# Engineered Magnetic Carbon-Based Adsorbents for the Removal of Water Priority Pollutants: An Overview

Authors: H. E. Reynel-Ávila; K. I. Camacho-Aguilar; A. Bonilla-Petriciolet; D. I. Mendoza-Castillo; H. A. González-Ponce; R. Trejo-Valencia
Journal: Adsorption Science & Technology
 (2021)

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## Abstract

This review covers the preparation, characterization, and application of magnetic adsorbents obtained from carbon-based sources and their application in the adsorption of both inorganic and organic pollutants from water. Different preparation routes to obtain magnetic adsorbents from activated carbon, biochar, hydrochar, graphene, carbon dots, carbon nanotubes, and carbon nanocages, including the magnetic phase incorporated on the solid surface, are described and discussed. The performance of these adsorbents is analyzed for the removal of fluoride, arsenic, heavy metals, dyes, pesticides, pharmaceuticals, and other emerging and relevant water pollutants. Properties of these adsorbents and the corresponding adsorption mechanisms have been included in this review. Overall, this type of magnetic adsorbents offers an alternative for facing the operational problems associated to adsorption process in water treatment. However, some gaps have been identified in the proper physicochemical characterization of these adsorbents, the development of green and low-cost preparation methods for their industrial production and commercialization, the regeneration and final disposal of spent adsorbents, and their application in the multicomponent adsorption of water pollutants.


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## Body

## 1. Introduction

Adsorption has been widely used for water and wastewater purification because of its significant benefits in terms of low cost, easy operation, limited energy consumption, selectivity, and flexibility for process design and scale-up [1, 2]. In this sense, several types of adsorbents have been prepared, characterized, and tested to remove both organic and inorganic pollutants from water. They include activated carbon (AC) [3], zeolites [4, 5], ion exchange resins [6, 7], clays [8], and alternative materials like hydrogels [9], polymers [10], and their composites, carbon nanomaterials (CNMs) [11, 12], metal oxides [13], and magnetic nanoparticles (NPs) [14]. All these adsorbents show different physicochemical and mechanical properties, adsorption capacities, as well as advantages and drawbacks for water treatment at industrial level.Functionalized nanomaterials have attracted increasing attention for advanced applications due to their outstanding properties (e.g., long-term stability, low toxicity, and high dispersion) [15]. Iron oxide nanoparticles (IONP) have special magnetic properties with different active sites that can be utilized in diverse applications in biomedicine and environmental fields [15, 16]. The direct application of IONP, especially as adsorbents in water treatment, implies some drawbacks that restrict their use such as leaching in low pH range, low structural stability due to oxidative conditions, their aggregation in the solution, and the significant mass loss in an equipment with continuous operation that implies water flow [15, 16]. Several studies have focused on the preparation of composites to provide more stability for magnetic phases using different substrates like carbon nanotubes (CNTs), graphene, mesoporous carbon-materials and AC [17], ion exchange resins [18, 19], zeolites [20], and polymers like chitosan [10].Therefore, the preparation of adsorbents employing carbon sources and iron has been found to offer several advantages for environmental remediation. Magnetic carbon-based materials are interesting due to magnetic metal particles incorporated on the material structure, chemical inertness, thermal stability, and electrical conductivity obtained from the carbon phase [11]. They have been introduced in various fields including catalysts, magnetic resonance imaging, drug/gene/RNA delivery carriers, energy storage, super capacitance, enzymes immobilization, adsorption, CO2 capture, and biosensors [11, 12]. A key characteristic of these materials is their easy recovery using an external magnetic field, which allows their application and handling in diverse operations.Magnetic carbon-based adsorbents are characterized by a magnetic source supported on the surface of carbon materials. These materials show a certain affinity for the separation/purification of a specific target substance and their magnetic properties facilitate different industrial tasks (e.g., deflection and mixing) [21]. The main advantage of this type of adsorbents is its easy recovery from fluid using magnetic decantation where the adsorbent is retained by the magnetic field. Therefore, the magnetic properties of adsorbents enable the use of alternative and intensified equipment (e.g., magnetically stabilized fluidized beds), thus, offering new alternatives for water treatment [21]. According to Mehta et al. [22], the use of magnetism for water purification dates to 1873 thus being an old concept. However, the attention of researchers on magnetic adsorbents has exponentially increased during the last decades. A basic search in Scopus using the phrase “magnetic AND adsorbent” generates a record of 1,284 papers published in 2020 where a considerable increment in the publications has occurred during the last decade thus accumulating more than 8,800 papers on this topic.A variety of carbon supports (or holders) can be used to prepare magnetic carbon adsorbents such as AC, biochar (BC), fullerenes, nanotubes, and other alternative compounds (e.g., nitro-phenol, polyurethane, yeast alcohol dehydrogenase, low-density polyethylene, acetate, acetylene, and oleates) [11, 12]. These materials can be produced from low-cost feedstock like agricultural orange peel waste [23], pinewood [24], chestnut shell [25], empty fruit bunch from palm [26], rice straw [27, 28], coconut shell [29], potato stems and leaves [30], and banana biomass [31].In this sense, the carbon-based feedstock and iron compounds can be utilized to prepare new composite materials thus taking advantage of their unique characteristics to obtain outstanding magnetic adsorbents with enhanced properties for the pollutant(s) removal in water treatment and other environmental applications [32, 33].With this in mind, this review focuses on the preparation of a number of carbon-based magnetic adsorbents from different routes and their application to remove priority water pollutants. Adsorbent properties and removal performance for the adsorption of several priority water pollutants (e.g., arsenic, pharmaceuticals, heavy metals, dyes, fluoride, pesticides, and radionuclides) are discussed and analyzed. Some research gaps and pending topics to be analyzed in future studies of these adsorbents are also outlined.


## 2. Sources of Carbon Materials Employed as Supports for Preparing Magnetic Adsorbents

Carbon is one of the most prevalent elements in nature with a significant scientific interest, and it is also one of the key components in organic molecules [34]. The carbon atoms can exist in different allotropic forms due to their orbital hybridization and electronic configuration, and they include fullerenes, graphene, CNTs, nanocapsules, carbon and graphene quantum dots, onions, or nanocages, which have their own physical and chemical properties. Figure 1 shows some allotropic forms of carbon [35]. Some of these carbon allotropes can be utilized as supports to prepare carbon-based composites but AC [36] and BC [25] are the most used. Each carbon allotrope has different structure, surface functionality, area, porosity, and physicochemical properties. One of the main features to select a carbon material is related to the particle size, and, in this sense, they can be classified arbitrarily into macroparticulated (e.g., BC, AC, and other nongraphitic carbon materials) and nanoparticulated (e.g., CNTs, carbon nanocages CNCs, and graphene). The most important characteristics of some carbon supports are described below.Figure 1
Description of the structure forms of carbon materials. Adapted from [35, 186–188].BC is a solid material rich in carbon that can be obtained from the biomass thermal decomposition, usually at lower temperatures than those commonly used for the preparation of other adsorbents, in total or partial absence of oxygen [24, 25, 37]. It mainly contains oxygenated functional groups (e.g., hydroxyl, carbonyl, and carboxylate) and has unique properties such as cation exchange capacity with a great potential to adsorb different water pollutants [37]. These characteristics depend on the biomass precursor and the methodology (i.e., preparation conditions) to obtain the BC.AC is essentially referred as a carbonaceous solid that has been treated to obtain a high surface area and to develop or to suppress specific surface functional groups in order of tailoring its chemical properties for specific applications [36, 38]. Its structure is amorphous and graphite-like form [38]. Generally, the physical activation to obtain AC includes the treatment of a char under CO2, steam flow, or other gas, while the chemical activation refers to the impregnation and/or surface functionalization of char/precursor with different reagents and compounds [36, 38]. Both physical and chemical activations contribute to develop specific porous morphology (i.e., surface area and pore network) and surface chemistry (i.e., surface functionalities like carbonyl, carboxyl, phenols, and lactones) [38, 39]. Consequently, the activation protocols can be optimized to obtain high porosity, surface area, adsorption capacity, mechanical strength, and physicochemical stability of the final product for the desired application at hand [38]. These properties are also determined by the nature of precursor and the technology utilized to obtain the adsorbent [36].On the other hand, graphene consists of sp2-hybridized carbons with a two-dimensional (2D) structure. This material is described as a free-standing single-layer carbon sheet with a hexagonally packed lattice structure with a theoretical specific surface area of ~2630 m2/g and outstanding electronic, thermal, mechanical, and optical properties [40–43]. This material offers a wide window for its surface chemistry modification, and, consequently, it has shown a promising performance as adsorbent of different water pollutants [42, 43]. Normally, the graphene oxide (GO) and its reduced form (RGO) can be prepared from graphite. GO is the main precursor of graphene [44]. It is soluble in water with low conductivity and contains a variety of oxygen functional groups due to the oxidation route of graphite to obtain GO, while RGO has a limited solubility in water but good conductivity [45]. The oxygen-containing functional groups of graphene are useful to anchor ions by both coordinate or/and electrostatic interactions [32, 44]. Therefore, GO has been widely applied in water pollution control. Nevertheless, the separation and recovery of graphene from the working medium are restricted by its high dispersibility in water, thus, leading to the generation of wastes that could be hazardous materials for the environment.CNTs consist of graphene sheets that are perfectly rolled into cylindrical tubes. They can be classed as single- and multiwalled carbon nanotubes (SWCNTs and MWCNTs) [46]. SWCNTs are classified in three crystallographic configurations according to the mode of graphene sheet is rolled up (i.e., chiral, armchair, and zigzag). Two opposite C–C bonds of each hexagon are parallel to the tube axis in the zigzag conformation, whereas the armchair conformation implies that the C–C bonds are perpendicular to the axis. In the chiral configuration, the opposite C–C bonds lie at an angle to the tube axis, thus, generating a so-called helical nanotube chiral [47]. Trojanowicz [48] stated that the CNTs have the simplest chemical composition and atomic configuration, but they can also show the most widely diversity of structures and properties. The thermal, electrical, and mechanical properties of these materials can be exploited in a variety of applications [49]. CNTs also exhibit excellent adsorption properties to bind various organic and inorganic adsorbates [49]. Moreover, the surface chemistry modification and sidewall functionalization of these materials allow their use as support phases to immobilize particles improving their performance as adsorbents in water treatment [49, 50].CNCs (or nanoshells) have 3D spherical structure consisting of a graphitic shell and hollow interior with high surface area [33]. In CNCs, the graphitic walls can isolate magnetic NPs from environment acting as a shield that avoids oxidation and ensures a long-term stability of the magnetic core [34]. CNCs have been applied in data storage, drug and gene delivery, catalysis, environmental remediation, and sensing due to their electrical and physical properties and geometrical structure [33, 51].Carbon quantum dots (CQDs) are a class of structures consisting of quasispherical carbon nanoparticles with sizes of ~10 nm [52]. They are mainly composed of sp3 hybridized carbon and are usually amorphous. CQDs are fluorescent due to the quantum confinement effect that allows to obtain optoelectronic and photoluminescent properties [52]. The color of CQDs turns to fluorescent light blue under UV light irradiation. However, the fluorescent properties of CQDs are also affected by the emitting properties of carbon precursor used as feedstock [53]. Graphene quantum dots (GQDs) are zero-dimensional structures, but they are composed by graphene nanosheets “cut” until reaching a size of < 20 nm [52, 53]. GQDs are mainly composed of sp2 hybridized carbon and have crystalline structure. Therefore, they are better recognized as graphene disks in the size range of 1-20 nm. Abbas et al. [52] have indicated that the main difference between the GQDs and graphene is their band gap values. Graphene is a zero-band gap material, while GQDs show band gap due to their quantum confinement and edge effects that generate fluorescence properties. CQDs and GQDs are interesting materials for semiconductors, light-emitting diodes, detection of heavy metal ions, and wastewater treatment as catalysts or adsorbents. These materials are characterized by their high stability, biocompatibility, low toxicity, high dispersibility in water, photostability, and low manufacturing cost [53].Overall, all these carbon-based materials can be used to prepare magnetic adsorbents for water treatment. In the next section, an overview of the synthesis of magnetic carbon-based adsorbents is provided.


## 3. Synthesis of Magnetic Carbon-Based Adsorbents

The most common metallic NPs utilized to prepare magnetic materials are nickel, cobalt, and iron [12, 34]. Nevertheless, the iron compounds are commonly utilized due to their low cost and magnetic characteristics [12]. Siddiqui et al. [12] have reviewed the main sources of iron and they comprise ferrous sulfate FeSO4, ferric nitrate Fe(NO3)3, ferric oxide Fe2O3, ferrous ferric oxide Fe3O4, ferric chloride FeCl3, and iron ores like magnetite and maghemite. As mentioned by Meng et al. [23], the iron compounds display numerous advantages: they can be used to modify supports at low temperatures (around 180 °C), they have low toxicity for ecosystems and human health thus being safe and environmentally friendly, and they also offer physical stability to supports and good magnetic performance. These characteristics can be exploited in water purification and treatment.Several methods have been used to synthesize magnetic carbon composites (CCs), and, practically, each synthesis route applies more than two stages for obtaining the final material. These preparation protocols can vary according to the carbon source nature, but all approaches generally include the impregnation with iron salts and chemical coprecipitation of IONPs. In this section, the conventional synthesis methods besides recent advances for the preparation of magnetic carbon-based materials are analyzed.


### 3.1. Magnetic Versions of Activated Carbon (AC), Biochar (BC), and Hydrochar (HC)

Generally, various stages are necessary to produce magnetic AC and BC. First, the carbonization of precursor is required, and it can be performed by traditional pyrolysis or hydrothermal method. In a second stage, the impregnation with iron phases in liquid phase is performed to modify AC or BC. Alternatively, the iron salts can be mixed with a carbon-precursor and then the carbonization step is carried out.In the direct synthesis, an impregnation stage is required where the support precursor (e.g., a lignocellulosic biomass) is mixed with iron salts or iron phases; then, the pyrolysis or hydrothermal stage is performed for obtaining magnetic BC or HC. Otherwise, the first stage of an indirect synthesis is the precursor carbonization, and, once BC or HC has been obtained, the second stage consists of the impregnation of carbon-based material with a magnetic phase of iron oxides for finally obtaining magnetic BC or HC. These procedures are illustrated in Figure2(a).Figure 2
General steps for the preparation of: (a) magnetic hydrochar (HC) and magnetic biochar (BC) by direct or indirect synthesis and (b) magnetic activated carbon (AC) by direct or indirect synthesis.
(a)(b)The direct synthesis of magnetic AC implies the addition of chemical substances during impregnation stage and the activation in the subsequent stage of carbonization by hydrothermal treatment or pyrolysis, as shown in Figure2(b). Note that the production of magnetic AC by indirect synthesis relies on the activation stage that can be performed after carbonization by chemical and/or physical pathways and then followed by the impregnation to incorporate magnetic species. A relevant advantage of the synthesis of AC, HC, and BC, as carbon-based supports, is the use of low-cost raw materials as precursors. In this sense, researchers have prepared AC and BC using biomass sources with noncommercial value like orange peels [23], chestnut shell [25], empty fruit bunch from palm [26], and rice straw [27]. Also, alternative carbon sources like industrial and urban residues (e.g., Tetra pack, PET bottles, and tires) can be utilized to obtain these carbon supports [54–56]. Once the precursor for the carbon matrix preparation has been selected and acondicionated (this stage generally includes washing, particle size reduction, and pretreatment), the carbonization stage is the next step. Note that several methods for biomass carbonization can be chosen and some of them are discussed below.Pyrolysis involves the formation of a low-developed porous solid matrix (usually called as char) where the precursor is submitted to a thermal treatment without oxygen at temperatures from 600 to 1000 °C. This char can be also obtained via thermal treatment under the presence of oxygen, and this process is commonly referred as carbonization [57, 58]. For BC and char production, pyrolysis or carbonization is the only stage employed in the preparation route, but an additional activation stage is needed for obtaining AC, which can involve the use of different reagents. For instance, an oxidizing gas like CO2 or steam at 600-1200 °C can be utilized to promote the formation of a well-developed pore structure [57, 58].On the other hand, the hydrothermal carbonization (HTC) is the thermochemical conversion process that transforms biomass under the presence of pressurized water (at subcritical conditions) into a carbon-based material usually referred as HC (i.e., hydrochar) [59]. This process is regarded as a green route to prepare new materials from biomasses and other feedstocks in a closed reactor or autoclave under the presence of water at low temperatures (150-250 °C). HTC offers some advantages in comparison to the conventional thermal treatments because not only helps to generate a surface area rich in functional groups but it also implies a reduced energy consumption and low-cost. Raw HC obtained at common operating conditions has a low specific surface area (<100 m2/g) but contains a significant amount of oxygenated functionalities if water is the reaction medium to prepare this adsorbent [23, 60–63]. For example, Cai et al. [64] reported the preparation of a magnetic BC for chromium adsorption using peanut shells, deionized water, hexamethylenediamine, and FeCl3•6H2O. The adsorbent was obtained via HTC at 220 °C for 12 h. The maximum adsorption capacity of this magnetic material was 142.86 mg/g and could be reused in 3 removal cycles. Figure 3 illustrates the methodology used to produce magnetic BC from peanut shell [64]. Note that HC with high surface area and porosity can be prepared if a postactivation step is performed.Figure 3
HTC used to prepare magnetic adsorbents for Cr (VI) removal from aqueous solution [64].Herein, it is convenient to highlight that alternative technologies can be utilized to prepare the carbon-based support, and they include the application of microwave and plasma [26, 58, 65]. For instance, the main objective of microwave-assisted pyrolysis is to reduce the preparation time and to enhance the adsorption properties of the solid matrix [58]. In microwave instruments, the precursor pyrolysis/carbonization and adsorbent activation can be carried out. This technology offers a heating process that is uniform, thus, it is feasible to homogenize the bulk properties of the final product [58]. Microwave power and radiation time can impact on the char textural parameters like surface area and pore volume [66].As indicated, another important stage is the impregnation with magnetic salts for conferring magnetic properties to BC, AC, or HC. This task can be performed via:(1)
The nonmagnetic iron oxides (i.e., hematite and goethite that can be transformed in magnetic phases) or iron salts can be mixed with the carbon precursor, before its carbonization, in the aqueous solution at a given temperature and time to ensure its impregnation. The impregnated precursor can be carbonized to obtain directly the magnetic adsorbents(2)
Char or AC can be mixed with the magnetic salts in an aqueous solution following the next alternatives for the support impregnation: (1) with a chemical synthesis of magnetic iron oxide using, for example, sol-gel, or coprecipitation methods; and (2) with magnetic iron oxides already synthesized by thermal decomposition, chemical reduction, sol-gel, or coprecipitation. A detailed description of each approach can be found in the interesting review of Noor et al. [58]The final magnetic material could acquire different structural, chemical, and physical characteristics depending on the preparation conditions. For instance, the precursor (biomass or other carbon source), temperature, and impregnation ratio could have a significant impact on the final adsorbent properties. Figure4 illustrates three examples for the preparation of magnetic adsorbents with different methods and stages.Figure 4
Preparation of magnetic biochar (BC) and hydrochar (HC) using several methods: (a) gelatin modified-magnetic BC [25], (b) magnetic BC by direct pyrolysis [24], and (c) dendrimer-like magnetic HC by direct hydrothermal carbonization [23]. Additional information for the magnetic iron oxides preparation can be found in Noor et al. [58].
(a)(b)(c)


### 3.2. Magnetic Graphene-Based Materials

GO and RGO are other preferred carbon matrices to prepare magnetic adsorbents. They have been considered as better graphene derivative nanomaterials than pure graphene, and, compared to raw or commercial chars, they offer high surface areas for the adsorbent preparation. However, these nanopowder adsorbents can aggregate easily in a liquid-phase thus making difficult their separation from aqueous media where additional steps (e.g., centrifugation and granulation by binder) are needed [29]. Magnetic modification is an alternative solution for the recovery and reuse of those materials. For this purpose, magnetic forms of graphene-based materials can be prepared first by GO or RGO synthesis and then modified with magnetic NPs (usually iron oxides).In general, GO and RGO can be obtained by several synthesis methods such as mechanical cleaving (exfoliation), chemical exfoliation by oxidation, chemical synthesis, arc discharge, and thermal chemical vapor deposition (CVD) [67–70]. However, the most usual method to prepare magnetic form of GO or RGO is the exfoliation by oxidation of graphite flakes with the direct or indirect Hummers-Offeman procedure [71]. There is also an alternative method that consists in biomass carbonization with specific reagents to promote graphitization and to obtain graphene-like carbon nanosheets [72, 73]. An overview of graphene-based preparation methods is given in the next subsections.


#### 3.2.1. Magnetic GO and RGO Synthesis by Graphite Oxidation Method (GOM)

Basically, the chemical exfoliation is a top-down method where the graphite precursor in solution is exfoliated by incorporating large alkali ions between the graphite layers [74]. Herein, it is convenient to remark that the main method to obtain GO implies a mixture of powdered flake graphite, sulfuric acid, and sodium nitrate, which is cooled at 0 °C with an ice-bath. Potassium permanganate should be carefully added to the mixture under vigorous agitation, preventing that the temperature can exceed 20 °C. Then, the temperature is increased to 35 °C and maintained for 30 min. After this period, water is added and slowly stirred thus causing a violent effervescence and a final temperature of ~98 °C. The diluted color brown suspension is maintained at this temperature for 15 min, and warm water is used to dilute the suspension. Hydrogen peroxide is utilized to reduce the residual permanganate and manganese dioxide to colorless soluble manganese sulfate. This hydrogen peroxide treatment causes that the suspension turns bright yellow, which is a characteristic of GO [71]. RGO can be prepared from GO applying an additional method for reduction that can be carried out by chemical or physical routes [44]. Chemical reagents such as hydrazine hydrate [44], NH3 [75], and L-ascorbic acid [76] have been employed for the chemical reduction of GO. On the other hand, the physical reduction can be performed via thermal reduction [44], hydrothermal reduction [77], and microwave-assisted reduction [78].Magnetic GO or magnetic RGO can be obtained from the corresponding graphene precursor with different methods to modify its structure for preparing the magnetic composite. The most conventional procedure consists of the material impregnation with IONPs at given time and temperature. Figure5 provides the general procedure for obtaining magnetic versions of GO and RGO.Figure 5
General steps for the preparation of magnetic graphene oxide (GO) and magnetic reduced graphene oxide (RGO) by GCEM.Some variations in GO production and its postimpregnation for magnetic modification have been developed by several researchers. Specifically, a magnetic graphene/iron oxide composite for the uranium removal was prepared by Zong et al. [79]. GO synthesis was done with a modified Hummers and Offeman method where 500 mL of H2SO4 solution, 4 g of graphite, and 3 g of NaNO3 were mixed. This suspension was stirred in an ice-water bath, and 18 g of KMnO4 was slowly added during 2.5 h. The mixture was stirred for 5 days at <25 °C and 560 mL of 5 wt% H2SO4 was added dropwise for 2.5 h and stirred at 98 °C. The temperature decreased to 55 °C, and 12 mL of H2O2 (about 30 wt%) was also added dropwise and then stirred for 2.5 h at room temperature. The mixture was centrifuged for 20 min at 19,000 rpm, the liquid and solid phases were separated with bath sonication and potent stirring, and the final product was washed with distilled water. Magnetic GO was obtained by impregnation using 0.50 g of GO and a 300 mL container with 0.58 g FeCl2·4H2O (i.e., Fe2+ : Fe3+ molar ratio of 1 : 2) and 1.56 g FeCl3·6H2O. An ammonia solution (28 wt%) was slowly added, adjusted the pH at 10.5, and stirred for 8 h at 90 °C. The final black solution was filtered and washed with distilled water until obtaining a pH 7 in the filtrated solution. Besides, Ghorbanian et al. [80] reported the synthesis of a magnetic nanocomposite with GO and a chitosan matrix functionalized with 1,5-diphenylcarbazone (DPC) and magnetite for lead extraction from water. GO was prepared with a modified Hummers and Offeman method where graphite powder was poured into a 9 : 1 mixture of concentrated H2SO4/H3PO4 (360 : 40). KMnO4 was slowly added to the mixture, and it was heated up to 50 °C and stirred for 24 h, and the final temperature was decreased to room temperature. 400 mL of pure ice and H2O2 (30%, v/v) was added to this mixture. GO was washed with water, centrifuged, and dried at 60 °C. Acylated GO was obtained from GO and dried SOCl2 with reflux at 70 °C for 24 h. Anhydrous dimethylformamide was used to wash this mixture and then dried. Toluene and GO-Cl were mixed by sonication, and DPC was added to the solution, the mixture was heated and refluxed for 24 h, rinsed with methanol, and dried at room temperature to obtain GO-DPC. Acetic acid solution (2% v/v) was used to dissolve chitosan in an ultrasonic bath to generate a homogeneous solution for magnetic modification. Chitosan solution and magnetic NPs were stirred for 2 h to obtain a uniform suspension. GO-DPC was added to a reaction flask with 15 glutaraldehyde, the mixture pH was adjusted at 9.5 by drop wise of 0.1 mol/L NaOH, and the solution was maintained at 80 °C for 1 h. The magnetic composite was collected by the magnet, washed with double-distilled water and ethanol to neutral pH, and dried at 50 °C.It is important to remark that GO is more suitable than RGO for adsorption applications, but some researchers have carried out some experiments to remove water pollutants. As example, magnetic GO and RGO prepared by annealing reduction at 500 °C under N2 (magnetic annealing-RGO) and by chemical reduction with hydrazine hydrate (magnetic chemically-RGO) were studied by Huang et al. [44]. Magnetic GO was the best adsorbent with competitive adsorption capacities of tetracycline, Cd2+, and As5+ due to its oxygenated functional groups.


#### 3.2.2. Production of Pseudographene by Biomass Carbonization Method (BCM)

Biomass is a renewable carbon-containing source available worldwide [81]. According to Wang et al. [81], the global production of biomass is estimated in 146 billion tons, which is generated as residue by industry, agriculture, forestry, and other sources. Therefore, several studies have used biomasses as inexpensive raw materials with the aim of solving environmental pollution problems. The development of biomass-based CNMs implies an important effort to contribute to the science progress. However, the use of biomasses to prepare high performance CNMs is still challenging due to its high oxygen content, strong chemical bonding, and complex structure [81]. Several methods for preparing CNMs from biomasses have been studied including CVD (in situ and two-stage), pyrolytic transformation (e.g., thermo-chemical activation, catalytic graphitization, and catalytic graphitization coupled with thermo-chemical activation), mechanical activation, cyclic oxidation, combustion, and microwave-assisted pyrolysis [58, 81]. A comprehensive discussion of these methodologies is given in the reviews of Noor et al. [58] and Wang et al. [81].Particularly, the pyrolytic transformation by catalytic graphitization is the most used method to obtain pseudographene [81, 82]. Conventional graphitization is a type of pyrolysis that requires graphitizable precursors and is carried out at high temperature (>2000 °C), which increases the process cost and security risks thus limiting its industrial scalability [82]. As an alternative method, the catalytic graphitization is a simple strategy consisting of the precursor carbonization using transition metals as catalysts [82]. This process allows that graphitizable and nongraphitizable carbon materials can be converted into crystalline materials at temperatures <1000 °C and, consequently, thus reducing the energy consumption and costs [82]. Figure 6 shows some routes to prepare CNMs [81]. Basically, the modification technique to obtain magnetic materials consists of a biomass (carbon precursor) pretreatment and its impregnation with an activating agent and/or catalyst and the final carbonization via conventional or nonconventional methods. The use of metals from group 4-7 (e.g., Fe, Co, Ni, and Mn) contributes to the conversion of amorphous carbon to graphitic carbon via the reduction of the corresponding activation energy. In fact, they are ideal as graphitization catalysts due to their 2-5 electrons in the d-shell orbitals that allow the formation of strong bonds between carbon-based materials and metal carbides [81]. Some examples of BCM routes are described below.Figure 6
Preparation of carbon nanomaterials from biomasses [81].Graphene-like nanosheet materials with high surface area can be prepared from simple BCM route using coconut shell, FeCl3 and ZnCl2 as carbon precursor, graphitic catalyst precursor, and activating agent, respectively [72]. ZnCl2 and coconut shell were mixed in a 3 M FeCl3 solution, and the impregnation was performed by evaporation at 80 °C for 2 h under stirring and a final drying at 100 °C. The activation and graphitization of the coconut shell were performed at 900 °C for 1 h with N2 atmosphere in a tubular furnace. Magnetic composites were prepared at 800 and 1000 °C forming the magnetic species CFe3 and α-Fe. Moreover, sugar has been used as a carbon precursor to prepare magnetic graphene-like nanosheets for U6+ adsorption [73]. The disaccharide sugar was slowly heated at 200 °C for 1 h under N2 flow in a furnace to achieve its caramelization. The furnace temperature was increased to 750 °C within 1 h and then maintained for 3 h to convert caramel to inorganic carbon. The pyrolyzed sugar was milled, and the final powder was utilized as a sugar-based pseudographene carbon. The oxidized pseudographene form was prepared using a treatment with ozone in water at rate of 5 g/h for 1 h and sonication, and the final product was washed with deionized water and dried at 80 °C for 8 h. The magnetic phase impregnation was done with a fast in situ synthesis of magnetite where a solution of FeCl3·6H2O and FeCl2·4H2O (2:1 molar ratio of Fe3+:Fe2+) was dropwise added into oxidized pseudographene sample at room temperature under vigorous stirring and N2 purging. Solution pH was adjusted to ≥10 and maintained at 80 °C for 1 h with continuous stirring where a black precipitate was formed. The final product was washed, separated with an external magnetic field, and dried at 60 °C for 12 h under vacuum.


#### 3.2.3. Magnetic Carbon Nanotubes (CNTs)

CNTs are also nanomaterials utilized to prepare magnetic adsorbents. A number of methods has been reported for the preparation of magnetic iron oxide/CNTs composites by routes that firstly include the preparation of CNTs (e.g., CVD, arc discharge, and vapor phase growth) [83] and the subsequent modification with MNPs using sol–gel [84], solvothermal [85], reverse microemulsion [86], hydrothermal [87, 88], high-temperature decomposition [89], or coprecipitation method [90–92].For CNTs synthesis, the CVD is the most conventional method where a carbon precursor, catalyst and growth promoter are usually needed. As example, MWCNTs can be prepared via catalytic CVD of hexane using magnesium/iron layered double hydroxide as catalyst precursor [90]. MWCNTs were purified with a 3 M HNO3 solution at room temperature for 24 h, filtered and washed with distilled water. H2SO4/HNO3 mixture (3 : 1 v/v) and sonication were applied to activate MWCNTs at room temperature. 0.05 M Fe(NO3)3 solution and activated MWCNTs were mixed under stirring, and, subsequently, an ammonia solution (2.5 wt.%) was slowly added until reaching pH 9.5. Filtration and washing with distilled water were used to obtain the final product that was dried at 100 °C for 12 h. Finally, MWCNTs-IONPs were obtained via an annealing at 500 °C for 1.5 h under Ar flow.Typically, hydrocarbons are sources for CNT synthesis; nevertheless, some studies employed alternative precursors in order to propose a green synthesis. Ma [93] prepared SWCNTs by spray pyrolysis with ethanol (carbon precursor), ferrocene (catalyst), and thiophene (growth promoter). Thiophene and ferrocene were dissolved in ethanol by sonication, and the final solution was employed in spray pyrolysis. A tubular furnace with a quartz tube was heated at 1000-1150 °C under Ar flow. The mixture (ethanol-ferrocene-thiophene) was sprayed through a nozzle to the furnace and pyrolyzed, and the final sample was collected. For purification stage, the pristine sample was heated at 400 °C in continuous oxygen flow to oxidize iron NPs, and the oxidized sample was further heated at 800-900 °C for 1 h under Ar flow and exposed to 12 M HCl treatment at 100 °C for 4 h. The final product was filtrated and washed until obtaining a neutral pH.Ma et al. [17] reported the application of arc discharge evaporation of a carbon electrode with an iron catalyst to obtain SWCNTs. This synthesis was done using two electrodes that were located in the center of a water-cooled stainless-steel chamber. Pure graphite-rod and graphite-rod containing 4 wt% of iron catalyst were the cathode and anode, respectively. The direct current arc discharge was obtained with 120 A in a gas mixture of Ar and H2. After 30 min of arc evaporation, ~500 mg of iron NPs- SWCNTs was obtained. The product was heated at 350 °C for 6 h in air to oxidize iron NPs and to remove the amorphous carbon.Once CNTs have been obtained, a modification and/or functionalization stage is necessary to obtain magnetic CNTs. Note that interesting purification and modification methods for magnetic CNTs preparation have been reported. For instance, commercial MWCNTs can be functionalized with dibenzo-18-crown-6 moieties for amoxicillin adsorption [87]. The partial oxidation and impurity removal of MWCNTs were done by dispersion in concentrated HNO3 at 130 °C for 30 min. For the magnetic modification stage, the pretreated MWCNTs were added to a mixture obtained from ammonium iron sulfate hexahydrate dissolved in water and a hydrazine hydrate solution. This suspension was stirred and sonicated, and the solution pH was adjusted to 11-13 and refluxed at boiling point for 2 h. Filtration and washing of magnetic MWCNTs were done with water and ethanol, and the product was dried for 24 h under vacuum. Ethanol was used to disperse magnetic MWCNTs and sonicated for 10 min to do the crown-functionalization. This system was mixed with a dicyclohexylcarbodiimide ethanolic solution, stirred for 10 min and, finally, a solution of 4,4’-diaminodibenzo-18-crown-6 was added to the mixture, which was stirred at room temperature for 24 h. The final products were washed with water and dried for 12 h under vacuum.In addition, magnetic MWCNTs were prepared to remove As5+ and As3+ from water [91]. Commercial MWCNTs were treated with HNO3 solution (70%) at 70 °C for 12 h to incorporate oxygenated functionalities with the aim of increasing their affinity for the IONPs. Fe3+/Fe2+ solution (molarratio=2) and oxidized MWCNTs were mixed by ultrasonication for 4 h. Then, the magnetic material was obtained via the addition dropwise of a 6 M NaOH solution until reaching pH 8. In a recent study, magnetic MWCNTs were embedded in a hydrophilic polyvinylidene fluoride (PVDF) membrane for the adsorption of As3+ [50]. First, copper-ferrite was obtained from the dissolution of ethylene glycol, FeCl3, CuCl2·2H2O, polyethylene glycol, and sodium acetate. This mixture was heated up for 8 h at 200 °C using a teflon-lined autoclave and cooled to room temperature. The substrate for MWCNTs membrane preparation was a flat-sheet PVDF membrane. Specifically, 12 mg of MWCNTs was mixed with 30 mL of pure water, and this mixture was added to the PVDF membrane where CuFe2O4 particles were dispersed in water, sonicated, and then injected onto the CNT membrane.It is important to mention that in several papers related to the use of CNTs as supports to prepare carbon-based adsorbents, CNTs were purchased (i.e., they were available commercial products), and a modification step was used to obtain the adsorbent [87, 91]. Only few studies have reported the CNTs synthesis [17, 93] because this step could be expensive, and CNTs are difficult to obtain in laboratory with a suitable quality and reproducible properties.


#### 3.2.4. Magnetic Carbon Nanocages (CNCs)

CNCs have interesting applications in energy and environmental protection [33]. They can be utilized to prepare hybrid nanomaterials with multifunctional properties [33]. Currently, various synthesis routes have been reported to prepare CNCs including pyrolysis of organic precursors and sol-gel method, CVD, templating by using different metal particles, and arc discharge [94]. However, these approaches have used pyridine, ethanol, and acetylene as carbon sources, which are unsustainable and expensive due to the use of fossil precursors [94]. Therefore, the utilization of porous carbon materials obtained from biomass precursors is an alternative employing pyrolysis, HTC, template-directed synthesis (soft, hard, and dual template), and direct synthesis. Biomass graphitization was proved to be promising to obtain CNCs structures, especially, for environmental applications [94].A low-cost, simple, and environmentally friendly method to prepare magnetic CNCs, with multiform pore structure, from the lignin carbonization at low temperature was reported by Qin et al. [94]. They prepared CNCs with lignin, NaOH, formalin solutions, and Fe(NO3)2·9H2O. A conventional pyrolysis was carried out at 600 °C for 3 h, and the final material was used for methyl orange adsorption.Cho et al. [95] synthesized magnetic CNCs using sugar as carbon precursor, and this material was applied for methylene blue adsorption, see Figure 7. Magnetic NPs were soaked in a sugar solution for 30 min with a sugar/magnetite ratio of 1 : 2, then, the water was vaporized under magnetic stirring at 85 °C for 120 min. The dried and impregnated sugar compound was pyrolyzed at 500 °C for 30 min in a tubular reactor. The final adsorbent showed a methylene blue adsorption capacity of 52.6 mg/g.Figure 7
Preparation of novel magnetic CNC adsorbent via pyrolysis of sugar for methylene blue adsorption in aqueous solutions [95].Zuo et al. [96] proposed a green protocol to synthesize magnetic CNCs that were modified with diethylenetriamine (DETA) and gold using glucose as carbon source where the final adsorbent was applied in the adsorption of methylene blue from aqueous solution. CNCs were synthetized via the HTC of the glucose solution at 180 °C for 3 h. CNCs were treated with ethanol and DETA and, finally, impregnated with Fe3O4 NPs diluted in chloroform/ethanol solution at room temperature for 24 h under stirring. A solution of ethylene glycol/water was mixed with the black solid product where a HAuCl4 solution was dropwise added and stirred at room temperature for 1 h. Finally, NaBH4 solution was added to this mixture and stirred for 2 h under N2 atmosphere to obtain the final magnetic product.Petala et al. [33] also reported a green one-step and simple method to prepare magnetic CNCs from pine resin, iron nitrate impregnation, and pyrolysis at 1000 °C. The morphology, textural, and surface properties of magnetic CNCs were analyzed with surface, spectroscopic, and microscopic techniques. Results indicated that the magnetic CNCs presented a homogeneous distribution of core-shell-type magnetic NPs within the carbon matrix where the surface area was 177 m2/g with both micropores and mesopores. These magnetic CNCs showed an adsorption capacity of 263.9 mg/g for the removal of As3+ from aqueous solutions at pH 7.A low-cost and easily scalable method was proposed by Rudakov et al. [34] to obtain magnetic CNCs via the simple thermolysis of precursors based on a mixture of citrate acid and transition metal (nickel, cobalt, or iron) acetate salts. The effect of thermolysis temperature (in a range of 500-850 °C) on magnetic CNCs structural properties was studied. The theory of Ostwald ripening, Arrhenius law for diffusion, and instrumental characterization were used to analyze the thermal dependence of the particle size. Superparamagnetic characteristics were observed for nickel samples annealed at <700 °C. CNCs prepared with cobalt at 600 °C showed higher saturation magnetization than CNCs with nickel, while iron nanoparticles were larger than those of cobalt and nickel thus showing ferromagnetic behavior.


#### 3.2.5. Magnetic Carbon Quantum Dots (CQDs) and Magnetic Graphene Quantum Dots (GQDs)

The synthesis of CQDs and GQDs usually involves at least 2 stages. First, it is necessary to obtain the quantum dots and then the corresponding magnetic properties are developed in the second stage [52]. Some authors have reported the functionalization of material surface to add functional groups that can interact with a specific adsorbate. CQDs and GQDs can be prepared from various natural carbon sources, but citric acid is the most common one because it consists of carbonyl, carboxylic, and hydroxyl groups [52]. However, other available and low-cost raw biomasses with similar chemical composition can be employed to prepare CQDs and GQDs [52].Chemical structure, quantum size, and photo-luminescent properties of these materials depend on the feedstock chemical structure and the preparation route [52]. The next examples describe interesting synthesis methods to obtain magnetic CQDs and GQDs. For instance, a typical procedure to prepare CQDs employs a mixture of citric acid, dicyandiamide, and water, which is agitated until a clear solution is obtained [97]. This solution is transferred to a stainless autoclave and heated to 160 °C for 4 h. The final product is collected and centrifuged. The magnetic composite can be obtained by coprecipitation where CQDs are dispersed in deionized water by sonication and mixed with FeCl3·6H2O solution at room temperature under N2 flow with vigorous stirring. The temperature is increased up to 80 °C, and FeCl2·4H2O is slowly added to the solution containing Fe3+/CQDs and stirred for additional 30 min. Finally, ammonia is added dropwise to adjust the solution pH at 10. The black precipitate can be magnetically separated and washed several times and, subsequently, dried at room temperature [97]. On the other hand, Tadesse et al. [98] proposed a hydrothermal method to prepare nitrogen-doped magnetic CQDs using lemon juice and ethylenediamine. These reagents were mixed and heated at 200 °C for 3 h to obtain a black paste, which was washed with water to remove insoluble matter. Dichloromethane was added to obtain a brown solution, and a coprecipitation reaction was employed for the magnetic impregnation where metallic salts of Fe3+/Fe2+ and CQDs were mixed in aqueous solution. NaOH was added drop wise to this system, and the final product was a magnetic CQDs soluble in water. Recently, Nuengmatcha et al. [99] reported magnetic mercapto-functionalized GQDs for Cd2+ adsorption. GQDs were prepared using citric acid (2 g) heated at 260 °C where 100 mL of 0.25 M NaOH was added when the color changed to yellow. Maghemite was the magnetic phase and produced by mixing 5 g of FeCl3·6H2O, 2.5 g of FeSO4·7H2O, and deionized water. Subsequently, 20 mL of 28% NH4OH was added, and the solution was heated at 80 °C for 30 min under N2 atmosphere. GQD solution was mixed with maghemite, and this suspension was heated at 80 °C for 30 min, washed with deionized water, and dried at 90 °C. Magnetic GQDs were modified with C2H5OH and H(CH2)Si(OCH3)3. Kahrizi et al. [100] also reported a similar procedure to prepare magnetic GQDs combined with hydroxyapatite for Cd2+ adsorption.


### 3.3. Magnetic Carbon-Based Adsorbents Prepared from Low-Cost Feedstocks

One advantage of magnetic carbon-based adsorbents is the possibility of using a wide variety of carbon supports (or holders). However, the preparation and regeneration of adsorbents based on CNTs, graphene, and fullerenes as template are relatively difficult and expensive thus limiting their application at industrial scale [101]. The preparation of carbon materials via simple and low-cost procedures is highly desirable to reach the scale-up and commercialization of magnetic adsorbents [101]. The use of low-cost feedstocks is an alternative to achieve this target. It is necessary to apply raw materials that are abundantly available in nature or produced as by-product and wastes in agro-industrial and other processes. Examples of low-cost feedstocks for the preparation of carbon-based materials include biomasses and urban wastes such as chestnut shell [25], rice straw [27], banana peel [31], pomelo peel [101], rubber tires [102], Tetra pak residues [55], and sewage sludge [103, 104]. AC, BC, and other carbon-based supports can be obtained from the processing of these wastes via thermal decomposition (e.g., via pyrolysis or HTC) to prepare suitable adsorbents.For example, a magnetic AC derived from the carbonization of waste rubber tires and iron impregnation was combined with polyethylenimine to prepare an adsorbent for the removal of methyl red in batch and column experiments [102]. This adsorbent showed a strong dye affinity due to the abundance of hydroxyl and amine groups with an adsorption capacity of 526 mg/g in batch conditions and a breakthrough time of 150 min. This dye adsorption process was also exothermic. Huang et al. [101] synthesized a magnetic adsorbent using pomelo peels as precursor. This biomass is considered as inedible to humans and is discarded in landfills. These authors proposed a one-pot synthesis method to obtain a magnetic material with a core-shell structure to adsorb apolar parabens and nonpolar fluoroquinolones. This adsorbent showed a competitive removal for both compounds. Also, Deng et al. [105] reported a hybrid magnetic adsorbent obtained from carbon dots and CNTs for carbamazepine removal. Specifically, carbon dots were prepared via HTC of a mixture of diaminoethane, citric, and nitric acids. Magnetic CNTs and carbon dots were mixed in a rotovapor to prepare this adsorbent, which showed an adsorption capacity of 65 mg/g at pH 7. Carbamazepine adsorption was fast and achieved 80% removal within the first 3 h of contact time. This adsorbent was easily separated and was regenerated up to 6 times with a capacity loss less than 2.2%Herein, it should be pointed out that the compounds used to confer magnetic properties in an adsorbent can be also obtained from low cost materials such as urban and industrial wastes (e.g., sewage sludge) [104]. One illustrative example is the iron salts utilized in anaerobic biological wastewater treatment system [104] and chemical precipitation [106]. Sewage sludge contains high amounts of iron species that can be converted to iron oxides with both magnetic and adsorption properties [103, 104]. For instance, a magnetic alkali-acid adsorbent was prepared via the pyrolysis of municipal sewage sludge (containing polyferric sulfate) for the tetracycline removal [103]. Results showed an adsorption capacity of 286 mg/g where the preparation method affected the adsorption properties of this material. Tetracycline adsorption was dominated by π-π stacking interaction and strong pore filling effect. Another interesting example is the application of electric arc furnace dust to prepare magnetic adsorbents for water treatment [107]. This material contained a significant amount of iron (37%) and is generated as by-product from steel industrial sector.


### 3.4. Techniques for the Characterization of Magnetic Carbon-Based Adsorbents

It is important to highlight that the use of instrumental techniques for adsorbent characterization provides key and useful results for understanding the structures and mechanisms involved in the adsorbent preparation route as well as the interactions adsorbate-adsorbent and material performance. The use of these instruments is essential to validate the synthesis routes and analyze the surface chemistry changes of adsorbent after its application to explain its adsorption properties and mechanisms. For the characterization of magnetic adsorbents, there are several techniques that can be used:(1)
Surface chemistry, structural, and morphology characterization using Fourier Transform Infrared Spectroscopy (FTIR), X-Ray Diffraction (XRD), N2 adsorption/desorption isotherms, X-ray Photoelectron Spectroscopy (XPS), High Resolution Transmission Electronic Microscopy (HRTEM), and Transmission Electronic Microscopy (TEM)(2)
Magnetic properties measurement with Vibrating Sample Magnetometry (VSM) and Mössbauer Spectroscopy (MS)In particular, the electronic microscopy provides important and useful information for understanding the adsorbent performance by (1) analyzing their morphology and chemical composition and (2) studying the specific structures and textures such as the arrangement and dimensions of aromatic layers and interlayer spacing [108]. FTIR analysis gives valuable information about the main surface functional groups, and XRD analysis contributes to study the crystalline structure, while MS is employed to determine oxidation states, electronic spin-state, coordination number, and environment for coordinating compounds. It is convenient to indicate that if iron compounds are analyzed, then the technique is known as Iron-57 Mössbauer Spectroscopy [109–111]. XPS helps to identify the functional states of elements and their chemical bonds on the adsorbent surface [112]. N2 adsorption/desorption isotherms give information about the adsorbent textural parameters (i.e., surface area, porosity distribution, and pore volume) [113]. Magnetometry measures the magnetic properties like magnetic moment, permeability, and saturation magnetization. Each instrumental method provides relevant, comparative, and complementary information about the magnetic adsorbents. Based on the fact that the carbon precursor and adsorbent synthesis method generate the possibility to obtain a wide spectrum of materials, the physicochemical properties of magnetic adsorbents can vary substantially. Therefore, a proper and detailed characterization of these adsorbents is fundamental to explain their performance in water treatment and other applications.


## 3.1. Magnetic Versions of Activated Carbon (AC), Biochar (BC), and Hydrochar (HC)

Generally, various stages are necessary to produce magnetic AC and BC. First, the carbonization of precursor is required, and it can be performed by traditional pyrolysis or hydrothermal method. In a second stage, the impregnation with iron phases in liquid phase is performed to modify AC or BC. Alternatively, the iron salts can be mixed with a carbon-precursor and then the carbonization step is carried out.In the direct synthesis, an impregnation stage is required where the support precursor (e.g., a lignocellulosic biomass) is mixed with iron salts or iron phases; then, the pyrolysis or hydrothermal stage is performed for obtaining magnetic BC or HC. Otherwise, the first stage of an indirect synthesis is the precursor carbonization, and, once BC or HC has been obtained, the second stage consists of the impregnation of carbon-based material with a magnetic phase of iron oxides for finally obtaining magnetic BC or HC. These procedures are illustrated in Figure2(a).Figure 2
General steps for the preparation of: (a) magnetic hydrochar (HC) and magnetic biochar (BC) by direct or indirect synthesis and (b) magnetic activated carbon (AC) by direct or indirect synthesis.
(a)(b)The direct synthesis of magnetic AC implies the addition of chemical substances during impregnation stage and the activation in the subsequent stage of carbonization by hydrothermal treatment or pyrolysis, as shown in Figure2(b). Note that the production of magnetic AC by indirect synthesis relies on the activation stage that can be performed after carbonization by chemical and/or physical pathways and then followed by the impregnation to incorporate magnetic species. A relevant advantage of the synthesis of AC, HC, and BC, as carbon-based supports, is the use of low-cost raw materials as precursors. In this sense, researchers have prepared AC and BC using biomass sources with noncommercial value like orange peels [23], chestnut shell [25], empty fruit bunch from palm [26], and rice straw [27]. Also, alternative carbon sources like industrial and urban residues (e.g., Tetra pack, PET bottles, and tires) can be utilized to obtain these carbon supports [54–56]. Once the precursor for the carbon matrix preparation has been selected and acondicionated (this stage generally includes washing, particle size reduction, and pretreatment), the carbonization stage is the next step. Note that several methods for biomass carbonization can be chosen and some of them are discussed below.Pyrolysis involves the formation of a low-developed porous solid matrix (usually called as char) where the precursor is submitted to a thermal treatment without oxygen at temperatures from 600 to 1000 °C. This char can be also obtained via thermal treatment under the presence of oxygen, and this process is commonly referred as carbonization [57, 58]. For BC and char production, pyrolysis or carbonization is the only stage employed in the preparation route, but an additional activation stage is needed for obtaining AC, which can involve the use of different reagents. For instance, an oxidizing gas like CO2 or steam at 600-1200 °C can be utilized to promote the formation of a well-developed pore structure [57, 58].On the other hand, the hydrothermal carbonization (HTC) is the thermochemical conversion process that transforms biomass under the presence of pressurized water (at subcritical conditions) into a carbon-based material usually referred as HC (i.e., hydrochar) [59]. This process is regarded as a green route to prepare new materials from biomasses and other feedstocks in a closed reactor or autoclave under the presence of water at low temperatures (150-250 °C). HTC offers some advantages in comparison to the conventional thermal treatments because not only helps to generate a surface area rich in functional groups but it also implies a reduced energy consumption and low-cost. Raw HC obtained at common operating conditions has a low specific surface area (<100 m2/g) but contains a significant amount of oxygenated functionalities if water is the reaction medium to prepare this adsorbent [23, 60–63]. For example, Cai et al. [64] reported the preparation of a magnetic BC for chromium adsorption using peanut shells, deionized water, hexamethylenediamine, and FeCl3•6H2O. The adsorbent was obtained via HTC at 220 °C for 12 h. The maximum adsorption capacity of this magnetic material was 142.86 mg/g and could be reused in 3 removal cycles. Figure 3 illustrates the methodology used to produce magnetic BC from peanut shell [64]. Note that HC with high surface area and porosity can be prepared if a postactivation step is performed.Figure 3
HTC used to prepare magnetic adsorbents for Cr (VI) removal from aqueous solution [64].Herein, it is convenient to highlight that alternative technologies can be utilized to prepare the carbon-based support, and they include the application of microwave and plasma [26, 58, 65]. For instance, the main objective of microwave-assisted pyrolysis is to reduce the preparation time and to enhance the adsorption properties of the solid matrix [58]. In microwave instruments, the precursor pyrolysis/carbonization and adsorbent activation can be carried out. This technology offers a heating process that is uniform, thus, it is feasible to homogenize the bulk properties of the final product [58]. Microwave power and radiation time can impact on the char textural parameters like surface area and pore volume [66].As indicated, another important stage is the impregnation with magnetic salts for conferring magnetic properties to BC, AC, or HC. This task can be performed via:(1)
The nonmagnetic iron oxides (i.e., hematite and goethite that can be transformed in magnetic phases) or iron salts can be mixed with the carbon precursor, before its carbonization, in the aqueous solution at a given temperature and time to ensure its impregnation. The impregnated precursor can be carbonized to obtain directly the magnetic adsorbents(2)
Char or AC can be mixed with the magnetic salts in an aqueous solution following the next alternatives for the support impregnation: (1) with a chemical synthesis of magnetic iron oxide using, for example, sol-gel, or coprecipitation methods; and (2) with magnetic iron oxides already synthesized by thermal decomposition, chemical reduction, sol-gel, or coprecipitation. A detailed description of each approach can be found in the interesting review of Noor et al. [58]The final magnetic material could acquire different structural, chemical, and physical characteristics depending on the preparation conditions. For instance, the precursor (biomass or other carbon source), temperature, and impregnation ratio could have a significant impact on the final adsorbent properties. Figure4 illustrates three examples for the preparation of magnetic adsorbents with different methods and stages.Figure 4
Preparation of magnetic biochar (BC) and hydrochar (HC) using several methods: (a) gelatin modified-magnetic BC [25], (b) magnetic BC by direct pyrolysis [24], and (c) dendrimer-like magnetic HC by direct hydrothermal carbonization [23]. Additional information for the magnetic iron oxides preparation can be found in Noor et al. [58].
(a)(b)(c)


## 3.2. Magnetic Graphene-Based Materials

GO and RGO are other preferred carbon matrices to prepare magnetic adsorbents. They have been considered as better graphene derivative nanomaterials than pure graphene, and, compared to raw or commercial chars, they offer high surface areas for the adsorbent preparation. However, these nanopowder adsorbents can aggregate easily in a liquid-phase thus making difficult their separation from aqueous media where additional steps (e.g., centrifugation and granulation by binder) are needed [29]. Magnetic modification is an alternative solution for the recovery and reuse of those materials. For this purpose, magnetic forms of graphene-based materials can be prepared first by GO or RGO synthesis and then modified with magnetic NPs (usually iron oxides).In general, GO and RGO can be obtained by several synthesis methods such as mechanical cleaving (exfoliation), chemical exfoliation by oxidation, chemical synthesis, arc discharge, and thermal chemical vapor deposition (CVD) [67–70]. However, the most usual method to prepare magnetic form of GO or RGO is the exfoliation by oxidation of graphite flakes with the direct or indirect Hummers-Offeman procedure [71]. There is also an alternative method that consists in biomass carbonization with specific reagents to promote graphitization and to obtain graphene-like carbon nanosheets [72, 73]. An overview of graphene-based preparation methods is given in the next subsections.


### 3.2.1. Magnetic GO and RGO Synthesis by Graphite Oxidation Method (GOM)

Basically, the chemical exfoliation is a top-down method where the graphite precursor in solution is exfoliated by incorporating large alkali ions between the graphite layers [74]. Herein, it is convenient to remark that the main method to obtain GO implies a mixture of powdered flake graphite, sulfuric acid, and sodium nitrate, which is cooled at 0 °C with an ice-bath. Potassium permanganate should be carefully added to the mixture under vigorous agitation, preventing that the temperature can exceed 20 °C. Then, the temperature is increased to 35 °C and maintained for 30 min. After this period, water is added and slowly stirred thus causing a violent effervescence and a final temperature of ~98 °C. The diluted color brown suspension is maintained at this temperature for 15 min, and warm water is used to dilute the suspension. Hydrogen peroxide is utilized to reduce the residual permanganate and manganese dioxide to colorless soluble manganese sulfate. This hydrogen peroxide treatment causes that the suspension turns bright yellow, which is a characteristic of GO [71]. RGO can be prepared from GO applying an additional method for reduction that can be carried out by chemical or physical routes [44]. Chemical reagents such as hydrazine hydrate [44], NH3 [75], and L-ascorbic acid [76] have been employed for the chemical reduction of GO. On the other hand, the physical reduction can be performed via thermal reduction [44], hydrothermal reduction [77], and microwave-assisted reduction [78].Magnetic GO or magnetic RGO can be obtained from the corresponding graphene precursor with different methods to modify its structure for preparing the magnetic composite. The most conventional procedure consists of the material impregnation with IONPs at given time and temperature. Figure5 provides the general procedure for obtaining magnetic versions of GO and RGO.Figure 5
General steps for the preparation of magnetic graphene oxide (GO) and magnetic reduced graphene oxide (RGO) by GCEM.Some variations in GO production and its postimpregnation for magnetic modification have been developed by several researchers. Specifically, a magnetic graphene/iron oxide composite for the uranium removal was prepared by Zong et al. [79]. GO synthesis was done with a modified Hummers and Offeman method where 500 mL of H2SO4 solution, 4 g of graphite, and 3 g of NaNO3 were mixed. This suspension was stirred in an ice-water bath, and 18 g of KMnO4 was slowly added during 2.5 h. The mixture was stirred for 5 days at <25 °C and 560 mL of 5 wt% H2SO4 was added dropwise for 2.5 h and stirred at 98 °C. The temperature decreased to 55 °C, and 12 mL of H2O2 (about 30 wt%) was also added dropwise and then stirred for 2.5 h at room temperature. The mixture was centrifuged for 20 min at 19,000 rpm, the liquid and solid phases were separated with bath sonication and potent stirring, and the final product was washed with distilled water. Magnetic GO was obtained by impregnation using 0.50 g of GO and a 300 mL container with 0.58 g FeCl2·4H2O (i.e., Fe2+ : Fe3+ molar ratio of 1 : 2) and 1.56 g FeCl3·6H2O. An ammonia solution (28 wt%) was slowly added, adjusted the pH at 10.5, and stirred for 8 h at 90 °C. The final black solution was filtered and washed with distilled water until obtaining a pH 7 in the filtrated solution. Besides, Ghorbanian et al. [80] reported the synthesis of a magnetic nanocomposite with GO and a chitosan matrix functionalized with 1,5-diphenylcarbazone (DPC) and magnetite for lead extraction from water. GO was prepared with a modified Hummers and Offeman method where graphite powder was poured into a 9 : 1 mixture of concentrated H2SO4/H3PO4 (360 : 40). KMnO4 was slowly added to the mixture, and it was heated up to 50 °C and stirred for 24 h, and the final temperature was decreased to room temperature. 400 mL of pure ice and H2O2 (30%, v/v) was added to this mixture. GO was washed with water, centrifuged, and dried at 60 °C. Acylated GO was obtained from GO and dried SOCl2 with reflux at 70 °C for 24 h. Anhydrous dimethylformamide was used to wash this mixture and then dried. Toluene and GO-Cl were mixed by sonication, and DPC was added to the solution, the mixture was heated and refluxed for 24 h, rinsed with methanol, and dried at room temperature to obtain GO-DPC. Acetic acid solution (2% v/v) was used to dissolve chitosan in an ultrasonic bath to generate a homogeneous solution for magnetic modification. Chitosan solution and magnetic NPs were stirred for 2 h to obtain a uniform suspension. GO-DPC was added to a reaction flask with 15 glutaraldehyde, the mixture pH was adjusted at 9.5 by drop wise of 0.1 mol/L NaOH, and the solution was maintained at 80 °C for 1 h. The magnetic composite was collected by the magnet, washed with double-distilled water and ethanol to neutral pH, and dried at 50 °C.It is important to remark that GO is more suitable than RGO for adsorption applications, but some researchers have carried out some experiments to remove water pollutants. As example, magnetic GO and RGO prepared by annealing reduction at 500 °C under N2 (magnetic annealing-RGO) and by chemical reduction with hydrazine hydrate (magnetic chemically-RGO) were studied by Huang et al. [44]. Magnetic GO was the best adsorbent with competitive adsorption capacities of tetracycline, Cd2+, and As5+ due to its oxygenated functional groups.


### 3.2.2. Production of Pseudographene by Biomass Carbonization Method (BCM)

Biomass is a renewable carbon-containing source available worldwide [81]. According to Wang et al. [81], the global production of biomass is estimated in 146 billion tons, which is generated as residue by industry, agriculture, forestry, and other sources. Therefore, several studies have used biomasses as inexpensive raw materials with the aim of solving environmental pollution problems. The development of biomass-based CNMs implies an important effort to contribute to the science progress. However, the use of biomasses to prepare high performance CNMs is still challenging due to its high oxygen content, strong chemical bonding, and complex structure [81]. Several methods for preparing CNMs from biomasses have been studied including CVD (in situ and two-stage), pyrolytic transformation (e.g., thermo-chemical activation, catalytic graphitization, and catalytic graphitization coupled with thermo-chemical activation), mechanical activation, cyclic oxidation, combustion, and microwave-assisted pyrolysis [58, 81]. A comprehensive discussion of these methodologies is given in the reviews of Noor et al. [58] and Wang et al. [81].Particularly, the pyrolytic transformation by catalytic graphitization is the most used method to obtain pseudographene [81, 82]. Conventional graphitization is a type of pyrolysis that requires graphitizable precursors and is carried out at high temperature (>2000 °C), which increases the process cost and security risks thus limiting its industrial scalability [82]. As an alternative method, the catalytic graphitization is a simple strategy consisting of the precursor carbonization using transition metals as catalysts [82]. This process allows that graphitizable and nongraphitizable carbon materials can be converted into crystalline materials at temperatures <1000 °C and, consequently, thus reducing the energy consumption and costs [82]. Figure 6 shows some routes to prepare CNMs [81]. Basically, the modification technique to obtain magnetic materials consists of a biomass (carbon precursor) pretreatment and its impregnation with an activating agent and/or catalyst and the final carbonization via conventional or nonconventional methods. The use of metals from group 4-7 (e.g., Fe, Co, Ni, and Mn) contributes to the conversion of amorphous carbon to graphitic carbon via the reduction of the corresponding activation energy. In fact, they are ideal as graphitization catalysts due to their 2-5 electrons in the d-shell orbitals that allow the formation of strong bonds between carbon-based materials and metal carbides [81]. Some examples of BCM routes are described below.Figure 6
Preparation of carbon nanomaterials from biomasses [81].Graphene-like nanosheet materials with high surface area can be prepared from simple BCM route using coconut shell, FeCl3 and ZnCl2 as carbon precursor, graphitic catalyst precursor, and activating agent, respectively [72]. ZnCl2 and coconut shell were mixed in a 3 M FeCl3 solution, and the impregnation was performed by evaporation at 80 °C for 2 h under stirring and a final drying at 100 °C. The activation and graphitization of the coconut shell were performed at 900 °C for 1 h with N2 atmosphere in a tubular furnace. Magnetic composites were prepared at 800 and 1000 °C forming the magnetic species CFe3 and α-Fe. Moreover, sugar has been used as a carbon precursor to prepare magnetic graphene-like nanosheets for U6+ adsorption [73]. The disaccharide sugar was slowly heated at 200 °C for 1 h under N2 flow in a furnace to achieve its caramelization. The furnace temperature was increased to 750 °C within 1 h and then maintained for 3 h to convert caramel to inorganic carbon. The pyrolyzed sugar was milled, and the final powder was utilized as a sugar-based pseudographene carbon. The oxidized pseudographene form was prepared using a treatment with ozone in water at rate of 5 g/h for 1 h and sonication, and the final product was washed with deionized water and dried at 80 °C for 8 h. The magnetic phase impregnation was done with a fast in situ synthesis of magnetite where a solution of FeCl3·6H2O and FeCl2·4H2O (2:1 molar ratio of Fe3+:Fe2+) was dropwise added into oxidized pseudographene sample at room temperature under vigorous stirring and N2 purging. Solution pH was adjusted to ≥10 and maintained at 80 °C for 1 h with continuous stirring where a black precipitate was formed. The final product was washed, separated with an external magnetic field, and dried at 60 °C for 12 h under vacuum.


### 3.2.3. Magnetic Carbon Nanotubes (CNTs)

CNTs are also nanomaterials utilized to prepare magnetic adsorbents. A number of methods has been reported for the preparation of magnetic iron oxide/CNTs composites by routes that firstly include the preparation of CNTs (e.g., CVD, arc discharge, and vapor phase growth) [83] and the subsequent modification with MNPs using sol–gel [84], solvothermal [85], reverse microemulsion [86], hydrothermal [87, 88], high-temperature decomposition [89], or coprecipitation method [90–92].For CNTs synthesis, the CVD is the most conventional method where a carbon precursor, catalyst and growth promoter are usually needed. As example, MWCNTs can be prepared via catalytic CVD of hexane using magnesium/iron layered double hydroxide as catalyst precursor [90]. MWCNTs were purified with a 3 M HNO3 solution at room temperature for 24 h, filtered and washed with distilled water. H2SO4/HNO3 mixture (3 : 1 v/v) and sonication were applied to activate MWCNTs at room temperature. 0.05 M Fe(NO3)3 solution and activated MWCNTs were mixed under stirring, and, subsequently, an ammonia solution (2.5 wt.%) was slowly added until reaching pH 9.5. Filtration and washing with distilled water were used to obtain the final product that was dried at 100 °C for 12 h. Finally, MWCNTs-IONPs were obtained via an annealing at 500 °C for 1.5 h under Ar flow.Typically, hydrocarbons are sources for CNT synthesis; nevertheless, some studies employed alternative precursors in order to propose a green synthesis. Ma [93] prepared SWCNTs by spray pyrolysis with ethanol (carbon precursor), ferrocene (catalyst), and thiophene (growth promoter). Thiophene and ferrocene were dissolved in ethanol by sonication, and the final solution was employed in spray pyrolysis. A tubular furnace with a quartz tube was heated at 1000-1150 °C under Ar flow. The mixture (ethanol-ferrocene-thiophene) was sprayed through a nozzle to the furnace and pyrolyzed, and the final sample was collected. For purification stage, the pristine sample was heated at 400 °C in continuous oxygen flow to oxidize iron NPs, and the oxidized sample was further heated at 800-900 °C for 1 h under Ar flow and exposed to 12 M HCl treatment at 100 °C for 4 h. The final product was filtrated and washed until obtaining a neutral pH.Ma et al. [17] reported the application of arc discharge evaporation of a carbon electrode with an iron catalyst to obtain SWCNTs. This synthesis was done using two electrodes that were located in the center of a water-cooled stainless-steel chamber. Pure graphite-rod and graphite-rod containing 4 wt% of iron catalyst were the cathode and anode, respectively. The direct current arc discharge was obtained with 120 A in a gas mixture of Ar and H2. After 30 min of arc evaporation, ~500 mg of iron NPs- SWCNTs was obtained. The product was heated at 350 °C for 6 h in air to oxidize iron NPs and to remove the amorphous carbon.Once CNTs have been obtained, a modification and/or functionalization stage is necessary to obtain magnetic CNTs. Note that interesting purification and modification methods for magnetic CNTs preparation have been reported. For instance, commercial MWCNTs can be functionalized with dibenzo-18-crown-6 moieties for amoxicillin adsorption [87]. The partial oxidation and impurity removal of MWCNTs were done by dispersion in concentrated HNO3 at 130 °C for 30 min. For the magnetic modification stage, the pretreated MWCNTs were added to a mixture obtained from ammonium iron sulfate hexahydrate dissolved in water and a hydrazine hydrate solution. This suspension was stirred and sonicated, and the solution pH was adjusted to 11-13 and refluxed at boiling point for 2 h. Filtration and washing of magnetic MWCNTs were done with water and ethanol, and the product was dried for 24 h under vacuum. Ethanol was used to disperse magnetic MWCNTs and sonicated for 10 min to do the crown-functionalization. This system was mixed with a dicyclohexylcarbodiimide ethanolic solution, stirred for 10 min and, finally, a solution of 4,4’-diaminodibenzo-18-crown-6 was added to the mixture, which was stirred at room temperature for 24 h. The final products were washed with water and dried for 12 h under vacuum.In addition, magnetic MWCNTs were prepared to remove As5+ and As3+ from water [91]. Commercial MWCNTs were treated with HNO3 solution (70%) at 70 °C for 12 h to incorporate oxygenated functionalities with the aim of increasing their affinity for the IONPs. Fe3+/Fe2+ solution (molarratio=2) and oxidized MWCNTs were mixed by ultrasonication for 4 h. Then, the magnetic material was obtained via the addition dropwise of a 6 M NaOH solution until reaching pH 8. In a recent study, magnetic MWCNTs were embedded in a hydrophilic polyvinylidene fluoride (PVDF) membrane for the adsorption of As3+ [50]. First, copper-ferrite was obtained from the dissolution of ethylene glycol, FeCl3, CuCl2·2H2O, polyethylene glycol, and sodium acetate. This mixture was heated up for 8 h at 200 °C using a teflon-lined autoclave and cooled to room temperature. The substrate for MWCNTs membrane preparation was a flat-sheet PVDF membrane. Specifically, 12 mg of MWCNTs was mixed with 30 mL of pure water, and this mixture was added to the PVDF membrane where CuFe2O4 particles were dispersed in water, sonicated, and then injected onto the CNT membrane.It is important to mention that in several papers related to the use of CNTs as supports to prepare carbon-based adsorbents, CNTs were purchased (i.e., they were available commercial products), and a modification step was used to obtain the adsorbent [87, 91]. Only few studies have reported the CNTs synthesis [17, 93] because this step could be expensive, and CNTs are difficult to obtain in laboratory with a suitable quality and reproducible properties.


### 3.2.4. Magnetic Carbon Nanocages (CNCs)

CNCs have interesting applications in energy and environmental protection [33]. They can be utilized to prepare hybrid nanomaterials with multifunctional properties [33]. Currently, various synthesis routes have been reported to prepare CNCs including pyrolysis of organic precursors and sol-gel method, CVD, templating by using different metal particles, and arc discharge [94]. However, these approaches have used pyridine, ethanol, and acetylene as carbon sources, which are unsustainable and expensive due to the use of fossil precursors [94]. Therefore, the utilization of porous carbon materials obtained from biomass precursors is an alternative employing pyrolysis, HTC, template-directed synthesis (soft, hard, and dual template), and direct synthesis. Biomass graphitization was proved to be promising to obtain CNCs structures, especially, for environmental applications [94].A low-cost, simple, and environmentally friendly method to prepare magnetic CNCs, with multiform pore structure, from the lignin carbonization at low temperature was reported by Qin et al. [94]. They prepared CNCs with lignin, NaOH, formalin solutions, and Fe(NO3)2·9H2O. A conventional pyrolysis was carried out at 600 °C for 3 h, and the final material was used for methyl orange adsorption.Cho et al. [95] synthesized magnetic CNCs using sugar as carbon precursor, and this material was applied for methylene blue adsorption, see Figure 7. Magnetic NPs were soaked in a sugar solution for 30 min with a sugar/magnetite ratio of 1 : 2, then, the water was vaporized under magnetic stirring at 85 °C for 120 min. The dried and impregnated sugar compound was pyrolyzed at 500 °C for 30 min in a tubular reactor. The final adsorbent showed a methylene blue adsorption capacity of 52.6 mg/g.Figure 7
Preparation of novel magnetic CNC adsorbent via pyrolysis of sugar for methylene blue adsorption in aqueous solutions [95].Zuo et al. [96] proposed a green protocol to synthesize magnetic CNCs that were modified with diethylenetriamine (DETA) and gold using glucose as carbon source where the final adsorbent was applied in the adsorption of methylene blue from aqueous solution. CNCs were synthetized via the HTC of the glucose solution at 180 °C for 3 h. CNCs were treated with ethanol and DETA and, finally, impregnated with Fe3O4 NPs diluted in chloroform/ethanol solution at room temperature for 24 h under stirring. A solution of ethylene glycol/water was mixed with the black solid product where a HAuCl4 solution was dropwise added and stirred at room temperature for 1 h. Finally, NaBH4 solution was added to this mixture and stirred for 2 h under N2 atmosphere to obtain the final magnetic product.Petala et al. [33] also reported a green one-step and simple method to prepare magnetic CNCs from pine resin, iron nitrate impregnation, and pyrolysis at 1000 °C. The morphology, textural, and surface properties of magnetic CNCs were analyzed with surface, spectroscopic, and microscopic techniques. Results indicated that the magnetic CNCs presented a homogeneous distribution of core-shell-type magnetic NPs within the carbon matrix where the surface area was 177 m2/g with both micropores and mesopores. These magnetic CNCs showed an adsorption capacity of 263.9 mg/g for the removal of As3+ from aqueous solutions at pH 7.A low-cost and easily scalable method was proposed by Rudakov et al. [34] to obtain magnetic CNCs via the simple thermolysis of precursors based on a mixture of citrate acid and transition metal (nickel, cobalt, or iron) acetate salts. The effect of thermolysis temperature (in a range of 500-850 °C) on magnetic CNCs structural properties was studied. The theory of Ostwald ripening, Arrhenius law for diffusion, and instrumental characterization were used to analyze the thermal dependence of the particle size. Superparamagnetic characteristics were observed for nickel samples annealed at <700 °C. CNCs prepared with cobalt at 600 °C showed higher saturation magnetization than CNCs with nickel, while iron nanoparticles were larger than those of cobalt and nickel thus showing ferromagnetic behavior.


### 3.2.5. Magnetic Carbon Quantum Dots (CQDs) and Magnetic Graphene Quantum Dots (GQDs)

The synthesis of CQDs and GQDs usually involves at least 2 stages. First, it is necessary to obtain the quantum dots and then the corresponding magnetic properties are developed in the second stage [52]. Some authors have reported the functionalization of material surface to add functional groups that can interact with a specific adsorbate. CQDs and GQDs can be prepared from various natural carbon sources, but citric acid is the most common one because it consists of carbonyl, carboxylic, and hydroxyl groups [52]. However, other available and low-cost raw biomasses with similar chemical composition can be employed to prepare CQDs and GQDs [52].Chemical structure, quantum size, and photo-luminescent properties of these materials depend on the feedstock chemical structure and the preparation route [52]. The next examples describe interesting synthesis methods to obtain magnetic CQDs and GQDs. For instance, a typical procedure to prepare CQDs employs a mixture of citric acid, dicyandiamide, and water, which is agitated until a clear solution is obtained [97]. This solution is transferred to a stainless autoclave and heated to 160 °C for 4 h. The final product is collected and centrifuged. The magnetic composite can be obtained by coprecipitation where CQDs are dispersed in deionized water by sonication and mixed with FeCl3·6H2O solution at room temperature under N2 flow with vigorous stirring. The temperature is increased up to 80 °C, and FeCl2·4H2O is slowly added to the solution containing Fe3+/CQDs and stirred for additional 30 min. Finally, ammonia is added dropwise to adjust the solution pH at 10. The black precipitate can be magnetically separated and washed several times and, subsequently, dried at room temperature [97]. On the other hand, Tadesse et al. [98] proposed a hydrothermal method to prepare nitrogen-doped magnetic CQDs using lemon juice and ethylenediamine. These reagents were mixed and heated at 200 °C for 3 h to obtain a black paste, which was washed with water to remove insoluble matter. Dichloromethane was added to obtain a brown solution, and a coprecipitation reaction was employed for the magnetic impregnation where metallic salts of Fe3+/Fe2+ and CQDs were mixed in aqueous solution. NaOH was added drop wise to this system, and the final product was a magnetic CQDs soluble in water. Recently, Nuengmatcha et al. [99] reported magnetic mercapto-functionalized GQDs for Cd2+ adsorption. GQDs were prepared using citric acid (2 g) heated at 260 °C where 100 mL of 0.25 M NaOH was added when the color changed to yellow. Maghemite was the magnetic phase and produced by mixing 5 g of FeCl3·6H2O, 2.5 g of FeSO4·7H2O, and deionized water. Subsequently, 20 mL of 28% NH4OH was added, and the solution was heated at 80 °C for 30 min under N2 atmosphere. GQD solution was mixed with maghemite, and this suspension was heated at 80 °C for 30 min, washed with deionized water, and dried at 90 °C. Magnetic GQDs were modified with C2H5OH and H(CH2)Si(OCH3)3. Kahrizi et al. [100] also reported a similar procedure to prepare magnetic GQDs combined with hydroxyapatite for Cd2+ adsorption.


## 3.2.1. Magnetic GO and RGO Synthesis by Graphite Oxidation Method (GOM)

Basically, the chemical exfoliation is a top-down method where the graphite precursor in solution is exfoliated by incorporating large alkali ions between the graphite layers [74]. Herein, it is convenient to remark that the main method to obtain GO implies a mixture of powdered flake graphite, sulfuric acid, and sodium nitrate, which is cooled at 0 °C with an ice-bath. Potassium permanganate should be carefully added to the mixture under vigorous agitation, preventing that the temperature can exceed 20 °C. Then, the temperature is increased to 35 °C and maintained for 30 min. After this period, water is added and slowly stirred thus causing a violent effervescence and a final temperature of ~98 °C. The diluted color brown suspension is maintained at this temperature for 15 min, and warm water is used to dilute the suspension. Hydrogen peroxide is utilized to reduce the residual permanganate and manganese dioxide to colorless soluble manganese sulfate. This hydrogen peroxide treatment causes that the suspension turns bright yellow, which is a characteristic of GO [71]. RGO can be prepared from GO applying an additional method for reduction that can be carried out by chemical or physical routes [44]. Chemical reagents such as hydrazine hydrate [44], NH3 [75], and L-ascorbic acid [76] have been employed for the chemical reduction of GO. On the other hand, the physical reduction can be performed via thermal reduction [44], hydrothermal reduction [77], and microwave-assisted reduction [78].Magnetic GO or magnetic RGO can be obtained from the corresponding graphene precursor with different methods to modify its structure for preparing the magnetic composite. The most conventional procedure consists of the material impregnation with IONPs at given time and temperature. Figure5 provides the general procedure for obtaining magnetic versions of GO and RGO.Figure 5
General steps for the preparation of magnetic graphene oxide (GO) and magnetic reduced graphene oxide (RGO) by GCEM.Some variations in GO production and its postimpregnation for magnetic modification have been developed by several researchers. Specifically, a magnetic graphene/iron oxide composite for the uranium removal was prepared by Zong et al. [79]. GO synthesis was done with a modified Hummers and Offeman method where 500 mL of H2SO4 solution, 4 g of graphite, and 3 g of NaNO3 were mixed. This suspension was stirred in an ice-water bath, and 18 g of KMnO4 was slowly added during 2.5 h. The mixture was stirred for 5 days at <25 °C and 560 mL of 5 wt% H2SO4 was added dropwise for 2.5 h and stirred at 98 °C. The temperature decreased to 55 °C, and 12 mL of H2O2 (about 30 wt%) was also added dropwise and then stirred for 2.5 h at room temperature. The mixture was centrifuged for 20 min at 19,000 rpm, the liquid and solid phases were separated with bath sonication and potent stirring, and the final product was washed with distilled water. Magnetic GO was obtained by impregnation using 0.50 g of GO and a 300 mL container with 0.58 g FeCl2·4H2O (i.e., Fe2+ : Fe3+ molar ratio of 1 : 2) and 1.56 g FeCl3·6H2O. An ammonia solution (28 wt%) was slowly added, adjusted the pH at 10.5, and stirred for 8 h at 90 °C. The final black solution was filtered and washed with distilled water until obtaining a pH 7 in the filtrated solution. Besides, Ghorbanian et al. [80] reported the synthesis of a magnetic nanocomposite with GO and a chitosan matrix functionalized with 1,5-diphenylcarbazone (DPC) and magnetite for lead extraction from water. GO was prepared with a modified Hummers and Offeman method where graphite powder was poured into a 9 : 1 mixture of concentrated H2SO4/H3PO4 (360 : 40). KMnO4 was slowly added to the mixture, and it was heated up to 50 °C and stirred for 24 h, and the final temperature was decreased to room temperature. 400 mL of pure ice and H2O2 (30%, v/v) was added to this mixture. GO was washed with water, centrifuged, and dried at 60 °C. Acylated GO was obtained from GO and dried SOCl2 with reflux at 70 °C for 24 h. Anhydrous dimethylformamide was used to wash this mixture and then dried. Toluene and GO-Cl were mixed by sonication, and DPC was added to the solution, the mixture was heated and refluxed for 24 h, rinsed with methanol, and dried at room temperature to obtain GO-DPC. Acetic acid solution (2% v/v) was used to dissolve chitosan in an ultrasonic bath to generate a homogeneous solution for magnetic modification. Chitosan solution and magnetic NPs were stirred for 2 h to obtain a uniform suspension. GO-DPC was added to a reaction flask with 15 glutaraldehyde, the mixture pH was adjusted at 9.5 by drop wise of 0.1 mol/L NaOH, and the solution was maintained at 80 °C for 1 h. The magnetic composite was collected by the magnet, washed with double-distilled water and ethanol to neutral pH, and dried at 50 °C.It is important to remark that GO is more suitable than RGO for adsorption applications, but some researchers have carried out some experiments to remove water pollutants. As example, magnetic GO and RGO prepared by annealing reduction at 500 °C under N2 (magnetic annealing-RGO) and by chemical reduction with hydrazine hydrate (magnetic chemically-RGO) were studied by Huang et al. [44]. Magnetic GO was the best adsorbent with competitive adsorption capacities of tetracycline, Cd2+, and As5+ due to its oxygenated functional groups.


## 3.2.2. Production of Pseudographene by Biomass Carbonization Method (BCM)

Biomass is a renewable carbon-containing source available worldwide [81]. According to Wang et al. [81], the global production of biomass is estimated in 146 billion tons, which is generated as residue by industry, agriculture, forestry, and other sources. Therefore, several studies have used biomasses as inexpensive raw materials with the aim of solving environmental pollution problems. The development of biomass-based CNMs implies an important effort to contribute to the science progress. However, the use of biomasses to prepare high performance CNMs is still challenging due to its high oxygen content, strong chemical bonding, and complex structure [81]. Several methods for preparing CNMs from biomasses have been studied including CVD (in situ and two-stage), pyrolytic transformation (e.g., thermo-chemical activation, catalytic graphitization, and catalytic graphitization coupled with thermo-chemical activation), mechanical activation, cyclic oxidation, combustion, and microwave-assisted pyrolysis [58, 81]. A comprehensive discussion of these methodologies is given in the reviews of Noor et al. [58] and Wang et al. [81].Particularly, the pyrolytic transformation by catalytic graphitization is the most used method to obtain pseudographene [81, 82]. Conventional graphitization is a type of pyrolysis that requires graphitizable precursors and is carried out at high temperature (>2000 °C), which increases the process cost and security risks thus limiting its industrial scalability [82]. As an alternative method, the catalytic graphitization is a simple strategy consisting of the precursor carbonization using transition metals as catalysts [82]. This process allows that graphitizable and nongraphitizable carbon materials can be converted into crystalline materials at temperatures <1000 °C and, consequently, thus reducing the energy consumption and costs [82]. Figure 6 shows some routes to prepare CNMs [81]. Basically, the modification technique to obtain magnetic materials consists of a biomass (carbon precursor) pretreatment and its impregnation with an activating agent and/or catalyst and the final carbonization via conventional or nonconventional methods. The use of metals from group 4-7 (e.g., Fe, Co, Ni, and Mn) contributes to the conversion of amorphous carbon to graphitic carbon via the reduction of the corresponding activation energy. In fact, they are ideal as graphitization catalysts due to their 2-5 electrons in the d-shell orbitals that allow the formation of strong bonds between carbon-based materials and metal carbides [81]. Some examples of BCM routes are described below.Figure 6
Preparation of carbon nanomaterials from biomasses [81].Graphene-like nanosheet materials with high surface area can be prepared from simple BCM route using coconut shell, FeCl3 and ZnCl2 as carbon precursor, graphitic catalyst precursor, and activating agent, respectively [72]. ZnCl2 and coconut shell were mixed in a 3 M FeCl3 solution, and the impregnation was performed by evaporation at 80 °C for 2 h under stirring and a final drying at 100 °C. The activation and graphitization of the coconut shell were performed at 900 °C for 1 h with N2 atmosphere in a tubular furnace. Magnetic composites were prepared at 800 and 1000 °C forming the magnetic species CFe3 and α-Fe. Moreover, sugar has been used as a carbon precursor to prepare magnetic graphene-like nanosheets for U6+ adsorption [73]. The disaccharide sugar was slowly heated at 200 °C for 1 h under N2 flow in a furnace to achieve its caramelization. The furnace temperature was increased to 750 °C within 1 h and then maintained for 3 h to convert caramel to inorganic carbon. The pyrolyzed sugar was milled, and the final powder was utilized as a sugar-based pseudographene carbon. The oxidized pseudographene form was prepared using a treatment with ozone in water at rate of 5 g/h for 1 h and sonication, and the final product was washed with deionized water and dried at 80 °C for 8 h. The magnetic phase impregnation was done with a fast in situ synthesis of magnetite where a solution of FeCl3·6H2O and FeCl2·4H2O (2:1 molar ratio of Fe3+:Fe2+) was dropwise added into oxidized pseudographene sample at room temperature under vigorous stirring and N2 purging. Solution pH was adjusted to ≥10 and maintained at 80 °C for 1 h with continuous stirring where a black precipitate was formed. The final product was washed, separated with an external magnetic field, and dried at 60 °C for 12 h under vacuum.


## 3.2.3. Magnetic Carbon Nanotubes (CNTs)

CNTs are also nanomaterials utilized to prepare magnetic adsorbents. A number of methods has been reported for the preparation of magnetic iron oxide/CNTs composites by routes that firstly include the preparation of CNTs (e.g., CVD, arc discharge, and vapor phase growth) [83] and the subsequent modification with MNPs using sol–gel [84], solvothermal [85], reverse microemulsion [86], hydrothermal [87, 88], high-temperature decomposition [89], or coprecipitation method [90–92].For CNTs synthesis, the CVD is the most conventional method where a carbon precursor, catalyst and growth promoter are usually needed. As example, MWCNTs can be prepared via catalytic CVD of hexane using magnesium/iron layered double hydroxide as catalyst precursor [90]. MWCNTs were purified with a 3 M HNO3 solution at room temperature for 24 h, filtered and washed with distilled water. H2SO4/HNO3 mixture (3 : 1 v/v) and sonication were applied to activate MWCNTs at room temperature. 0.05 M Fe(NO3)3 solution and activated MWCNTs were mixed under stirring, and, subsequently, an ammonia solution (2.5 wt.%) was slowly added until reaching pH 9.5. Filtration and washing with distilled water were used to obtain the final product that was dried at 100 °C for 12 h. Finally, MWCNTs-IONPs were obtained via an annealing at 500 °C for 1.5 h under Ar flow.Typically, hydrocarbons are sources for CNT synthesis; nevertheless, some studies employed alternative precursors in order to propose a green synthesis. Ma [93] prepared SWCNTs by spray pyrolysis with ethanol (carbon precursor), ferrocene (catalyst), and thiophene (growth promoter). Thiophene and ferrocene were dissolved in ethanol by sonication, and the final solution was employed in spray pyrolysis. A tubular furnace with a quartz tube was heated at 1000-1150 °C under Ar flow. The mixture (ethanol-ferrocene-thiophene) was sprayed through a nozzle to the furnace and pyrolyzed, and the final sample was collected. For purification stage, the pristine sample was heated at 400 °C in continuous oxygen flow to oxidize iron NPs, and the oxidized sample was further heated at 800-900 °C for 1 h under Ar flow and exposed to 12 M HCl treatment at 100 °C for 4 h. The final product was filtrated and washed until obtaining a neutral pH.Ma et al. [17] reported the application of arc discharge evaporation of a carbon electrode with an iron catalyst to obtain SWCNTs. This synthesis was done using two electrodes that were located in the center of a water-cooled stainless-steel chamber. Pure graphite-rod and graphite-rod containing 4 wt% of iron catalyst were the cathode and anode, respectively. The direct current arc discharge was obtained with 120 A in a gas mixture of Ar and H2. After 30 min of arc evaporation, ~500 mg of iron NPs- SWCNTs was obtained. The product was heated at 350 °C for 6 h in air to oxidize iron NPs and to remove the amorphous carbon.Once CNTs have been obtained, a modification and/or functionalization stage is necessary to obtain magnetic CNTs. Note that interesting purification and modification methods for magnetic CNTs preparation have been reported. For instance, commercial MWCNTs can be functionalized with dibenzo-18-crown-6 moieties for amoxicillin adsorption [87]. The partial oxidation and impurity removal of MWCNTs were done by dispersion in concentrated HNO3 at 130 °C for 30 min. For the magnetic modification stage, the pretreated MWCNTs were added to a mixture obtained from ammonium iron sulfate hexahydrate dissolved in water and a hydrazine hydrate solution. This suspension was stirred and sonicated, and the solution pH was adjusted to 11-13 and refluxed at boiling point for 2 h. Filtration and washing of magnetic MWCNTs were done with water and ethanol, and the product was dried for 24 h under vacuum. Ethanol was used to disperse magnetic MWCNTs and sonicated for 10 min to do the crown-functionalization. This system was mixed with a dicyclohexylcarbodiimide ethanolic solution, stirred for 10 min and, finally, a solution of 4,4’-diaminodibenzo-18-crown-6 was added to the mixture, which was stirred at room temperature for 24 h. The final products were washed with water and dried for 12 h under vacuum.In addition, magnetic MWCNTs were prepared to remove As5+ and As3+ from water [91]. Commercial MWCNTs were treated with HNO3 solution (70%) at 70 °C for 12 h to incorporate oxygenated functionalities with the aim of increasing their affinity for the IONPs. Fe3+/Fe2+ solution (molarratio=2) and oxidized MWCNTs were mixed by ultrasonication for 4 h. Then, the magnetic material was obtained via the addition dropwise of a 6 M NaOH solution until reaching pH 8. In a recent study, magnetic MWCNTs were embedded in a hydrophilic polyvinylidene fluoride (PVDF) membrane for the adsorption of As3+ [50]. First, copper-ferrite was obtained from the dissolution of ethylene glycol, FeCl3, CuCl2·2H2O, polyethylene glycol, and sodium acetate. This mixture was heated up for 8 h at 200 °C using a teflon-lined autoclave and cooled to room temperature. The substrate for MWCNTs membrane preparation was a flat-sheet PVDF membrane. Specifically, 12 mg of MWCNTs was mixed with 30 mL of pure water, and this mixture was added to the PVDF membrane where CuFe2O4 particles were dispersed in water, sonicated, and then injected onto the CNT membrane.It is important to mention that in several papers related to the use of CNTs as supports to prepare carbon-based adsorbents, CNTs were purchased (i.e., they were available commercial products), and a modification step was used to obtain the adsorbent [87, 91]. Only few studies have reported the CNTs synthesis [17, 93] because this step could be expensive, and CNTs are difficult to obtain in laboratory with a suitable quality and reproducible properties.


## 3.2.4. Magnetic Carbon Nanocages (CNCs)

CNCs have interesting applications in energy and environmental protection [33]. They can be utilized to prepare hybrid nanomaterials with multifunctional properties [33]. Currently, various synthesis routes have been reported to prepare CNCs including pyrolysis of organic precursors and sol-gel method, CVD, templating by using different metal particles, and arc discharge [94]. However, these approaches have used pyridine, ethanol, and acetylene as carbon sources, which are unsustainable and expensive due to the use of fossil precursors [94]. Therefore, the utilization of porous carbon materials obtained from biomass precursors is an alternative employing pyrolysis, HTC, template-directed synthesis (soft, hard, and dual template), and direct synthesis. Biomass graphitization was proved to be promising to obtain CNCs structures, especially, for environmental applications [94].A low-cost, simple, and environmentally friendly method to prepare magnetic CNCs, with multiform pore structure, from the lignin carbonization at low temperature was reported by Qin et al. [94]. They prepared CNCs with lignin, NaOH, formalin solutions, and Fe(NO3)2·9H2O. A conventional pyrolysis was carried out at 600 °C for 3 h, and the final material was used for methyl orange adsorption.Cho et al. [95] synthesized magnetic CNCs using sugar as carbon precursor, and this material was applied for methylene blue adsorption, see Figure 7. Magnetic NPs were soaked in a sugar solution for 30 min with a sugar/magnetite ratio of 1 : 2, then, the water was vaporized under magnetic stirring at 85 °C for 120 min. The dried and impregnated sugar compound was pyrolyzed at 500 °C for 30 min in a tubular reactor. The final adsorbent showed a methylene blue adsorption capacity of 52.6 mg/g.Figure 7
Preparation of novel magnetic CNC adsorbent via pyrolysis of sugar for methylene blue adsorption in aqueous solutions [95].Zuo et al. [96] proposed a green protocol to synthesize magnetic CNCs that were modified with diethylenetriamine (DETA) and gold using glucose as carbon source where the final adsorbent was applied in the adsorption of methylene blue from aqueous solution. CNCs were synthetized via the HTC of the glucose solution at 180 °C for 3 h. CNCs were treated with ethanol and DETA and, finally, impregnated with Fe3O4 NPs diluted in chloroform/ethanol solution at room temperature for 24 h under stirring. A solution of ethylene glycol/water was mixed with the black solid product where a HAuCl4 solution was dropwise added and stirred at room temperature for 1 h. Finally, NaBH4 solution was added to this mixture and stirred for 2 h under N2 atmosphere to obtain the final magnetic product.Petala et al. [33] also reported a green one-step and simple method to prepare magnetic CNCs from pine resin, iron nitrate impregnation, and pyrolysis at 1000 °C. The morphology, textural, and surface properties of magnetic CNCs were analyzed with surface, spectroscopic, and microscopic techniques. Results indicated that the magnetic CNCs presented a homogeneous distribution of core-shell-type magnetic NPs within the carbon matrix where the surface area was 177 m2/g with both micropores and mesopores. These magnetic CNCs showed an adsorption capacity of 263.9 mg/g for the removal of As3+ from aqueous solutions at pH 7.A low-cost and easily scalable method was proposed by Rudakov et al. [34] to obtain magnetic CNCs via the simple thermolysis of precursors based on a mixture of citrate acid and transition metal (nickel, cobalt, or iron) acetate salts. The effect of thermolysis temperature (in a range of 500-850 °C) on magnetic CNCs structural properties was studied. The theory of Ostwald ripening, Arrhenius law for diffusion, and instrumental characterization were used to analyze the thermal dependence of the particle size. Superparamagnetic characteristics were observed for nickel samples annealed at <700 °C. CNCs prepared with cobalt at 600 °C showed higher saturation magnetization than CNCs with nickel, while iron nanoparticles were larger than those of cobalt and nickel thus showing ferromagnetic behavior.


## 3.2.5. Magnetic Carbon Quantum Dots (CQDs) and Magnetic Graphene Quantum Dots (GQDs)

The synthesis of CQDs and GQDs usually involves at least 2 stages. First, it is necessary to obtain the quantum dots and then the corresponding magnetic properties are developed in the second stage [52]. Some authors have reported the functionalization of material surface to add functional groups that can interact with a specific adsorbate. CQDs and GQDs can be prepared from various natural carbon sources, but citric acid is the most common one because it consists of carbonyl, carboxylic, and hydroxyl groups [52]. However, other available and low-cost raw biomasses with similar chemical composition can be employed to prepare CQDs and GQDs [52].Chemical structure, quantum size, and photo-luminescent properties of these materials depend on the feedstock chemical structure and the preparation route [52]. The next examples describe interesting synthesis methods to obtain magnetic CQDs and GQDs. For instance, a typical procedure to prepare CQDs employs a mixture of citric acid, dicyandiamide, and water, which is agitated until a clear solution is obtained [97]. This solution is transferred to a stainless autoclave and heated to 160 °C for 4 h. The final product is collected and centrifuged. The magnetic composite can be obtained by coprecipitation where CQDs are dispersed in deionized water by sonication and mixed with FeCl3·6H2O solution at room temperature under N2 flow with vigorous stirring. The temperature is increased up to 80 °C, and FeCl2·4H2O is slowly added to the solution containing Fe3+/CQDs and stirred for additional 30 min. Finally, ammonia is added dropwise to adjust the solution pH at 10. The black precipitate can be magnetically separated and washed several times and, subsequently, dried at room temperature [97]. On the other hand, Tadesse et al. [98] proposed a hydrothermal method to prepare nitrogen-doped magnetic CQDs using lemon juice and ethylenediamine. These reagents were mixed and heated at 200 °C for 3 h to obtain a black paste, which was washed with water to remove insoluble matter. Dichloromethane was added to obtain a brown solution, and a coprecipitation reaction was employed for the magnetic impregnation where metallic salts of Fe3+/Fe2+ and CQDs were mixed in aqueous solution. NaOH was added drop wise to this system, and the final product was a magnetic CQDs soluble in water. Recently, Nuengmatcha et al. [99] reported magnetic mercapto-functionalized GQDs for Cd2+ adsorption. GQDs were prepared using citric acid (2 g) heated at 260 °C where 100 mL of 0.25 M NaOH was added when the color changed to yellow. Maghemite was the magnetic phase and produced by mixing 5 g of FeCl3·6H2O, 2.5 g of FeSO4·7H2O, and deionized water. Subsequently, 20 mL of 28% NH4OH was added, and the solution was heated at 80 °C for 30 min under N2 atmosphere. GQD solution was mixed with maghemite, and this suspension was heated at 80 °C for 30 min, washed with deionized water, and dried at 90 °C. Magnetic GQDs were modified with C2H5OH and H(CH2)Si(OCH3)3. Kahrizi et al. [100] also reported a similar procedure to prepare magnetic GQDs combined with hydroxyapatite for Cd2+ adsorption.


## 3.3. Magnetic Carbon-Based Adsorbents Prepared from Low-Cost Feedstocks

One advantage of magnetic carbon-based adsorbents is the possibility of using a wide variety of carbon supports (or holders). However, the preparation and regeneration of adsorbents based on CNTs, graphene, and fullerenes as template are relatively difficult and expensive thus limiting their application at industrial scale [101]. The preparation of carbon materials via simple and low-cost procedures is highly desirable to reach the scale-up and commercialization of magnetic adsorbents [101]. The use of low-cost feedstocks is an alternative to achieve this target. It is necessary to apply raw materials that are abundantly available in nature or produced as by-product and wastes in agro-industrial and other processes. Examples of low-cost feedstocks for the preparation of carbon-based materials include biomasses and urban wastes such as chestnut shell [25], rice straw [27], banana peel [31], pomelo peel [101], rubber tires [102], Tetra pak residues [55], and sewage sludge [103, 104]. AC, BC, and other carbon-based supports can be obtained from the processing of these wastes via thermal decomposition (e.g., via pyrolysis or HTC) to prepare suitable adsorbents.For example, a magnetic AC derived from the carbonization of waste rubber tires and iron impregnation was combined with polyethylenimine to prepare an adsorbent for the removal of methyl red in batch and column experiments [102]. This adsorbent showed a strong dye affinity due to the abundance of hydroxyl and amine groups with an adsorption capacity of 526 mg/g in batch conditions and a breakthrough time of 150 min. This dye adsorption process was also exothermic. Huang et al. [101] synthesized a magnetic adsorbent using pomelo peels as precursor. This biomass is considered as inedible to humans and is discarded in landfills. These authors proposed a one-pot synthesis method to obtain a magnetic material with a core-shell structure to adsorb apolar parabens and nonpolar fluoroquinolones. This adsorbent showed a competitive removal for both compounds. Also, Deng et al. [105] reported a hybrid magnetic adsorbent obtained from carbon dots and CNTs for carbamazepine removal. Specifically, carbon dots were prepared via HTC of a mixture of diaminoethane, citric, and nitric acids. Magnetic CNTs and carbon dots were mixed in a rotovapor to prepare this adsorbent, which showed an adsorption capacity of 65 mg/g at pH 7. Carbamazepine adsorption was fast and achieved 80% removal within the first 3 h of contact time. This adsorbent was easily separated and was regenerated up to 6 times with a capacity loss less than 2.2%Herein, it should be pointed out that the compounds used to confer magnetic properties in an adsorbent can be also obtained from low cost materials such as urban and industrial wastes (e.g., sewage sludge) [104]. One illustrative example is the iron salts utilized in anaerobic biological wastewater treatment system [104] and chemical precipitation [106]. Sewage sludge contains high amounts of iron species that can be converted to iron oxides with both magnetic and adsorption properties [103, 104]. For instance, a magnetic alkali-acid adsorbent was prepared via the pyrolysis of municipal sewage sludge (containing polyferric sulfate) for the tetracycline removal [103]. Results showed an adsorption capacity of 286 mg/g where the preparation method affected the adsorption properties of this material. Tetracycline adsorption was dominated by π-π stacking interaction and strong pore filling effect. Another interesting example is the application of electric arc furnace dust to prepare magnetic adsorbents for water treatment [107]. This material contained a significant amount of iron (37%) and is generated as by-product from steel industrial sector.


## 3.4. Techniques for the Characterization of Magnetic Carbon-Based Adsorbents

It is important to highlight that the use of instrumental techniques for adsorbent characterization provides key and useful results for understanding the structures and mechanisms involved in the adsorbent preparation route as well as the interactions adsorbate-adsorbent and material performance. The use of these instruments is essential to validate the synthesis routes and analyze the surface chemistry changes of adsorbent after its application to explain its adsorption properties and mechanisms. For the characterization of magnetic adsorbents, there are several techniques that can be used:(1)
Surface chemistry, structural, and morphology characterization using Fourier Transform Infrared Spectroscopy (FTIR), X-Ray Diffraction (XRD), N2 adsorption/desorption isotherms, X-ray Photoelectron Spectroscopy (XPS), High Resolution Transmission Electronic Microscopy (HRTEM), and Transmission Electronic Microscopy (TEM)(2)
Magnetic properties measurement with Vibrating Sample Magnetometry (VSM) and Mössbauer Spectroscopy (MS)In particular, the electronic microscopy provides important and useful information for understanding the adsorbent performance by (1) analyzing their morphology and chemical composition and (2) studying the specific structures and textures such as the arrangement and dimensions of aromatic layers and interlayer spacing [108]. FTIR analysis gives valuable information about the main surface functional groups, and XRD analysis contributes to study the crystalline structure, while MS is employed to determine oxidation states, electronic spin-state, coordination number, and environment for coordinating compounds. It is convenient to indicate that if iron compounds are analyzed, then the technique is known as Iron-57 Mössbauer Spectroscopy [109–111]. XPS helps to identify the functional states of elements and their chemical bonds on the adsorbent surface [112]. N2 adsorption/desorption isotherms give information about the adsorbent textural parameters (i.e., surface area, porosity distribution, and pore volume) [113]. Magnetometry measures the magnetic properties like magnetic moment, permeability, and saturation magnetization. Each instrumental method provides relevant, comparative, and complementary information about the magnetic adsorbents. Based on the fact that the carbon precursor and adsorbent synthesis method generate the possibility to obtain a wide spectrum of materials, the physicochemical properties of magnetic adsorbents can vary substantially. Therefore, a proper and detailed characterization of these adsorbents is fundamental to explain their performance in water treatment and other applications.


## 4. Use of Magnetic Adsorbents for Water Pollutant(s) Removal

Water pollution is undoubtedly a relevant environmental problem where the magnetic carbon-based adsorbents have found to be effective to contribute to its resolution. Adsorption capacities of these materials vary as a function of the adsorbent properties (e.g., surface area and functionalities), the carbon precursor and synthesis route, as well as the adsorption operation conditions like solution pH, temperature, pollutant concentration, among others. Therefore, the adsorption of representative pollutants such as arsenic, pharmaceuticals, heavy metals, dyes, fluoride, pesticides, and other relevant compounds using magnetic carbon-based adsorbents is analyzed and discussed, including their removal performances. Several tables are reported to summarize recent studies about the adsorption of water pollutants on magnetic adsorbents where the synthesis route, experimental conditions, adsorption capacities, and properties are shown.


### 4.1. Arsenic

Arsenic (As) is a geogenic pollutant of water supplies that is a major problem for public health and, consequently, a current and relevant environmental problem for the population of several countries of Southeast Asia, Latin America, and Europe. Natural sources and anthropogenic activities (pesticide usage, fossil fuel combustion, and mining) are the main causes of arsenic pollution [27]. It shows a severe toxicity to humans, and, consequently, the US Environmental Protection Agency (EPA) [114] and World Health Organization (WHO) [115] have recommended a maximum threshold of 10 ppb for arsenic concentration in the water used for human consumption with the aim of protecting consumers supplied by public water systems [26, 33, 116]. However, it has been calculated that over 100 million people can be exposed to arsenic-polluted water [117]. Chronic exposure to arsenic could cause dermal lesions, hypertension, diabetes, cancer, and peripheral vascular disease [115, 118]. This pollutant can occur in oxidation states of +5, +3, 0, and -3, and it is frequently found as arsenates or arsenites [115]. Therefore, the toxicity of this pollutant strongly depends on its chemical nature. Arsenate (AsO4)3 with (+5) or arsenite (AsO3)3 with (+3) are the most frequent forms of arsenic in water where arsenite is 20 times more toxic than arsenate [16, 119]. This toxic pollutant can be removed from water using magnetic carbon-based adsorbents. This adsorption process could imply surface complexation and electrostatic attraction between the magnetic adsorbents and arsenic species in the aqueous solution [27, 119]. Table 1 shows recent studies of arsenic adsorption using magnetic forms of AC, CNTs, BC, CNCs, GO, and RGO.Table 1
Removal of arsenic from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAs specieAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic MWCNTs by microwave-assisted processFe3O4 and γ-Fe2O3Commercial MWCNTsAs3+As5+1.7230.1897440--153[49]Magnetic CNTs by catalytic CVD vapor deposition with alkali-activated methodFe3O4 and γ-Fe2O3EthanolAs3+As5+8.139.745.52527.2662.1[119]Sulfhydryl-functionalized MWCNTs with CVD synthesis and high-temperature treatmentFe3O4 and γ-Fe2O3EthanolAs3+19.1272527.3139.9[89]Magnetic BC by thermal impregnation of biomass with natural hematite and direct pyrolysis procedureγ-Fe2O3PinewoodAs5+0.429722--193.1[24]Magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+As5+54.1826.76852512.870.20[189]Magnetic MWCNTs by oxidation and coprecipitationFe3O4Commercial MWCNTsAs3+As5+14.2616.856.833039.37119.09[91]Magnetic RGO/CNT composites by graphite exfoliation and coprecipitationFe3O4Commercial MWCNTs and graphiteAs3+As5+9.115.1725----[190]Si-magnetic GO by graphite exfoliation and coprecipitation and sol-gel coatedSi-coated Fe3O4GraphiteAs3+As5+7.511.41425----[191]Aerogel magnetic CNCs by sol-gel impregnation and pyrolysisFe3CCitric acidAs5+56.2725--290[29]Magnetic AC by impregnation using iron and manganese oxidesγ-Fe2O3Commercial ACAs5+19.353250.35649.4[116]Magnetic BC by hydrothermal impregnation and carbonizationFe3O4Orange peelAs5+81.36245396[23]Magnetic CNCs by thermal impregnation with iron salts and pyrolysis methodFe3CPine resinAs3+263.9356.674----177[33]Magnetic AC by coprecipitation, impregnation and carbonization processFe3O4Cigarette sootAs3+As5+80.99107.96732510.77575.6[16]Gelatin modified–magnetic BC by pyrolysis and impregnation by coprecipitationγ-Fe2O3Chestnut shellAs5+45.842542--[25]Magnetic CNCs by coprecipitation, impregnation, and hydrothermal synthesisFe3O4GlucoseAs5+20.051-22535.1--[15]Magnetic SWCNTs prepared by arc discharge evaporationFe3O4 and γ-Fe2O3GraphiteAs5+49.65425----[17]Magnetic BC by thermal impregnation and pyrolysis with microwave heatingFe3O4Empty fruit bunch from palmAs5+88N. D.25--890[26]Calcium-based magnetic BC by coprecipitation impregnation and pyrolysisFe3O4Rice strawAs3+6.34525----[27]Magnetic CNTs by inverse coprecipitation and impregnation with Ni-Zn-ferriteNi-Zn-FerriteCommercial MWCNTsAs5+6622515214[92]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteAs5+2-12142534148.2[44]3D magnetic GO hydrogel by graphite exfoliation, coprecipitation, and one-pot method combining GO sheets, Fe3O4, and polyacrylamide hydrochlorideFe3O4GraphiteAs3+As5+25.174. 27.76.22510.5--[192]MWCNT membranes modified with CuFe2O4 by coprecipitation and using polyvinylidene fluoride (PVDF) membrane supportCu ferriteCommercial MWCNTsAs3+31.25725----[50]Chitosan magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+457.32549.3152.38[120]MGO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+993------Multifunctionalized magnetic GO by coprecipitation and multiple impregnationFe3O4Commercial GOAs3+As5+62.719.372523--[76]1,4-butane sultone modified magnetic AC by carbonization, activation, and finally magnetic impregnation with magnetic phase coprecipitatedFe3O4Pistachio shellAs3+151.515.52511.6--[143]Magnetic BC by coprecipitation, pyrolysis, and high-energy ball milling impregnationFe3O4 and γ-Fe2O3Slovak LigniteAs5+19.93.925--10.6[193]HTC with iron salt followed by NaOH additionFeCl3Olive pomaceAs5+3.5525----[194]Pyrolysis and two step magnetizationγ-Fe2O3Corn strawAs5+6.7772517.5115.43[195]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Ntim and Mitra [49] used iron oxide supported on MWCNTs as arsenic adsorbent. MWCNTs were microwave-assisted functionalized and then dispersed in an aqueous solution of FeCl3:FeSO4 via ultrasonication. This magnetic material showed adsorption capacities of 189 and 1723 μg/g for As5+ and As3+, respectively. Kinetics and isotherms of arsenic adsorption were fitted with the pseudo second-order, Langmuir, and Freundlich models. These authors concluded that arsenic adsorption on this magnetic adsorbent could occur via multiple interactions where the complexation with adsorbent oxyhydroxide sites played a key role.On the other hand, a novel magnetic adsorbent prepared from orange peel as precursor was studied by Meng et al. [23]. This adsorbent was obtained using hydrothermal process with an iron solution. The influence of operation variables such as solution pH, temperature, and coexisting inorganic coadsorbates on As5+ adsorption was investigated. An As5+ adsorption capacity of 81.3 mg/g was obtained with an iron/biomass ratio of 10 wt%. Solution pH affected the arsenic adsorption process, and this removal was also endothermic. The characterization results indicated the formation of a dendrimer-like structure that surrounded the crystal iron NPs inside the branch with the amorphous carbon. Also, an adsorption−reduction phenomenon that included inner reduction and complex adsorption was identified with the characterization data. Removal efficiency after 3 cycles of adsorption-regeneration was found 89% where deadsorbent showed good mechanical stability with a low iron release (i.e., <0.3 mg/L).Sahu et al. [16] prepared a novel Fe3O4 AC using as precursor cigarette soot. FTIR, Zeta potential, N2 physisorption, EDX, TEM, SEM, XRD, and VSM were used in the adsorbent characterization and to confirm the magnetic phase formation. This adsorbent showed 575.6 m2/g of surface area and 10.77 emu/g of magnetic properties. As5+ adsorption was affected by solution pH where it was reduced with pH increment, while As3+ adsorption increased from pH 3 to 7 and then decreased. Experimental adsorption data were correlated with pseudo second-order and Langmuir models. The highest adsorption capacities were 80 and 110 mg/g for As3+ and As5+ at pH 7, respectively. Regeneration studies were performed with 0.5 M NaOH, and results indicated that the adsorption capacities of this adsorbent did not decrease significantly up to 4 consecutive regeneration cycles. The adsorption of As3+ and As5+ species was mainly associated to the hydroxyl groups on the adsorbent surface. Finally, it was concluded that a monodentate complex formation prevailed for As3+ adsorption, while both monodentate and bidentate complex formation and electrostatic attraction were involved in As5+ adsorption.Multicomponent adsorption of As3+ and Cd2+ was studied using calcium-based magnetic BC with rice straw as carbon source and iron salts [27]. Results demonstrated that the iron favored As3+ adsorption, while calcium enhanced Cd2+ uptake. In the experiments with one adsorbate, the adsorption of both pollutants depended on solution pH where the maximum removal rate was obtained at pH 6 with maximum adsorption capacities of 10.07 and 6.34 mg/g for Cd2+ and As3+, respectively. Multicomponent adsorption of these adsorbates included synergistic and competitive effects. In the binary solutions, As3+ adsorption decreased in 15–33% due to the presence of Cd2+ as coadsorbate, while Cd2+ adsorption increased in 3–16% due to the presence of As3+. The formation of type B ternary surface complexes and electrostatic interactions were associated to the multicomponent adsorption effects observed for the binary solution Cd2++As3+.Graphite powder and iron salts were used to prepare a magnetic GO for the As3+ adsorption from aqueous solution [120]. The characteristics of this magnetic GO were studied with FTIR, XRD, and Field Emission SEM/EDX instruments. A central composite design (CCD) was employed to study the As3+ adsorption at batch conditions where the impact of As3+ concentration, contact time, pH, and adsorbent dosage were analyzed by response surface methodology (RSM). The solution pH impacted the As3+ adsorption where the highest removal was obtained in the range of 2–6. As3+ removal was 99.95% at pH 7, adsorbent dosage of 0.3 g/L, contact time of 77 min, and an initial As3+ concentration of 100 mg/L. 0.1 M NaOH was used to regenerate the magnetic GO where its removal performance decreased up to 80% after 4 adsorption-desorption cycles. FTIR analysis confirmed that As3+ adsorption involved a monodentate complexation between arsenic oxyanions and magnetic GO surface functionalities.It is important to highlight that arsenic adsorption studies have been carried out mainly at batch conditions, and only few authors have reported packed bed columns for this purpose [117]. Particularly, Xu et al. [117] reported the breakthrough curves for the As5+ adsorption with a magnetic composite obtained from bagasse biomass and iron oxide. The biomass was first impregnated with iron salts in microwave oven, then, it was sonicated with ethanol and subsequently carbonized at 500 °C. Breakthrough curves of As5+ adsorption were quantified at different conditions of bed height, solution flow rate, pH, and As5+ feed concentration. Results showed that the increment of As5+ feed concentration reduced the exhaustion time and breakthrough points. The increment of solution pH and bed height decreased the As5+ adsorption rate. This adsorbent can be regenerated with 1 M EDTA to recover its As5+ adsorption capacity.


### 4.2. Pharmaceuticals

Pharmaceutical products, once used or expired, are considered a special type of waste in the environment that have been catalogued as chemicals of emerging concern to the public because of their potential to pollute water [115, 121, 122]. The global pharmaceutical consumption is estimated as ~1,000,000 tons/year with 15 g/year as per capita use [123]. Several pharmaceutical molecules cannot be totally absorbed and metabolized, thus, they are excreted and released to the environment. Therefore, a significant amount of pharmaceutics is discharged into the environment during its production, delivery, use, application, and excretion [115, 124]. For example, the tetracycline (TC) is an important antibiotic widely utilized as antimicrobial in livestock industry and human therapy. It has been established that 50–80% of TC used in the farming industry can be excreted as unmodified parent compounds via urine and feces [125]. Besides, conventional water treatment plants are not designed to remove pollutants at trace concentrations, and, consequently, the degradation or separation of this and other pharmaceutical compounds is not effective [122, 126]. Pharmaceutical molecules could be found in concentrations ranging from ng/L to μg/L in ground waters, wastewaters, and surface waters [124]. Wastewaters could contain significant amounts of more than 55 pharmaceuticals over the 150 daily used compounds [127–129]. Most of these compounds have been categorized as essential by the WHO. The bioaccumulation of these compounds represents a serious eco-toxicological risk and implies adverse effects like organism drug resistance, metabolism disruptions, and bacteria strain proliferation [125, 129–131]. There are no international regulations to establish the threshold concentration for pharmaceuticals in the environment, which is mainly due to the lack of studies reporting the long-term effects caused by a chronic exposure to these emerging pollutants and their metabolites [132, 133]. The concentration of pharmaceutical compounds can be effectively reduced in water via adsorption [123]. Carbamazepine (CBZ), atenolol, erythromycin, diclofenac, ibuprofen (IBP), and naproxen are the common adsorbates analyzed in adsorption studies. A compilation of the magnetic carbon-based adsorbents utilized for pharmaceuticals removal is presented in Table 2.Table 2
Removal of pharmaceuticals from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic MWCNTs by hydrolysis impregnationFe3O4Commercial MWCNTsAmoxicillin33.564.627----[87]Magnetic AC by coprecipitation impregnationFe3O4Commercial ACNaproxen87.79325----[196]Magnetic MWCNTs with dibenzo-18-crown-6 by hydrolysis impregnationFe3O4Dibenzo-18-crown-6Amoxicillin263.1525----[88]Magnetic AC by coprecipitation impregnationFe3O4Commercial ACCarbamazepine182.9--25161241[134]Magnetic GO nanoplatelets by coprecipitationFe3O4Commercial GOAmoxicillin106.38525--543.2[135]Magnetic BC by impregnation with iron salts and direct HTCFe3O4Sugarcane bagasseTetracycline48.356.8309.7348.35[197]Magnetic AC by ball milling impregnationFe3O4Commercial coconut shell-based ACTetracyclineCarbamazepine45.3135.162520.8486[198]Magnetic BC by pyrolysis and ball milling impregnationFe3O4Coconut shellTetracyclineCarbamazepine94.262.762519365Chitosan-magnetic GO by coprecipitationFe3O4Commercial GOCiprofloxacin282.952514.76388.3[199]Magnetic AC by direct impregnation with hydrothermal method and functionalized with silanesFe3O4Commercial ACCarbamazepineClofibric acidIbuprofen114.378.7166.77252.65960.9[200]Magnetic MWCNTs by coprecipitation impregnationFe3O4Commercial MWCNTsAmoxicillin355.85725----[201]Magnetic GO spongeFe3O4GraphiteTetracycline47310351.14--[124]Magnetic carbon microspheres by pyrolysis and direct hydrothermal impregnationFe3O4GlucoseSulfonamide27.8542542.31228[136]Magnetic BC by pyrolysis and impregnationγ -Fe2O3Astragalus membranaceus residuesCiprofloxacin68.962523.96203.7[202]Pyrolysis of sewage sludge and alkali-acid treatmentγ-Fe2O3Sewage sludgeTetraciclyne286.91745--141.78[103]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteTetracycline252.02-122534148.2[44]Magnetic carbon via carbonizationα-FeMetal-organic frameworkTetracycline511.0674555.51171.7[203]Magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteChlorpheniramine472.01025--221[204]Magnetic AC by impregnation with iron and cobaltCobalt ferriteCommercial ACAmoxicillinParacetamol444.2399.97253.07893.8[205]Magnetic AC by simultaneous pyrolysis, impregnation, and activationγ-Fe2O3Corn stalksNorfloxacin7.691025--760.7[206]Magnetic BC yolk shell by calcinationFe3O4Resorcinol and formaldehydeSulfamethazine312.562519.77247[207]Pyrolysis of bones at 500 °C, coprecipitationFe3O4Chicken boneTetracycline98.892–102664.7328.06[171]GO/diethylenetriaminepentaacetic acidFe3O4Commercial GOTetracyclineCiprofloxacin294.12111.73330--176[208]Manganese-based magnetic BC by pyrolysis and coprecipitation impregnationFe3O4Potato stems and leavesNorfloxacinCiprofloxacinEnrofloxacin6.948.377.193309.8252[209]Magnetic GO-polyaniline by graphite exfoliation and coprecipitationFe3O4GraphiteCiprofloxacin106.38625----[210]Nitrogenated magnetic RGOFe3O4Commercial GONorfloxacinKetoprofen158.1468.06.825--38.2[75]Magnetic BC by pyrolysis and impregnated by oxidative hydrolysisFe3O4 and γ-Fe2O3Pine sawdustSulfamethoxazole19.094.52547.8 Amp∗m/kg125.8[211]Magnetic RGO hydrogelFe3O4Commercial RGOTetracyclineCiprofloxacin4.762.7862514.566.8[212]Polyglycerol mediatedSPMGOFe3O4Commercial GOTetracycline684.937256.81--[213]Carbon dot modified magnetic CNTs by coprecipitation impregnation and hydrothermal modificationFe3O4Commercial CNTs and citric acid for carbon dotsCarbamazepine657255.64184.1[105]Magnetic AC by direct impregnation and hydrothermal methodNi ferriteCommercial ACIbuprofenKetoprofen172.1985.64225256.25564.4[214]Magnetic CNTs by coprecipitation/hydrothermal impregnationFe3O4Commercial CNTsKetoprofenDiclofenacIbuprofen7.917.99.0525-----[215]Phenol resin melted at 40 °C, soft-templating, and impregnationFe3O4Phenolic resinMinocycline6------[1]Magnetic GO-SO3H by graphite exfoliation and coprecipitationFe3O4GraphiteIbuprofenTetracycline160.83500.6877303555.4--[131]Magnetic BC by carbonization and thermal activation procedureFe0White rot fungus ofPhanerochaete chrysosporiumDiclofenac361.25--21.651986[216]Magnetic GO-SiFe3O4GraphiteSulfamethoxazole15.4672526.98--[217]β-cyclodextrin- magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteSulfamethazine238.532530--[218]Magnetic CNT by hydrolysis impregnationMn ferriteCommercial CNTsBezafibrate33.472523.896.526[219]Humic acid coated magnetic BC by direct impregnation pyrolysis and coated after with humic acidFe3O4Potato stems and leavesNorfloxacinCiprofloxacinEnrofloxacin9.9711.468.410304.0426.28[30]Magnetic RGO sulfonated by pyrolysis, and inverse coprecipitation impregnationFe3O4Plastic bottle wasteGaramycinAmpicillin4565005.53.025254.9600[220]Magnetic BC by pyrolysis and coprecipitation impregnationFe3O4Banana biomassFurazolidone37.867.53041166.9[31]Magnetic AC by hydrothermal carbonization and thermally activated with pyrolysisFe3O4 and Fe0GlucoseBio sludgeIron sludgeSulfanilamideSulfadiazineSulfamethazineSulfamethoxazole63.7140.9178.6181.8625171385[221]Magnetic AC by coprecipitation impregnationFe3O4Commercial wood ACTetracycline208.332022.2--[222]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Baghdadi et al. [134] reported the preparation of a magnetic nanocomposite using a commercial AC and the CBZ adsorption tests. Different instrumental techniques (SEM, FTIR, N2 physisorption, VSM, XRD, and SEM) were utilized to characterize the surface chemistry, textural parameters, and magnetic properties of this adsorbent. CBZ adsorption from urban wastewater was optimized with a CCD by analyzing different operating conditions (total dissolved solids TDS, CBZ concentration, and adsorbent dosage). It was observed that a high magnetite content for the adsorbent preparation caused the blockage of composite porous structure and the reduction of CBZ adsorption capacities. The maximum CBZ adsorption capacities ranged from 182.9 to 280 mg/g. Besides, the CBZ adsorption decreased slightly with TDS concentration. Authors explained that CBZ adsorption was associated to carboxylic groups, and it was also concluded that the removal of CBZ was exothermic and spontaneous.The adsorption of amoxicillin (AMX), which is an antibiotic, on magnetic graphene nanoplatelets (GNPs) from aqueous solution was reported by Kerkez-Kuyumcu et al. [135]. Magnetite NPs and GNPs were used to obtain this adsorbent. Results showed that the magnetic GNPs outperformed GNPs and magnetite alone. The increase in solution pH reduced AMX adsorption, and this adsorbent showed a maximum adsorption capacity of 14.10 mg/g. Electrostatic and π– π interactions were associated to the AMX adsorption mechanism with magnetic GNPs. Pseudo second-order kinetic model fitted AMX adsorption, which was spontaneous and exothermic. Magnetic GNPs were regenerated with 0.15 M NaOH, and the adsorbent was utilized during 4 adsorption-desorption cycles where its adsorption capacity remained as 35%.Fe3O4 NPs and glucose were the feedstocks to obtain reusable magnetic carbon microspheres (CMs) via HTC [136]. This adsorbent was utilized to remove the antibiotic sulfonamide. Magnetic CMs samples were also calcined at 600 °C for 1 h to improve their surface properties thus obtaining a pore volume of 0.448 m3/g and surface area of 1228 m2/g. Pseudo second-order and Langmuir equations correlated the antibiotic adsorption data. The adsorption capacity of magnetic CMs decreased with pH and temperature, and the highest value of 24.22 mg/g was obtained at 10 °C and pH 4. Magnetic CMs were regenerated with NaOH thus obtaining an adsorption capacity of 18.31 mg/g after the antibiotic desorption, and this adsorbent was reused 4 times.Another type of antibiotics that represents a hidden danger to human health is the fluoroquinolones (FQs). Enrofloxacin (ENR), norfloxacin (NOR), and ciprofloxacin (CIP) were employed as FQs adsorbates to study the adsorption properties of a humic acid-magnetic BC [30]. These authors prepared a magnetic BC from potato stems and leaves, which were coated with humic acid (HA), see Figure 8. Humic acid-magnetic BC showed the presence of oxygenated functional groups that conferred its adsorption capacity. It exhibited FQ uptakes up to 1.8-3.4 times higher than those reported for raw and magnetic BC for these compounds. Specifically, this magnetic material showed adsorption capacities of 6.0, 7.5, and 7.1 mg/g for adsorbates ENR, NOR, and CIP, respectively, at 35 °C. The adsorption experimental data were adjusted and analyzed with Langmuir isotherm and pseudo second-order kinetic. FQ adsorption on this magnetic carbon-based adsorbent was associated to π-π, H-bond, hydrophobic, and electrostatic interactions.Figure 8
Humic acid coated magnetic biochar (MBC) derived from potato leaves and stems for fluoroquinolone antibiotics removal from water [30].Liyanage et al. [133] proposed the preparation of magnetic adsorbent using the IONP precipitation to modify a commercial Douglas fir BC. This magnetic BC was applied to remove 3 emerging water pollutants: caffeine (CF), IBP, and acetylsalicylic acid (ASA) in adsorption systems at batch conditions. This magnetic adsorbent showed a surface area of 322 m2/g, which was lower than that of BC (468.2 m2/g). The adsorption of these pharmaceuticals depended on solution pH and temperature. Authors concluded that H-bonding, electrostatic, and π-π interactions were present at different pH conditions. The adsorption capacities of this adsorbent were 80, 40, and 140 mg/g for CF, IBP, and ASA, respectively, at pH 8 and 35 °C. Competitive experiments in binary CF/IBP solutions showed a decrement in its adsorption capacity of 13.6 and 52.3%, respectively. Surface protonation and CF polarity contributed to generate strong adsorbate-adsorbent interactions thus leading to high adsorption capacities. Adsorbent regeneration was carried out with methanol and water, and results showed that the adsorption capacity remained almost constant during 5 adsorption-desorption cycles.Wei et al. [123] prepared 7 deep eutectic solvents (DESs) known as green sustainable solvents that were used to regulate the preparation of a magnetic composite from MOF MUiO-66-NH2 and Fe3O4. The removal of pharmaceuticals mefenamic acid (MF) and ofloxacin (OX) was analyzed with this nanoadsorbent, labelled as DES-MUiO-66-NH2. Under optimal conditions, the adsorption capacities were up to 97.60 and 79.22 mg/g for OX and MF, respectively. Hydrogen bonding, hydrophobic interaction, π-π stacking, chelation, and electrostatic interactions were the main forces involved in the adsorption mechanisms. Density functional theory calculations demonstrated the formation of chelation. It was also concluded that DES structures determined the adsorption properties of DESMUiO-66-NH2, thus, offering a green preparation route of tailored adsorbents for emerging water pollutants. The presence of coions (e.g., sulphates, nitrates, chlorides, calcium, potassium, and sodium) did not affect the adsorption. Desorption and regeneration tests were also carried out.


### 4.3. Heavy Metals

Heavy metals are also relevant water pollutants that are characterized by low biodegradability and high chemical stability. Heavy metals are toxic for ecosystems and human beings at certain concentration thresholds. Toxicological effects of heavy metals include reproductive problems, neurological disorder, renal disease, gastrointestinal bleeding, lung disease, hypertension, and cancer [137]. Lead (Pb), cadmium (Cd), copper (Cu), zinc (Zn), nickel (Ni), chromium (Cr), mercury (Hg), and manganese (Mn) are common heavy metals found in the environment and considered as priority water pollutants [137–139]. Water pollution by heavy metals is associated to the several industrial activities including, for instance, chemical processing, oil refining, electronic manufacturing, and mineral smelting [139]. Different magnetic adsorbents have been used in heavy metal adsorption, and Table 3 describes a survey of magnetic carbon-based materials used for this purpose.Table 3
Removal of heavy metals from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic CNTs by in situ coprecipitation modificationγ-Fe2O3Commercial CNTsCr6+11.25632543.29119.09[223]Magnetic BC by impregnation and direct pyrolysisγ-Fe2O3Peanut hullsCr6+77.5452536.79145.25[140]Magnetic GO by hummers method and impregnation in situ hydrothermal synthesisFe3O4GraphiteCr6+31.872512182[224]Amino functionalized magnetic GO by hummer method and impregnation in situ hydrothermal synthesisFe3O4GraphiteCr6+123.422530.257.55[225]Nitrogen doped magnetic AC by impregnation and direct pyrolysis processes using glucose as nitrogen sourceFe3O4 and Fe3CGlucose and melamineCr6+29.46725130.756.2[226]Carboxyl functionalized magnetic CNTs by solvothermal methodFe3O4Commercial CNTsCr6+22.2222570.62--[227]Chitin-magnetic CNTs by simple millingFe3O4Commercial CNTsCr6+10.72255.77569.1[228]Dithiocarbamate functionalized magnetic RGO by hummer method, reduction with hydrobromic acid, and magnetic impregnation by coprecipitation.Fe3O4GraphiteCu2+Cd2+Pb2+Hg2+113.64116.28147.06181.82566625--194.8[141]Magnetic fluorine and nitrogen codoped carbonFe3O4Melamine and polyvinylidene fluorideCr6+740.7153.4182.7[229]Magnetic AC high temperature carbonization and activationFe0, Fe3O4, and Fe3CActivated sludgeCr6+2033257.6114.24[230]Magnetic BC by iron salts impregnation and hydrothermal pyrolysisγ-Fe2O3Pinewood sawdustHg2+167.272515.5843.29[142]One step hydrothermal method with iron salt and hexamethylenediamineγ-Fe2O3Peanut hullCr6+142.86--25--62.4[64]Magnetic AC by low temperature carbonization, impregnation, and high temperature for magnetic modification and activationFe3O4Termite fecesCr6+663251.46699[231]1,4-Butane sultone modified magnetic AC by carbonization, activation, and finally magnetic impregnation with magnetic phase coprecipitatedFe3O4Pistachio shellPb2+Cd2+147.05119.045.52511.6--[143]Magnetic BC by pyrolysis and impregnation with coprecipitation of magnetic phaseFe3O4Banana peelsZn2+Cu2+Hg2+72.875.983.462539.55323.2[232]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteCd2+2-122342534148.2[44]Impregnation with humic acid, solvothermal process, and calcinationFe3O4Layered double hydroxidesCu2+Cd2+Pb2+400.0375.0200.0625--132.4[233]Magnetic BC modified with MnO by pyrolysis and impregnation with magnetic phaseFe3O4Palm kernel cake residueCd2+Cr3+Hg2+Pb2+18.6019.9249.6413.6972520.9489.38[144]Direct pyrolysis and sonochemical methodFe3O4Biogas residueCu2+Pb2+75.76 181.825--39.9679.64[234]Pyrolysis at 600 °C and physical comixingFe3O4Wheat stalk and rice huskPb2+73.34 - 179.552526.1 - 28.613.96 - 224.6[235]Pyrolysis at 500 °C, impregnation with iron saltγ-Fe2O3Blooms of alga EnteromorphaCr6+11.1322539.29--[236]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Peanut hulls are an abundant residual biomass with low cost that can be employed to prepare a magnetic BC for Cr6+ adsorption [140]. The best adsorbent was obtained via pyrolysis at 650 °C with an adsorption capacity of 77.54 mg/g. Adsorption studies showed that low solution pH and the particle size of magnetic BC were relevant variables to remove this pollutant. Characterization results suggested that iron oxide was crucial to obtain the magnetic properties of adsorbent. Cr6+ was desorbed up to 55.9% using NaOH. The removal mechanism of this pollutant involved an electrostatic attraction of the anionic chromium to the protonated –OH2+ of maghemite.Fu and Huang [141] analyzed the removal of Hg2+, Pb2+, Cd2+, and Cu2+ using a RGO that was functionalized with magnetic dithiocarbamate (DTC). A modified Hummers method was implemented to prepare GO, and the reduced and functionalized RGO composite was obtained via GO bromination, polyethylenimine nucleophilic substitution, reaction with CS2, and loading of Fe3O4 NPs. XRD, TEM, FTIR, and XPS techniques allowed the characterization of this magnetic adsorbent. The surface area of this adsorbent was 194.8 m2/g. The increment of solution pH from 2 to 4 improved the heavy metal adsorption. This adsorbent exhibited high adsorption capacities with the next trend: 165 mg/g of Hg2+>135mg/g of Pb2+>105mg/g of Cd2+>90mg/g of Cu2+. These experimental adsorption data were fitted with the pseudo second-order kinetic and Langmuir isotherm. Nanocomposite regeneration was done with a one-step organic reaction obtaining satisfactory heavy metal uptakes in 5 adsorption-regeneration cycles.Magnetic CCs and BC were prepared using pinewood sawdust, and they were subsequently applied for Hg2+ removal [142]. Pinewood sawdust was soaked in iron solutions and hydrothermally treated. Magnetic BC was obtained via pyrolysis, while magnetic CCs were prepared by calcination. Magnetic BC showed a surface area of 80.35 m2/g, which was higher than magnetic CCs (i.e., 43.29 m2/g); their adsorption capacities were 31.80 and 167.22 mg/g, respectively. These results suggested that textural parameters of these magnetic materials did not play a relevant role for Hg2+ adsorption. This finding was supported on the fact that magnetic CCs contained higher amounts of hydroxyl, lactone, and carboxyl groups than those identified for the surface of magnetic BC. Additionally, it was identified that magnetic CCs contained γ-Fe2O3 with a high crystallization degree. In fact, this adsorbent showed better regeneration and magnetic properties. Hg2+ adsorption mechanism implied coprecipitation, surface complexation, and electrostatic attraction.Heavy metals and antibiotics usually coexist in wastewater thus magnifying its toxicological profile. Therefore, Huang et al. [44] studied the application of magnetic GO and its reduced forms via chemical and annealing routes to remove As5+, Cd2+, and TC. The adsorption properties of these adsorbents and the corresponding mechanism for these pollutants were analyzed. In aqueous solutions with only one adsorbate, the adsorption of these pollutants was affected by solution pH and the adsorption capacities showed the next trend: magneticannealingRGO<magneticchemicallyRGO<magneticGO. In particular, the magnetic GO showed the best adsorption capacities with values of 13.9, 234 and 252 mg/g for TC, Cd2+, and As5+, respectively. The interaction effects of Cd2+ and TC in the multiadsorbate solutions were not significant. The presence of TC in the solution decreased significantly the As5+ adsorption, while As5+ did not affect TC removal in multicomponent solutions. The adsorption of As5+ and Cd2+ in the multiadsorbate solutions increased by 30 and 65%, respectively.A green synthesis was proposed to prepare a magnetic adsorbent with AC, 1,4-butane sultone, and Fe3O4 NPs for the removal of Cd2+, As3+, and Pb2+ under ultrasound [143]. Adsorption results showed that the heavy metal uptake under ultrasound conditions was fast and increased during the first 10 min. Nevertheless, the adsorption capacity decreased at operating times >10 min, and this phenomenon was associated to the release of metallic species from adsorbent surface. The maximum adsorption capacities in the aqueous solutions with one adsorbate were 95, 130, and 140 mg/g for Cd2+, As3+, and Pb2+, respectively. Competitive (i.e., multiadsorbate) adsorption experiments indicated that the adsorption capacities reduced in 12, 21, and 22% for Pb2+, As3+, and Cd2+, respectively. Thermodynamic parameters confirmed that the adsorption of these pollutants was feasible, exothermic, and spontaneous. Characterization techniques supported that the mechanisms of adsorption implied the heavy metal complexation with the SO3H and OH groups from the magnetic adsorbent surface.Maneechakr and Mongkollertlop [144] prepared and tested a MnO2-modified magnetic BC for the removal of Hg2+, Pb2+, Cr3+, and Cd2+. This magnetic adsorbent was obtained from Fe3O4 and palm kernel cake residue. Different techniques (SEM-EDS, FTIR, Boehm titration, N2 physisorption, XRD, and VSM) were utilized to characterize the adsorbent physicochemical properties. As expected, the pollutant adsorption was enhanced with increments of solution pH. Adsorption temperature did not show a high impact on the heavy metal removal although the process was endothermic. The maximum experimental adsorption capacities of Cd2+, Cr3+, Pb2+, and Hg2+ were 19.90, 21.20, 49.64, and 13.69 mg/g, respectively. Experimental data were modeled, and thermodynamic parameters were also obtained.


### 4.4. Pesticides and Other Pest Controllers

Pests and associated-diseases cause around 30% of global crop loss [145]. The pesticides are quite toxic chemical compounds tailored to kill off pests via their environment spread [146]. The biotransformation of these compounds is difficult thus causing their bioaccumulation for long periods. Agriculture production has increased the usage of pesticides, herbicides, insecticides, and fungicides thus generating an additional source of water and soil pollution [146, 147]. In particular, their residues can be still found on fruits and vegetables, and they could enter into water resources due to their microbial degradation resistance and chemical stability in the water [146, 148]. To illustrate the serious environmental problem associated to these pollutants, it can be indicated that studies performed in the United States detected 5 or more pesticides in several samples obtained from different streams, while ~400,000 tons of pesticides are used annually in China [149, 150]. In Europe, pesticides have been considered among the main pollutants of drinking water supplies [151].Since these chemicals are nonselective, they can be toxic for wildlife populations and humans that are the nontarget organisms [146]. Long-term exposure to these substances could lead to serious health effects like neurodegenerative diseases, cancer, hypertension, reproductive, endocrinal, mutagenic, genotoxic, and respiratory effects [146–148]. In particular, glyphosate is a pesticide widely used in agriculture and nonagriculture areas [147]. It causes acute toxic endocrinal, mutagenic, and carcinogenic effects [147]. On the other hand, acetochlor is an herbicide used to control gramineae weeds and has been reported in surface waters of United States at 2.5 μg/L, which is an enough concentration to induce health damage [148]. Also, atrazine is one of the most frequently detected pesticides in freshwater in United States. Therefore, a concentration limit of 3 ng/L was established by EPA for this compound in drinking water [114].Adsorption is effective to remove these toxic substances from water sources. Table4 summarizes the adsorption of pesticides and other pest controllers using magnetic carbon-based adsorbents. For instance, a hybrid composite obtained from the decoration of RGO with MnFe2O4 microspheres was used as adsorbent to remove glyphosate [147]. N2 physisorption, XPS, XRD, FTIR, and TEM analyses were performed for the adsorbent characterization. The glyphosate adsorption on this magnetic composite was associated to ion exchange and electrostatic interactions where 39 mg/g was the maximum adsorption capacity at 5 °C. Kinetic data were fitted with the pseudo second-order model, while Freundlich equation correlated the experimental isotherms. Glyphosate adsorption on this composite was exothermic at 5–45 °C. Surface area of this composite was 305.7 m2/g with the predominance of mesopores where TEM and SEM analyses also confirmed a proper dispersion of MnFe2O4 microspheres on the graphene nanosheets.Table 4
Removal of pesticides and other pest controllers from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic GO by chemical exfoliation and coprecipitation impregnationMn ferriteGraphiteGlyphosate33.444.725--305.7[147]Magnetic AC by direct impregnation with hydrothermal method and functionalized with silanesFe3O4Commercial ACBisphenol A126.97252.65960.9[200]Magnetic GO modified with Cu MOF andβ-cyclodextrin by coprecipitation impregnation and chemical modificationFe3O4Commercial GOThiamethoxamImidaclopridAcetamipridNitempyramDinotefuranClothianidinThiacloprid2.883.112.962.561.772.883.21----10.47250.33[237]Phenyl-modified magnetic GO/mesoporous silica by hierarchical bridge-pore structureFe3O4GraphiteAvemerctinImidaclopridPyridabenDichlorvosAcetamipridDursbanIsocarbophosPhoxim9.216.4012.7247.785.118.012.888.23--2525446.5[238]Magnetic BC by direct molten salt methodFe3O4Fir dustDichlorophenolAtrazine298.12102.17--2540.02404[239]Palm carbonization at 773 K, liquid phase reduction method for iron impregnationFe0PalmGlyphosate80.0425--253.97[153]Magnetic MWCNTs modified with Zn MOF by coprecipitation impregnation and chemical coordination methodFe3O4Commercial MWCNTsTriazophosDiazinonPhosaloneProfenofosMethidathionEthopropSulfotepIsazofos3.122.593.803.892.342.182.843.004--53.56128[152]Carboxilated magnetic GO modified with silica-coated magnetite by covalent couplingFe3O4GraphiteChlorpyrifosMalathionParathion13561.935.672533133[154]Magnetic CNTs functionalized with imidazole zeolite by thermal procedureFe3O4Commercial carboxylic-CNTsTetrabromobisphenol77.077309.65--[240]Magnetic GO by electrochemical exfoliationNiOGraphiteMethylparabenEthylparabenPropylparabenButylparaben3.125.288.4210.46525--227.5[241]Magnetic GO-AC by chemical exfoliation, solvothermal impregnationMn ferriteGraphite and commercial vegetal origin ACGlyphosate6.784.725--19.77[242]Chemical activation with H3PO4 for AC production, composite produced by coprecipitation methodFe3O4Peanut shellsAtrazine62.325.07----189.50[156]Magnetic AC coated with by pyrolysis, microwave activation and coprecipitation impregnationFe3O4Waste tyreMethylparabenPropylparaben85.990.0625---1281[155]Pyrolysis of bagasse at 600 °C, impregnation of salts, activation with KOHZn ferriteSugarcane bagasseImidacloprid313.06255.99660.0[243]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), metal-organic framework (MOF), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).MWCNTs and MOF ZIF-8 were utilized to obtain a magnetic adsorbent for the adsorption of organophosphorus pesticides from soil and water [152]. Isazofos, sulfotep, ethoprop, methidathion, profenofos, phosalone, diazinon, and triazophos were considered as adsorbates for this study. Multicomponent solutions with concentrations ranging from 0.2 to 8 mg/L were prepared with these 8 pesticides. Results of this study suggested that coordination-polymerization was involved in the incorporation of ZIF-8 particles on the magnetic MWCNTs surface. Adsorbent pore structure contained meso and macropores with a surface area of 127.95 m2/g. The adsorption capacities of this magnetic adsorbent for tested pollutants ranged from 2.18 to 3.89 mg/g where the lowest and highest removal were for ethoprop and profenofos, respectively. The authors determined that these adsorption capacities were lower than those reported in previous papers, and this finding was associated to the competitive (i.e., antagonistic) adsorption in multicomponent system in comparison to individual pesticide solutions. Solution pH played an important role in pesticides adsorption with pH 4 as an optimum condition. Langmuir model was outperformed by Freundlich equation to correlate the experimental data. It was concluded that the active sites of this magnetic adsorbent and pesticide molecules interacted via a valence-electron-driven adsorption with electrons exchanging or sharing.The glyphosate adsorption mechanism using a modified BC was reported by Jiang et al. [153]. A liquid-phase chemical reduction was employed to functionalize palm-based BC with nano-zero-valent iron. SEM, TEM, FTIR, and XPS techniques were utilized to characterize the final composite, which showed a surface rich in oxygenated functionalities and complex ligands with 253.97 m2/g of specific surface area. Experimental adsorption data were processed and analyzed with Langmuir and pseudo second-order equations. Authors concluded that the maximum glyphosate adsorption was obtained at pH 4, which was twice (i.e., 80 mg/g) than that of raw BC. The presence of phosphate or Cd2+ at low concentrations did not affect the glyphosate adsorption. But, an antagonistic effect was identified in the treatment of agricultural wastewaters that were polluted with organic compounds. Electrostatic forces, complexation, and hydrogen bonding were associated to the glyphosate adsorption mechanism using this magnetic adsorbent.Organophosphorus pesticide adsorption on GO-based silica coated magnetic NPs functionalized with 2-phenylethylamine was studied [154]. Malathion, parathion, and chlorpyrifos were considered as the target pollutants. Magnetic and physical properties of this adsorbent were characterized via VSM, N2 adsorption/desorption, Zeta potential, XRD, TEM, and FTIR. This adsorbent was spherical in shape and agglomerated, showing 33 emu/g of magnetic saturation and 133 m2/g of surface area. No significant differences in adsorption performance were found at different pH. This study showed that the interaction of pesticides with the adsorbent was not affected by deprotonation/protonation caused by pH adjustment. Pesticide adsorption capacities in aqueous solutions ranged from 10.9 to 11.1 where the minimum and maximum removal were for parathion and chlorpyrifos. Note that the parathion and chlorpyrifos adsorption was caused by π–π interactions and hydrogen bonding, while hydrogen bonding governed the malathion adsorption. These findings explained the order of adsorption capacities. Dubinin–Radushkevich and Sips models fitted the experimental adsorption data. Acetone was used for adsorbent regeneration where the recovery of tested pesticides was 89–100% in 10 adsorption–desorption cycles.Mashile et al. [155] reported the synthesis of a recyclable magnetic adsorbent using chitosan and waste tyre AC for the simultaneous adsorption of propylparaben and methylparaben. Adsorbent characterization was done with FTIR, SEM, TEM, and XRD. Surface area of this composite was 1281 m2/g. Pseudo second-order kinetic model described the adsorption of these pollutants. Redlich-Peterson and Langmuir models were used to correlate the binary adsorption of propylparaben and methylparaben. It was calculated that the maximum Langmuir monolayer adsorption capacities for propylparaben and methylparaben were 90.0 and 85.9 mg/g, respectively. This magnetic composite was chemically stable and useful after 7 cycles of adsorption-desorption.Agani et al. [156] evaluated the atrazine adsorption from water using a fixed-bed column packed with a magnetic composite prepared from AC, chitosan, and magnetite. XRD and FTIR techniques allowed to analyze the composite surface chemistry. Experimental designs based on CCD and RSM optimized the adsorption operating variables (i.e., flow rate, bed depth, atrazine initial concentration, and pH). The impact of these operating variables on adsorption process was also analyzed. The experimental results indicated the preparation of a mesoporous adsorbent with 188.50 m2/g of surface area and 62.32 mg/g of atrazine adsorption capacity. Yoon–Nelson, Yan, Bohart–Adams, and Thomas models were used to fit the breakthrough curves. These models allowed to analyze the limiting step of mass transfer for atrazine adsorption with this composite. Bohart-Adams model offered the best correlations for the adsorption data. Composite regeneration and atrazine desorption was studied with NaOH and HCl, thus, confirming the recycling potential of this magnetic material.


### 4.5. Fluoride

Fluorine is a geogenic water pollutant with a wide environmental distribution [157]. Different studies have documented its natural existence in soil, rocks, and groundwater [157]. Also, fluoride has been detected in effluents and wastewaters from fertilizers, electroplating, metal processing, cement, electronic manufacturing, and other industrial sectors, which also contributes as anthropogenic sources of water pollution [158, 159]. Fluoride can contribute to bone tissue development in human beings, but its chronic exposure can cause dental and skeletal fluorosis [157, 159]. The prevalence of dental fluorosis has been reported in more than 50 countries where the population of China is significantly affected by this disease [157]. It has been estimated that fluoride concentration in drinking water exceeds the WHO limit concentration (1.5 mg/L) in more than 25 countries [158]. As a result, over 300 million of people around the world are exposed to develop health problems associated to a chronic fluoride exposure. Herein, it is convenient to highlight that recent epidemiological advances have demonstrated that soft tissues are also affected by fluoride, and its toxic effect is known as nonskeletal fluorosis [159], which also could include damage to the respiratory, renal, immune, endocrine, digestive, central nervous, and cardiovascular systems [157, 159]. Therefore, low-cost and effective methods for the reduction of fluoride concentrations in water are required and demanded in particular for low-income countries.Adsorption is the most commercial technology for fluoride water depollution. Table5 summarizes the adsorption of fluoride using magnetic carbon-based adsorbents. For example, Mohan et al. [160] prepared a corn stover BC with slow pyrolysis at 500 °C, which was magnetized with an aqueous Fe3+/Fe2+ solution and treated with NaOH. BC with and without magnetic properties was characterized by Raman, energy dispersive X-Ray fluorescence (EDXRF), TEM, SEM-EDX, FTIR, and XRD analyses where magnetic moment and textural parameters were also measured. Maximum fluoride adsorption capacities were 6.0 and 4.11 mg/g for BC without and with magnetic properties, respectively, at 25 °C and pH 2. An exothermic fluoride adsorption was identified for both adsorbents at 25–45 °C. Fluoride adsorption kinetics were adjusted with the pseudo first order model. Fluoride adsorption in real ground water was reduced by the interference of solids and other ions such as Na+, Cl-, and NO3-.Table 5
Removal of fluoride from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceImpregnation methodγ-Fe2O3Cotton cellulose18.64 – 925--2.23[244]Pyrolysis at 500 °C and coprecipitation methodFe3O4Corn stover4.112255.13.61[160]Chemical deposition of Fe3O4γ-Fe2O3Graphite77.1272522.66--[245]Impregnation methodFe3O4Yak dung3.985 – 625--79.49[246]BC impregnation with iron salt, pyrolysis at 600 °C.Fe3O4Douglas fir biochar7.5815.5725--494[161]Impregnation with CaCl2 and FeCl3. Carbonization at 300–700 °C during 2 hγ-Fe2O3Cattle dung157.525–45--19.2[247]Impregnation with FeCl3 and pyrolysis after impregnation.γ-Fe2O3Bovine bone5.238254.4341.77[162]Oak shell calcination at 800 °C and iron salt impregnationFe3O4Oak shell454.5469.46226.78[163]AC impregnation and pyrolysis at 500 °C during 2 h.Fe3O4Pea peel4.712–1025-55---[164]Adsorbent nomenclature: biochar (BC).Dewage et al. [161] prepared a Douglas fir BC with Fe3O4 and α-Fe2O3. N2 physisorption, XPS, XRD, TEM, and SEM/EDX were applied to characterize BC precursor and the magnetic BC. Adsorbent magnetization and generation of additional adsorption sites were obtained with the dispersion of Fe3O4 and α-Fe2O3 particles. In fact, the magnetic adsorbent showed higher fluoride and nitrate adsorption capacities than those of BC. An endothermic and pH-dependent fluoride removal was identified. Experimental isotherms were analyzed and correlated with Langmuir model. Fluoride and nitrate adsorption capacities of magnetic BC were 9 and 15 mg/g, respectively, which outperformed the values reported for other oxide-based adsorbents and BC. Adsorption mechanism of both adsorbates (i.e., fluoride and nitrate) implied the hydrogen bond formation with the participation of protonated surface hydroxyls on the iron oxides.BCs and their magnetic versions were prepared with bovine bone and peanut hull for fluoride adsorption [162]. XPS, FTIR, XRD, SEM-EDX, and VSM were used to analyze the surface chemistry and magnetic properties of these adsorbents. A prepyrolysis approach (i.e., biomass+ironsalts+pyrolysis) enhanced the fluoride adsorption capacity of the magnetic BC in comparison to the adsorbent obtained from a postpyrolysis where BC was mixed with Fe3+/Fe2+ solution. Fluoride adsorption capacity of bovine-based magnetic adsorbent was >5 mg/g mainly due to γ-Fe2O3 and hydroxyapatite, which outperformed the nonmagnetic BC. It was inferred an ion exchange process in this endothermic fluoride removal. Freundlich model fitted the experimental adsorption isotherms of magnetic BC. Fluoride desorption was studied with 0.1 M NaOH solution, and results indicated that the magnetic BC maintained an acceptable adsorption performance for several regeneration cycles.A nanocomposite obtained from Fe3O4 and oak shell AC was used and assessed in fluoride adsorption [163]. Surface areas reported were 226.78 and 65.33 m2/g for AC/Fe3O4 and Fe3O4, respectively. Freundlich equation fitted satisfactorily the fluoride adsorption isotherms where the maximum adsorption capacity of AC/Fe3O4 was 454.54 mg/g, which is an outstanding performance for adsorbents reported for fluoride removal considering that their adsorption capacities ranged usually from 1 to 10 mg/g. The pH increment did not favor the fluoride adsorption and thermodynamic calculations confirmed an endothermic fluoride removal employing this magnetic adsorbent.Sahu et al. [164] evaluated the fluoride adsorption with a magnetic AC prepared using pea peel biomass impregnated with FeCl3 and pyrolyzed at 500 °C. Fluoride removal tests were performed with column and agitated tank modes. Initial fluoride concentration, solution pH, adsorbent dosage, and contact time were the operating parameters analyzed at batch adsorption conditions. The maximum fluoride adsorption capacity was 4.71 mg/g; it was established that water defluoridation was endothermic and pH dependent. Freundlich model was better than Langmuir model to fit fluoride adsorption isotherms. In the case of column studies, the breakthrough curves were analyzed with Clark, Yoon-Nelson, Adams-Bohart, and Thomas equations. This magnetic adsorbent showed a promising performance for water defluoridation in both batch and column operation modes. Fluoride adsorption mechanism was governed by fluoride-adsorbent interactions involving ketone, methyl, and hydroxyl groups, while the iron species imparted a positive charge to the adsorbent surface that generated electrostatic attraction forces for binding fluoride ions.


### 4.6. Dyes, Other Organic Pollutants, and Radionuclides

Dyes are complex organic molecules that are the most evident indicator of water pollution [165]. These compounds affect the aesthetic of aquatic systems and interfere with the sunlight transmission thus impacting the photosynthesis [165]. Dye classification includes different categories like nonionic (disperse dyes), cationic (basic dyes), and anionic (reactive, acid, and direct dyes), which can also consider their chemical structures like azo, anthraquinone, indigo, triphenylmethyl, and phthalocyanine derivative [165, 166]. These organic compounds are toxic and persistent pollutants with low degradability that can cause serious health effects with mutagenic and carcinogenic impacts on organisms [167–169]. Textile and dyeing industrial sectors are considered as the main contributors to this environmental pollution due to a significant release of dyes and related compounds into the water sources. It has been estimated that more than 100,000 commercial dyes are known, and their production is ~1.6 million tons of dyes/year where 10-15% can be released in wastewaters thus affecting the ecosystems [166, 168]. Dye adsorption with magnetic carbon-based adsorbents has proved to be effective. For illustration, Table 6 summarizes the dye adsorption using magnetic carbon-based adsorbents.Table 6
Removal of dyes, organic pollutants and radionuclides from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceOne-pot method--CNTsRhodamine BCongo redMalachite greenMethylene blueNeutral red28.052.076.082.0101.0253.64186.3[248]Impregnation-pyrolisisFe3O4Empty fruit brunchMethylene blueOrange G31.2532.362-101025----[170]Impregnation methodFe3O4Coconut shell-activated carbonSunset yellow22.33 – 10--16.55-28.74238-372[249]Electromagnetization techniqueFe3O4Brown marine macroalgaeAcid orange 738253026.79336.97[250]Pyrolisis of SrFe12O19 and BCSrFe12O19Sewage sludgeMalachite green388.6572511.11--[251]Pyrolysis of rubber tires, impregnation with iron, and functionalization with polyethylenimineFe3O4Waste rubber tiresMethyl red526.0--25--153[102]β-Cyclodextrin-L-glutamic acid-magnetic GOFe3O4GraphiteEstradiol85.8072590.43298.9[252]One step coprecipitationFe3O4SludgeAcid orange 720.795.22258.4965.47[253]CoprecipitationFe3O4Bone charReactive 5G blue91.58--509.79142.43[254]Pyrolysis of bones at 500 °C, coprecipitationFe3O4Chicken boneRhodamine B109.662 – 102664.7328.06[171]Magnetic BC by impregnation and direct pyrolysisZn ferriteRice strawEstradiol153.25--2.242357.8[28]Coprecipitation methodFe3O4Pineapple crown leaf wasteMethyl violet16.765--15.095.11-314.08[255]Microwave methodγ-Fe2O3Sugarcane bagasseMethylene blue36.142 – 10----54.49-109.07[256]Thermal graphitizationFe3O4BambooMethylene blue286.62 – 1025----[257]Impregnation of husk with ZnCl2, carbonization at 400 °C, wet impregnation of iron saltFe3O4Rice huskMethylene blueMethyl orange17.7813.21325--375.02[2]Pyrolysis of straw at 500 °C, impregnation with iron saltFe0Corn strawMalachite green515.7762538.780.1[167]Ball-mill extrusion with Fe3O4Fe3O4ACBCMethylene blue310.0500.0--2533.834.975.490.6[258]Pyrolysis at 650 °C, impregnation with iron salt, and carbonization at 900 °CK2FeO4Lotus seedpodEstradiol98.73725147828.37[172]Hummer method and exfoliation of GOFe3O4GraphiteMethylene blueOrange GAlizarine cyanine green91%71%70%7------[259]Carbothermal magnetization by microwave-assisted impregnation with zinc and iron onto agriculture shell wastesZn ferriteWalnut shellMethylene blue130725--1000[260]Coprecipitation methodFe3O4GO and celluloseCongo redAcid red 1Reactive red 245.0947.3246.213-6308.9197.8[168]Pyrolysis at 700 °C and impregnation with iron salt and cetyl trimethyl ammonium bromideFe3O4Nut shellsAcid chrome blue K108.83502.08--[261]Direct mixing of the polymer matrix with the nanofillersFe3O4ACMethylene blue10.63635–651.28[262]Hydrothermal carbonizationFe3O4 and Fe0CarbohydrateMethylene blue570258766[263]Sol-gel and coprecipitationSpinel ferriteEthylene glycol60Cobalt152+154Europium82.51136.98925----[177]CoprecipitationFe3O4GOCesium362725----[176]Adsorbent nomenclature: activated carbon (AC), biochar (BC), and graphene oxide (GO).Mubarak et al. [170] tested orange-G and methylene blue removal with a magnetic BC, which was prepared using the empty fruit bunch. This biomass was first treated with FeCl3 and pyrolyzed in a microwave muffle. Dye removal was optimized via the analysis of contact time, stirring speed, adsorbent dosage, and pH. Methylene blue adsorption was maximum with a 125 rpm stirring, 1.0 g of adsorbent ratio, and 120 min of contact time at pH 10. The best removal conditions for orange-G were 125 rpm stirring, 1.0 g of adsorbent dosage, 120 min of contact time, and pH 2. 32.36 and 31.25 mg/g were the maximum adsorption capacities for orange-G and methylene blue dyes, respectively. Experimental data followed a pseudo second-order kinetic.Oladipo and Ifebajo [171] prepared a magnetic chicken bone BC for the adsorption of rhodamine B (RB) and TC. This adsorbent displayed a pHpzc of 8.3 with a magnetization value of 64.7 emu/g and 328 m2/g of surface area. The magnetic adsorbent was utilized for the adsorption of TC and RB with single and two-stage stirred adsorbers. This configuration reduced adsorbent fouling, mass transfer resistances, and pressure drops. The configuration of two-stage stirred adsorbers was optimized to obtain 98 and 96% RB and TC removal with 22.2 and 33.2 g of adsorbent for initial concentrations of 100 mg/L and 180 min of contact time. Freundlich equation correlated the adsorption results where the experimental adsorption capacities were 109.66 and 93.11 mg/g for RB and TC, respectively.Estradiol is an endocrine disrupting chemical that has become of public concern. Therefore, Yin et al. [28] analyzed Cu2+ and 17β-estradiol (E2) adsorption on activated and magnetic BC. One-step method was utilized to obtain these adsorbents at 300, 500, and 700 °C. Oxygenated functional groups, pore volume, and surface area of the magnetic adsorbent were higher than those of BC without modification. Also, the magnetic adsorbent showed better adsorption capacities for the removal of these pollutants in single and binary aqueous solutions. The adsorbent obtained at 300 °C showed the highest adsorption capacity of 85.93 mg/g for Cu2+, and the adsorbent prepared at 700 °C had an adsorption capacity of 153.2 mg/g for E2 in single aqueous solutions. Langmuir and pseudo second-order equations fitted the E2 and Cu2+ adsorption. Solution pH affected the adsorption of both pollutants. Binary experiments indicated an antagonistic (i.e., competition) adsorption. It appeared that Cu2+ adsorption occurred via a chemical complexation with the oxygenated functionalities, while E2 adsorption implied π-π interactions and hydrogen bonds.Also, a graphene-like magnetic adsorbent was synthesized with K2FeO4 and lotus seedpod for its application in the adsorption of 17β-estradiol (E2) [172]. Adsorption variables (e.g., foreign ions, humic acids, ionic strength, and solution pH) including the presence of other water pollutants like microplastics (MPs) and Al2O3 NPs were analyzed, and their impact on the E2 adsorption was established. Surface area of this adsorbent was 828.37 m2/g and displayed some graphene-like properties. E2 removal was interpreted with Langmuir isotherm and pseudo second-order kinetic. Sulfate ions, ionic strength, and solution pH impacted on E2 adsorption, while background electrolytes (e.g., NO3-, Cl-, Ca2+, K+, and Na+) and humic acids did not reduce the removal of this pollutant. MPs and Al2O3 significantly reduced the adsorption equilibrium time, but without a significant effect on the final E2 removal. The corresponding adsorption mechanism implied multiple interactions such as electrostatic π-π interactions besides micropore filling effects.GO–carboxymethyl cellulose and Fe3O4 were the feedstocks to prepare a magnetic composite to adsorb dye reactive red 2 (RR2), acid red 1 (AR1), and congo red (CR) [168]. FTIR, XRD, VSM, N2 physisorption, TGA, and SEM/TEM techniques were used to characterize the main adsorbent properties. This magnetic adsorbent showed adsorption capacities of 46.21, 47.32, and 45.09 mg/g for RR2, AR1, and CR, respectively. Freundlich equation showed the best fit for dye adsorption equilibrium experiments. Thermodynamic calculations confirmed an endothermic dye removal at tested operating conditions. Adsorption of these dyes on the magnetic composite was associated to surface complexation, π−π stacking, hydrogen bonding, and electrostatic forces. Particularly, there was a complex formation involving Fe3O4, while the composite and dye molecules interacted via electrostatic interactions with hydroxyl and carboxyl groups. NaOH solution (0.1 M) regenerated this adsorbent with an effectiveness of 65% up to adsorption-desorption cycles.Radionuclides are elements that emit alpha, beta, gamma rays, or neutrons [173], and they can occur naturally (e.g., terrestrial and cosmogenic) or anthropogenic (e.g., nuclear plants, weapons, testing sites, lignit burning, and fertilizers use) [173, 174]. Some radionuclides can be found in water due to the rock lixiviation and accidents in nuclear facilities [173, 175]. These radioactive elements can have a long life-time and radioactivity. The toxicology of these pollutants is associated to neurological damage, birth defects, and cancer [173, 175, 176]. Some magnetic adsorbents have prepared and tested to remove radionuclides. For instance, a magnetic GO was utilized for the cesium adsorption [176]. This adsorbent was prepared via coprecipitation reaction of iron salts and characterized with FTIR, Mössbauer, XRD, and TEM techniques. The adsorption capacity was 362 mg/g where Langmuir model was employed in the data correlation. Cesium removal was favored with pH, and it was concluded that an ion exchange was involved in its adsorption mechanism. Maksoud et al. [177] prepared carbon-modified zirconia/spinel ferrite nanostructures for the removal of cobalt and europium. The adsorption of these radionuclides was assessed at different conditions of pH and temperature. The adsorption was endothermic with adsorption capacities of 137 and 83 mg/g for europium and cobalt. Langmuir and pseudo second-order models were employed to fit the adsorption equilibrium and kinetics.


## 4.1. Arsenic

Arsenic (As) is a geogenic pollutant of water supplies that is a major problem for public health and, consequently, a current and relevant environmental problem for the population of several countries of Southeast Asia, Latin America, and Europe. Natural sources and anthropogenic activities (pesticide usage, fossil fuel combustion, and mining) are the main causes of arsenic pollution [27]. It shows a severe toxicity to humans, and, consequently, the US Environmental Protection Agency (EPA) [114] and World Health Organization (WHO) [115] have recommended a maximum threshold of 10 ppb for arsenic concentration in the water used for human consumption with the aim of protecting consumers supplied by public water systems [26, 33, 116]. However, it has been calculated that over 100 million people can be exposed to arsenic-polluted water [117]. Chronic exposure to arsenic could cause dermal lesions, hypertension, diabetes, cancer, and peripheral vascular disease [115, 118]. This pollutant can occur in oxidation states of +5, +3, 0, and -3, and it is frequently found as arsenates or arsenites [115]. Therefore, the toxicity of this pollutant strongly depends on its chemical nature. Arsenate (AsO4)3 with (+5) or arsenite (AsO3)3 with (+3) are the most frequent forms of arsenic in water where arsenite is 20 times more toxic than arsenate [16, 119]. This toxic pollutant can be removed from water using magnetic carbon-based adsorbents. This adsorption process could imply surface complexation and electrostatic attraction between the magnetic adsorbents and arsenic species in the aqueous solution [27, 119]. Table 1 shows recent studies of arsenic adsorption using magnetic forms of AC, CNTs, BC, CNCs, GO, and RGO.Table 1
Removal of arsenic from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAs specieAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic MWCNTs by microwave-assisted processFe3O4 and γ-Fe2O3Commercial MWCNTsAs3+As5+1.7230.1897440--153[49]Magnetic CNTs by catalytic CVD vapor deposition with alkali-activated methodFe3O4 and γ-Fe2O3EthanolAs3+As5+8.139.745.52527.2662.1[119]Sulfhydryl-functionalized MWCNTs with CVD synthesis and high-temperature treatmentFe3O4 and γ-Fe2O3EthanolAs3+19.1272527.3139.9[89]Magnetic BC by thermal impregnation of biomass with natural hematite and direct pyrolysis procedureγ-Fe2O3PinewoodAs5+0.429722--193.1[24]Magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+As5+54.1826.76852512.870.20[189]Magnetic MWCNTs by oxidation and coprecipitationFe3O4Commercial MWCNTsAs3+As5+14.2616.856.833039.37119.09[91]Magnetic RGO/CNT composites by graphite exfoliation and coprecipitationFe3O4Commercial MWCNTs and graphiteAs3+As5+9.115.1725----[190]Si-magnetic GO by graphite exfoliation and coprecipitation and sol-gel coatedSi-coated Fe3O4GraphiteAs3+As5+7.511.41425----[191]Aerogel magnetic CNCs by sol-gel impregnation and pyrolysisFe3CCitric acidAs5+56.2725--290[29]Magnetic AC by impregnation using iron and manganese oxidesγ-Fe2O3Commercial ACAs5+19.353250.35649.4[116]Magnetic BC by hydrothermal impregnation and carbonizationFe3O4Orange peelAs5+81.36245396[23]Magnetic CNCs by thermal impregnation with iron salts and pyrolysis methodFe3CPine resinAs3+263.9356.674----177[33]Magnetic AC by coprecipitation, impregnation and carbonization processFe3O4Cigarette sootAs3+As5+80.99107.96732510.77575.6[16]Gelatin modified–magnetic BC by pyrolysis and impregnation by coprecipitationγ-Fe2O3Chestnut shellAs5+45.842542--[25]Magnetic CNCs by coprecipitation, impregnation, and hydrothermal synthesisFe3O4GlucoseAs5+20.051-22535.1--[15]Magnetic SWCNTs prepared by arc discharge evaporationFe3O4 and γ-Fe2O3GraphiteAs5+49.65425----[17]Magnetic BC by thermal impregnation and pyrolysis with microwave heatingFe3O4Empty fruit bunch from palmAs5+88N. D.25--890[26]Calcium-based magnetic BC by coprecipitation impregnation and pyrolysisFe3O4Rice strawAs3+6.34525----[27]Magnetic CNTs by inverse coprecipitation and impregnation with Ni-Zn-ferriteNi-Zn-FerriteCommercial MWCNTsAs5+6622515214[92]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteAs5+2-12142534148.2[44]3D magnetic GO hydrogel by graphite exfoliation, coprecipitation, and one-pot method combining GO sheets, Fe3O4, and polyacrylamide hydrochlorideFe3O4GraphiteAs3+As5+25.174. 27.76.22510.5--[192]MWCNT membranes modified with CuFe2O4 by coprecipitation and using polyvinylidene fluoride (PVDF) membrane supportCu ferriteCommercial MWCNTsAs3+31.25725----[50]Chitosan magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+457.32549.3152.38[120]MGO by graphite exfoliation and coprecipitationFe3O4GraphiteAs3+993------Multifunctionalized magnetic GO by coprecipitation and multiple impregnationFe3O4Commercial GOAs3+As5+62.719.372523--[76]1,4-butane sultone modified magnetic AC by carbonization, activation, and finally magnetic impregnation with magnetic phase coprecipitatedFe3O4Pistachio shellAs3+151.515.52511.6--[143]Magnetic BC by coprecipitation, pyrolysis, and high-energy ball milling impregnationFe3O4 and γ-Fe2O3Slovak LigniteAs5+19.93.925--10.6[193]HTC with iron salt followed by NaOH additionFeCl3Olive pomaceAs5+3.5525----[194]Pyrolysis and two step magnetizationγ-Fe2O3Corn strawAs5+6.7772517.5115.43[195]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Ntim and Mitra [49] used iron oxide supported on MWCNTs as arsenic adsorbent. MWCNTs were microwave-assisted functionalized and then dispersed in an aqueous solution of FeCl3:FeSO4 via ultrasonication. This magnetic material showed adsorption capacities of 189 and 1723 μg/g for As5+ and As3+, respectively. Kinetics and isotherms of arsenic adsorption were fitted with the pseudo second-order, Langmuir, and Freundlich models. These authors concluded that arsenic adsorption on this magnetic adsorbent could occur via multiple interactions where the complexation with adsorbent oxyhydroxide sites played a key role.On the other hand, a novel magnetic adsorbent prepared from orange peel as precursor was studied by Meng et al. [23]. This adsorbent was obtained using hydrothermal process with an iron solution. The influence of operation variables such as solution pH, temperature, and coexisting inorganic coadsorbates on As5+ adsorption was investigated. An As5+ adsorption capacity of 81.3 mg/g was obtained with an iron/biomass ratio of 10 wt%. Solution pH affected the arsenic adsorption process, and this removal was also endothermic. The characterization results indicated the formation of a dendrimer-like structure that surrounded the crystal iron NPs inside the branch with the amorphous carbon. Also, an adsorption−reduction phenomenon that included inner reduction and complex adsorption was identified with the characterization data. Removal efficiency after 3 cycles of adsorption-regeneration was found 89% where deadsorbent showed good mechanical stability with a low iron release (i.e., <0.3 mg/L).Sahu et al. [16] prepared a novel Fe3O4 AC using as precursor cigarette soot. FTIR, Zeta potential, N2 physisorption, EDX, TEM, SEM, XRD, and VSM were used in the adsorbent characterization and to confirm the magnetic phase formation. This adsorbent showed 575.6 m2/g of surface area and 10.77 emu/g of magnetic properties. As5+ adsorption was affected by solution pH where it was reduced with pH increment, while As3+ adsorption increased from pH 3 to 7 and then decreased. Experimental adsorption data were correlated with pseudo second-order and Langmuir models. The highest adsorption capacities were 80 and 110 mg/g for As3+ and As5+ at pH 7, respectively. Regeneration studies were performed with 0.5 M NaOH, and results indicated that the adsorption capacities of this adsorbent did not decrease significantly up to 4 consecutive regeneration cycles. The adsorption of As3+ and As5+ species was mainly associated to the hydroxyl groups on the adsorbent surface. Finally, it was concluded that a monodentate complex formation prevailed for As3+ adsorption, while both monodentate and bidentate complex formation and electrostatic attraction were involved in As5+ adsorption.Multicomponent adsorption of As3+ and Cd2+ was studied using calcium-based magnetic BC with rice straw as carbon source and iron salts [27]. Results demonstrated that the iron favored As3+ adsorption, while calcium enhanced Cd2+ uptake. In the experiments with one adsorbate, the adsorption of both pollutants depended on solution pH where the maximum removal rate was obtained at pH 6 with maximum adsorption capacities of 10.07 and 6.34 mg/g for Cd2+ and As3+, respectively. Multicomponent adsorption of these adsorbates included synergistic and competitive effects. In the binary solutions, As3+ adsorption decreased in 15–33% due to the presence of Cd2+ as coadsorbate, while Cd2+ adsorption increased in 3–16% due to the presence of As3+. The formation of type B ternary surface complexes and electrostatic interactions were associated to the multicomponent adsorption effects observed for the binary solution Cd2++As3+.Graphite powder and iron salts were used to prepare a magnetic GO for the As3+ adsorption from aqueous solution [120]. The characteristics of this magnetic GO were studied with FTIR, XRD, and Field Emission SEM/EDX instruments. A central composite design (CCD) was employed to study the As3+ adsorption at batch conditions where the impact of As3+ concentration, contact time, pH, and adsorbent dosage were analyzed by response surface methodology (RSM). The solution pH impacted the As3+ adsorption where the highest removal was obtained in the range of 2–6. As3+ removal was 99.95% at pH 7, adsorbent dosage of 0.3 g/L, contact time of 77 min, and an initial As3+ concentration of 100 mg/L. 0.1 M NaOH was used to regenerate the magnetic GO where its removal performance decreased up to 80% after 4 adsorption-desorption cycles. FTIR analysis confirmed that As3+ adsorption involved a monodentate complexation between arsenic oxyanions and magnetic GO surface functionalities.It is important to highlight that arsenic adsorption studies have been carried out mainly at batch conditions, and only few authors have reported packed bed columns for this purpose [117]. Particularly, Xu et al. [117] reported the breakthrough curves for the As5+ adsorption with a magnetic composite obtained from bagasse biomass and iron oxide. The biomass was first impregnated with iron salts in microwave oven, then, it was sonicated with ethanol and subsequently carbonized at 500 °C. Breakthrough curves of As5+ adsorption were quantified at different conditions of bed height, solution flow rate, pH, and As5+ feed concentration. Results showed that the increment of As5+ feed concentration reduced the exhaustion time and breakthrough points. The increment of solution pH and bed height decreased the As5+ adsorption rate. This adsorbent can be regenerated with 1 M EDTA to recover its As5+ adsorption capacity.


## 4.2. Pharmaceuticals

Pharmaceutical products, once used or expired, are considered a special type of waste in the environment that have been catalogued as chemicals of emerging concern to the public because of their potential to pollute water [115, 121, 122]. The global pharmaceutical consumption is estimated as ~1,000,000 tons/year with 15 g/year as per capita use [123]. Several pharmaceutical molecules cannot be totally absorbed and metabolized, thus, they are excreted and released to the environment. Therefore, a significant amount of pharmaceutics is discharged into the environment during its production, delivery, use, application, and excretion [115, 124]. For example, the tetracycline (TC) is an important antibiotic widely utilized as antimicrobial in livestock industry and human therapy. It has been established that 50–80% of TC used in the farming industry can be excreted as unmodified parent compounds via urine and feces [125]. Besides, conventional water treatment plants are not designed to remove pollutants at trace concentrations, and, consequently, the degradation or separation of this and other pharmaceutical compounds is not effective [122, 126]. Pharmaceutical molecules could be found in concentrations ranging from ng/L to μg/L in ground waters, wastewaters, and surface waters [124]. Wastewaters could contain significant amounts of more than 55 pharmaceuticals over the 150 daily used compounds [127–129]. Most of these compounds have been categorized as essential by the WHO. The bioaccumulation of these compounds represents a serious eco-toxicological risk and implies adverse effects like organism drug resistance, metabolism disruptions, and bacteria strain proliferation [125, 129–131]. There are no international regulations to establish the threshold concentration for pharmaceuticals in the environment, which is mainly due to the lack of studies reporting the long-term effects caused by a chronic exposure to these emerging pollutants and their metabolites [132, 133]. The concentration of pharmaceutical compounds can be effectively reduced in water via adsorption [123]. Carbamazepine (CBZ), atenolol, erythromycin, diclofenac, ibuprofen (IBP), and naproxen are the common adsorbates analyzed in adsorption studies. A compilation of the magnetic carbon-based adsorbents utilized for pharmaceuticals removal is presented in Table 2.Table 2
Removal of pharmaceuticals from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic MWCNTs by hydrolysis impregnationFe3O4Commercial MWCNTsAmoxicillin33.564.627----[87]Magnetic AC by coprecipitation impregnationFe3O4Commercial ACNaproxen87.79325----[196]Magnetic MWCNTs with dibenzo-18-crown-6 by hydrolysis impregnationFe3O4Dibenzo-18-crown-6Amoxicillin263.1525----[88]Magnetic AC by coprecipitation impregnationFe3O4Commercial ACCarbamazepine182.9--25161241[134]Magnetic GO nanoplatelets by coprecipitationFe3O4Commercial GOAmoxicillin106.38525--543.2[135]Magnetic BC by impregnation with iron salts and direct HTCFe3O4Sugarcane bagasseTetracycline48.356.8309.7348.35[197]Magnetic AC by ball milling impregnationFe3O4Commercial coconut shell-based ACTetracyclineCarbamazepine45.3135.162520.8486[198]Magnetic BC by pyrolysis and ball milling impregnationFe3O4Coconut shellTetracyclineCarbamazepine94.262.762519365Chitosan-magnetic GO by coprecipitationFe3O4Commercial GOCiprofloxacin282.952514.76388.3[199]Magnetic AC by direct impregnation with hydrothermal method and functionalized with silanesFe3O4Commercial ACCarbamazepineClofibric acidIbuprofen114.378.7166.77252.65960.9[200]Magnetic MWCNTs by coprecipitation impregnationFe3O4Commercial MWCNTsAmoxicillin355.85725----[201]Magnetic GO spongeFe3O4GraphiteTetracycline47310351.14--[124]Magnetic carbon microspheres by pyrolysis and direct hydrothermal impregnationFe3O4GlucoseSulfonamide27.8542542.31228[136]Magnetic BC by pyrolysis and impregnationγ -Fe2O3Astragalus membranaceus residuesCiprofloxacin68.962523.96203.7[202]Pyrolysis of sewage sludge and alkali-acid treatmentγ-Fe2O3Sewage sludgeTetraciclyne286.91745--141.78[103]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteTetracycline252.02-122534148.2[44]Magnetic carbon via carbonizationα-FeMetal-organic frameworkTetracycline511.0674555.51171.7[203]Magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteChlorpheniramine472.01025--221[204]Magnetic AC by impregnation with iron and cobaltCobalt ferriteCommercial ACAmoxicillinParacetamol444.2399.97253.07893.8[205]Magnetic AC by simultaneous pyrolysis, impregnation, and activationγ-Fe2O3Corn stalksNorfloxacin7.691025--760.7[206]Magnetic BC yolk shell by calcinationFe3O4Resorcinol and formaldehydeSulfamethazine312.562519.77247[207]Pyrolysis of bones at 500 °C, coprecipitationFe3O4Chicken boneTetracycline98.892–102664.7328.06[171]GO/diethylenetriaminepentaacetic acidFe3O4Commercial GOTetracyclineCiprofloxacin294.12111.73330--176[208]Manganese-based magnetic BC by pyrolysis and coprecipitation impregnationFe3O4Potato stems and leavesNorfloxacinCiprofloxacinEnrofloxacin6.948.377.193309.8252[209]Magnetic GO-polyaniline by graphite exfoliation and coprecipitationFe3O4GraphiteCiprofloxacin106.38625----[210]Nitrogenated magnetic RGOFe3O4Commercial GONorfloxacinKetoprofen158.1468.06.825--38.2[75]Magnetic BC by pyrolysis and impregnated by oxidative hydrolysisFe3O4 and γ-Fe2O3Pine sawdustSulfamethoxazole19.094.52547.8 Amp∗m/kg125.8[211]Magnetic RGO hydrogelFe3O4Commercial RGOTetracyclineCiprofloxacin4.762.7862514.566.8[212]Polyglycerol mediatedSPMGOFe3O4Commercial GOTetracycline684.937256.81--[213]Carbon dot modified magnetic CNTs by coprecipitation impregnation and hydrothermal modificationFe3O4Commercial CNTs and citric acid for carbon dotsCarbamazepine657255.64184.1[105]Magnetic AC by direct impregnation and hydrothermal methodNi ferriteCommercial ACIbuprofenKetoprofen172.1985.64225256.25564.4[214]Magnetic CNTs by coprecipitation/hydrothermal impregnationFe3O4Commercial CNTsKetoprofenDiclofenacIbuprofen7.917.99.0525-----[215]Phenol resin melted at 40 °C, soft-templating, and impregnationFe3O4Phenolic resinMinocycline6------[1]Magnetic GO-SO3H by graphite exfoliation and coprecipitationFe3O4GraphiteIbuprofenTetracycline160.83500.6877303555.4--[131]Magnetic BC by carbonization and thermal activation procedureFe0White rot fungus ofPhanerochaete chrysosporiumDiclofenac361.25--21.651986[216]Magnetic GO-SiFe3O4GraphiteSulfamethoxazole15.4672526.98--[217]β-cyclodextrin- magnetic GO by graphite exfoliation and coprecipitationFe3O4GraphiteSulfamethazine238.532530--[218]Magnetic CNT by hydrolysis impregnationMn ferriteCommercial CNTsBezafibrate33.472523.896.526[219]Humic acid coated magnetic BC by direct impregnation pyrolysis and coated after with humic acidFe3O4Potato stems and leavesNorfloxacinCiprofloxacinEnrofloxacin9.9711.468.410304.0426.28[30]Magnetic RGO sulfonated by pyrolysis, and inverse coprecipitation impregnationFe3O4Plastic bottle wasteGaramycinAmpicillin4565005.53.025254.9600[220]Magnetic BC by pyrolysis and coprecipitation impregnationFe3O4Banana biomassFurazolidone37.867.53041166.9[31]Magnetic AC by hydrothermal carbonization and thermally activated with pyrolysisFe3O4 and Fe0GlucoseBio sludgeIron sludgeSulfanilamideSulfadiazineSulfamethazineSulfamethoxazole63.7140.9178.6181.8625171385[221]Magnetic AC by coprecipitation impregnationFe3O4Commercial wood ACTetracycline208.332022.2--[222]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Baghdadi et al. [134] reported the preparation of a magnetic nanocomposite using a commercial AC and the CBZ adsorption tests. Different instrumental techniques (SEM, FTIR, N2 physisorption, VSM, XRD, and SEM) were utilized to characterize the surface chemistry, textural parameters, and magnetic properties of this adsorbent. CBZ adsorption from urban wastewater was optimized with a CCD by analyzing different operating conditions (total dissolved solids TDS, CBZ concentration, and adsorbent dosage). It was observed that a high magnetite content for the adsorbent preparation caused the blockage of composite porous structure and the reduction of CBZ adsorption capacities. The maximum CBZ adsorption capacities ranged from 182.9 to 280 mg/g. Besides, the CBZ adsorption decreased slightly with TDS concentration. Authors explained that CBZ adsorption was associated to carboxylic groups, and it was also concluded that the removal of CBZ was exothermic and spontaneous.The adsorption of amoxicillin (AMX), which is an antibiotic, on magnetic graphene nanoplatelets (GNPs) from aqueous solution was reported by Kerkez-Kuyumcu et al. [135]. Magnetite NPs and GNPs were used to obtain this adsorbent. Results showed that the magnetic GNPs outperformed GNPs and magnetite alone. The increase in solution pH reduced AMX adsorption, and this adsorbent showed a maximum adsorption capacity of 14.10 mg/g. Electrostatic and π– π interactions were associated to the AMX adsorption mechanism with magnetic GNPs. Pseudo second-order kinetic model fitted AMX adsorption, which was spontaneous and exothermic. Magnetic GNPs were regenerated with 0.15 M NaOH, and the adsorbent was utilized during 4 adsorption-desorption cycles where its adsorption capacity remained as 35%.Fe3O4 NPs and glucose were the feedstocks to obtain reusable magnetic carbon microspheres (CMs) via HTC [136]. This adsorbent was utilized to remove the antibiotic sulfonamide. Magnetic CMs samples were also calcined at 600 °C for 1 h to improve their surface properties thus obtaining a pore volume of 0.448 m3/g and surface area of 1228 m2/g. Pseudo second-order and Langmuir equations correlated the antibiotic adsorption data. The adsorption capacity of magnetic CMs decreased with pH and temperature, and the highest value of 24.22 mg/g was obtained at 10 °C and pH 4. Magnetic CMs were regenerated with NaOH thus obtaining an adsorption capacity of 18.31 mg/g after the antibiotic desorption, and this adsorbent was reused 4 times.Another type of antibiotics that represents a hidden danger to human health is the fluoroquinolones (FQs). Enrofloxacin (ENR), norfloxacin (NOR), and ciprofloxacin (CIP) were employed as FQs adsorbates to study the adsorption properties of a humic acid-magnetic BC [30]. These authors prepared a magnetic BC from potato stems and leaves, which were coated with humic acid (HA), see Figure 8. Humic acid-magnetic BC showed the presence of oxygenated functional groups that conferred its adsorption capacity. It exhibited FQ uptakes up to 1.8-3.4 times higher than those reported for raw and magnetic BC for these compounds. Specifically, this magnetic material showed adsorption capacities of 6.0, 7.5, and 7.1 mg/g for adsorbates ENR, NOR, and CIP, respectively, at 35 °C. The adsorption experimental data were adjusted and analyzed with Langmuir isotherm and pseudo second-order kinetic. FQ adsorption on this magnetic carbon-based adsorbent was associated to π-π, H-bond, hydrophobic, and electrostatic interactions.Figure 8
Humic acid coated magnetic biochar (MBC) derived from potato leaves and stems for fluoroquinolone antibiotics removal from water [30].Liyanage et al. [133] proposed the preparation of magnetic adsorbent using the IONP precipitation to modify a commercial Douglas fir BC. This magnetic BC was applied to remove 3 emerging water pollutants: caffeine (CF), IBP, and acetylsalicylic acid (ASA) in adsorption systems at batch conditions. This magnetic adsorbent showed a surface area of 322 m2/g, which was lower than that of BC (468.2 m2/g). The adsorption of these pharmaceuticals depended on solution pH and temperature. Authors concluded that H-bonding, electrostatic, and π-π interactions were present at different pH conditions. The adsorption capacities of this adsorbent were 80, 40, and 140 mg/g for CF, IBP, and ASA, respectively, at pH 8 and 35 °C. Competitive experiments in binary CF/IBP solutions showed a decrement in its adsorption capacity of 13.6 and 52.3%, respectively. Surface protonation and CF polarity contributed to generate strong adsorbate-adsorbent interactions thus leading to high adsorption capacities. Adsorbent regeneration was carried out with methanol and water, and results showed that the adsorption capacity remained almost constant during 5 adsorption-desorption cycles.Wei et al. [123] prepared 7 deep eutectic solvents (DESs) known as green sustainable solvents that were used to regulate the preparation of a magnetic composite from MOF MUiO-66-NH2 and Fe3O4. The removal of pharmaceuticals mefenamic acid (MF) and ofloxacin (OX) was analyzed with this nanoadsorbent, labelled as DES-MUiO-66-NH2. Under optimal conditions, the adsorption capacities were up to 97.60 and 79.22 mg/g for OX and MF, respectively. Hydrogen bonding, hydrophobic interaction, π-π stacking, chelation, and electrostatic interactions were the main forces involved in the adsorption mechanisms. Density functional theory calculations demonstrated the formation of chelation. It was also concluded that DES structures determined the adsorption properties of DESMUiO-66-NH2, thus, offering a green preparation route of tailored adsorbents for emerging water pollutants. The presence of coions (e.g., sulphates, nitrates, chlorides, calcium, potassium, and sodium) did not affect the adsorption. Desorption and regeneration tests were also carried out.


## 4.3. Heavy Metals

Heavy metals are also relevant water pollutants that are characterized by low biodegradability and high chemical stability. Heavy metals are toxic for ecosystems and human beings at certain concentration thresholds. Toxicological effects of heavy metals include reproductive problems, neurological disorder, renal disease, gastrointestinal bleeding, lung disease, hypertension, and cancer [137]. Lead (Pb), cadmium (Cd), copper (Cu), zinc (Zn), nickel (Ni), chromium (Cr), mercury (Hg), and manganese (Mn) are common heavy metals found in the environment and considered as priority water pollutants [137–139]. Water pollution by heavy metals is associated to the several industrial activities including, for instance, chemical processing, oil refining, electronic manufacturing, and mineral smelting [139]. Different magnetic adsorbents have been used in heavy metal adsorption, and Table 3 describes a survey of magnetic carbon-based materials used for this purpose.Table 3
Removal of heavy metals from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic CNTs by in situ coprecipitation modificationγ-Fe2O3Commercial CNTsCr6+11.25632543.29119.09[223]Magnetic BC by impregnation and direct pyrolysisγ-Fe2O3Peanut hullsCr6+77.5452536.79145.25[140]Magnetic GO by hummers method and impregnation in situ hydrothermal synthesisFe3O4GraphiteCr6+31.872512182[224]Amino functionalized magnetic GO by hummer method and impregnation in situ hydrothermal synthesisFe3O4GraphiteCr6+123.422530.257.55[225]Nitrogen doped magnetic AC by impregnation and direct pyrolysis processes using glucose as nitrogen sourceFe3O4 and Fe3CGlucose and melamineCr6+29.46725130.756.2[226]Carboxyl functionalized magnetic CNTs by solvothermal methodFe3O4Commercial CNTsCr6+22.2222570.62--[227]Chitin-magnetic CNTs by simple millingFe3O4Commercial CNTsCr6+10.72255.77569.1[228]Dithiocarbamate functionalized magnetic RGO by hummer method, reduction with hydrobromic acid, and magnetic impregnation by coprecipitation.Fe3O4GraphiteCu2+Cd2+Pb2+Hg2+113.64116.28147.06181.82566625--194.8[141]Magnetic fluorine and nitrogen codoped carbonFe3O4Melamine and polyvinylidene fluorideCr6+740.7153.4182.7[229]Magnetic AC high temperature carbonization and activationFe0, Fe3O4, and Fe3CActivated sludgeCr6+2033257.6114.24[230]Magnetic BC by iron salts impregnation and hydrothermal pyrolysisγ-Fe2O3Pinewood sawdustHg2+167.272515.5843.29[142]One step hydrothermal method with iron salt and hexamethylenediamineγ-Fe2O3Peanut hullCr6+142.86--25--62.4[64]Magnetic AC by low temperature carbonization, impregnation, and high temperature for magnetic modification and activationFe3O4Termite fecesCr6+663251.46699[231]1,4-Butane sultone modified magnetic AC by carbonization, activation, and finally magnetic impregnation with magnetic phase coprecipitatedFe3O4Pistachio shellPb2+Cd2+147.05119.045.52511.6--[143]Magnetic BC by pyrolysis and impregnation with coprecipitation of magnetic phaseFe3O4Banana peelsZn2+Cu2+Hg2+72.875.983.462539.55323.2[232]Magnetic GO by graphite exfoliation and coprecipitation and magnetic RGO reduced by hydrazine hydrateFe3O4GraphiteCd2+2-122342534148.2[44]Impregnation with humic acid, solvothermal process, and calcinationFe3O4Layered double hydroxidesCu2+Cd2+Pb2+400.0375.0200.0625--132.4[233]Magnetic BC modified with MnO by pyrolysis and impregnation with magnetic phaseFe3O4Palm kernel cake residueCd2+Cr3+Hg2+Pb2+18.6019.9249.6413.6972520.9489.38[144]Direct pyrolysis and sonochemical methodFe3O4Biogas residueCu2+Pb2+75.76 181.825--39.9679.64[234]Pyrolysis at 600 °C and physical comixingFe3O4Wheat stalk and rice huskPb2+73.34 - 179.552526.1 - 28.613.96 - 224.6[235]Pyrolysis at 500 °C, impregnation with iron saltγ-Fe2O3Blooms of alga EnteromorphaCr6+11.1322539.29--[236]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).Peanut hulls are an abundant residual biomass with low cost that can be employed to prepare a magnetic BC for Cr6+ adsorption [140]. The best adsorbent was obtained via pyrolysis at 650 °C with an adsorption capacity of 77.54 mg/g. Adsorption studies showed that low solution pH and the particle size of magnetic BC were relevant variables to remove this pollutant. Characterization results suggested that iron oxide was crucial to obtain the magnetic properties of adsorbent. Cr6+ was desorbed up to 55.9% using NaOH. The removal mechanism of this pollutant involved an electrostatic attraction of the anionic chromium to the protonated –OH2+ of maghemite.Fu and Huang [141] analyzed the removal of Hg2+, Pb2+, Cd2+, and Cu2+ using a RGO that was functionalized with magnetic dithiocarbamate (DTC). A modified Hummers method was implemented to prepare GO, and the reduced and functionalized RGO composite was obtained via GO bromination, polyethylenimine nucleophilic substitution, reaction with CS2, and loading of Fe3O4 NPs. XRD, TEM, FTIR, and XPS techniques allowed the characterization of this magnetic adsorbent. The surface area of this adsorbent was 194.8 m2/g. The increment of solution pH from 2 to 4 improved the heavy metal adsorption. This adsorbent exhibited high adsorption capacities with the next trend: 165 mg/g of Hg2+>135mg/g of Pb2+>105mg/g of Cd2+>90mg/g of Cu2+. These experimental adsorption data were fitted with the pseudo second-order kinetic and Langmuir isotherm. Nanocomposite regeneration was done with a one-step organic reaction obtaining satisfactory heavy metal uptakes in 5 adsorption-regeneration cycles.Magnetic CCs and BC were prepared using pinewood sawdust, and they were subsequently applied for Hg2+ removal [142]. Pinewood sawdust was soaked in iron solutions and hydrothermally treated. Magnetic BC was obtained via pyrolysis, while magnetic CCs were prepared by calcination. Magnetic BC showed a surface area of 80.35 m2/g, which was higher than magnetic CCs (i.e., 43.29 m2/g); their adsorption capacities were 31.80 and 167.22 mg/g, respectively. These results suggested that textural parameters of these magnetic materials did not play a relevant role for Hg2+ adsorption. This finding was supported on the fact that magnetic CCs contained higher amounts of hydroxyl, lactone, and carboxyl groups than those identified for the surface of magnetic BC. Additionally, it was identified that magnetic CCs contained γ-Fe2O3 with a high crystallization degree. In fact, this adsorbent showed better regeneration and magnetic properties. Hg2+ adsorption mechanism implied coprecipitation, surface complexation, and electrostatic attraction.Heavy metals and antibiotics usually coexist in wastewater thus magnifying its toxicological profile. Therefore, Huang et al. [44] studied the application of magnetic GO and its reduced forms via chemical and annealing routes to remove As5+, Cd2+, and TC. The adsorption properties of these adsorbents and the corresponding mechanism for these pollutants were analyzed. In aqueous solutions with only one adsorbate, the adsorption of these pollutants was affected by solution pH and the adsorption capacities showed the next trend: magneticannealingRGO<magneticchemicallyRGO<magneticGO. In particular, the magnetic GO showed the best adsorption capacities with values of 13.9, 234 and 252 mg/g for TC, Cd2+, and As5+, respectively. The interaction effects of Cd2+ and TC in the multiadsorbate solutions were not significant. The presence of TC in the solution decreased significantly the As5+ adsorption, while As5+ did not affect TC removal in multicomponent solutions. The adsorption of As5+ and Cd2+ in the multiadsorbate solutions increased by 30 and 65%, respectively.A green synthesis was proposed to prepare a magnetic adsorbent with AC, 1,4-butane sultone, and Fe3O4 NPs for the removal of Cd2+, As3+, and Pb2+ under ultrasound [143]. Adsorption results showed that the heavy metal uptake under ultrasound conditions was fast and increased during the first 10 min. Nevertheless, the adsorption capacity decreased at operating times >10 min, and this phenomenon was associated to the release of metallic species from adsorbent surface. The maximum adsorption capacities in the aqueous solutions with one adsorbate were 95, 130, and 140 mg/g for Cd2+, As3+, and Pb2+, respectively. Competitive (i.e., multiadsorbate) adsorption experiments indicated that the adsorption capacities reduced in 12, 21, and 22% for Pb2+, As3+, and Cd2+, respectively. Thermodynamic parameters confirmed that the adsorption of these pollutants was feasible, exothermic, and spontaneous. Characterization techniques supported that the mechanisms of adsorption implied the heavy metal complexation with the SO3H and OH groups from the magnetic adsorbent surface.Maneechakr and Mongkollertlop [144] prepared and tested a MnO2-modified magnetic BC for the removal of Hg2+, Pb2+, Cr3+, and Cd2+. This magnetic adsorbent was obtained from Fe3O4 and palm kernel cake residue. Different techniques (SEM-EDS, FTIR, Boehm titration, N2 physisorption, XRD, and VSM) were utilized to characterize the adsorbent physicochemical properties. As expected, the pollutant adsorption was enhanced with increments of solution pH. Adsorption temperature did not show a high impact on the heavy metal removal although the process was endothermic. The maximum experimental adsorption capacities of Cd2+, Cr3+, Pb2+, and Hg2+ were 19.90, 21.20, 49.64, and 13.69 mg/g, respectively. Experimental data were modeled, and thermodynamic parameters were also obtained.


## 4.4. Pesticides and Other Pest Controllers

Pests and associated-diseases cause around 30% of global crop loss [145]. The pesticides are quite toxic chemical compounds tailored to kill off pests via their environment spread [146]. The biotransformation of these compounds is difficult thus causing their bioaccumulation for long periods. Agriculture production has increased the usage of pesticides, herbicides, insecticides, and fungicides thus generating an additional source of water and soil pollution [146, 147]. In particular, their residues can be still found on fruits and vegetables, and they could enter into water resources due to their microbial degradation resistance and chemical stability in the water [146, 148]. To illustrate the serious environmental problem associated to these pollutants, it can be indicated that studies performed in the United States detected 5 or more pesticides in several samples obtained from different streams, while ~400,000 tons of pesticides are used annually in China [149, 150]. In Europe, pesticides have been considered among the main pollutants of drinking water supplies [151].Since these chemicals are nonselective, they can be toxic for wildlife populations and humans that are the nontarget organisms [146]. Long-term exposure to these substances could lead to serious health effects like neurodegenerative diseases, cancer, hypertension, reproductive, endocrinal, mutagenic, genotoxic, and respiratory effects [146–148]. In particular, glyphosate is a pesticide widely used in agriculture and nonagriculture areas [147]. It causes acute toxic endocrinal, mutagenic, and carcinogenic effects [147]. On the other hand, acetochlor is an herbicide used to control gramineae weeds and has been reported in surface waters of United States at 2.5 μg/L, which is an enough concentration to induce health damage [148]. Also, atrazine is one of the most frequently detected pesticides in freshwater in United States. Therefore, a concentration limit of 3 ng/L was established by EPA for this compound in drinking water [114].Adsorption is effective to remove these toxic substances from water sources. Table4 summarizes the adsorption of pesticides and other pest controllers using magnetic carbon-based adsorbents. For instance, a hybrid composite obtained from the decoration of RGO with MnFe2O4 microspheres was used as adsorbent to remove glyphosate [147]. N2 physisorption, XPS, XRD, FTIR, and TEM analyses were performed for the adsorbent characterization. The glyphosate adsorption on this magnetic composite was associated to ion exchange and electrostatic interactions where 39 mg/g was the maximum adsorption capacity at 5 °C. Kinetic data were fitted with the pseudo second-order model, while Freundlich equation correlated the experimental isotherms. Glyphosate adsorption on this composite was exothermic at 5–45 °C. Surface area of this composite was 305.7 m2/g with the predominance of mesopores where TEM and SEM analyses also confirmed a proper dispersion of MnFe2O4 microspheres on the graphene nanosheets.Table 4
Removal of pesticides and other pest controllers from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceMagnetic GO by chemical exfoliation and coprecipitation impregnationMn ferriteGraphiteGlyphosate33.444.725--305.7[147]Magnetic AC by direct impregnation with hydrothermal method and functionalized with silanesFe3O4Commercial ACBisphenol A126.97252.65960.9[200]Magnetic GO modified with Cu MOF andβ-cyclodextrin by coprecipitation impregnation and chemical modificationFe3O4Commercial GOThiamethoxamImidaclopridAcetamipridNitempyramDinotefuranClothianidinThiacloprid2.883.112.962.561.772.883.21----10.47250.33[237]Phenyl-modified magnetic GO/mesoporous silica by hierarchical bridge-pore structureFe3O4GraphiteAvemerctinImidaclopridPyridabenDichlorvosAcetamipridDursbanIsocarbophosPhoxim9.216.4012.7247.785.118.012.888.23--2525446.5[238]Magnetic BC by direct molten salt methodFe3O4Fir dustDichlorophenolAtrazine298.12102.17--2540.02404[239]Palm carbonization at 773 K, liquid phase reduction method for iron impregnationFe0PalmGlyphosate80.0425--253.97[153]Magnetic MWCNTs modified with Zn MOF by coprecipitation impregnation and chemical coordination methodFe3O4Commercial MWCNTsTriazophosDiazinonPhosaloneProfenofosMethidathionEthopropSulfotepIsazofos3.122.593.803.892.342.182.843.004--53.56128[152]Carboxilated magnetic GO modified with silica-coated magnetite by covalent couplingFe3O4GraphiteChlorpyrifosMalathionParathion13561.935.672533133[154]Magnetic CNTs functionalized with imidazole zeolite by thermal procedureFe3O4Commercial carboxylic-CNTsTetrabromobisphenol77.077309.65--[240]Magnetic GO by electrochemical exfoliationNiOGraphiteMethylparabenEthylparabenPropylparabenButylparaben3.125.288.4210.46525--227.5[241]Magnetic GO-AC by chemical exfoliation, solvothermal impregnationMn ferriteGraphite and commercial vegetal origin ACGlyphosate6.784.725--19.77[242]Chemical activation with H3PO4 for AC production, composite produced by coprecipitation methodFe3O4Peanut shellsAtrazine62.325.07----189.50[156]Magnetic AC coated with by pyrolysis, microwave activation and coprecipitation impregnationFe3O4Waste tyreMethylparabenPropylparaben85.990.0625---1281[155]Pyrolysis of bagasse at 600 °C, impregnation of salts, activation with KOHZn ferriteSugarcane bagasseImidacloprid313.06255.99660.0[243]Adsorbent nomenclature: activated carbon (AC), biochar (BC), carbon nanocages (CNCs), carbon nanotubes (CNTs), graphene oxide (GO), metal-organic framework (MOF), multiwalled carbon nanotubes (MWCNTs), single-walled carbon nanotubes (SWCNTs), and reduced graphene oxide (RGO).MWCNTs and MOF ZIF-8 were utilized to obtain a magnetic adsorbent for the adsorption of organophosphorus pesticides from soil and water [152]. Isazofos, sulfotep, ethoprop, methidathion, profenofos, phosalone, diazinon, and triazophos were considered as adsorbates for this study. Multicomponent solutions with concentrations ranging from 0.2 to 8 mg/L were prepared with these 8 pesticides. Results of this study suggested that coordination-polymerization was involved in the incorporation of ZIF-8 particles on the magnetic MWCNTs surface. Adsorbent pore structure contained meso and macropores with a surface area of 127.95 m2/g. The adsorption capacities of this magnetic adsorbent for tested pollutants ranged from 2.18 to 3.89 mg/g where the lowest and highest removal were for ethoprop and profenofos, respectively. The authors determined that these adsorption capacities were lower than those reported in previous papers, and this finding was associated to the competitive (i.e., antagonistic) adsorption in multicomponent system in comparison to individual pesticide solutions. Solution pH played an important role in pesticides adsorption with pH 4 as an optimum condition. Langmuir model was outperformed by Freundlich equation to correlate the experimental data. It was concluded that the active sites of this magnetic adsorbent and pesticide molecules interacted via a valence-electron-driven adsorption with electrons exchanging or sharing.The glyphosate adsorption mechanism using a modified BC was reported by Jiang et al. [153]. A liquid-phase chemical reduction was employed to functionalize palm-based BC with nano-zero-valent iron. SEM, TEM, FTIR, and XPS techniques were utilized to characterize the final composite, which showed a surface rich in oxygenated functionalities and complex ligands with 253.97 m2/g of specific surface area. Experimental adsorption data were processed and analyzed with Langmuir and pseudo second-order equations. Authors concluded that the maximum glyphosate adsorption was obtained at pH 4, which was twice (i.e., 80 mg/g) than that of raw BC. The presence of phosphate or Cd2+ at low concentrations did not affect the glyphosate adsorption. But, an antagonistic effect was identified in the treatment of agricultural wastewaters that were polluted with organic compounds. Electrostatic forces, complexation, and hydrogen bonding were associated to the glyphosate adsorption mechanism using this magnetic adsorbent.Organophosphorus pesticide adsorption on GO-based silica coated magnetic NPs functionalized with 2-phenylethylamine was studied [154]. Malathion, parathion, and chlorpyrifos were considered as the target pollutants. Magnetic and physical properties of this adsorbent were characterized via VSM, N2 adsorption/desorption, Zeta potential, XRD, TEM, and FTIR. This adsorbent was spherical in shape and agglomerated, showing 33 emu/g of magnetic saturation and 133 m2/g of surface area. No significant differences in adsorption performance were found at different pH. This study showed that the interaction of pesticides with the adsorbent was not affected by deprotonation/protonation caused by pH adjustment. Pesticide adsorption capacities in aqueous solutions ranged from 10.9 to 11.1 where the minimum and maximum removal were for parathion and chlorpyrifos. Note that the parathion and chlorpyrifos adsorption was caused by π–π interactions and hydrogen bonding, while hydrogen bonding governed the malathion adsorption. These findings explained the order of adsorption capacities. Dubinin–Radushkevich and Sips models fitted the experimental adsorption data. Acetone was used for adsorbent regeneration where the recovery of tested pesticides was 89–100% in 10 adsorption–desorption cycles.Mashile et al. [155] reported the synthesis of a recyclable magnetic adsorbent using chitosan and waste tyre AC for the simultaneous adsorption of propylparaben and methylparaben. Adsorbent characterization was done with FTIR, SEM, TEM, and XRD. Surface area of this composite was 1281 m2/g. Pseudo second-order kinetic model described the adsorption of these pollutants. Redlich-Peterson and Langmuir models were used to correlate the binary adsorption of propylparaben and methylparaben. It was calculated that the maximum Langmuir monolayer adsorption capacities for propylparaben and methylparaben were 90.0 and 85.9 mg/g, respectively. This magnetic composite was chemically stable and useful after 7 cycles of adsorption-desorption.Agani et al. [156] evaluated the atrazine adsorption from water using a fixed-bed column packed with a magnetic composite prepared from AC, chitosan, and magnetite. XRD and FTIR techniques allowed to analyze the composite surface chemistry. Experimental designs based on CCD and RSM optimized the adsorption operating variables (i.e., flow rate, bed depth, atrazine initial concentration, and pH). The impact of these operating variables on adsorption process was also analyzed. The experimental results indicated the preparation of a mesoporous adsorbent with 188.50 m2/g of surface area and 62.32 mg/g of atrazine adsorption capacity. Yoon–Nelson, Yan, Bohart–Adams, and Thomas models were used to fit the breakthrough curves. These models allowed to analyze the limiting step of mass transfer for atrazine adsorption with this composite. Bohart-Adams model offered the best correlations for the adsorption data. Composite regeneration and atrazine desorption was studied with NaOH and HCl, thus, confirming the recycling potential of this magnetic material.


## 4.5. Fluoride

Fluorine is a geogenic water pollutant with a wide environmental distribution [157]. Different studies have documented its natural existence in soil, rocks, and groundwater [157]. Also, fluoride has been detected in effluents and wastewaters from fertilizers, electroplating, metal processing, cement, electronic manufacturing, and other industrial sectors, which also contributes as anthropogenic sources of water pollution [158, 159]. Fluoride can contribute to bone tissue development in human beings, but its chronic exposure can cause dental and skeletal fluorosis [157, 159]. The prevalence of dental fluorosis has been reported in more than 50 countries where the population of China is significantly affected by this disease [157]. It has been estimated that fluoride concentration in drinking water exceeds the WHO limit concentration (1.5 mg/L) in more than 25 countries [158]. As a result, over 300 million of people around the world are exposed to develop health problems associated to a chronic fluoride exposure. Herein, it is convenient to highlight that recent epidemiological advances have demonstrated that soft tissues are also affected by fluoride, and its toxic effect is known as nonskeletal fluorosis [159], which also could include damage to the respiratory, renal, immune, endocrine, digestive, central nervous, and cardiovascular systems [157, 159]. Therefore, low-cost and effective methods for the reduction of fluoride concentrations in water are required and demanded in particular for low-income countries.Adsorption is the most commercial technology for fluoride water depollution. Table5 summarizes the adsorption of fluoride using magnetic carbon-based adsorbents. For example, Mohan et al. [160] prepared a corn stover BC with slow pyrolysis at 500 °C, which was magnetized with an aqueous Fe3+/Fe2+ solution and treated with NaOH. BC with and without magnetic properties was characterized by Raman, energy dispersive X-Ray fluorescence (EDXRF), TEM, SEM-EDX, FTIR, and XRD analyses where magnetic moment and textural parameters were also measured. Maximum fluoride adsorption capacities were 6.0 and 4.11 mg/g for BC without and with magnetic properties, respectively, at 25 °C and pH 2. An exothermic fluoride adsorption was identified for both adsorbents at 25–45 °C. Fluoride adsorption kinetics were adjusted with the pseudo first order model. Fluoride adsorption in real ground water was reduced by the interference of solids and other ions such as Na+, Cl-, and NO3-.Table 5
Removal of fluoride from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceImpregnation methodγ-Fe2O3Cotton cellulose18.64 – 925--2.23[244]Pyrolysis at 500 °C and coprecipitation methodFe3O4Corn stover4.112255.13.61[160]Chemical deposition of Fe3O4γ-Fe2O3Graphite77.1272522.66--[245]Impregnation methodFe3O4Yak dung3.985 – 625--79.49[246]BC impregnation with iron salt, pyrolysis at 600 °C.Fe3O4Douglas fir biochar7.5815.5725--494[161]Impregnation with CaCl2 and FeCl3. Carbonization at 300–700 °C during 2 hγ-Fe2O3Cattle dung157.525–45--19.2[247]Impregnation with FeCl3 and pyrolysis after impregnation.γ-Fe2O3Bovine bone5.238254.4341.77[162]Oak shell calcination at 800 °C and iron salt impregnationFe3O4Oak shell454.5469.46226.78[163]AC impregnation and pyrolysis at 500 °C during 2 h.Fe3O4Pea peel4.712–1025-55---[164]Adsorbent nomenclature: biochar (BC).Dewage et al. [161] prepared a Douglas fir BC with Fe3O4 and α-Fe2O3. N2 physisorption, XPS, XRD, TEM, and SEM/EDX were applied to characterize BC precursor and the magnetic BC. Adsorbent magnetization and generation of additional adsorption sites were obtained with the dispersion of Fe3O4 and α-Fe2O3 particles. In fact, the magnetic adsorbent showed higher fluoride and nitrate adsorption capacities than those of BC. An endothermic and pH-dependent fluoride removal was identified. Experimental isotherms were analyzed and correlated with Langmuir model. Fluoride and nitrate adsorption capacities of magnetic BC were 9 and 15 mg/g, respectively, which outperformed the values reported for other oxide-based adsorbents and BC. Adsorption mechanism of both adsorbates (i.e., fluoride and nitrate) implied the hydrogen bond formation with the participation of protonated surface hydroxyls on the iron oxides.BCs and their magnetic versions were prepared with bovine bone and peanut hull for fluoride adsorption [162]. XPS, FTIR, XRD, SEM-EDX, and VSM were used to analyze the surface chemistry and magnetic properties of these adsorbents. A prepyrolysis approach (i.e., biomass+ironsalts+pyrolysis) enhanced the fluoride adsorption capacity of the magnetic BC in comparison to the adsorbent obtained from a postpyrolysis where BC was mixed with Fe3+/Fe2+ solution. Fluoride adsorption capacity of bovine-based magnetic adsorbent was >5 mg/g mainly due to γ-Fe2O3 and hydroxyapatite, which outperformed the nonmagnetic BC. It was inferred an ion exchange process in this endothermic fluoride removal. Freundlich model fitted the experimental adsorption isotherms of magnetic BC. Fluoride desorption was studied with 0.1 M NaOH solution, and results indicated that the magnetic BC maintained an acceptable adsorption performance for several regeneration cycles.A nanocomposite obtained from Fe3O4 and oak shell AC was used and assessed in fluoride adsorption [163]. Surface areas reported were 226.78 and 65.33 m2/g for AC/Fe3O4 and Fe3O4, respectively. Freundlich equation fitted satisfactorily the fluoride adsorption isotherms where the maximum adsorption capacity of AC/Fe3O4 was 454.54 mg/g, which is an outstanding performance for adsorbents reported for fluoride removal considering that their adsorption capacities ranged usually from 1 to 10 mg/g. The pH increment did not favor the fluoride adsorption and thermodynamic calculations confirmed an endothermic fluoride removal employing this magnetic adsorbent.Sahu et al. [164] evaluated the fluoride adsorption with a magnetic AC prepared using pea peel biomass impregnated with FeCl3 and pyrolyzed at 500 °C. Fluoride removal tests were performed with column and agitated tank modes. Initial fluoride concentration, solution pH, adsorbent dosage, and contact time were the operating parameters analyzed at batch adsorption conditions. The maximum fluoride adsorption capacity was 4.71 mg/g; it was established that water defluoridation was endothermic and pH dependent. Freundlich model was better than Langmuir model to fit fluoride adsorption isotherms. In the case of column studies, the breakthrough curves were analyzed with Clark, Yoon-Nelson, Adams-Bohart, and Thomas equations. This magnetic adsorbent showed a promising performance for water defluoridation in both batch and column operation modes. Fluoride adsorption mechanism was governed by fluoride-adsorbent interactions involving ketone, methyl, and hydroxyl groups, while the iron species imparted a positive charge to the adsorbent surface that generated electrostatic attraction forces for binding fluoride ions.


## 4.6. Dyes, Other Organic Pollutants, and Radionuclides

Dyes are complex organic molecules that are the most evident indicator of water pollution [165]. These compounds affect the aesthetic of aquatic systems and interfere with the sunlight transmission thus impacting the photosynthesis [165]. Dye classification includes different categories like nonionic (disperse dyes), cationic (basic dyes), and anionic (reactive, acid, and direct dyes), which can also consider their chemical structures like azo, anthraquinone, indigo, triphenylmethyl, and phthalocyanine derivative [165, 166]. These organic compounds are toxic and persistent pollutants with low degradability that can cause serious health effects with mutagenic and carcinogenic impacts on organisms [167–169]. Textile and dyeing industrial sectors are considered as the main contributors to this environmental pollution due to a significant release of dyes and related compounds into the water sources. It has been estimated that more than 100,000 commercial dyes are known, and their production is ~1.6 million tons of dyes/year where 10-15% can be released in wastewaters thus affecting the ecosystems [166, 168]. Dye adsorption with magnetic carbon-based adsorbents has proved to be effective. For illustration, Table 6 summarizes the dye adsorption using magnetic carbon-based adsorbents.Table 6
Removal of dyes, organic pollutants and radionuclides from aqueous solution using magnetic carbon-based adsorbents: preparation, removal operating conditions, and adsorption properties.
Synthesis routeMagnetic sourceCarbon sourceAdsorbateAdsorption capacity (mg/g)pHT (°C)Magnetization (emu/g)BET area (m2/g)ReferenceOne-pot method--CNTsRhodamine BCongo redMalachite greenMethylene blueNeutral red28.052.076.082.0101.0253.64186.3[248]Impregnation-pyrolisisFe3O4Empty fruit brunchMethylene blueOrange G31.2532.362-101025----[170]Impregnation methodFe3O4Coconut shell-activated carbonSunset yellow22.33 – 10--16.55-28.74238-372[249]Electromagnetization techniqueFe3O4Brown marine macroalgaeAcid orange 738253026.79336.97[250]Pyrolisis of SrFe12O19 and BCSrFe12O19Sewage sludgeMalachite green388.6572511.11--[251]Pyrolysis of rubber tires, impregnation with iron, and functionalization with polyethylenimineFe3O4Waste rubber tiresMethyl red526.0--25--153[102]β-Cyclodextrin-L-glutamic acid-magnetic GOFe3O4GraphiteEstradiol85.8072590.43298.9[252]One step coprecipitationFe3O4SludgeAcid orange 720.795.22258.4965.47[253]CoprecipitationFe3O4Bone charReactive 5G blue91.58--509.79142.43[254]Pyrolysis of bones at 500 °C, coprecipitationFe3O4Chicken boneRhodamine B109.662 – 102664.7328.06[171]Magnetic BC by impregnation and direct pyrolysisZn ferriteRice strawEstradiol153.25--2.242357.8[28]Coprecipitation methodFe3O4Pineapple crown leaf wasteMethyl violet16.765--15.095.11-314.08[255]Microwave methodγ-Fe2O3Sugarcane bagasseMethylene blue36.142 – 10----54.49-109.07[256]Thermal graphitizationFe3O4BambooMethylene blue286.62 – 1025----[257]Impregnation of husk with ZnCl2, carbonization at 400 °C, wet impregnation of iron saltFe3O4Rice huskMethylene blueMethyl orange17.7813.21325--375.02[2]Pyrolysis of straw at 500 °C, impregnation with iron saltFe0Corn strawMalachite green515.7762538.780.1[167]Ball-mill extrusion with Fe3O4Fe3O4ACBCMethylene blue310.0500.0--2533.834.975.490.6[258]Pyrolysis at 650 °C, impregnation with iron salt, and carbonization at 900 °CK2FeO4Lotus seedpodEstradiol98.73725147828.37[172]Hummer method and exfoliation of GOFe3O4GraphiteMethylene blueOrange GAlizarine cyanine green91%71%70%7------[259]Carbothermal magnetization by microwave-assisted impregnation with zinc and iron onto agriculture shell wastesZn ferriteWalnut shellMethylene blue130725--1000[260]Coprecipitation methodFe3O4GO and celluloseCongo redAcid red 1Reactive red 245.0947.3246.213-6308.9197.8[168]Pyrolysis at 700 °C and impregnation with iron salt and cetyl trimethyl ammonium bromideFe3O4Nut shellsAcid chrome blue K108.83502.08--[261]Direct mixing of the polymer matrix with the nanofillersFe3O4ACMethylene blue10.63635–651.28[262]Hydrothermal carbonizationFe3O4 and Fe0CarbohydrateMethylene blue570258766[263]Sol-gel and coprecipitationSpinel ferriteEthylene glycol60Cobalt152+154Europium82.51136.98925----[177]CoprecipitationFe3O4GOCesium362725----[176]Adsorbent nomenclature: activated carbon (AC), biochar (BC), and graphene oxide (GO).Mubarak et al. [170] tested orange-G and methylene blue removal with a magnetic BC, which was prepared using the empty fruit bunch. This biomass was first treated with FeCl3 and pyrolyzed in a microwave muffle. Dye removal was optimized via the analysis of contact time, stirring speed, adsorbent dosage, and pH. Methylene blue adsorption was maximum with a 125 rpm stirring, 1.0 g of adsorbent ratio, and 120 min of contact time at pH 10. The best removal conditions for orange-G were 125 rpm stirring, 1.0 g of adsorbent dosage, 120 min of contact time, and pH 2. 32.36 and 31.25 mg/g were the maximum adsorption capacities for orange-G and methylene blue dyes, respectively. Experimental data followed a pseudo second-order kinetic.Oladipo and Ifebajo [171] prepared a magnetic chicken bone BC for the adsorption of rhodamine B (RB) and TC. This adsorbent displayed a pHpzc of 8.3 with a magnetization value of 64.7 emu/g and 328 m2/g of surface area. The magnetic adsorbent was utilized for the adsorption of TC and RB with single and two-stage stirred adsorbers. This configuration reduced adsorbent fouling, mass transfer resistances, and pressure drops. The configuration of two-stage stirred adsorbers was optimized to obtain 98 and 96% RB and TC removal with 22.2 and 33.2 g of adsorbent for initial concentrations of 100 mg/L and 180 min of contact time. Freundlich equation correlated the adsorption results where the experimental adsorption capacities were 109.66 and 93.11 mg/g for RB and TC, respectively.Estradiol is an endocrine disrupting chemical that has become of public concern. Therefore, Yin et al. [28] analyzed Cu2+ and 17β-estradiol (E2) adsorption on activated and magnetic BC. One-step method was utilized to obtain these adsorbents at 300, 500, and 700 °C. Oxygenated functional groups, pore volume, and surface area of the magnetic adsorbent were higher than those of BC without modification. Also, the magnetic adsorbent showed better adsorption capacities for the removal of these pollutants in single and binary aqueous solutions. The adsorbent obtained at 300 °C showed the highest adsorption capacity of 85.93 mg/g for Cu2+, and the adsorbent prepared at 700 °C had an adsorption capacity of 153.2 mg/g for E2 in single aqueous solutions. Langmuir and pseudo second-order equations fitted the E2 and Cu2+ adsorption. Solution pH affected the adsorption of both pollutants. Binary experiments indicated an antagonistic (i.e., competition) adsorption. It appeared that Cu2+ adsorption occurred via a chemical complexation with the oxygenated functionalities, while E2 adsorption implied π-π interactions and hydrogen bonds.Also, a graphene-like magnetic adsorbent was synthesized with K2FeO4 and lotus seedpod for its application in the adsorption of 17β-estradiol (E2) [172]. Adsorption variables (e.g., foreign ions, humic acids, ionic strength, and solution pH) including the presence of other water pollutants like microplastics (MPs) and Al2O3 NPs were analyzed, and their impact on the E2 adsorption was established. Surface area of this adsorbent was 828.37 m2/g and displayed some graphene-like properties. E2 removal was interpreted with Langmuir isotherm and pseudo second-order kinetic. Sulfate ions, ionic strength, and solution pH impacted on E2 adsorption, while background electrolytes (e.g., NO3-, Cl-, Ca2+, K+, and Na+) and humic acids did not reduce the removal of this pollutant. MPs and Al2O3 significantly reduced the adsorption equilibrium time, but without a significant effect on the final E2 removal. The corresponding adsorption mechanism implied multiple interactions such as electrostatic π-π interactions besides micropore filling effects.GO–carboxymethyl cellulose and Fe3O4 were the feedstocks to prepare a magnetic composite to adsorb dye reactive red 2 (RR2), acid red 1 (AR1), and congo red (CR) [168]. FTIR, XRD, VSM, N2 physisorption, TGA, and SEM/TEM techniques were used to characterize the main adsorbent properties. This magnetic adsorbent showed adsorption capacities of 46.21, 47.32, and 45.09 mg/g for RR2, AR1, and CR, respectively. Freundlich equation showed the best fit for dye adsorption equilibrium experiments. Thermodynamic calculations confirmed an endothermic dye removal at tested operating conditions. Adsorption of these dyes on the magnetic composite was associated to surface complexation, π−π stacking, hydrogen bonding, and electrostatic forces. Particularly, there was a complex formation involving Fe3O4, while the composite and dye molecules interacted via electrostatic interactions with hydroxyl and carboxyl groups. NaOH solution (0.1 M) regenerated this adsorbent with an effectiveness of 65% up to adsorption-desorption cycles.Radionuclides are elements that emit alpha, beta, gamma rays, or neutrons [173], and they can occur naturally (e.g., terrestrial and cosmogenic) or anthropogenic (e.g., nuclear plants, weapons, testing sites, lignit burning, and fertilizers use) [173, 174]. Some radionuclides can be found in water due to the rock lixiviation and accidents in nuclear facilities [173, 175]. These radioactive elements can have a long life-time and radioactivity. The toxicology of these pollutants is associated to neurological damage, birth defects, and cancer [173, 175, 176]. Some magnetic adsorbents have prepared and tested to remove radionuclides. For instance, a magnetic GO was utilized for the cesium adsorption [176]. This adsorbent was prepared via coprecipitation reaction of iron salts and characterized with FTIR, Mössbauer, XRD, and TEM techniques. The adsorption capacity was 362 mg/g where Langmuir model was employed in the data correlation. Cesium removal was favored with pH, and it was concluded that an ion exchange was involved in its adsorption mechanism. Maksoud et al. [177] prepared carbon-modified zirconia/spinel ferrite nanostructures for the removal of cobalt and europium. The adsorption of these radionuclides was assessed at different conditions of pH and temperature. The adsorption was endothermic with adsorption capacities of 137 and 83 mg/g for europium and cobalt. Langmuir and pseudo second-order models were employed to fit the adsorption equilibrium and kinetics.


## 5. Patents and Status of the Commercialization of Magnetic Carbon-Based Adsorbents

There are several patents related to the preparation of magnetic adsorbents, and some of them are summarized in Table7. For instance, Kirsten et al. [178] obtained the patent WO2003053860A1 related to the preparation of ferromagnetic adsorbents derived from fly ash for the removal of metallic ions from wastewater. The patent JP2005137973A describes the preparation of a magnetic adsorbent combining iron oxide and porous adsorbents (e.g., activated carbon, zeolite, silica gel, and alumina) to treat water polluted with heavy metals, organic compounds, and microorganisms [179]. The patent JP2005046728A covers the production of magnetic adsorbent containing aminopropyl group for the adsorption of arsenic from water [180]. In the patent KR20060024312A, a wastewater treatment system was proposed that included a superconducting magnetic separation and activated carbon as adsorbent [181]. Sony Corp [182] patented a composite obtained from porous carbon material derived from plant-material and an oxide semiconductor. This composite can be applied for the adsorption of organic compounds, cosmetics, and photocatalysis. The University of Jinan obtained the patent CN105688825A, which was related to a method for the preparation of a magnetic adsorbent using ferrous metal-organic framework [183]. FeCl3, La(NO3)3, and sodium citrate were utilized in the adsorbent synthesis. This adsorbent can be employed for the removal of phosphate in water. In 2018, the Carbonxt Group obtained the patent AU2018203359 B2 associated to the impregnation of iron oxide on activated carbon with additives such as halogen or halide [184]. These additives were useful to enhance the oxidation of mercury contained in contaminated streams. In 2019, Honda Motor Co. obtained the patent number US20190091661A1 related to the preparation of magnetic adsorbents using different carbon allotropes. These magnetic adsorbents were tested to remove drugs, oil, and heavy metals [185].Table 7
Summary of patents related to the preparation of carbon-based magnetic adsorbents.
AdsorbentAdsorbatePatent (year)StatusReferenceFly ash-ferromagnetic saltsMetallic ionsWO2003053860A1, 2003Active[178]Magnetic adsorbents using activated carbon, zeolite, silica gel, and aluminaHeavy metals, organic compounds, and microorganismsJP2005137973A, 2005Pending since 2005[179]Aminopropyl groups-zirconium ferriteArsenicJP2005046728A, 2005Active[264]Porous carbon material composite obtained from plant-derived material and an oxide semiconductorOrganic compounds and other applications in cosmetics and photocatalysisUS20160243529A1, 2009Abandoned[182]Magnetic nanoparticlesSelenatesJP6494468B2, 2009Active[265]Hierarchical magnetic nanoparticle-enzyme mesoporous assemblies embedded in macroporous scaffoldsAromatic compoundsUS20180087043A1, 2013Active[266]Magnetic nanoparticles decorated activated carbon nanocompositesMethylene blue and methyl orange dyesUS20160243523A1, 2014Abandoned[267]Magnetic adsorbent using polyacrylamide solution and ferriteHeavy metals and phosphateUS10569250B2, 2015Active[268]Ferrous metal-organic frameworkPhosphateCN105688825A, 2016Active[183]Activated carbon impregnated with iron oxideMercuryAU2018203359B2, 2018Active[184]Carbon allotropes surrounding the ferromagnetic particlesHeavy metals, drugs and oilsUS20190091661A1, 2019Abandoned[185]Herein, it is convenient to remark that the industrial exploitation of these patents has not been reached. For example, Carbonxt Grupo is an Australian company that produces powder activated carbons, and its catalog of commercial products does not contain neither the patented adsorbent nor the corresponding adsorption system. Overall, the number of patents related to magnetic adsorbents is limited in comparison to the wide portfolio of adsorbents reported in the literature. It is clear that some magnetic materials can outperform the adsorption capacities reported for other commercial adsorbents like activated carbon, zeolites, or alumina. However, the large-scale production of these adsorbents imply additional technological and economical challenges to be resolved with the aim of exploiting these materials in water purification and other applications.


## 6. Conclusions and Perspectives of Magnetic Carbon-Based Adsorbents for Water Purification

Adsorption is a successful and mature technology for water treatment and purification due to its economic and operational advantages. In this direction, the magnetic adsorbents obtained from carbon precursors have gained a significant attention in this field due to their attractive features, which combine the magnetic characteristics of metals supported and those of the carbon matrix to promote their selectivity and performance for the adsorption of a wide spectrum of both organic and inorganic pollutants. The magnetic properties allow the adsorbents to be easily separated and recovered employing an external magnetic field thus contributing to their reutilization and reducing the limitations caused by the application of nanodimension adsorbent particles. Therefore, the preparation of magnetic adsorbents with iron and carbon matrices can be considered as a win-win approach, which takes advantage and outstanding properties of both phases: magnetic particles and carbon supports. This review enables readers to broaden their vision and analyze the progress and developments on this type of adsorbents to remove important pollutants such as fluoride, dyes, pharmaceuticals, heavy metals, arsenic, and other relevant compounds in the context of environmental pollution. To date, a great effort has been made to offer novel and competitive magnetic adsorbents, thus, enriching the experimental evidence related to the applications of these materials. It is evident the scarce of magnetic adsorbents produced at commercial stage and their limited number of patents with respect to the number of publications related to these materials. Overall, these indicators highlight the necessity of further development and research of improved magnetic adsorbents to achieve commercial products and consolidating their use in real life applications. In this direction, there are important topics to be researched and studied in future publications:(1)
The identification and selection of alternative green and low-cost feedstocks for the adsorbent preparation(2)
The study of the preparation conditions to control the adsorbent properties especially at large scale production(3)
The development of specific, low-cost, and green preparation methods to improve the adsorbent selectivity for target pollutant(s)(4)
The application of residual biomasses and wastes as feedstocks to avoid secondary pollution and to reduce the environmental impacts and costs of adsorbent production(5)
The proper characterization of the physicochemical properties of these adsorbents in order to determine the adsorption mechanism(6)
The evaluation of the adsorbent performance in real water systems and operating with dynamic conditions (column operation)(7)
The regeneration, reuse, and final disposal of the adsorbent to determine its lifetime and the corresponding life cycle analysisIn particular, the overcoming of technical challenges involved in the scale-up and industrial production of novel magnetic adsorbents is fundamental to reach a successful commercialization. Despite the various gaps and current challenges, an extensive and increasing progress is evident in this relevant topic for water treatment and purification.



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