# A Facile Review on the Sorption of Heavy Metals and Dyes Using Bionanocomposites

Authors: Uyiosa Osagie Aigbe; Kingsley Eghonghon Ukhurebor; Robert Birundu Onyancha; Benedict Okundaye; Kaushik Pal; Otolorin Adelaja Osibote; Ese Lawrence Esiekpe; Heri Septya Kusuma; Handoko Darmokoesoemo
Journal: Adsorption Science & Technology
 (2022)

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## Abstract

Presently, hazardous metal and dye removal from wastewater is one of the major areas of research focus. For the elimination of these contaminants, many approaches have been devised and applied. However, the accomplishment of various water treatment processes has largely depended on the medium utilized and the associated problem with the leaching of harmful compounds into the water process with most commercial and chemically manufactured materials for water treatment processes. Hence, this study is aimed at reviewing existing studies on the sorption of heavy metals (HMs) and dyes using bionanocomposites (BNCs). The key focus of this review is on the development of eco-friendly, effective, and appropriate nanoadsorbents that could accomplish superior and enhanced contaminant sequestration using BNCs owing to their biodegradability, biocompatible, environmentally friendly, and not posing as secondary waste to the environment. The sorption of most pollutants was observed to be pH, sorbent dosage, and initial contaminant concentration-dependent, with most contaminants’ elimination taking place in the pH range of 2-10. The sorption process of HMs and dyes to various BNCs was superlatively depicted utilizing the Langmuir (LNR) and Freundlich (FL) as well as the pseudo-second-order (PSO) models, suggestive of the sorption process of a monolayer and multilayer and the chemisorption process, the rate-limiting stage in surface sorption. The established sorption capacities for the reviewed sorption process for various contaminants ranged from 1.47 to 740.97 mg/g. Future prospective for the treatment and remediation of contaminated water using BNCs was also discussed.


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## Body

## 1. Introduction

An energetic base for living organisms and which is utilized in humans’ everyday endeavours is water. Owing to the fast manufacturing expansion, physical water reserves are impacted by various contaminants [1]. Notably, the World Health Organization (WHO) reports that an estimated 748 million of the global population are impacted by the supply of safe drinking water and water for sanitation. Alarming is the reported case of about 2.5 billion individuals without proper access to sanitation and about 3,900 infants that die daily owing to deficient water quality and infectious diseases; accordingly, water contamination by various contaminants has become a frightening issue globally as revealed by these reported figures [2].Globally, humans have had the right to use water as an abundant, free resource for many centuries. This condition has dramatically changed in modern times, and water shortage has now become one of the menaces to the human community’s long-term growth [3]. This problem is expected to grow at an exponential rate, making it a wide-reaching systemic risk. The global blue water scarcity statistics at a high spatial resolution was calculated by Mekonen and Hoekstra on a month by month basis, and according to this assessment, about four billion people, or two-thirds of the world’s inhabitants, suffer from severe water shortage at least one month in every year, with half of these numbers living in India and China. Furthermore, they reported that 0.5 billion people around the globe are affected by this issue annually (Figure 1) [4].Figure 1
Recorded global water scarcity between 1996 and 2005 [4].Most of the obliterations of the quality of air, water, and soil which are critical for life sustenance on earth are due to the fast-growing global population and industrialization [5]. An imperative constraint for economic growth is the accelerated urbanization and industrialization as well as the swift increase in water consumption and the issue of water scarcity [6]. Water quality has exceptionally declined owing to the untreated effluents discharged into streams, lakes, and oceans by refining metal plating, mining, paint and dyes, and textile productions [5]. Water use in these industries has increased by as much as 22% (industry), 70% (agriculture), and 8.0% (household) of available freshwater, resulting in a massive amount of wastewater containing several contaminants. Without a doubt, the discharge of effluent from commercial and industrial sectors, as well as untreated sewage from households and chemical contaminants such as HMs, pharmaceuticals, pesticides, and dyes, is among the several compounds, released into freshwater supplies, which are harmful not only to humans but also to animals, plants, and the ecosystem in general [4, 7, 8].Presently, one of the utmost global environmental problems is the pollution of water with HMs and other toxic chemicals, released from mining, refining, electroplating, chemical plants, metallurgy, agriculture, and household effluents [9]. A serious hazard is posed to an individual’s health, environment, and other ecological receptors by HMs such as lead (Pb), zinc (Zn), copper (Cu), and mercury (Hg). Biologically, owing to HMs accumulating in the food chain, they cannot be degraded by microorganisms when released into the ecosystem [6]. Grave health issues, as well as decreased growth and development, cancer, organ injury, impairment to the nervous system, rheumatoid arthritis, kidney injury, and death in extreme cases, are caused by HMs [10]. High doses of metals are mostly received through food by children than adults, due to a huge amount of food consumed for their body weight than adults. Table 1 gives some details of the impact of excessive intake of heavy metal ion (HMI) and their noxiousness in the ecological perspective as well as their maximum allowed level (MCL) as recognized by the United States Environmental Protection Agency (USEPA) [11].Table 1
Impact of excessive intake HMI, their noxiousness in the ecological perspective, and their MCL [11].
HMsNoxiousnessMCL (mg·L-1)AsVisceral tumours, skin symptoms, and vascular disease.0.05CdHuman carcinogen, kidney injury, and renal disease.0.01CrCarcinogenic, headache, diarrhoea, nausea, and vomiting.0.05CuInsomnia, liver impairment, and Wilson disease.0.25NiHuman carcinogens, dermatitis, nausea, compulsive asthma, and coughing.0.20ZnHeightened thirst, depression, fatigue, and nervous signs.0.80PbImpairment to the developing brain, circulatory system, nervous system illnesses, and kidney disease.0.006HgCirculatory and nervous systems, rheumatoid arthritis, and kidney injury.0.00003Among these noxious and aromatic contaminants released into water bodies without prior and proper treatment, the textile industry is a primary user of synthetic or noxious dyes for product colouring [12]. Dye is a major source of serious contamination owing to the fast industrial development and extensive utilization [13, 14]. Dyes have been used for textiles, paint, pigments, and other purposes for thousands of years. In the clothing, paper, plastics, leather, food, and cosmetic industries, dyes and pigments are commonly used to dye goods. The majority of dyes are poisonous and must be discarded before being discharged into waterways [15]. The global textile production is projected to be valued at around a trillion United States Dollars (USD), and its overall global export contribution is about 7.0% and with the global engagement of 35 million individuals. The greatest major and vicious contamination form triggered by textile production is the contamination of water owing to dye industries. Wastewaters from textiles are both visually contaminated and have elevated salinity, ecotoxicity, and chemical oxygen demand. Also, owing to their enhanced omnipresence in surface water, it negatively affects the health of humans, wildlife, and marine ecology [16]. A major consideration has been drawn by pollution of water through the discharged dye from paper production, food processing, textile dyeing, paints, and cosmetic industries owing to community health and ecosystem hazards. At present, the worldwide colourant market is about 32 billion USD and is projected to grow to about 42 billion USD in 2021. Yearly, the total of synthetic dyes manufactured is estimated to be over 700,000 tons, and more than 15% of these are discharged into water annually. Water polluted by these dyes are noxious, xenobiotic, and carcinogenic, and they are grouped according to their chromophore structure into the solvent, reactive, basic, vat, and direct dyes. Exclusively, 47% of synthetic dyes are decomposable [17].At present, about a hundred thousand different dyes are commercially manufactured, and in terms of volume, 1.6 million tons of dyes are consumed annually. As a result, 10-15% of the product is lost during usage. A dyeing process involves organic dyes and water usage in several industries, including textile, leather, paper, cosmetics, plastics, and food [15]. Dye-containing wastewaters such as water sources polluted with dye molecules are coloured organics with low biodegradability, resulting from these processes. Dyes, especially azo dyes, are tenacious, withstanding aerobic digestion and oxidizing agents. The multiple benzene rings in azo dyes cause this severe resistance. According to statistics, 1-20% of global dye output is lost in textile effluents, negatively impacting human metabolism, ecosystems, and natural processes such as eutrophication. Coloured effluents released into the aquatic media block sunlight, preventing algal and aquatic plants from the photosynthesis process [4]. Furthermore, azo dyes and their metabolites have been shown to have negative effects on people and animals owing to their noxiousness, carcinogenicity, and mutagenicity. When they are dissolved in water-soluble solutions, they are categorized based on their functional groups, colour, and ionic charges. The last form of classification, which is based on dye molecule ionization and has a significant impact on dye sorption performance, is more important. As a result, they can be divided into two categories: ionic and nonionic. Nonionic dyes are classified as cask and disperse dyes, while ionic dyes are classified as cationic (basic) and anionic (reactive, direct, and acidic) dyes [15].The dyes mentioned in Table2 are mainly carcinogenic and should be handled efficiently in dye processing plants to keep them from being released into the ecosystem. The properties, applications, and toxicity of individual dye forms are mentioned in Table 2 [18].Table 2
Classification of dyes, their properties, applications, and noxiousness to the environment [4].
Types of dyeDye propertiesDye applicationsDye noxiousnessExamplesAcidicAnionic, water-solubleWool, silk, ink-jet printing, nylon, paper, and leatherCarcinogenicAcid red 183 (AR-183), acid orange 10 (AO-10), acid red 18 (AR-18), sunset yellow (SY), acid green 27 (AG-27), methyl orange (MO), amido black 10B (AB-10B), and indigo carmine (IC)CationicWater-soluble and releases colour cationsAntiseptic for biomedicine, paper, PAN, treated polyesters, and nylonCarcinogenicMethyl blue (MB), basic violet 10 (BV-10), Janus green (JG), basic green 5 (BG-5), and rhodamine 6G (R-6G)DisperseNonionic, for aqueous/hydrophobic dispersions, and water-insolubleNylon, polyester, acrylic fibers, cellulose (CLL), and CLL acetateSkin allergenic and carcinogenicDisperse orange 3 (DO-3), disperse red (DR), disperse red 1 (DR-1), and disperse yellow 1 (DY-1)DirectWater-soluble, anionic, and chelate with metal saltsCotton, paper, leather, and regenerated CLLCancer of bladderCongo red (CR), direct red 23 (DR-23), and direct blue 86 (DB-86)ReactiveGenerates brighter colours and a high wash grip due to the covalent bond to the fibersWool, cotton, ink-jet printing of textiles, and nylonDermatitis, conjunctivitis allergic reaction, rhinitis, and work-related asthmaReactive black 5 (RB-5), reactive green 19 (RG-19), reactive blue 4 (RB-4), reactive red 195 (RR-195), reactive red 198 (RR-198), reactive red 120 (RR-120), reactive blue, and 19 (RB-19)VatWater-insoluble and reduction into weakly acidic leucon form by NaOHCLL and fibersVat blue 4, (VB-4), vat green 11 (VG-11), vat orange 15 (VO-15), vat orange 28 (VO-28), and vat yellow 20 (VY-20)Therefore, capable technologies for water treatment have been recognized to raise water resource potential and reduce the water contamination challenges and fears [2]. Over the years, nanomaterials (NMs) have earned huge interest in various fields like electron devices, health care, energy, and environmental protection field. Under the nanoscale, unique features like surface effect, effect of small size, quantum effect, and effect of the macro quantum tunnel are exhibited by NMs. These features contribute to their remarkable sorption capacity and reactivity; together, they are advantageous for the sorption of HM ions and dyes. Extensive research has been conducted on NMs to study their uses in pollutants in water treatment, and they have shown significant promise as a viable alternative to removing contaminants from wastewater [6].In the development and application of NMs (nanoparticles (NPs), nanotubes (NTs), nanofibers, and nanowires) in science and engineering, there has been improved attention on their research. NPs were chosen for contaminant removal from wastewater because of their low cost and qualities (particle size, shape, even distribution of particle size, crystal structure, component distribution, purity, aggregation control, and stabilisation). Organic or inorganic NPs with high porosity, small size, and broad surface area make full use of their interface with dye or HM molecules via multiple contaminant binding sites, resulting in high sorption efficacy [19].In respect of water purification technology as well as treatment of potable water, desalination, and treatment of water, nanocomposites (NCs) play a considerable part to provide substantial machinery for water purification at a reduced price employing a reduced amount of energy and further reducing the environmental effects. To prevent various environmental issues such as the treatment of water polluted with HMs, organic contaminants, inorganic anions, pathogen, dyes, and industrial effluents, they have been applied extensively using zero-valent metal NPs, metal oxide NPs, carbon nanotubes (CNTs), bionanocomposites (BNCs), biopolymers (BPs), etc. [2].When their sizes approach the nanoscale, and as the atom segment at the material’s surface gains momentum, NMs such as NPs, CNTs, nanosheets, and nanofibers have shown distinct chemical and physical properties due to their nanoscale dimensions. For example, they have massive surface-to-volume ratios or massive interfacial reactivity. NPs have a large surface-to-volume ratio and a high percentage of surface-associated atoms and molecules [19].To meet the aforementioned requirements, a wide range of sorbents with dimensions below the nanoscale have been established over the last few decades as nanotechnology has progressed. These NMs have a large reactive surface area for a low density, and they can be synthesized at a lower cost and extract dyestuff in a much smaller quantity than activated carbon. Several nanoadsorbents in various shapes and dimensionalities (D) of NPs, (0D), nanofibers and nanotubes (1D), nanosheets (2D), and nanoflowers (3D) have been investigated in terms of dye removal. The 0D nanoadsorbents are those whose external dimensions are between 1 and 100 nanometres (nm) [4].There has recently been a lot of interest in using the sorption technique to remove certain dyes from solutions on different adsorbent surfaces. Clays, fly ash, peat, activated carbon, polymers, and alumina are only a few examples of different adsorbents. The procedure is well-known for being simple and effective in treating concentrated dyes [20].Although there are no stand-alone methods to fully decolourize or remove HMI from wastewater due to the overwhelming variety of azo dye chemophysical and structural properties, the growth of industries with dye by-product contamination, combined with declining water supplies, necessitates the development of new methods and materials to recycle wastewater. Natural materials, BPs, and BNCs have all gained a lot of publicity as possible adsorbents in this regard. Natural materials are biodegradable and biocompatible, making them environmentally friendly. Protein-based sorbents have distinct advantages over traditional polysaccharide-based adsorbents like CLL, chitosan (CS), and lignin due to their structural and chemical diversity. Furthermore, certain proteins can self-assemble and transform into highly organized nanofibrils that can withstand high temperatures and salt concentrations and have strength and stiffness similar to steel and silk [21].A variety of HMs and synthetic dye wastewater disposal methods have been developed to reduce their environmental effects [22]. HM and dye sequestration from water bodies has substantial importance to the ecosystem, and developing effective and cost-effective removal techniques is a going continuous effort. These methods comprise of the sorption of pollutants to mineral or carbon-based matrix [23], photocatalysis or oxidation processes [24], chemical precipitation [25], ion exchange [26], microbiological or enzymatic decomposition [27], coagulation [28], reverse-osmosis [29], membrane filtration, etc. [30].Sorption of inorganic or organic matrices, photocatalysis and/or oxidation processes, microbiological or enzymatic decomposition, and so on are some of the technologies. Because of its convenience, ease of use, and simplicity of design, the sorption process is regarded as the most successful of the various available water treatment technologies [22, 23].The process of sorption is a distinctive technique for the confiscation of contaminants from water-soluble solutions by putting them precisely on the surface of the adsorbent [28]. For the purification of effluent media, sorption is a popular industrial separation technique. It is a mass transfer operation in which a solid material attracts dissolved solutes to its surface and thereby selectively removes them from an aqueous solution [3]. As a result, it entails the interphase aggregation of material concentrations at a surface or in the interphase. The removal of dye from aqueous media is a popular application for this separation technique [31]. It is used in the clothing, leather, dyeing, cosmetics, plastics, fruit, and paper industries, among others, where water recovery is critical [20].Consequently, this paper is aimed at reviewing existing studies on the sorption of HMs and dyes using BNCs. The paper examines some of the most recent developments for the removal of HMs and dyes from wastewater using BNCs. The major emphasis of this review is on the development of eco-friendly, effective, and appropriate nanoadsorbents that could accomplish superior and enhanced contaminant sequestration using BNCs owing to their biodegradability, biocompatible, environmentally friendly, and not posing as secondary waste to the environment. Consequently, the roles of NMs for the treatment and remediation of wastewater and contaminants in water are presented systematically and comprehensively drawn from existing publications. Future prospectives for the treatment and remediation of contaminated water vis-à-vis water purification technology in the form of suggestions and recommendations are also discussed.


## 2. BNCs as a Sorbent for the Treatment of Wastewater Contaminated with HMs and Dyes

BNCs have evolved over the last few decades into a standard word describing a naturally occurring polymer (BP) in combination with an inorganic component that appears at least a nm scale measurement (<1000 nm) because of their widespread availability. They have gained international attention, and their environmental friendliness contributes to green chemistry [32]. They are divided into groups based on their origin, the types of matrix used, and the size and shape of the reinforcements. BNCs are classified as layered structures, particulate, and elongated particles based on the morphology of the particles used for reinforcement [33, 34]. Isodimensional particles are mostly used as supports for specific BNCs, and the strengthening force is moderate because of the low aspect ratio. This sort of support is used to increase flammability resistance, reduce permeability, and lower the cost of composites. BNCs (CNTs and CLL nanofibrils) are used as a support in elongated particles [35].Natural species (mainly BPs) and mineral solids with a wide range of shapes and structures bonded at the nanoscale scale make up BNCs (biohybrid materials). In terms of preparation methodology, characteristics, functions, biocompatibility, biodegradability, and applications, they differ from NCs. BNCs are also known as biocomposites, NCs, nano-BNCs, green composites, biohybrids, or biobased plastics, even though the name is new to the public (bioplastics) [36]. BPs are polymers that occur naturally and have potential use in disciplines such as agricultural science, sanitary products, wastewater treatment, and medicine delivery [37].BPs are often made up of nontoxic monomers and are carbon neutral. Because biomass morphology is often structured at the nanoscale, BPs make it easier to make NMs. BPs are chemically distinct and have a wide range of physiological features. BPs, in particular, form molecular capsules by intramolecular hydrogen bonding [38].Natural biodegradable BPs include plant carbohydrates (starch, CLL, CS, alginate, agar, carrageenan, etc.) and plant and animal source proteins (soy protein, corn zein, wheat gluten, gelatine, collagen, whey protein, casein, etc.), synthetic biodegradable BPs like polylactic acid (poly(L-lactide) (PLA), poly(glycolic acid) (PGA), poly(-caprolactone) (PCL), poly(butylene succinate) (PBS), poly(vinyl alcohol) (PVA), and other synthetic biodegradable BPs, and BPs produced by microbial fermentation (poly(hydroxyalkanoates) (PHAs) such as poly(-hydroxybutyrate) (PHAs) comprising of poly(β-hydroxybutyrate) (PHB), poly(3-hydroxybutyrate-co-3-hydroxyvalerate) (PHBV), etc., and microbial polysaccharides, like pullulan and curdlan) [39].As for BPs, the polysaccharides like CS, CLL, starch, alginate, and polylactide are generally utilized for the preparation of BNCs. The major BPs employed are shown in Figure2, and from an environmental perspective, polysaccharides are the ideal BPs owing to their characteristic biodegradability, creation from renewable supplies, accessibility, lack of noxiousness, and relative minimal cost [40].Figure 2
Chemical structures of BPs generally employed for the creation of BNCs [40].Polysaccharides originating from plants and microbial biofilms, such as CS, starch, dextran, and CLL, are commonly used in NM fabrication. Starch, for example, can combine metals or metal oxides to generate polymeric NCs. Because of its broad compatibility, CS is also used in nanotechnology applications. CS has been utilized for colour removal and wastewater treatment in particular. Metals can be attached to BPs to create BP NMs (Figure3) [38].Figure 3
BP sources and their utilization in preparation of green polymeric NMs (M+:MI) [38].In situ polymerization, solution blending, casting, and melt processing are commonly used to make BNCs. Other synthesis processes including electrospinning and processing have recently gained popularity under supercritical conditions. In situ polymerization, melt processing or blending, and solution casting or blending are commonly used in the creation of polymer NCs, with the purpose of optimal NP dispersion during processing [37, 41].They have improved mechanical behaviour because of the large aspect ratio of this support. Based on particle dispersion in the matrix, layer-supported BNCs (layered polymer NCs) are divided into three secondary classes. When there is no barrier between layers due to particle-particle interactions, phase/flocculated separated NCs are formed, and because specific components are not separated, they are referred to as microcomposites. As a result, they act as dissolved microparticles in the polymeric matrix. When polymer chains are intercalated between sheets of layered NPs, intercalated NCs are formed, and exfoliated NCs are formed when individual layers are detached. Mechanical characteristics, biodegradability, and biocompatibility are all outstanding. They are increasingly being used in biomedical applications (drug delivery systems, vaccination, wound dressing, and tissue engineering), BNC films (low-cost, environmentally friendly, and renewable food packaging materials with enhanced antimicrobial activity), and as an emerging sorbent for dye and HM ion removal [36, 42].In this study by Song et al. [43], CLL/clay composite was created for the sorption of Drimarine yellow HF-3GL direct dye. The prepared composite was characterized using SEM, which showed the morphology before and after the sorption of the dye onto the composite. It was noticed that the composite had a rough and porous surface and the surface becomes smooth after sorption of dye as shown in Figure 4. The sorption of this dye was also observed to be optimally removed at pH 2, and this was ascribed to the interaction between the created positive active sites on the composite surface and the dye. The pseudo-second-order (PSO) and the Redlich-Peterson models best described the sorption process using the nonlinear kinetic (KNT) and equilibrium isotherm (IST), while the thermodynamic (TMD) factors showed that the sorption process was spontaneous, exothermic, and reasonable. NaOH showed a high desorption efficiency and the composites showed high efficiency of 90-96.07% and 97-98.23% for the dye removal using the respective dyes (composite I and II).Figure 4
(a) CLL/clay composite SEM before and (b) after sorption of yellow HF-3GL direct dye [43].
(a)(b)(c)(d)To obtain films that possess optimal functional properties such as biodegradability, nonnoxiousness, and bioadhesion, natural biodegradable CS-based thin-film nanogels (TNGs) were prepared for the sequestration of HMI. 2-Hydroxyethyl methacrylate (HEMA) and acrylic acid (AA) were grafted to the CS through the redox initiator system of ammonium persulfate (APS), and complex catalyst CuSO4/glycine in the presence of foaming agent sorbitol was created. A new thin-film (CS-g-P(HEMA-co-AA)/nano-CaO nanogel) created from the blend of CS-g-P (HEMA-co-AA) copolymers altered with snail shell was employed to capture active noxious HMI. The sorption of Cr (VI) to TNG was best defined using the Langmuir (LNR) and the LNR-Freundlich (FL) as well as the PSO sorption models. The determined sorption capacity was calculated to be 149.7 mg/g at a temperature of 25°C [44].While guar gum/bentonite BNCs prepared using the solution intercalation technique were employed for the removal of Pb (II) and crystal violet dye (CV), the SEM images in Figure5 show the micrographs of the BNCs (a) indicating the existence of a solid bounded network structure with pores or voids present within the surface. With the BNC surface being irregular and permeable, it offered a good platform for CV and Pb (II) sorption. After sorption of CV and Pb (II), a smooth surface presence on the surface of the sorbent was noticed, indicating that the pores or voids are being filled by the contaminants. Their particle sizes ranged from 3 to 11 nm according to the TEM analysis.Figure 5
SEM images of (a) BNCs and (b, c) contaminants loaded BNCs with their respective EDX spectral [45].
(a)(b)(c)The point of zero charge (pHPZC) of the BNCs was found to be 2.2, with optimum sorption capacity noticed at pH 5.1 and 7.6 for Pb (II) (97.94 mg/g) and CV (39.149 mg/g). From the KNT and IST studies, it was found that the sorption of both Pb (II) and CV was best defined using the PSO and LNR (CV) and FL (Pb (II)). While the sorption process was depicted physisorption, spontaneous and endothermic with enhanced uncertainty, an efficient regeneration efficiency was observed up to five cycles using 0.1 M HCl. The synthesized BNCs were successfully applied for the sequestration of HMs from the electroplating battery industrial and medical effluents before and after spiking it with CV dye solution [45].A new sorbent was created in this study by the alteration of CS applied for the confiscation of Cu (II) and Cr (VI). To develop a crosslinked gel, Schiff-based was created from the CS reaction with 3-methyl-1-phenyl-5-(piperidin-1-yl)-1H-pyrazole-4-carbaldehyde, which was crosslinked with epichlorohydrin (ECSBNC). To get a magnetic sorbent material, Fe3O4 NPs were integrated into the altered CS gel. Figure 6 shows the SEM images of Fe3O4, ECSBNC, and ECSBNC loaded with Cu (II) and Cr (VI). Aggregation of spherical-shaped NPs of various sizes was visible on the surface of Fe3O4 (Figure 6(a)). The Schiff base of CS containing Fe3O4 NPs had an uneven flake-like structure, as seen in Figure 6(b). Cu (II) and Cr (VI) sorption on the surface of the adsorbent is shown in Figures 6(c) and 6(d), respectively. The sorption looks to be consistent across the entire surface. The data of the sorption process were well fitted employing the LNR and PSO models, with a determined sorption capacity of 90.90 and 83.33 mg/g for Cu (II) and Cr (VI), respectively. While the parameters of TMDs show that the sorption process was endothermic and spontaneous, the desorption studies also show an effective recovery of the sorbate species and the possibility of sorbent material reuse [46].Figure 6
SEM images of (a) Fe3O4, (b) ECSBNC, and ECSBNC loaded with (c) Cu (II) and (d) Cr (VI) [46].
(a)(b)(c)(d)A green technique was used to create a BNC-based protein concentrate; its nanofibrils and montmorillonite nanoclay (WPF/MMT) were employed for the removal of cationic dye (Chrysoidine-G (CG), Bismarck brown-R (BBR)), acid dyes (acid red-88 (AC88), acid red-114 (AR114)), direct dyes (direct violet-51 (DV51), congo red (CR)), and reactive dyes (reactive black-5 (RB5), reactive orange-16 (RO16)). It was observed that the BNCs sorbed the CG cationic dye much faster than the other dye type, and with a greater than 93% removal efficiency for a wide concentration range of CG dye, while the PSO and the linear Nerst models best depict the sorption of these dyes to the BNCs [21].In this study, a BNC created from cyclodextrin-polycaprolactone titanium dioxide was employed as a biosorbent for confiscation of Pb (II). Titanium dioxide was prepared through the sol-gel method and was integrated into the polymer blend (CD-PCL) through the solution blending technique. The CD-PCL-TiO2 nanocomposite’s size, shape, and aggregation were studied using TEM. As shown in Figure 7, CD-PCL-TiO2 exhibited a variety of morphological characteristics, including a rod-like structure with an average diameter of 395 nm and a few rectangular shapes. Aggregation of CD-PCL-TiO2 was also noticed. The particles adhere to one another, resulting in an uneven crystal structure. However, there are no visible TiO2 NPs, which is due to TiO2 being evenly dispersed throughout the BNC matrix [47].Figure 7
SEM image of CD-PCL-TiO2 BNCs [47].Optimum removal sorption of Pb (II) was 98% noticed at pH 9.7, using a 10 ppm and a dosage of 0.005 g. The surface charge of the BNCs was more negative at higher pHs when the pH of the solution is higher than the point of zero charge (pHpzc) of 8.80. Hence, there is electrostatic attraction between the sorbent and the sorbate (Figure8). The sorption of Pb (II) to the BNCs followed the LNR and PSO models [47].Figure 8
Impact of pH on the sorption of Pb (II) to the BNCs [47].A new circular method was employed to tackle issues relating to noxious secondary water using TiO2 nanorods (NRs), and functionalized gum ghatti (Gg) BP-based BNCs (TGB-hydrogel (TGB-H)) created via the free radical graft polymerization were used for brilliant green (BG) dye. The dye sorbed TGB-hydrogel was subsequently treated at 550°C for 3 h and reused for the degradation of antibiotic ciprofloxacin (CIP) photocatalytically. Thereafter, the sent photocatalyst was restored and employed for the sorption BG dye to finish the round. The sorption process was ideally defined using the LNR and PSO models. The determined sorption capacity was found to be 740.97 mg/g, and the sorption process was found to be spontaneous and endothermic using the TMD studies, indicatives of physical sorption owing to the low calculated value of ΔH°. The high photocatalytic efficiency of 88.7% was found for CIP using the acquired photocatalyst owing to the recombination delay of the charge carriers, high light sorption, and the elevated surface area. The high-resolution transmission scanning electron microscope (HR-TEM) was used to determine the morphologies and particle sizes of the synthesized materials (TiO2 NRs and TGB-H). The HR-TEM images shown in Figures 9(a) and 9(b) depict the created TiO2 with NR-like morphology with an average width and length of approximately 4 and 45 nm. Bundles of NRs were created due to the surface polar functionalities, while Figure 9(c) shows a crystalline domain with a lattice fringe of 0.326 nm which relates to the 101 crystallographic planes of the rutile TiO2 NRs. The polycrystalline nature of TiO2 NRs was confirmed using the selected area electron-diffraction (SAED) (Figure 9(d)), and the visible bright spots were attributed to the 110, 101, 111, and 211 crystalline plane refection of the rutile TiO2 NRs, while the HR-TEM images in Figures 9(e) and 9(f) show the well-distributed TiO2 NRs in the crosslinked polymer matrix of the hydrogel network [48].Figure 9
HR-TEM images of (a, b) of TiO2 NRs, (c) crystalline domain TiO2 NRs, (d) SAED patterns of TiO2 NRs, and (e, f) TGB-H [48].The sorption of the cationic BG dye was attributed to the electrostatic interaction, van der Waals forces, ion exchange,π−π interactions, hydrogen bonding, and Yoshida hydrogen bonding interactions, and based on the FTIR data, the possible interaction between the sites of the dye and the TGB-H sorbent (Figure 10), a loss of the carbonyl, and -C-O peaks of the dye sorbed TGB-H was observed, which was indicative of the -COO- groups being involved BG dye sorption enabled by the interaction between the -COO- groups of the TGB-H and the positively charged nitrogen centre of the dye.Figure 10
The mechanism of interaction between the BG dye and TGB-H sorbent [48].Magnetic chitosan (CS@Fe3O4) NCs prepared using the solvothermal technique and which were altered using graphene oxide (GO) to create CS@Fe3O4GO NCs were employed as a sorbent for Cr (VI) confiscation from water-soluble solution. The XRD result of the sorbent in Figure 9 showed excellent agreement with the elemental study. Fe3O4 were allocated XRD peaks in the 2θ range of 35°, 43°, 54°, 57°, and 63°, the shoulder observed at 30°. Based on the result of XRD, no crystalline CS and carbon were present in the sorbent (Figure 11).Figure 11
XRD pattern of prepared NCs for Cr (VI) removal [49].Optimum removal of Cr (VI) was noticed at pH 2, with determined sorption capacities of 84.84, 82, and 10.28 mg/g applying CS@Fe3O4, CS@Fe3O4GO, and Fe3O4. Improved sorption at the acidic pH was ascribed to the sorbent surface protonation owing to H+ ions, which enhances the electrostatic attraction between the negatively and positively charged sorbent surface and chromate ions. With the increase in the solution pH, a drop in the sorption capacity is observed (Figure 12).Figure 12
Impact of pH on the sorption of Cr (VI) [49].The KNT and IST reactions associated well with the PSO and FL models, with a determined sorption capacity of 142.32 and 100.1 mg/g for CS@Fe3O4 and CS@Fe3O4GO. TMD parameter assessment shows that the interaction between the sorbate and the sorbent was spontaneous and endothermic. Also, the reusability studies indicated that the sorbent can be reused for four regeneration cycles. Results show that the created sorbent could be employed in the sequestration of Cr (VI) ions [49].Biodegradable xanthan gum/montmorillonite (XG/MMT) BNCs were employed for the sequestration of Pb (II) from industrial and synthetic effluents. The sorption process was perfectly illustrated using the PSO and the FL models, while the TMD study shows that the sorption process was spontaneous and endothermic. The sorbent was efficiently restored utilizing 0.05 M HCl for five runs, showing that this BNC was a promising and prospective sorbent for practical applications [50].Mahdavinia and Mosallanezhad [51] report in this study the preparation of a magnetic BNC sorbent based on k-carrageenan through the in situ technique which was crosslinked by CS polysaccharide via electrostatic attraction. The prepared magnetic BNC sorbent was used in the MB removal from water-soluble solution as shown in Figure 13.Figure 13
Schematics showing the steps of preparation of the magnetic BNC sorbent for MB removal [51].From the pH experimental result, the sorption of MB to the magnetic BNCs was via electrostatic attraction between positively charged MB dye and negatively sulfate pendants on the BNCs and optimum removal for MB was noticed at pH 12. The sorption of MB to the BNCs was ideally defined using the LNR and a determined sorption capacity of 130.4 and 123.1 mg/g using nonmagnetic and magnetic sorbents. The TMD result showed that the sorption process was spontaneous, endothermic, and improved randomness. With the rising temperature, the negative value of∆G° improved progressively which was indicative of sturdier sorptive forces between the MB and BNCs [51].Synthesized starch/CLL nanowhisker hydrogel composite was effective sequestration of MB. The sorption of MB to the hydrogel composite was best depicted using the LNR and PSO models. The determined sorption capacity of 2050 mg/g was obtained using this hydrogel composite for MB removal. The possible mechanism of sorption of MB to the hydrogel composite was ascribed to the combined hydrogen bonds, hydrophobic interaction, and electrostatic interactions between the negative charges’ groups in the sorbent (-COO-) and the positive charge MB (Figure 14) [52].Figure 14
Possible mechanism of sorption of MB to hydrogel composite [52].In this study, starch and sodium montmorillonite (starch/Na-MMT) NCs were created using an acetic acid solution using the intercalation method and employed in the sequestration of Co (II) and Ni (II) ions. Optimum confiscation of both HMI was detected at pH 4.5 and 6 for metal concentration of 100 and 140 mg/L of Co (II) and Ni (II) with a determined removal yield of 78.07 and 97.1%. The experimental data fitted well to the FL IST, which was indicative of a multilayer sorption process for both HMI [53].Starch/poly (N,N-diethylaminoethyl methacrylate) copolymer was created through the grafting polymerization of N,N-diethylaminoethyl methacrylate monomers to heated starch utilizing as an initiator of a ceric ammonium nitrate/nitric acid mixture. To convert the created copolymer to hydrogels, it was subjected to crosslinking treatment employing epichlorohydrin in an alkaline medium. The created hydrogel was employed for anionic dye DR-81 removal from water-soluble solution. The swelling ratio of the created hydrogel was found to be 100. The sorption of DR-81 to the hydrogel was best described using the LNR model, and the determined sorption capacity was 112 mg/g [54].In this study, CS/Ag-substituted hydroxyapatite NCs were prepared and applied as a sorbent for the confiscation of basic dye, HM, and microbes. The morphology of the CS utilized had a heterogeneous surface and was rough with intermittent pores. No change was noticed in the NCs with the introduction of Ag-substituted hydroxyapatite. The rough surface of the beads with intermittent pores provided improved surface area and sufficient sites for the sorption of pollutants to the surface of the beads (Figure15). Optimum sorption capacities using this sorbent were observed at pH 7 for both dye (rhodamine B-RhB) and HM (Cu II). The LNR and PSO model best depicted the interaction between the Cu (II) and RhB, and the determined sorption capacity was found to be 40.11 and 127.61 mg/g. The percentage of sequestration efficiency for Cu (II) and RhB from tap water and untreated river water ranged from 86.7 to 94.4%, and microbial load decontamination was 99.99% [55].Figure 15
Morphology of CS/Ag-hydroxyapatite [55].While in the study by Eivazzadeh-Keihan et al. [56], a synthesized magnetic guanidinylated CS (MGCS) BNC was applied as an effective sorbent for the elimination of HMs such as Cu (II), Pb (II), and Cr (VI) and in vitro hyperthermia for cancer treatment. According to the pH result for Pb (II) sorption to the BNCs, it was reported that the maximum percentage removal occurred at pH 7 (90.56%). The sorption process of Pb (II) to the BNCs was best described using the LNR and the PSO models, with a maximum monolayer coverage capacity of 60.60 mg.g-1. While for the in vitro treatment of cancer, it was discovered that specific sorption rate and saturation magnetization values obtained were 70.56 w.g-1 and 43.66 emu/g using an alternating magnetic field.Also, in the study by Peralta et al. [57], a magnetic CS composite (MCSC) was synthesized by implanting a CS matrix into the magnetic materials using the one-step method. The synthesized MCSC was employed for the sequestration of noxious Cu (II), Ni (II), and Pb (II) ions from water. The isoelectric point (pHIEP) of the prepared MCSC was determined to be about 8.0. Since each HMs showed comparable sorption behaviour, the impact of pH on Cu (II) was evaluated as a model. A significant increase in the percentage of Cu (II) removed was noticed as the solution pH was increased from pH 2, with a maximum percentage of Cu (II) removed noticed at pH 7. Low removal at pH lower than 3 was ascribed to the CS solubilization in an acidic medium. The sorption process of individual HMs was best depicted using the LNR and the PSO models, with maximum sorption capacities of 220.9 (Pb (II)), 216.8 (Cu (II)), and 108.9 (Ni (II)) mg.g-1, respectively. Based on the experimental results from existing and reviewed studies, BNCs were found to be promising nanosorbents for the confiscation of HMs and dye ions. A listing of BNMs was utilized in the biosorption of various HMs and dyes with their optimum pH, IST, and KNT models, and TMD parameters best depicting the interaction between the sorbates and BNCs and values of determined sorption capacity are summarized in Table 3.Table 3
A description of several experimental conditions for HM and dye confiscation, including optimum pH, IST and KNT models, TMDs, and sorption capacity of several BNMs.
BNCsHMIOptimum pHMaximum sorption capacity (mg·g-1 expect stated)IST/KNT modelsTMDs (∆H°and∆G°-kJ·mol−1)ReferencesMagnetic layered double hydroxide/guar gum BNCsCd (II)10258LNR and PSO—[85]CS-lignin-titania NCsBB dye5.815.8FL and PSO—[84]Biodegradable hydrogel based on starch immobilized humic acidMB and Pb (II)4.0-9.0 and 4.0-6.0110 and 58LNR and PSOSpontaneous and exothermal[86]Nickel sulphide incorporated polyacrylamide grafted gum karaya BNC hydrogelR-6G7.01244.71LNR and PSOSpontaneous and endothermic[87]CS-montmorillonite/polyaniline NCsMB—111Temkin and PSO—[88]CS and gum arabic NPsCu (II)10303/344.8LNR and PSO—[89]Alumina/CS (AlCS) compositeCr (VI)3.08.62D-R/PSO and intraparticle diffusionSpontaneous, endothermic, and randomness[90]Magnetic CLL/GOMB6.070.03LNR and PSOSpontaneous, exothermic, and favourable[91]CS/Ag BNCsCu (II), Pb (II), and Cd (VI)5.5-6.597, 88, and 89%——[92]Zn-based magnetic zeolitic imidazolate framework BNCs using basil seed mucilageMB and Eriochrome Black T10 and 2.09.09 and 13.21FL/Elovich and PSOSpontaneous and endothermic[93]Partially hydrolysed polyacrylamide/CLL nanocrystal NC hydrogelsMB6.5358.42LNR and PSO—[94]Carboxylated CLL filtersMB and Pb (II)6.076.92 and 81.30LNR—[95]BNCs of eggshell/Ag-FeAs (V), Pb (II), and Hg (II)—17.7, 27.8, and 15.9FL, Sip, and Redlich-Peterson/Elovich, PSO, and Elovich—[96]S. cerevisiae-AgNP BNCsPb (II), Cu (II), Hg (II), Zn (II), Mn (II), Ni (II), Cr (VI), and As (V)6.0-Cu (II)91.75, 43.58, 19.72, 22.56, 12.47, 6.25, and 9.65%LNR and PSO for Cu (II)—[97]Cationic CLL hydrogels cross-linked by poly(ethylene glycol)Anionic dyes (AR13, AB92, and AR112)2.0440, 462, and 329LNR and PSO—[98]Polyaniline/carboxymethyl CLL/TiO2 NCsCR2.694.3LNR, Hill, Sips, Redlich-Peterson, Khan, Toth, and Koble-Corrigan/PSOSpontaneous and endothermic[75]BPs (CS)/nanoclay compositesCu (II) and Ni (II)—176 and 144——[99]Cationic starch/Na-montmorillonite BNCsAcid scarlet dye7.443.7Sips and PSO—[100]Gum ghatti and acrylic acid-based biodegradable hydrogelsMB and RhB7.0909.09 and 819.67LNR and PSO—[101]l-Methionine montmorillonite encapsulated guar gum-g-polyacrylonitrile copolymer hybrid NCsPb (II) and Cu (II)5.0125 and 90.91LNR and PSOSpontaneous, endothermic, and randomness[69]Hydrolysed polyacrylamide grafted xanthan gum and incorporated nanosilica NCsMB and MV497.5 and 378.8LNR and PSOSpontaneous, endothermic, and randomness[74]Chitin BNCs obtained from carb shellsPb (II), Cu (II), Ni (II), Cd (II), and Zn (II)10142, 166.6, 138.8, 100, and 142.85FL and Temkin and PSOSpontaneous and endothermic[102]CS-based nanocomposite containing mesoporous nanosilica MCM-41Pb (II)6.0125.85LNR and PSO—[103]Magnetic layered double hydroxide/guar gum polymer BNCsCr (VI)6.0101LNR and PSO—[104]CS/Mg-Al-layered double hydroxide NCsPb (II) and Cd (II)3.0333.3 and 140.8LNR and PSO—[105]Hybrid BNCs from CLL nanowhisker and Mg/Al-CO3-LDHCationic dyes (MB, MG, CV, JG, Fuc, and CR dyes)1321-27PSO—[106]CS coated iron-oxide NCsAs (III)6.0267.2FL and PSO—[72]Hybrid BNCs from CLL and clayDrimarine yellow HF-3GL direct dye2.048.9691 and 46.7548Redlich-Peterson and PSOSpontaneous and endothermic[107]Functionalised mesoporous KCC-1 and CS-oleic acidPb (II)9.068LNR and PSOSpontaneous, endothermic, and randomness[108]CS-coated bentoniteAs (V)—1.47LNR and PSONonspontaneous, endothermic, and randomness[109]Fe2O3-CS-cherry kernel shell pyrolytic charcoal composite beadsCr (VI)2.047.576LNR and PSOSpontaneous and endothermic[77]Starch-graft-acrylic acid/montmorillonite superabsorbent NC hydrogelsPb (II) and Cu (II)4.0—FL and PSO—[110]Xanthan gum/n-acetyl cysteine modified mica BNCsPb (II), Cu (II), and Ni (II)4.5 and 4.0530.54, 177.2, and 51.48LNR and PSOSpontaneous, endothermic, and with enhanced randomness[59]CS/polyvinyl alcohol/talc composite (CSPTC)CR, MO, Pb (II), and Cr (VI)87%, 74%, and 380 and 200 mg/g—LNR/PSO—[111]Magnetic CS/GO compositePb (II)5.0112.35LNR/PSO—[112]Goethite/GO/CS NCsAs (III)3.0289.42FL and Sips and PSOSpontaneous and endothermic[113]CSGOAs (III)7.345LNR and PSOSpontaneous and exothermic[114]Fe@polyethyleneimineAs(III)5.00.002μg/L——[115]


## 3. Factors Affecting Sorption of HMs and Dyes Using BNCs

To bind HM to diverse sorbents, ion exchange, complexation, coordination, microprecipitation, chelation, mechanism combination, and electrostatic interaction are all used. The sorption conditions like temperature, pH, sorbent dosage, sorption system types, and volume treated, sorbent physicochemical features like chemical and textural functionality, and sorbate qualities are all taken into account when determining the mechanism of sorption [26]. The pH, temperature, and coexisting are the most important parameters for the sorption of contaminants, and this has an impact on the efficacy of NMs for contaminants removal [58].


### 3.1. pH Impact on the Sorption of HM and Dyes to BNCs

The optimum pH selection is important in sorption studies [49]. In the process of sorption in a water-soluble medium, an important variable and a controlling factor are the medium pH [59]. An effective parameter for sorption, the solubility of contaminants in solution, sorbent functional group activity, and ionic competition are the pH [60].During the sorption process, it changes the charges on the sorbent’s surface, the degree of ionization, and the sorbate speciation, hence leading to the interaction between pollutants and NMs [54, 61]. The value of pH indicates the H+ level of concentration in water, and electrostatic interaction and ion exchange are considerably affected by the concentration of H+ [58]. The adjustment of the pHpzc of the sorbents by the surface modification improves the electrostatic interactions between the sorbent surface and contaminants. Remarkably, the sorbent has a positive and negative charge when the pH is less than pHpzc and more than pHpzc [61, 62]. It was observed in this study that the sorption of MB to starch-g-PAAc/CNW nanocomposites (NCs) under varying solution pH was due to the variation in the electrostatic attraction and the dipolar interaction between the sorbent and sorbed molecules as depicted in Figure 16. At low pH values, there was competition for the sorption sites on the sorbent between the surplus protons (H+) and the MB cationic groups. Also, at these pH values, there was a suppression of the ionization of the carboxyl groups, which reduced the electrostatic interaction between the MB dye molecules and the sorbent. An increase in the sorption capacity was also observed as the pH value was increased from pH 2-5. As noticed, as the pH preconditions close to the pKa of carboxyl groups, there was an increase in the negative charge density within the hydrogel/hydrogel NC matrixes leading to improved sorption capacity. The optimum sorption capacity of MB to the NCs was determined to be at pH 5, as a subsequent increase in the solution pH (>pH 5) did not substantially enhance the sorption capacity [52].Figure 16
Sorption of MB to hydrogel NCs at various pH [52].For the removal of Cr (VI), a novel CS-g-PMMA/silica BP-based hybrid NC manufactured using an emulsifier-free emulsion polymerization approach was used. As the solution pH was adjusted from pH 1 to 4/5, greater Cr (VI) removal was seen, with optimum Cr (VI) removal observed at pH 4 using these NCs. The ionization of functional groups on the chelating surfaces of the sorbent, which involves the competitive reactions of protonation and complex binding, resulted in enhanced Cr (VI) removal at higher pH. The reduced sorption of the sorbate to the sorbent at lower pH (acidic medium) was owing to a significant quantity of hydrogen ions competing with Cr (VI) ions for active sites on the sorbent surface [32].In the study by Abdel-Halim [54], it was observed that the optimum percentage of dye removal (95.65%) was obtained at pH 1 as depicted in Figure 17. As the pH was increased to higher pH, the percentage of dye removed decreased to 0% at pH 10. The improvement and decrease in the percentage of dye sequestered in the sturdy acidic and alkaline mediums were ascribed to the sorbent surface charge owing to the amino group involved in its structure protonation. The ion exchange mechanism was suggestive of the hydrogel amino protonation in the first phase, while in the second phase was due to the anionic dye molecules from the negative centre bonding to the protonated amino groups. The high concentration of OH groups at pH 10 led to no protonation of the amino groups, hence leading to the nonavailability of ion exchange sites to attract the negatively charged dye anions.Figure 17
Impact of sorbate pH on the sorption of anionic dye [54].The percentage removal of MI to grafted crosslinked chitosan beads was shown to be lower at lower pH levels, owing to the protonation of the CS amine group, which causes an electrical repulsion between the MI and the amine group on the chitosan. The surface of the beads becomes deprotonated and negatively charged as the pH rises. As a result, the elimination of these HMI was increased until an optimum value (pH 5-Pb (II) and Cu (II), pH 6-Zn (II) and Cd (II), and pH 7-Ni (II)) is reached. The insoluble metal hydroxide begins to precipitate from the solution above the optimum value of removal, resulting in a reduction in MI removal (Figure18) [63].Figure 18
pH impact on the sequestration of HMI by BNCs [63].The pH was reported in this study to influence the sorption of several cationic dyes using a biodegradable magnetic composite microsphere (MCM). It was observed that the sorption capacities for the three dyes were enhanced with varying in the solution pH from 2 to 10, with a rapid increase at pH 4.5. With the subsequent increase in the solution pH above 5, the uptake of dyes was slowly enhanced and until a maximum level is attained. Optimum confiscation efficiency for these dyes is attained at a pH range of 5-10. In strong acidic mediums, the protonation of the carboxyl and amino groups in MCM resulted in a positively charged surface on the magnetic MCM, hence resulting in a reduction in the sorption capacities of these cationic dyes at low pH conditions. At elevated pH conditions, the amino and carboxyl groups are deprotonated and the surface charge on the sorbent surface becomes negative. This leads to improved removal of the cationic dyes owing to the interaction between the sorbate and the sorbent electrostatically (Figure19) [64].Figure 19
Impact of solution pH on the uptake of the different cationic dyes employing MCM [64].The effect of pH on anionic dye and HMI sorption was studied using BNCs. The BNCs’ pHPZC was discovered to be 8.2. When the pH was more than pHPZC, sorption favours positively charged sorbates, and when the pH is less than pHPZC, sorption favours negatively charged sorbates. Pb (II), Ni (II), and CR had sorption capacities of 47.98, 42.91, and 40 mg/g observed at pH 5, 4, and 2.1. Reduced competition between H+ and the positively charged MI was one of the reasons for the higher sorption capacity with an increase in pH, while the electrostatic interaction between the positively charged CR solution and the negatively charged sites in the acidic pH resulted in the enhanced sorption capacity [65].Using multiwalled CNTs/CS (MWCNTs/CS) NCs, the effect of solution pH (2-10) on the elimination of Cu (II), Cd (II), Zn (II), and Ni (II) was investigated. Owing to the protons (H+) and the target MI competing for the active sites of the sorbent, confiscation of these MI was shown to be significantly low in the pH ranges of 2-5. Individual MI elimination was also enhanced at higher pH levels, which was attributable to MI hydrolysis (Figure 20) [66].Figure 20
Impact of solution pH on the sorption of HMI to MWCNTs/CS NCs [66].pH was observed in the study by Kazemi and Javanbakht [60] to influence the sorption of MB to the BNCs. As shown in Figure 21, it was noticed that enhanced solution pH led to improvement in the percentage of MB removed to the BNCs, with optimum removal noticed at pH 11. At low pH, reduced removal was due to competition between the hydronium ion and MB for the negative charged functional groups on the surface of the sorbent. With an increase in pH, more ligands were freed and the negative charge generated caused the sorption of dye molecules to the surface of the sorbent. In detail, the general sorption of most HMI and dyes utilizing BNCs was observed to be in the pH range of 2-10 in the research publications examined, as presented in Table 3.Figure 21
Impact of pH on the sorption of MB to BNCs [60].


### 3.2. Impact of Time of Contact

The contact period between the NPs and various pollutants has a significant impact on the rate of removal throughout the sorption and redox processes. Various KNT models are used to investigate the effects of contact duration, and the rate of sorption of various pollutants to NMs rapidly reaches its highest point in the early stages before gradually slowing down till equilibrium is reached [67].The sorption rate of MB onto various hydrogel composite was noticed to be swift during the first 15 min and a subsequent marginal increase in the sorption capacity with a reduced rate attaining equilibrium at about 60 min as depicted in Figure22. The distinctive sorption rate at the start subsequently ascribed to the accessibility and availability of sorption sites in the hydrogels. At the start of the sorption experiments, most sorption sites were available for molecules of MB interaction and hence the rapid rate of sorption. With longer contact time, the sorption sites become filled and the sorption rate is slowly reduced reaching a continuous value (dynamic equilibrium). Hence, the sorptive capacities of the hydrogels were saturated after 60 min and the time was deemed as perfect [52].Figure 22
Impact of contact time on the sorption of MB onto various hydrogels [52].The impact of time of contact on the sorption of Pb (II), Ni (II), and Co (II) to hydroxyapatite/CS composite was explored at an initial metal concentration of 10 mg/L at a time of contact of 5-60 min in this study. Optimum confiscation efficiency was noticed within 5 min of time of contact, and thereafter, the rate of confiscation became slow. No further change was noticed after 30 min for Pb (II) (93.5%) and 40 min for Ni (II) (80%) and Co (II) (88.72%). Equilibrium was established at this point (Figure23) [68].Figure 23
Impact of time of contact on Ni (II), Pb (II), and Co (II) to hydroxyapatite/CS composite [68].The sorption of Pb (II) and Cu (II) to BNCs was rapid within the first 150 minutes due to the abundance of active sites on the sorbent surface. As a result of the reduced active sites on the sorbent surface, the sorption of these HMI became slow after 150 min and no further change was detected. At 150 min, the determined sorption capacity for Pb (II) and Cu (II) was 32.65 and 25.74 mg/g, respectively [69]. Swift sorption of various HMI onto BNCs was noticed within the first 30, 45, and 55 min. An additional variation was not detected after the preliminary phase of the sorption process and with equilibrium attained subsequently. These phenomena were due to the abundant and well-supported available sites for binding of HMI and the binding sites been coated with HMI stemming in the repulsion of the HMI from the surface of the sorbent with time [63]. With an increase in the time of contact, the sorption capacities were noticed to increase. At 60 min of sorption process time of contact, the sorption capacities of MB were 87.9, 109.9, and 126.5 mg/g at MB initial concentrations of 100, 120, and 140 mg/L. With a further increase in the time of contact above 60 min, there was a slight change in the sorption capacity, and hence, 60 min time of contact was selected as the optimum time of contact (Figure 24) [70].Figure 24
Impact of time of contact on the sorption of MB to porous CLL-derived carbon/montmorillonite NCs [70].It was observed in this study that the rate of sorption for the interaction between Cu (II) and various BNCs at varying times of contact (0-90 min) was swift within the initial 45 min and with 96.4, 132.3, and 156.9 mg of Cu (II) sorbed per gram of CS/clay, CS/AuNP-clay, and CS/Ag/clay. Sorption equilibrium was attained at 60 min with 134.5, 174.1, and 181.5 mg of Cu (II) sorbed per gram of the Cs/clay, CS/AuNP-clay, and CS/Ag/clay. Owing to the quick diffusion of Cu (II) from the solution to the external surfaces of the various BNCs, there was a swift removal of Cu (II), while the slow rate of sorption was ascribed to the long diffusion range of Cu (II) into the CS/clay inner sphere or the exchange of ions in the CS/AuNP-clay and CS/Ag/clay inner surface (Figure25) [71].Figure 25
Impact of time of contact on the sorption of Cu (II) to various sorbents [71].The removal of As (III) with varied contact times revealed rapid sorption within the first 15 minutes, with only minor increments for the remainder of the sorption period up to 60 minutes. The fast sorption that occurs during the first 30 minutes leads sorption sites to become saturated, resulting in an accumulation of As (III) on the surface of CS@iron oxide (CSIO) NCs that negates the benefit of changing contact duration further. The sorption curves were smooth and continuous, leading to saturation, demonstrating that As (III) could form a monolayer on the surface of BNCs [72].


### 3.3. Impact of Initial Concentration on the Sorption of HMI and Dyes to BNCs

The direct link between the initial sorbate concentration and the accessibility of the sorbing sites on the sorbent surface determines the effect of this factor on the sorption of contaminants. Aggregation of sorbent particles and poor sorption at high concentrations are two major processes that influence sorbate concentration [26].Gupta et al. [68] reported in their study an increase in the sorption capacities of the biosorbent with an increase with the equilibrium concentration, and this increase in the equilibrium MI concentration for these various MI was in the order of Pb (II) > Co (II) > Ni (II) (Figure 26).Figure 26
Impact of equilibrium metal ion concentration on the sorption of MI to biosorbent [68].Initial metal concentrations had a significant impact on their confiscation from aqueous solutions. With an increase in the initial metal concentration from 10 to 150 mg/L, Pb (II) and Cu (II) sorption capacities on the NCs rose from 26.62 and 27.12 mg/g to 209.49 and 195.57 mg/g, respectively. When the initial As3+ concentration was increased from 5 to 100 mg/L, the sorption capacity of As (III) to the NCs rose from 11.50 to 38.24 mg/g. Higher initial metal ion concentrations resulted in higher mass gradient pressures between the aqueous solution and the NCs, which could act as a driving force to overcome mass transfer resistance [73]. It was observed in this study that the sorption of MB onto porous CLL-derived carbon/montmorillonite NCs improved with increasing initial MB concentration and equilibrium attained within 60 min after the gradual increase of the sorption capacity [70].In the study by Kazemi and Javanbakht [60], it was reported that the sorption capacity of MB to the BNCs increased with increasing dye concentration due to the mass transfer momentum force which is enhanced with an improved initial concentration of the solution as shown in Figure 27.Figure 27
Impact of initial concentration on the sequestration of MB to BNCs [60].Ghorai et al. [74] report in their study a decrease in the number of dye molecules removed (99.4-81.5%-MB and 99.1-87.7%-MV) as the initial dye concentration was improved from 400 to 700 and 350 to 650 ppm. At low initial dye concentration, the optimum numbers of molecules of dyes were sorb on the surface of sorbent guaranteeing an elevated sorption percentage, while the high concentration of dye molecules results in a lesser option percentage due to the saturation of the active sorption sites. The determined sorption capacity at concentrations of 400 and 350 mg/L for MB and MV was 497.5 and 378.8 mg/g at pH values of 8 and 9 and time of contact of 20 and 15 min. It was observed in this study that the level As (III) uptake with an increase in the initial MI concentration was influenced by the driving force of the concentration gradient of the solvated MI, while the reduction in the rate of As (III) uptake with improving sorbate concentration was attributed to the sorption site saturation, as a static number of sites on the sorbent sorb of a specific number of the sorbate. Also, an increase in the net active sites is relatively more at lower levels of As (III) concentration leading to enhanced As (III) sorption, and at higher As (III) concentrations, restricted accessibility of the sorption sites contributes to the decreased sorption of As (III) (Figure 28) [72].Figure 28
The impact of initial MI concentration on the sorption process [72].


### 3.4. Impact of Sorbent Dosage

One of the key factors influencing the sorption process operational cost is the sorbent dosage [75]. The dosage of NMs has a significant impact on the pollutants’ ability to be confiscated. In most publications, the appropriate dosage of the sorbent is chosen to achieve expected removal efficiency, which is important for the cost-effective deployment of NMs [67]. Because it governs the equilibrium between the sorbent and the sorbate, as well as the sorption cost for a single unit of a water-soluble solution, the amount of sorbent used in the sequestration of pollutants is extremely important. The number of contaminants sorbed tends to increase with improved sorbent dosage until equilibrium is achieved and it becomes constant. This rise in the number of contaminants sorbed with increasing sorbent dosage was owing to the enhanced quantity of active sites and also the superior surface area of the sorbent [76].Utilizing a hydrogel sorbent dosage of 0.5-5 g/L to treat the anion dye, it was noticed that the percentage of dye molecules removed increased from 31.2% using 0.5 g/L of sorbent to 100% using 2.5 g/L. Increasing the sorbent dosage above 2.5 g/L, the percentage of dye removed remained constant. The improvement in the percentage of dye removed with an increase in sorbent dosage was ascribed to the superior available sorbent exchangeable sites, and the levelling of the sorption dosage was also ascribed to the complete enervation of the dye upon employing 2.5 g/L dosage of the sorbent [54].In this study, the impact of sorbent dosage on the confiscation of Cr (VI) to the NCs was explored at various NC dosages ranging from 0.25 to 1.5 g/L and it was noticed the confiscation efficiency was enhanced with dosage increase and this remained unaffected when an optimum level of dosage was attained (Figure29). This was ascribed to the fact that an increase in the mass of sorbent enhanced the sorption site availability, hence improving the Cr (VI) removal. The sorption capacity was also observed to be impacted negatively by the intensification of the sorbent dosage, as the sorption capacity of the sorbent is inversely proportional to the sorbent mass (Figure 29). Hence, at enhanced dosage, lesser active sorption sites are used which result in a reduced ratio of sorbed ions to the mass of sorbent and thereby lowering the sorption capacity of the sorbent [49].Figure 29
Sorbent mass impact on the sorption of Cr (VI) [49].In this investigation, there was a significant rise in the percentage of HMI eliminated using bionanosorbent when the sorbent dose was increased from 2 to 6 g/L, with a further shift in the removal percentage when the sorbent dose was increased above 6 g/L. This was attributed to the development of equilibrium between the HMI sorbed into the sorbent and the residue unadsorbed in the mixture due to adequate binding sites for metal complexation and increasing the sorbent dose over 6 g/L [63].An increase in the sorption of MI was improved from 78 to 93.5% for Pb (II), 71 to 86% for Co (II), and 64 to 77% for Ni (II) as the sorbent dosage was improved from 1 to 3 g/L in this study. This was ascribed to enhanced surface area and accessible sorption sites at elevated sorbent dosage causing higher sequestration of various MI. A further improvement in the sorbent dosage, no significant improvement in the sequestration of these MI was noticed due to the MI concentration approaching equilibrium status between the solution phase and the solid (Figure30) [68].Figure 30
Impact of sorbent dosage on the sequestration of HMI to biosorbent [68].Altun and Ecevit reported an enhancement in the removal percentage of Cr (VI) ions as the nanosorbent dosage was increased, and the quantity of the substance held per unit sorbent dosage (qe) diminished. The increase in the percentage removal of Cr (VI) was due to the improvement in the number of active sites on the surface of the sorbent. With a further increase in the sorbent dosage, a decrease in the number of substances retained per unit sorbent mass was observed owing to the number of sorbates per sorbent particle [77].As observed in the study by Tanzifi et al. [75], where the impact of sorbent dosage range of 0.02-0.2 g was tested on the confiscation of dye molecules, it was noticed that the sorption efficiency of the biosorbent improved for the dye molecule removal with an increase in the sorbent dosage (0.02-0.08 g) used and with optimum sorption efficiency of 96% attained. A subsequent increase in the sorbent dosage to 0.14 g, a maximum sorption efficiency of 97.03% was reached as shown in Figure 31.Figure 31
Impact of sorbent dosage on the sorption of dye molecules [75].In the study by Wang et al., it was reported that an increase in the dosage of the BNCs resulted in a 78.3% increase in the removal of Pb (II) and a 63% increase in the removal of Cu (II). The availability of additional sorption sites and increased surface area with increasing BNC dosage resulted in better elimination of these MI [78].


## 3.1. pH Impact on the Sorption of HM and Dyes to BNCs

The optimum pH selection is important in sorption studies [49]. In the process of sorption in a water-soluble medium, an important variable and a controlling factor are the medium pH [59]. An effective parameter for sorption, the solubility of contaminants in solution, sorbent functional group activity, and ionic competition are the pH [60].During the sorption process, it changes the charges on the sorbent’s surface, the degree of ionization, and the sorbate speciation, hence leading to the interaction between pollutants and NMs [54, 61]. The value of pH indicates the H+ level of concentration in water, and electrostatic interaction and ion exchange are considerably affected by the concentration of H+ [58]. The adjustment of the pHpzc of the sorbents by the surface modification improves the electrostatic interactions between the sorbent surface and contaminants. Remarkably, the sorbent has a positive and negative charge when the pH is less than pHpzc and more than pHpzc [61, 62]. It was observed in this study that the sorption of MB to starch-g-PAAc/CNW nanocomposites (NCs) under varying solution pH was due to the variation in the electrostatic attraction and the dipolar interaction between the sorbent and sorbed molecules as depicted in Figure 16. At low pH values, there was competition for the sorption sites on the sorbent between the surplus protons (H+) and the MB cationic groups. Also, at these pH values, there was a suppression of the ionization of the carboxyl groups, which reduced the electrostatic interaction between the MB dye molecules and the sorbent. An increase in the sorption capacity was also observed as the pH value was increased from pH 2-5. As noticed, as the pH preconditions close to the pKa of carboxyl groups, there was an increase in the negative charge density within the hydrogel/hydrogel NC matrixes leading to improved sorption capacity. The optimum sorption capacity of MB to the NCs was determined to be at pH 5, as a subsequent increase in the solution pH (>pH 5) did not substantially enhance the sorption capacity [52].Figure 16
Sorption of MB to hydrogel NCs at various pH [52].For the removal of Cr (VI), a novel CS-g-PMMA/silica BP-based hybrid NC manufactured using an emulsifier-free emulsion polymerization approach was used. As the solution pH was adjusted from pH 1 to 4/5, greater Cr (VI) removal was seen, with optimum Cr (VI) removal observed at pH 4 using these NCs. The ionization of functional groups on the chelating surfaces of the sorbent, which involves the competitive reactions of protonation and complex binding, resulted in enhanced Cr (VI) removal at higher pH. The reduced sorption of the sorbate to the sorbent at lower pH (acidic medium) was owing to a significant quantity of hydrogen ions competing with Cr (VI) ions for active sites on the sorbent surface [32].In the study by Abdel-Halim [54], it was observed that the optimum percentage of dye removal (95.65%) was obtained at pH 1 as depicted in Figure 17. As the pH was increased to higher pH, the percentage of dye removed decreased to 0% at pH 10. The improvement and decrease in the percentage of dye sequestered in the sturdy acidic and alkaline mediums were ascribed to the sorbent surface charge owing to the amino group involved in its structure protonation. The ion exchange mechanism was suggestive of the hydrogel amino protonation in the first phase, while in the second phase was due to the anionic dye molecules from the negative centre bonding to the protonated amino groups. The high concentration of OH groups at pH 10 led to no protonation of the amino groups, hence leading to the nonavailability of ion exchange sites to attract the negatively charged dye anions.Figure 17
Impact of sorbate pH on the sorption of anionic dye [54].The percentage removal of MI to grafted crosslinked chitosan beads was shown to be lower at lower pH levels, owing to the protonation of the CS amine group, which causes an electrical repulsion between the MI and the amine group on the chitosan. The surface of the beads becomes deprotonated and negatively charged as the pH rises. As a result, the elimination of these HMI was increased until an optimum value (pH 5-Pb (II) and Cu (II), pH 6-Zn (II) and Cd (II), and pH 7-Ni (II)) is reached. The insoluble metal hydroxide begins to precipitate from the solution above the optimum value of removal, resulting in a reduction in MI removal (Figure18) [63].Figure 18
pH impact on the sequestration of HMI by BNCs [63].The pH was reported in this study to influence the sorption of several cationic dyes using a biodegradable magnetic composite microsphere (MCM). It was observed that the sorption capacities for the three dyes were enhanced with varying in the solution pH from 2 to 10, with a rapid increase at pH 4.5. With the subsequent increase in the solution pH above 5, the uptake of dyes was slowly enhanced and until a maximum level is attained. Optimum confiscation efficiency for these dyes is attained at a pH range of 5-10. In strong acidic mediums, the protonation of the carboxyl and amino groups in MCM resulted in a positively charged surface on the magnetic MCM, hence resulting in a reduction in the sorption capacities of these cationic dyes at low pH conditions. At elevated pH conditions, the amino and carboxyl groups are deprotonated and the surface charge on the sorbent surface becomes negative. This leads to improved removal of the cationic dyes owing to the interaction between the sorbate and the sorbent electrostatically (Figure19) [64].Figure 19
Impact of solution pH on the uptake of the different cationic dyes employing MCM [64].The effect of pH on anionic dye and HMI sorption was studied using BNCs. The BNCs’ pHPZC was discovered to be 8.2. When the pH was more than pHPZC, sorption favours positively charged sorbates, and when the pH is less than pHPZC, sorption favours negatively charged sorbates. Pb (II), Ni (II), and CR had sorption capacities of 47.98, 42.91, and 40 mg/g observed at pH 5, 4, and 2.1. Reduced competition between H+ and the positively charged MI was one of the reasons for the higher sorption capacity with an increase in pH, while the electrostatic interaction between the positively charged CR solution and the negatively charged sites in the acidic pH resulted in the enhanced sorption capacity [65].Using multiwalled CNTs/CS (MWCNTs/CS) NCs, the effect of solution pH (2-10) on the elimination of Cu (II), Cd (II), Zn (II), and Ni (II) was investigated. Owing to the protons (H+) and the target MI competing for the active sites of the sorbent, confiscation of these MI was shown to be significantly low in the pH ranges of 2-5. Individual MI elimination was also enhanced at higher pH levels, which was attributable to MI hydrolysis (Figure 20) [66].Figure 20
Impact of solution pH on the sorption of HMI to MWCNTs/CS NCs [66].pH was observed in the study by Kazemi and Javanbakht [60] to influence the sorption of MB to the BNCs. As shown in Figure 21, it was noticed that enhanced solution pH led to improvement in the percentage of MB removed to the BNCs, with optimum removal noticed at pH 11. At low pH, reduced removal was due to competition between the hydronium ion and MB for the negative charged functional groups on the surface of the sorbent. With an increase in pH, more ligands were freed and the negative charge generated caused the sorption of dye molecules to the surface of the sorbent. In detail, the general sorption of most HMI and dyes utilizing BNCs was observed to be in the pH range of 2-10 in the research publications examined, as presented in Table 3.Figure 21
Impact of pH on the sorption of MB to BNCs [60].


## 3.2. Impact of Time of Contact

The contact period between the NPs and various pollutants has a significant impact on the rate of removal throughout the sorption and redox processes. Various KNT models are used to investigate the effects of contact duration, and the rate of sorption of various pollutants to NMs rapidly reaches its highest point in the early stages before gradually slowing down till equilibrium is reached [67].The sorption rate of MB onto various hydrogel composite was noticed to be swift during the first 15 min and a subsequent marginal increase in the sorption capacity with a reduced rate attaining equilibrium at about 60 min as depicted in Figure22. The distinctive sorption rate at the start subsequently ascribed to the accessibility and availability of sorption sites in the hydrogels. At the start of the sorption experiments, most sorption sites were available for molecules of MB interaction and hence the rapid rate of sorption. With longer contact time, the sorption sites become filled and the sorption rate is slowly reduced reaching a continuous value (dynamic equilibrium). Hence, the sorptive capacities of the hydrogels were saturated after 60 min and the time was deemed as perfect [52].Figure 22
Impact of contact time on the sorption of MB onto various hydrogels [52].The impact of time of contact on the sorption of Pb (II), Ni (II), and Co (II) to hydroxyapatite/CS composite was explored at an initial metal concentration of 10 mg/L at a time of contact of 5-60 min in this study. Optimum confiscation efficiency was noticed within 5 min of time of contact, and thereafter, the rate of confiscation became slow. No further change was noticed after 30 min for Pb (II) (93.5%) and 40 min for Ni (II) (80%) and Co (II) (88.72%). Equilibrium was established at this point (Figure23) [68].Figure 23
Impact of time of contact on Ni (II), Pb (II), and Co (II) to hydroxyapatite/CS composite [68].The sorption of Pb (II) and Cu (II) to BNCs was rapid within the first 150 minutes due to the abundance of active sites on the sorbent surface. As a result of the reduced active sites on the sorbent surface, the sorption of these HMI became slow after 150 min and no further change was detected. At 150 min, the determined sorption capacity for Pb (II) and Cu (II) was 32.65 and 25.74 mg/g, respectively [69]. Swift sorption of various HMI onto BNCs was noticed within the first 30, 45, and 55 min. An additional variation was not detected after the preliminary phase of the sorption process and with equilibrium attained subsequently. These phenomena were due to the abundant and well-supported available sites for binding of HMI and the binding sites been coated with HMI stemming in the repulsion of the HMI from the surface of the sorbent with time [63]. With an increase in the time of contact, the sorption capacities were noticed to increase. At 60 min of sorption process time of contact, the sorption capacities of MB were 87.9, 109.9, and 126.5 mg/g at MB initial concentrations of 100, 120, and 140 mg/L. With a further increase in the time of contact above 60 min, there was a slight change in the sorption capacity, and hence, 60 min time of contact was selected as the optimum time of contact (Figure 24) [70].Figure 24
Impact of time of contact on the sorption of MB to porous CLL-derived carbon/montmorillonite NCs [70].It was observed in this study that the rate of sorption for the interaction between Cu (II) and various BNCs at varying times of contact (0-90 min) was swift within the initial 45 min and with 96.4, 132.3, and 156.9 mg of Cu (II) sorbed per gram of CS/clay, CS/AuNP-clay, and CS/Ag/clay. Sorption equilibrium was attained at 60 min with 134.5, 174.1, and 181.5 mg of Cu (II) sorbed per gram of the Cs/clay, CS/AuNP-clay, and CS/Ag/clay. Owing to the quick diffusion of Cu (II) from the solution to the external surfaces of the various BNCs, there was a swift removal of Cu (II), while the slow rate of sorption was ascribed to the long diffusion range of Cu (II) into the CS/clay inner sphere or the exchange of ions in the CS/AuNP-clay and CS/Ag/clay inner surface (Figure25) [71].Figure 25
Impact of time of contact on the sorption of Cu (II) to various sorbents [71].The removal of As (III) with varied contact times revealed rapid sorption within the first 15 minutes, with only minor increments for the remainder of the sorption period up to 60 minutes. The fast sorption that occurs during the first 30 minutes leads sorption sites to become saturated, resulting in an accumulation of As (III) on the surface of CS@iron oxide (CSIO) NCs that negates the benefit of changing contact duration further. The sorption curves were smooth and continuous, leading to saturation, demonstrating that As (III) could form a monolayer on the surface of BNCs [72].


## 3.3. Impact of Initial Concentration on the Sorption of HMI and Dyes to BNCs

The direct link between the initial sorbate concentration and the accessibility of the sorbing sites on the sorbent surface determines the effect of this factor on the sorption of contaminants. Aggregation of sorbent particles and poor sorption at high concentrations are two major processes that influence sorbate concentration [26].Gupta et al. [68] reported in their study an increase in the sorption capacities of the biosorbent with an increase with the equilibrium concentration, and this increase in the equilibrium MI concentration for these various MI was in the order of Pb (II) > Co (II) > Ni (II) (Figure 26).Figure 26
Impact of equilibrium metal ion concentration on the sorption of MI to biosorbent [68].Initial metal concentrations had a significant impact on their confiscation from aqueous solutions. With an increase in the initial metal concentration from 10 to 150 mg/L, Pb (II) and Cu (II) sorption capacities on the NCs rose from 26.62 and 27.12 mg/g to 209.49 and 195.57 mg/g, respectively. When the initial As3+ concentration was increased from 5 to 100 mg/L, the sorption capacity of As (III) to the NCs rose from 11.50 to 38.24 mg/g. Higher initial metal ion concentrations resulted in higher mass gradient pressures between the aqueous solution and the NCs, which could act as a driving force to overcome mass transfer resistance [73]. It was observed in this study that the sorption of MB onto porous CLL-derived carbon/montmorillonite NCs improved with increasing initial MB concentration and equilibrium attained within 60 min after the gradual increase of the sorption capacity [70].In the study by Kazemi and Javanbakht [60], it was reported that the sorption capacity of MB to the BNCs increased with increasing dye concentration due to the mass transfer momentum force which is enhanced with an improved initial concentration of the solution as shown in Figure 27.Figure 27
Impact of initial concentration on the sequestration of MB to BNCs [60].Ghorai et al. [74] report in their study a decrease in the number of dye molecules removed (99.4-81.5%-MB and 99.1-87.7%-MV) as the initial dye concentration was improved from 400 to 700 and 350 to 650 ppm. At low initial dye concentration, the optimum numbers of molecules of dyes were sorb on the surface of sorbent guaranteeing an elevated sorption percentage, while the high concentration of dye molecules results in a lesser option percentage due to the saturation of the active sorption sites. The determined sorption capacity at concentrations of 400 and 350 mg/L for MB and MV was 497.5 and 378.8 mg/g at pH values of 8 and 9 and time of contact of 20 and 15 min. It was observed in this study that the level As (III) uptake with an increase in the initial MI concentration was influenced by the driving force of the concentration gradient of the solvated MI, while the reduction in the rate of As (III) uptake with improving sorbate concentration was attributed to the sorption site saturation, as a static number of sites on the sorbent sorb of a specific number of the sorbate. Also, an increase in the net active sites is relatively more at lower levels of As (III) concentration leading to enhanced As (III) sorption, and at higher As (III) concentrations, restricted accessibility of the sorption sites contributes to the decreased sorption of As (III) (Figure 28) [72].Figure 28
The impact of initial MI concentration on the sorption process [72].


## 3.4. Impact of Sorbent Dosage

One of the key factors influencing the sorption process operational cost is the sorbent dosage [75]. The dosage of NMs has a significant impact on the pollutants’ ability to be confiscated. In most publications, the appropriate dosage of the sorbent is chosen to achieve expected removal efficiency, which is important for the cost-effective deployment of NMs [67]. Because it governs the equilibrium between the sorbent and the sorbate, as well as the sorption cost for a single unit of a water-soluble solution, the amount of sorbent used in the sequestration of pollutants is extremely important. The number of contaminants sorbed tends to increase with improved sorbent dosage until equilibrium is achieved and it becomes constant. This rise in the number of contaminants sorbed with increasing sorbent dosage was owing to the enhanced quantity of active sites and also the superior surface area of the sorbent [76].Utilizing a hydrogel sorbent dosage of 0.5-5 g/L to treat the anion dye, it was noticed that the percentage of dye molecules removed increased from 31.2% using 0.5 g/L of sorbent to 100% using 2.5 g/L. Increasing the sorbent dosage above 2.5 g/L, the percentage of dye removed remained constant. The improvement in the percentage of dye removed with an increase in sorbent dosage was ascribed to the superior available sorbent exchangeable sites, and the levelling of the sorption dosage was also ascribed to the complete enervation of the dye upon employing 2.5 g/L dosage of the sorbent [54].In this study, the impact of sorbent dosage on the confiscation of Cr (VI) to the NCs was explored at various NC dosages ranging from 0.25 to 1.5 g/L and it was noticed the confiscation efficiency was enhanced with dosage increase and this remained unaffected when an optimum level of dosage was attained (Figure29). This was ascribed to the fact that an increase in the mass of sorbent enhanced the sorption site availability, hence improving the Cr (VI) removal. The sorption capacity was also observed to be impacted negatively by the intensification of the sorbent dosage, as the sorption capacity of the sorbent is inversely proportional to the sorbent mass (Figure 29). Hence, at enhanced dosage, lesser active sorption sites are used which result in a reduced ratio of sorbed ions to the mass of sorbent and thereby lowering the sorption capacity of the sorbent [49].Figure 29
Sorbent mass impact on the sorption of Cr (VI) [49].In this investigation, there was a significant rise in the percentage of HMI eliminated using bionanosorbent when the sorbent dose was increased from 2 to 6 g/L, with a further shift in the removal percentage when the sorbent dose was increased above 6 g/L. This was attributed to the development of equilibrium between the HMI sorbed into the sorbent and the residue unadsorbed in the mixture due to adequate binding sites for metal complexation and increasing the sorbent dose over 6 g/L [63].An increase in the sorption of MI was improved from 78 to 93.5% for Pb (II), 71 to 86% for Co (II), and 64 to 77% for Ni (II) as the sorbent dosage was improved from 1 to 3 g/L in this study. This was ascribed to enhanced surface area and accessible sorption sites at elevated sorbent dosage causing higher sequestration of various MI. A further improvement in the sorbent dosage, no significant improvement in the sequestration of these MI was noticed due to the MI concentration approaching equilibrium status between the solution phase and the solid (Figure30) [68].Figure 30
Impact of sorbent dosage on the sequestration of HMI to biosorbent [68].Altun and Ecevit reported an enhancement in the removal percentage of Cr (VI) ions as the nanosorbent dosage was increased, and the quantity of the substance held per unit sorbent dosage (qe) diminished. The increase in the percentage removal of Cr (VI) was due to the improvement in the number of active sites on the surface of the sorbent. With a further increase in the sorbent dosage, a decrease in the number of substances retained per unit sorbent mass was observed owing to the number of sorbates per sorbent particle [77].As observed in the study by Tanzifi et al. [75], where the impact of sorbent dosage range of 0.02-0.2 g was tested on the confiscation of dye molecules, it was noticed that the sorption efficiency of the biosorbent improved for the dye molecule removal with an increase in the sorbent dosage (0.02-0.08 g) used and with optimum sorption efficiency of 96% attained. A subsequent increase in the sorbent dosage to 0.14 g, a maximum sorption efficiency of 97.03% was reached as shown in Figure 31.Figure 31
Impact of sorbent dosage on the sorption of dye molecules [75].In the study by Wang et al., it was reported that an increase in the dosage of the BNCs resulted in a 78.3% increase in the removal of Pb (II) and a 63% increase in the removal of Cu (II). The availability of additional sorption sites and increased surface area with increasing BNC dosage resulted in better elimination of these MI [78].


## 4. Isotherm Models, Kinetic Studies, Temperature, and Thermodynamic Studies

### 4.1. Isotherm Models

In equilibrium studies of IST and understanding the KNT of the sorption process, investigations including changing contact time and initial metal concentration are important criteria [72]. The IST is the relationship between the solute equilibrium concentration in the solution and the solute equilibrium concentration in the sorbent at a constant temperature [79].Selecting the ideal IST model for the process of sorption, the following conditions must be satisfied: (i) the IST model and the determined equilibrium data must be a good fit, (ii) the function of the IST must be thermodynamically realistic, and (iii) in ideal situations, analytical calculation of concentration from capacity and the other way around [16]. The sorption equilibrium data in most studies are assessed using the LNR, FL, Temkin, and Dubinin-Radushkevich (D-R) IST models [79].The LNR model, which was created to describe gas-solid phase sorption processes, is frequently employed to calculate the sorption capacity of different sorbents in solutions. The LNR IST is mostly written in the nonlinear and linearized form shown in the following:(1)qe=qmKLCeKLCe+1,Ceqe=1qeCe+1qmKL,whereKL (L/mg) and qm (mg/g) represent the LNR IST constant and the corresponding saturation sorption capacity [80].The earliest far-famed equation which described the sorption technique was the FL model. It is linked with an empirical equation and employed for a nonideal natural process that comprises of heterogeneous surface sorption [81]. On heterogeneous surfaces, the FL model has been employed to exemplify sorption processes. This IST provides useful information on surface heterogeneity, active site exponential distribution, and energetics. The FL IST is generally written in the nonlinear and linearized form shown in the following:
(2)qe=KFCe1/n,lnqm=1nlnCe+lnKF,where KF (mg/g) and 1/n represent the constant of FL IST that is an indicator of sorption capacity and the sorption capacity measurement [82].Sorbate-sorbate interactions are taken into account in the Temkin model. It is assumed that as the surface coverage increases, the heat of sorption of all molecules in the layer reduces linearly rather than logarithmically. The Temkin IST is generally written in the nonlinear and linearized form shown in the following:(3)qm=RTbTlnKTCe,qm=RTbTlnCe+RTbTlnKF,where R (8.314 J·mol−1·K−1), T (K), KT (L·g−1), and bT represent the gas constant, the absolute temperature, the equilibrium binding constant of the Temkin IST, and the heat of sorption (J·mol−1) relating to the Temkin IST constant. The D-R model is a semiempirical equation in which sorption occurs on heterogeneous surfaces via a pore-filling mechanism with Gaussian energy distribution. It has been used to quantitatively describe the sorption of gases on microporous sorbents. The nonlinear and linearized forms of the D-R IST are as follows:
(4)qe=qse−KDRε2,lnqe=lnqs−KDRε2,ε=RTln1+1Ce,where KDR (mol2·kJ−2) and qs (mg/g) are the D-R constant and the theoretical D-R saturation capacity [80].The least-squares approach is the most extensively used method by many studies to best fit the sorption IST. The models are tested for their ability to fit the experimental data with coefficients of determination that are near to unity in magnitude. However, it has the weakness of producing a large number of different outcomes, which radically changes the structure of error, contradicts error variance, and leads to sorption bias according to classic least-squares normalcy theories. In the case of optimum IST selection, nonlinear regression is the optimal method. In comparison to the linear methodology, the nonlinear methodology has the advantage of not changing the error distribution because all of the IST’s parameters are set on the same axis. The linear regression method was utilized to get the best appropriate IST [26]. Table 3 summarizes the best IST models for the confiscation of metal and dye using several BNCs, indicating that the LNR and FL models described the sorption process of various contaminants to BNCs and that these models appear to be the most precise representation of the sorption process.


### 4.2. Kinetic Studies

Various sorption processes occur via a multistep mechanism which includes the dispersion across the liquid film bordering the particle of solid (external mass transfer coefficient controls this process), the dispersion within the individual particles assuming a pore diffusion mechanism (intraparticle diffusion), and the physical and chemical sorption at a sorption site. The transient behaviour of a batch sorption process at various temperatures and initial concentrations of the adsorbate is studied using the Lagergren first-order and the PSO models [83].KNT research was generally employed by several scientists to study the mechanism by which the sorption process takes place. Preexisting models are applied in most sorption KNT research, and this acts as a guide in demonstrating the mechanism of sorption. Among the widely employed models to describe the sorption process are the pseudo-first-order (PFO), PSO, and particle diffusion models. An extensive range of standard models is existing to rationalize the sorption at various conditions, and the most appropriate is chosen for the given experimental conditions [16].Some models of sorption IST and KNT are briefly introduced in this review to better demonstrate the sorption behaviours of the following biomaterials. The determination of KNT is critical for the design of sorption systems as well as the reaction rate control step during the chemical reaction. The number of sorbates adsorbed on the sorbents (qt) and the contact time is described by sorption KNT (t). The PFO and PSO KNT models are extensively applied in sorption KNT. The sorption of liquid-solid phase systems based on the sorption capacity is defined by the PFO model, whereas the PSO model is based on the sorption capacity of the solid phases [6]. The nonlinearized and linearized forms of the PFO and PSO models are generally expressed as follows:
(5)dqtdt=Kqe−qt,logqe−qt=logqe−K12.303t,dqtdt=K2qe−qt2,tqt=1K2qe2+1qet,whereqe (mg/g), qt (mg/g), K and K1, and K2 indicate the equilibrium sorption capacity, the sorption capacity at a contact time t, PFO rate constants, and PSO rate constant [6].The sorption mechanism enhanced by NPs is quick in terms of KNT. As a result, using NPs in the wastewater treatment process opens up a new avenue for NPs use [19]. Table 3 shows the summary of some of the best reported suited KNT models for metal and dye removal using various BNCs, which indicated that the sorption process of BNCs was characteristically followed by the PSO model and this model appears to be the most accurate approximation of the sorption process attributable to chemisorption processes, which are indicative of a rate-limiting phase in the sorption step.


### 4.3. Temperature and Thermodynamic Studies

The basic idea of TMDs was established based on the premise that entropy change is the driving force in a system that is kept isolated, where energy cannot be obtained or lost to the surroundings. Both energy and entropy considerations must be considered in environmental engineering practice to determine which processes will occur spontaneously. The change in entropy (∆s°) and change in enthalpy ∆E° is linked with the process using
(6)lnK=−∆H°RT+∆S°R.The key measure of spontaneity is the change in Gibbs free energy (∆G°), and at a given temperature, reactions happen spontaneously if ∆G° is a negative quantity. Considering the sorption equilibrium constant K, the ∆G° of the sorption reaction is given by
(7)∆G°=−RTlnK,whereK is defined by equation (8). ∆H° and ∆S° are determined from the slope and intercept of the plot of ln K against 1/T [63].
(8)K=qeCe.In this study, experiments were carried out at 298, 303, and 313 K to assess the influence of temperature on HMI sorption by the EDTA-MCS/GO NCs while maintaining all other parameter constant, such as sorbate and sorbent concentrations, pH, and agitation speed. With an initial metal concentration of 50 ppm, the Pb (II) and Cu (II) sorption capacities declined dramatically from 134.82 and 95.91 mg/g to 119.91 and 60.6 mg/g, respectively, as the temperature rose from 298 to 313 K. In contrast, As (III) sorption capacity improved slightly from 11.50 to 11.96 mg/g as the temperature rose from 298 to 313 K. Pb (II) and Cu (II) sorption on the EDTA-MCS/GO NCs were shown to be exothermic processes, while As (III) sorption was shown to be mildly endothermic. As a result, the temperature had a substantial impact on metal ion sorption by the EDTA-MCS/GO NCs [73].The effect of solution temperature on MWCNT/CS NC elimination of Cu (II), Cd (II), Zn (II), and Ni (II) from the aqueous medium was investigated, and the findings are given in Figure32. The four distinct solution temperatures chosen to represent aqueous environment temperatures were 5.0°C (278 K), 15.0°C (288 K), 25.0°C (298 K), and 40.0°C (313 K). It was observed that increasing the temperature of the solution increased the percentage removal of MI from the aqueous medium, showing that the sorption process was endothermic [66].Figure 32
Impact of temperature on the sorption of MI to MWCNTs/CS [66].The impact of varying temperatures on Cu (II) using CS/Ag/clay BNCs was reported in this study. It was noticed the efficiency of Cu (II) removed (sorption capacity) to the BNCs was enhanced with improvement in the temperature applied until equilibrium attained (Figure33). The determined sorption capacity was 239 mg/g at 318 K at a pH of 7 for 60 min employing a dosage of sorbent of 0.3 g/L and a stirring speed of 160 rpm [71].Figure 33
Impact of varying temperature on the varying initial Cu (II) concentration to CS/Ag/clay composite [71].It was noticed that the efficiency of removal of brilliant black (BB) dye using CS-lignin-titania NCs was enhanced with increasing initial dye concentration and attaining equilibrium of 88% using 50 mg/L of the dye solution. An increase in the efficiency of removal of BB with intensifying concentration was attributed to the electrostatic interaction between the free dye molecules, and the sorbent and increase in the mass of BB dyes transfer to the sorbent active sites [84]. It was noticed in this study that the sorption process between the sorbate and the sorbent was endothermic and spontaneous. Intensification in the interaction temperature led to a reduction in ∆G° indicative of suitable sorption of permanganate at elevated temperatures, while a positive value of ∆S° indicated the enhanced possibility of the collision between the sites on the sorbent surface and the sorbate ions [82].


## 4.1. Isotherm Models

In equilibrium studies of IST and understanding the KNT of the sorption process, investigations including changing contact time and initial metal concentration are important criteria [72]. The IST is the relationship between the solute equilibrium concentration in the solution and the solute equilibrium concentration in the sorbent at a constant temperature [79].Selecting the ideal IST model for the process of sorption, the following conditions must be satisfied: (i) the IST model and the determined equilibrium data must be a good fit, (ii) the function of the IST must be thermodynamically realistic, and (iii) in ideal situations, analytical calculation of concentration from capacity and the other way around [16]. The sorption equilibrium data in most studies are assessed using the LNR, FL, Temkin, and Dubinin-Radushkevich (D-R) IST models [79].The LNR model, which was created to describe gas-solid phase sorption processes, is frequently employed to calculate the sorption capacity of different sorbents in solutions. The LNR IST is mostly written in the nonlinear and linearized form shown in the following:(1)qe=qmKLCeKLCe+1,Ceqe=1qeCe+1qmKL,whereKL (L/mg) and qm (mg/g) represent the LNR IST constant and the corresponding saturation sorption capacity [80].The earliest far-famed equation which described the sorption technique was the FL model. It is linked with an empirical equation and employed for a nonideal natural process that comprises of heterogeneous surface sorption [81]. On heterogeneous surfaces, the FL model has been employed to exemplify sorption processes. This IST provides useful information on surface heterogeneity, active site exponential distribution, and energetics. The FL IST is generally written in the nonlinear and linearized form shown in the following:
(2)qe=KFCe1/n,lnqm=1nlnCe+lnKF,where KF (mg/g) and 1/n represent the constant of FL IST that is an indicator of sorption capacity and the sorption capacity measurement [82].Sorbate-sorbate interactions are taken into account in the Temkin model. It is assumed that as the surface coverage increases, the heat of sorption of all molecules in the layer reduces linearly rather than logarithmically. The Temkin IST is generally written in the nonlinear and linearized form shown in the following:(3)qm=RTbTlnKTCe,qm=RTbTlnCe+RTbTlnKF,where R (8.314 J·mol−1·K−1), T (K), KT (L·g−1), and bT represent the gas constant, the absolute temperature, the equilibrium binding constant of the Temkin IST, and the heat of sorption (J·mol−1) relating to the Temkin IST constant. The D-R model is a semiempirical equation in which sorption occurs on heterogeneous surfaces via a pore-filling mechanism with Gaussian energy distribution. It has been used to quantitatively describe the sorption of gases on microporous sorbents. The nonlinear and linearized forms of the D-R IST are as follows:
(4)qe=qse−KDRε2,lnqe=lnqs−KDRε2,ε=RTln1+1Ce,where KDR (mol2·kJ−2) and qs (mg/g) are the D-R constant and the theoretical D-R saturation capacity [80].The least-squares approach is the most extensively used method by many studies to best fit the sorption IST. The models are tested for their ability to fit the experimental data with coefficients of determination that are near to unity in magnitude. However, it has the weakness of producing a large number of different outcomes, which radically changes the structure of error, contradicts error variance, and leads to sorption bias according to classic least-squares normalcy theories. In the case of optimum IST selection, nonlinear regression is the optimal method. In comparison to the linear methodology, the nonlinear methodology has the advantage of not changing the error distribution because all of the IST’s parameters are set on the same axis. The linear regression method was utilized to get the best appropriate IST [26]. Table 3 summarizes the best IST models for the confiscation of metal and dye using several BNCs, indicating that the LNR and FL models described the sorption process of various contaminants to BNCs and that these models appear to be the most precise representation of the sorption process.


## 4.2. Kinetic Studies

Various sorption processes occur via a multistep mechanism which includes the dispersion across the liquid film bordering the particle of solid (external mass transfer coefficient controls this process), the dispersion within the individual particles assuming a pore diffusion mechanism (intraparticle diffusion), and the physical and chemical sorption at a sorption site. The transient behaviour of a batch sorption process at various temperatures and initial concentrations of the adsorbate is studied using the Lagergren first-order and the PSO models [83].KNT research was generally employed by several scientists to study the mechanism by which the sorption process takes place. Preexisting models are applied in most sorption KNT research, and this acts as a guide in demonstrating the mechanism of sorption. Among the widely employed models to describe the sorption process are the pseudo-first-order (PFO), PSO, and particle diffusion models. An extensive range of standard models is existing to rationalize the sorption at various conditions, and the most appropriate is chosen for the given experimental conditions [16].Some models of sorption IST and KNT are briefly introduced in this review to better demonstrate the sorption behaviours of the following biomaterials. The determination of KNT is critical for the design of sorption systems as well as the reaction rate control step during the chemical reaction. The number of sorbates adsorbed on the sorbents (qt) and the contact time is described by sorption KNT (t). The PFO and PSO KNT models are extensively applied in sorption KNT. The sorption of liquid-solid phase systems based on the sorption capacity is defined by the PFO model, whereas the PSO model is based on the sorption capacity of the solid phases [6]. The nonlinearized and linearized forms of the PFO and PSO models are generally expressed as follows:
(5)dqtdt=Kqe−qt,logqe−qt=logqe−K12.303t,dqtdt=K2qe−qt2,tqt=1K2qe2+1qet,whereqe (mg/g), qt (mg/g), K and K1, and K2 indicate the equilibrium sorption capacity, the sorption capacity at a contact time t, PFO rate constants, and PSO rate constant [6].The sorption mechanism enhanced by NPs is quick in terms of KNT. As a result, using NPs in the wastewater treatment process opens up a new avenue for NPs use [19]. Table 3 shows the summary of some of the best reported suited KNT models for metal and dye removal using various BNCs, which indicated that the sorption process of BNCs was characteristically followed by the PSO model and this model appears to be the most accurate approximation of the sorption process attributable to chemisorption processes, which are indicative of a rate-limiting phase in the sorption step.


## 4.3. Temperature and Thermodynamic Studies

The basic idea of TMDs was established based on the premise that entropy change is the driving force in a system that is kept isolated, where energy cannot be obtained or lost to the surroundings. Both energy and entropy considerations must be considered in environmental engineering practice to determine which processes will occur spontaneously. The change in entropy (∆s°) and change in enthalpy ∆E° is linked with the process using
(6)lnK=−∆H°RT+∆S°R.The key measure of spontaneity is the change in Gibbs free energy (∆G°), and at a given temperature, reactions happen spontaneously if ∆G° is a negative quantity. Considering the sorption equilibrium constant K, the ∆G° of the sorption reaction is given by
(7)∆G°=−RTlnK,whereK is defined by equation (8). ∆H° and ∆S° are determined from the slope and intercept of the plot of ln K against 1/T [63].
(8)K=qeCe.In this study, experiments were carried out at 298, 303, and 313 K to assess the influence of temperature on HMI sorption by the EDTA-MCS/GO NCs while maintaining all other parameter constant, such as sorbate and sorbent concentrations, pH, and agitation speed. With an initial metal concentration of 50 ppm, the Pb (II) and Cu (II) sorption capacities declined dramatically from 134.82 and 95.91 mg/g to 119.91 and 60.6 mg/g, respectively, as the temperature rose from 298 to 313 K. In contrast, As (III) sorption capacity improved slightly from 11.50 to 11.96 mg/g as the temperature rose from 298 to 313 K. Pb (II) and Cu (II) sorption on the EDTA-MCS/GO NCs were shown to be exothermic processes, while As (III) sorption was shown to be mildly endothermic. As a result, the temperature had a substantial impact on metal ion sorption by the EDTA-MCS/GO NCs [73].The effect of solution temperature on MWCNT/CS NC elimination of Cu (II), Cd (II), Zn (II), and Ni (II) from the aqueous medium was investigated, and the findings are given in Figure32. The four distinct solution temperatures chosen to represent aqueous environment temperatures were 5.0°C (278 K), 15.0°C (288 K), 25.0°C (298 K), and 40.0°C (313 K). It was observed that increasing the temperature of the solution increased the percentage removal of MI from the aqueous medium, showing that the sorption process was endothermic [66].Figure 32
Impact of temperature on the sorption of MI to MWCNTs/CS [66].The impact of varying temperatures on Cu (II) using CS/Ag/clay BNCs was reported in this study. It was noticed the efficiency of Cu (II) removed (sorption capacity) to the BNCs was enhanced with improvement in the temperature applied until equilibrium attained (Figure33). The determined sorption capacity was 239 mg/g at 318 K at a pH of 7 for 60 min employing a dosage of sorbent of 0.3 g/L and a stirring speed of 160 rpm [71].Figure 33
Impact of varying temperature on the varying initial Cu (II) concentration to CS/Ag/clay composite [71].It was noticed that the efficiency of removal of brilliant black (BB) dye using CS-lignin-titania NCs was enhanced with increasing initial dye concentration and attaining equilibrium of 88% using 50 mg/L of the dye solution. An increase in the efficiency of removal of BB with intensifying concentration was attributed to the electrostatic interaction between the free dye molecules, and the sorbent and increase in the mass of BB dyes transfer to the sorbent active sites [84]. It was noticed in this study that the sorption process between the sorbate and the sorbent was endothermic and spontaneous. Intensification in the interaction temperature led to a reduction in ∆G° indicative of suitable sorption of permanganate at elevated temperatures, while a positive value of ∆S° indicated the enhanced possibility of the collision between the sites on the sorbent surface and the sorbate ions [82].


## 5. Reusability of BNCs for HMI and Dye Confiscation

Any sorbent material used in experimental applications should maintain its stability after many sorption remediations [111]. A sorbent’s sorption and desorption properties are critical for its possible application. To be economically viable and efficient, a sorbent should have high sorption capacity as well as outstanding desorption characteristics [74].In this study, the BNCs employed for the MB dye were regenerated and reutilized for four cycles. The result in Figure34 shows that the BNC sorbent was not reusable and showed the ability to sorb dye molecules after successive sorption cycles [60].Figure 34
Regeneration of BNCs for MB removal [60].To explain the sorption mechanism, desorption experiments were carried out at various pH values of 2, 7, and 10 and the highest percentage of dyes desorb was obtained at pH 2, with a percentage of 95.7 and 49.5 desorb for MB and MV. At the fourth cycle of desorption at pH 2, 85.6 and 83.5% of MB and MV were desorbed; hence, the BNCs depicted an efficient recycling ability for dye treatment [74].High removal capacity was observed in this study notwithstanding five cycles of continual sorption and desorption (Figure35). 87.00% sorption capacity was shown by the CSIO at the fifth cycle, which was relative to their original capacity, and a marginal loss of 13.00% sorptive potential was noticed due to acid-base treatment of the NCs during the process of regeneration [72].Figure 35
The cycle of sorbent regeneration for MI removal [72].In this work, 0.05 M NaOH was employed to regenerate iron-doped electrospun CS nanofiber mat (Fe@Cs) for As (III) sorption and desorption cycles. More than 90.00% of the MI was desorbed from the sorbent surface for individual three cycles (Figure36) [116].Figure 36
Sorption-desorption of Fe@CS for As (III) removal [116].


## 6. Mechanism of HM and Dye Sorption to BNCs

The sorption IST are crucial for the sorption mechanism route optimization, the surface properties and sorbent capacity expression, and the constructive design of the sorption as they describe the sorbent material interrelation with the contaminants. Knowledge of the sorption mechanism, surface features, and the degree of sorbent affinity is provided by the physicochemical factors complemented by the basic TMD theories [117]. The sorbent sorption efficiency can be evaluated employing different parameters such as the number of active sites on the surface of the sorbent, sorbate functional and structural behaviour, sorbent surface characteristics, the process of mass transport, process of pollutant diffusion, and sorbate and sorbent interactions [87].To determine the mechanism of CR sorption to the BNCs, the FTIR spectra of the NCs before and after CR sorption were explored in this study. Hydrogen bonding was observed to exist as hydroxyl, carboxyl, imine, and amine functional groups of the NCs and CR dye functional groups. It was also noticed that the FTIR peaks of real polyaniline (PAN) marginally shifted in the composite, indicative of the effect of TiO2 and carboxymethyl CLL (CMC). Peaks at wavenumbers of 1471 and 1543 cm-1 attributed to C=C benzenoid and C=C quinonoid bonds were noticed to shift in the composite to 1485 and 1570 cm-1 after sorption of molecules of dyes with PAN. Also, it was observed that the FTIR peaks at wavenumbers of 1647 cm-1 in CMC shift to 1658 cm-1 indicative of dye bonding with this group. There was also a minor shift in the peak due to the hydroxyl group relating to water in the sample and CMC indicative of bonding of dye molecules with the OH group of CMCs. The FTIR spectrum of the sorbent in Figure 37 after sorption shows evidence of the presence of the sorbate in the structure of the sorbent. Therefore, molecules of dye made a sturdy bond with the sorbent in chemical sorption, and at low pH, the molecules of dye sorbed onto the surface of the sorbent owing to the electrostatic force between negatively charged pigment and positively charged sorbent surface. Figure 38 depicts the mechanism of CR sorption onto NCs [75].Figure 37
Spectra of PAN/CMC/TiO2 NCs (a) before sorption, (b) after sorption, (c) after desorption, and (d) CR dye [75].Figure 38
Mechanism of CR sorption to NCs [75].In this study, the major mechanism of sorption of MB was attributed to the electrostatic interaction according to the pH studies. At lower pH, there were more protons available, and the amorphous carbon’s surface became C-OH2+. As a result, there was ionic repulsion between the positively charged surface and positively charged MB molecules, reducing the sorption ability. The surface C-OH2+ was converted to C-OH as the pH intensified, and the sorption ability improved without ionic repulsion. When the pH rises over 8, the surface C-OH bonds turn to C-O-, and the electrostatic interaction between positively charged dye ions and negatively charged sorption sites causes an enhanced MB dye sorption. This result showed that, while multipores were prominent in the sorption of MB to sorbent, the sorption ability could be increased by inducing the formation of micropores. The mechanism of MB sorption to the bionanosorbent is depicted in Figure 39 [70].Figure 39
Illustration of MB sorption mechanism to the BNCs [70].In this study, it was reported that extra active sites were provided by the CS-clay NCs for the confiscation of MI comprising of the cation exchange sites and extra surface area. The functional groups in CS were observed to coordinate with Cu (II) ion, with the MI acting as a Lewis acid receiving electron sets from the hydroxyl and amino groups of CS (Lewis base). As noticed in Figure40, some of the Cu (II) ions also usurp clay’s interlayer cations and this cooperative effect significantly improves the sorption performance of the CS-clay sorbent [71].Figure 40
Mechanism of Cu (II) sorption to CS/clay NCs [71].In the sorption of R-6G to the BNC hydrogel, the cationic dye was swiftly sorbed to the negative charge BNC surface due to van der Waals forces, hydrogen bonding, and electrostatic interactions. From the FTIR result, the characteristic peaks of the dye-loaded BNC hydrogel were broadened and shifted marginally when compared to the pure BNCs. The -OH/-NH stretching vibration, COO- stretching vibration, amide stretching vibration, COO- asymmetric stretching vibration, -NH in-plane bending vibration, and amide -C-N stretching vibration were observed to shift marginally from 3349 to 3362, 1710 to 1716, 1658 to 1651, 1565 to 1590, 1455 to 1456, and 1232 to 1218 cm-1. A new peak was noticed at 1153 cm-1 after sorption which was attributed to -COC- of R-6G and indicative of the bonding of dye molecules to the BNC hydrogel. These changes observed signify electrostatic and hydrogen bonding interaction between the functional groups of the sorbate and sorbent as shown in Figure 41 [87].Figure 41
Mechanism of sorption of R-6G to BNC hydrogel [87].The mechanism of sorption of dye molecules to the BNCs from FTIR result was due to specific electrostatic and H-bonding interactions between the cationic dye active sites and the silanol-OH and polysaccharide-OH groups, amide carbonyl groups, and COO groups of the BNCs as depicted in Figure42. The sorption mechanism can also be elucidated by the successive process of dye diffusion consisting of bulk diffusion, intraparticle diffusion, and surface sorption [74].Figure 42
Mechanism of sorption of (a) MB and (b) MV [74].
(a)(b)In this study, surface complexation between the surface functional groups (-NH2, -OH, and -OH2) of the CSGO and the H3AsO30 was reported to be the dominant mechanism of sorption of As (III) to CSGO NCs from the impact of pH, pHPZC, and FTIR study. A characteristic example of outer-sphere complex structure between H3AsO30 and OH group at the surface of CSGO and a characteristic monodentate bond mechanism is symbolized by equations (9) and (10) [114].
(9)OH+H3AsO3⟶O−H−O−As0<OHOH(10)OH+H3AsO3⟶O−As<OHOH+0H2O


## 7. Conclusion and Future Potential

The production of environmentally friendly sorbents which are considered as one of the promising techniques in water remediation has been made possible by BNC trends. Reportedly, various BP NCs with sorption capacities comparable to or greater than viable sorbents have been created over the last decades. This review paves the way for the novel bionanosorbents developed for the sequestration of environmental contaminants. The sorption of most contaminants was noticed to be dependent on the pH, sorbent dosage, and initial contaminant concentration, with most contaminants’ sorption, noticed within the pH range of 2-10. The sorption process of HMs and dyes to various BNCs was superlatively depicted utilizing the LNR and FL as well as the PSO models, suggestive of the sorption process of a monolayer and multilayer as well as the chemisorption process and the rate-limiting stage in surface sorption. The use of these NCs as sorbents in industrial and domestic environments is currently under investigation, and the majority of studies carried out are with synthetically polluted water achieved by the dissolution of contaminants in deionized water. To conduct full-scale researches, the structural stability of BNCs and their ecological noxiousness should be understood to show their useful functionality. Since there is presently limited fiscal information on the long-term use of BNCs for remediation of wastewater, financial assessments in this regard would aid in giving more understanding on the practicability and durability of these sorbents for contaminated water. Conclusively, it is suggested and recommended that more studies on BNC sorbents that would exhibit more excellent applicability, isolation, and efficiency as well as fast analysis for the trace determination, sorption, and elimination of inorganic and toxic substances in water samples should be the direction for future prospective for the treatment and remediation of contaminated water vis-à-vis water purification technology.



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*Source: 8030175-2022-03-07.xml*