# Adsorptive Removal of Cd(II) Ions from Wastewater Using Maleic Anhydride Nanocellulose

Authors: Hizkeal Tsade Kara; Sisay Tadesse Anshebo; Fedlu Kedir Sabir
Journal: Journal of Nanotechnology
 (2021)

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## Abstract

In this study, both pristine cellulose nanocrystalline (CNC) and maleic anhydride functionalized cellulose nanocrystalline (MA-CNC) were prepared from the stems ofEichhornia crassipes weed by the sulfuric acid hydrolysis method. The as-prepared adsorbents were characterized by using X-ray diffraction (XRD), Fourier-transform infrared (FTIR) spectroscopy, scanning electron microscopy (SEM), energy-dispersive X-ray (EDX), and Brunauer–Emmett–Teller (BET) instruments. These materials were applied for the removal of Cd(II) ions from WW. The uptake mechanism was fixed to both Langmuir and Freundlich adsorption isotherms with a maximum Cd(II) ion uptake capability (qmax) of 75.76 and 215.52 mg g−1 by CNC and MA-CNC adsorbents, respectively. Pseudo-second-order (PSO) kinetic model was well fitted to the uptake process. The adsorbent regeneration study was done after desorption of Cd(II) ions from the adsorbent by HCl washing. Results exhibited that the adsorbent was reused for the removal of Cd(II) ions from real WW after successive 13th cycle.


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## Body

## 1. Introduction

Currently, the pollution of the environment by different toxic pollutants, such as heavy metals, dyes, and pesticides, has stimulated great concern and is the most focusing issue in developing countries [1]. The sources for these pollutants are different natural and anthropogenic activities, such as domestic, industrial, and agricultural activities. These pollutants enter into the water bodies through the release of different pollutant-containing effluents. Among these, the pollution of the environment by heavy metals causes severe environmental effects because, unlike organic pollutants, heavy metals are nonbiodegradable. These heavy metals are arsenic (As), lead (Pb), chromium (Cr), copper (Cu), zinc (Zn), cobalt (Co), molybdenum (Mo), and manganese (Mn) [2]. Cd is one representative example of toxic metals entering the environment from industrial effluent and poses a potential risk to the whole environment in general and wastewater in particular because of its nonbiodegradable nature, carcinogenicity, persistence, and bioaccumulation. The presence of Cd can harmfully affect the achievement of the wastewater treatment processes and lead to serious risks to the environment [3]. Subsequently, the efficient removal of Cd(II) ions from real wastewater before its discharge into the environment was one of the best options for the quality of water.In the 21st century, a lot of technologies were tested to remediate augmented poisonous waste discharges from the wastewater [4]. These are chemical precipitation, chemically enhanced primary treatment (CEPT), filtration, reverse osmosis, solvent extraction, ion exchange, coagulation, and adsorption [5, 6]. Most of these technologies need high prices, have relatively low remediation capabilities, and call for further treatments [7]. For instance, chemically enhanced primary treatment (CEPT) methods can remove the Cd(II) ions levels partially, but the complete removal of Cd(II) ions is not guaranteed. Furthermore, this technique leads to the production of an increased number of alkaline sludge. The other abovementioned techniques have similar drawbacks, and more efficient treatment ways are required currently. Therefore, among these techniques, adsorption seems to be the most one owing to its simple operation, cost-friendly, very high remediation sensitivity, augmented uptake capability, and easy availability as adsorbent materials like activated carbon, carbon nanotubes (CNT), composites, and nanoparticles [8–13].Recently, most thematic adsorption studies focused on low-cost, renewable, and easily recyclable adsorbent materials, such as polymeric materials including cellulose, chitin, chitosan, gelatin, alginate, and starch for the eradication of noxious nutrients from aqueous media has been the 21st-century choices. Despite its increased properties, the limitations of cellulose-based materials in wastewater remediation processes have shown that the decreased hydrophilicity, low physical and chemical stability, and low pollutants uptake capability [14, 15]. This drawback can be resolved by bringing cellulose into nanocellulose in order to enhance its pollutant uptake capabilities [16]. Thus, in this study, cellulose nanocrystallines (CNCs) were selected as a good adsorbent for Cd(II) ions remediation from wastewater due to their bioavailability, biocompatibility, sustainability, environmentally friendly, renewability, having high aspect ratio, having better physical and chemical stability, and abundant active and reactive surface [17, 18].Several research studies were reported on CNC adsorbents with a high specific surface area ranging from 52 m2g−1 to 107 m2g−1, based on the preparation methods [19, 20]. It is known that the high surface areas and small particle sizes are very significant for the efficient Cd(II) ions removal mechanisms. CNCs characteristically have low removal capability and less dimensional stability. One can improve these problems through the functionalization of CNCs by adding extra anions or cations into the surface of CNCs [21–25]. Chemical surface modification of CNCs has substantial removal capabilities toward different pollutants from contaminated effluents [26–28].Previously, many research studies have been carried out on the CNMs based adsorbents synthesized from different biobased materials such as plant materials, date palm (Phoenix dactylifera L.) [29], Cotton residue [30], banana [31], corn husk [32], Erythrina brucei plant [33], and Millettia ferruginea plant [34]. To the best of the author’s knowledge, insufficient research papers are reported on the CNCs sorbents synthesized from the stems of Eichhornia crassipes weed. This material was completely waste material that has not any negative economic impact on societies. This material has plenty of hydroxyl, carbonyl, and ester functional groups that are responsible for the efficient adsorption of Cd(II) ions from wastewater. This is due to the presence of hydrogen bonding between the positively charged Cd(II) ions and OH functional groups of CNCs adsorbents. Thus, using waste material instead of useful material as Cd(II) ions removing reagent from wastewater is cost-effective for developing countries. Furthermore, most of the research studies reported in the literature were on the removal of Cd(II) ions from synthetic wastewater only, but there is a dearth of information regarding the removal of Cd(II) ions from real wastewater. Therefore, the study focused on the preparation and characterization of pristine CNC and maleic anhydride-modified MA-CNC adsorbents from the stems of Eichhornia crassipes weed to remove Cd(II) ions from real wastewater.


## 2. Materials and Methods

### 2.1. Materials and Chemicals

The stems ofEichhornia crassipes weed, for CNCs preparation, were collected from Southern Region “Ganta Garo” Lake abaya, Gamo Zone, Ethiopia. The wastewater (WW) sample was collected from the run-off Modgo River, Oromia Region, Ethiopia. All the reagent grades are toluene (99%, Loba Chemie Pvt. Ltd, India), ethanol (97%, Tradewell International Pvt. Ltd, India), sodium hydroxide (99%, Shraddha Associates (GUJ) Pvt. Ltd., India), conc. hydrochloric acid (35%, Loba Chemie Pvt. Ltd., India), conc. sulfuric acid (69%, Loba Chemie Pvt. Ltd., India), conc. nitric acid (69%, Loba Chemie Pvt. Ltd., India), sodium chlorite (80%, Shanghai ZZ New Material Tech. Co., Ltd., China), sodium bicarbonate (99%, Shraddha Associates (GUJ) Pvt. Ltd., India), and cadmium nitrate (Cd (NO3) 2 (SDFCL, India)).


### 2.2. Experimental Procedures

The stock solution of Cd(II) ions was prepared by taking a 1000 mL volumetric flask and adding the required amount in a gram of Cd(NO3)2 into the flask. Then, to this flask certain volume of distilled water was added. The dilute solutions were prepared by adding a sufficient amount of distilled water to the previously prepared stock solution of the Cd(II) ions. The collected WW physicochemical property (pH, EC, COD, BOD, TIN, TP, NO3−, Ca2+, and Mg2+) measurements were performed using different standard series. Next to this, it was spiked with 20 mg L−1 of Cd(II) ions solution and kept in suitable places for the experimental procedures.


### 2.3. Preparation of Cellulose Nanomaterials fromEichhornia crassipes

The stems of the collectedEichhornia crassipes weed sample were cut in the length of 8 mm, washed with distilled water several times to remove any dust particles, dried with the sun for 4 days, and ground using a grinder carefully to form coarse particles [35–38]. The coarse particles were treated with 100 mL of 2.5 M NaOH solution at 50°C for 3 hours to remove the lignin and hemicelluloses present in lignocellulosic biomass. This mixture was washed well with deionized water repeatedly until the pH of 7, and the washed liquid wastes were managed properly in the laboratory. Thereafter, the neutral mixture was filtered, centrifuged, and dried in the oven at 50°C for 10 hours. Then, it was ground into a pulp form and bleached with a ratio of 2 : 1 mixture volume of sodium chlorite (NaClO2) and glacial acetic acid for 3 hours at 80°C under mechanical stirring. Then, it was centrifuged, washed, and filtered to form cellulose suspension. This procedure was repeated with half the initial amount of bleaching agents. Even though the sulfuric acid hydrolysis method produces a large number of liquid wastes to the environment compared to organic acids, it removes all hemicellulose from cellulosic components and it makes the nanocellulose dispersed as a stable colloid system due to the esterification of the hydroxyl group by sulfate ions [8]. Therefore, the mixture was hydrolyzed by 100 mL of 6 M H2SO4 for 2 hours to break up the cell wall and to form a white nanocellulose suspension. During this process, a number of liquid wastes that are harmful to the working environments are produced. This problem was managed through a scientific and sensible liquid waste management system. Then, the produced white suspension was centrifuged at 16000 rpm to separate the nanocellulose and homogenized in homogenizer at about 12,000 rpm for 2.5 hours. The separated nanocellulose was washed repeatedly until the pH of 7, filtered, and dried to form cellulose nanocrystalline (CNC). Finally, the prepared CNC was kept in a suitable place for characterization purposes. The flowchart representation of CNC preparation is given in Figure 1.Figure 1
Flowchart of CNC preparation fromEichhornia crassipes.


#### 2.3.1. Preparation of Chemically Modified (Maleic Anhydride) Cellulose Nanocrystalline (CNC): Esterification

About 50% of the world’s maleic anhydride yield is used in the manufacture of unsaturated polyester resins (UPR), and here, it was used as esterification processes by combining with CNC. CNC properties were improved by the esterification process with maleic anhydride by modification of the method reported in the literature [39]. Firstly, the obtained CNC was washed with the help of glacial acetic acid in order to make the chemical modification of CNC easy and to exchange the solvent. For this purpose, 15 g of previously prepared CNC was mixed with maleic anhydride by consecutively washing and centrifuging with glacial acetic acid four times for the purposes of solvent exchange. Then, this mixture was placed in a 500 mL beaker containing 170 mL of acetic acid and 210 mL of toluene and homogenized in a magnetic stirrer at 50°C for 2 hrs. Next to the homogenization procedure, 2 mL of 0.12 M sulfuric acid was added, the sonication processes were carried out for 1 min with the help of ionic liquid, and then, 1.5 g of maleic acid anhydride was added. The reaction mixture was kept at room temperature for 90 min. After the completion of this reaction, the maleic anhydride functionalized cellulose nanomaterial suspension was sequentially washed and centrifuged with toluene, methanol, and dichloromethane solvents. The purpose of solvent exchange during the preparation of MA-CNC is to remove nonpolar liquid wastes and polar liquid wastes using these nonpolar and polar solvents, respectively. Using toluene and dichloromethane solvents, the nonpolar wastes are removed, and using methanol and water solvents, the polar wastes are removed from the MA-CNC adsorbents. The sequentially washed maleic anhydride functionalized cellulose nanomaterial suspension was filtered and dried to form maleic anhydride functionalized cellulose nanocrystalline (MA-CNC). The esterification reaction of CNC with maleic anhydride (MA) is given in Figure 2.Figure 2
Esterification of cellulose nanocrystalline (CNC) by using maleic anhydride (MA).


### 2.4. Characterization

The crystallite size of both CNC and MA-CNC adsorbents was characterized by using XRD (XRD-7000 X-ray diffractometer, Shimadzu Co., Japan) with Cu-Kα radiation (λ = 0.154 nm) at 40 kV and 40 mA under a 2θ diffraction angle from 0° to 80° at a scan rate of 2°/min. The functional group of the as-synthesized CNC and MA-CNC sorbent materials were identified using the Fourier-transform infrared spectroscopy (FTIR) (Perkin Elmer65, PerkinElmer, Inc., Waltham, USA). The surface morphology of the different treatment phases of both CNC and MA-CNC adsorbents was examined using a Hitachi S-4100 scanning electron microscope (SEM). The specific surface area measurement was determined by the Brunauer–Emmett–Teller (BET) analysis.


### 2.5. Adsorption Experiments

To determine the Cd(II) ion adsorption efficiency of CNC and MA-CNC adsorbents, batch experiments were conducted. In this experiment, each experimental parameter such as the initial concentration of Cd(II) ions ranged from 5 to 40 mg/L, the adsorbent dosage ranged from 0.04 to 1.5 g, the contact time ranged from 30 to 180 min, solution pH ranged from 2 to 12, and the temperature ranged from 20 to 45°C by making the rest parameters at fixed manner. Each of these parameters was accomplished in 100 mL flasks at the temperature of 20°C through shaking by an orbital shaker. Initially, the pH value of each solution was calibrated by the addition of 0.1 M HCl or 0.1 M NaOH solution, and the pH change was measured using a PH meter (pH 21 Hanna instrument). Then, each flask containing these solutions was covered with aluminum foil in all experiments to prevent any contaminant reactions with this solution, and after the reaction completion, it was carefully filtered with filtrate paper No. 42. After this, the measurement of this solution was done by an Atomic Absorption Spectrophotometer (Shimadzu, USA).


#### 2.5.1. Adsorption Isotherms

Here, measuring the adsorption isotherms helps to quantify the affinity of the removal of Cd(II) ions from wastewater by CNC and MA-CNC adsorbents. Mathematically, the affinity of the Cd(II) ion uptake for CNC and MA-CNC adsorbents was measured using adsorption isotherms. Thus, the adsorption of Cd(II) ions by using CNC and MA-CNC sorbents was done by using equations (1) and (2). From this equation, one can understand that the amount of Cd(II) ions adsorbed onto the CNC and MA-CNC adsorbents is equal to the amount of Cd(II) ions that were removed from the WW.(1)qe=CiCdII−CeCdIIS,(2)qt=CiCdII−CtCdIIS,where qe and qt represent the amount of heavy metal adsorbed on the adsorbent surface at equilibrium and at any specific time (mg g−1), respectively. Ci, Cd(II) and Ce, Cd(II) represent the initial and equilibrium concentration of the heavy metal in the WW sample (mg L−1), respectively, and Ct is the concentration of Cd(II) ions in wastewater samples (mgL−1) at a specific time. S represents the slurry dosage defined as the ratio between the mass of adsorbent CNC and MA-CNC adsorbents (g) to the initial volume of the water sample (L). Both the initial and the optimum amounts of Cd(II) ions were used to measure the percentage of Cd(II) ions removal as follows:(3)%CdIIion removal=CiCdII−CeCdIICiCdII×100%.The thermodynamic study of the adsorption process was studied by considering the fundamental thermodynamic parameters such as a change in Gibbs free energy (∆G), change in enthalpy (∆H), and change in entropy (∆S) values [34, 35]. Therefore, the thermodynamics of the removal of Cd(II) ions was performed by using all the optimum values of predetermined parameters, such as solution pH, sorbent dosage, Cd(II) ions initial concentration, and agitation speed by varying the temperature range from 20 to 45°C.


#### 2.5.2. Adsorption Kinetics

The Cd(II) ion remediation kinetic process from WW was performed using the contact time ranging from 30 to 180 min by making all parameters (solution pH, sorbent dose, shaking speed, and Cd(II) ions initial concentration) at optimum value.


### 2.6. Regeneration Experiment

For regeneration experiments, the modified (MA-CNC) sorbent was selected because of the high removal efficiency of Cd(II) ions from WW. The experiments were conducted after desorption of Cd(II) ions by the addition of 0.5 g MA-CNC adsorbent to a flask containing 10 mL of 0.1 M HCl solution. Then, this mixture was sonicated and centrifuged to separate the adsorbent from the mixture. The separated MA-CNC sorbent was then washed with deionized water four times, filtered, and dried. The regenerated adsorbent was reused for at least 13th frequent sequences as adsorbent without any significant efficient loss.


## 2.1. Materials and Chemicals

The stems ofEichhornia crassipes weed, for CNCs preparation, were collected from Southern Region “Ganta Garo” Lake abaya, Gamo Zone, Ethiopia. The wastewater (WW) sample was collected from the run-off Modgo River, Oromia Region, Ethiopia. All the reagent grades are toluene (99%, Loba Chemie Pvt. Ltd, India), ethanol (97%, Tradewell International Pvt. Ltd, India), sodium hydroxide (99%, Shraddha Associates (GUJ) Pvt. Ltd., India), conc. hydrochloric acid (35%, Loba Chemie Pvt. Ltd., India), conc. sulfuric acid (69%, Loba Chemie Pvt. Ltd., India), conc. nitric acid (69%, Loba Chemie Pvt. Ltd., India), sodium chlorite (80%, Shanghai ZZ New Material Tech. Co., Ltd., China), sodium bicarbonate (99%, Shraddha Associates (GUJ) Pvt. Ltd., India), and cadmium nitrate (Cd (NO3) 2 (SDFCL, India)).


## 2.2. Experimental Procedures

The stock solution of Cd(II) ions was prepared by taking a 1000 mL volumetric flask and adding the required amount in a gram of Cd(NO3)2 into the flask. Then, to this flask certain volume of distilled water was added. The dilute solutions were prepared by adding a sufficient amount of distilled water to the previously prepared stock solution of the Cd(II) ions. The collected WW physicochemical property (pH, EC, COD, BOD, TIN, TP, NO3−, Ca2+, and Mg2+) measurements were performed using different standard series. Next to this, it was spiked with 20 mg L−1 of Cd(II) ions solution and kept in suitable places for the experimental procedures.


## 2.3. Preparation of Cellulose Nanomaterials fromEichhornia crassipes

The stems of the collectedEichhornia crassipes weed sample were cut in the length of 8 mm, washed with distilled water several times to remove any dust particles, dried with the sun for 4 days, and ground using a grinder carefully to form coarse particles [35–38]. The coarse particles were treated with 100 mL of 2.5 M NaOH solution at 50°C for 3 hours to remove the lignin and hemicelluloses present in lignocellulosic biomass. This mixture was washed well with deionized water repeatedly until the pH of 7, and the washed liquid wastes were managed properly in the laboratory. Thereafter, the neutral mixture was filtered, centrifuged, and dried in the oven at 50°C for 10 hours. Then, it was ground into a pulp form and bleached with a ratio of 2 : 1 mixture volume of sodium chlorite (NaClO2) and glacial acetic acid for 3 hours at 80°C under mechanical stirring. Then, it was centrifuged, washed, and filtered to form cellulose suspension. This procedure was repeated with half the initial amount of bleaching agents. Even though the sulfuric acid hydrolysis method produces a large number of liquid wastes to the environment compared to organic acids, it removes all hemicellulose from cellulosic components and it makes the nanocellulose dispersed as a stable colloid system due to the esterification of the hydroxyl group by sulfate ions [8]. Therefore, the mixture was hydrolyzed by 100 mL of 6 M H2SO4 for 2 hours to break up the cell wall and to form a white nanocellulose suspension. During this process, a number of liquid wastes that are harmful to the working environments are produced. This problem was managed through a scientific and sensible liquid waste management system. Then, the produced white suspension was centrifuged at 16000 rpm to separate the nanocellulose and homogenized in homogenizer at about 12,000 rpm for 2.5 hours. The separated nanocellulose was washed repeatedly until the pH of 7, filtered, and dried to form cellulose nanocrystalline (CNC). Finally, the prepared CNC was kept in a suitable place for characterization purposes. The flowchart representation of CNC preparation is given in Figure 1.Figure 1
Flowchart of CNC preparation fromEichhornia crassipes.


### 2.3.1. Preparation of Chemically Modified (Maleic Anhydride) Cellulose Nanocrystalline (CNC): Esterification

About 50% of the world’s maleic anhydride yield is used in the manufacture of unsaturated polyester resins (UPR), and here, it was used as esterification processes by combining with CNC. CNC properties were improved by the esterification process with maleic anhydride by modification of the method reported in the literature [39]. Firstly, the obtained CNC was washed with the help of glacial acetic acid in order to make the chemical modification of CNC easy and to exchange the solvent. For this purpose, 15 g of previously prepared CNC was mixed with maleic anhydride by consecutively washing and centrifuging with glacial acetic acid four times for the purposes of solvent exchange. Then, this mixture was placed in a 500 mL beaker containing 170 mL of acetic acid and 210 mL of toluene and homogenized in a magnetic stirrer at 50°C for 2 hrs. Next to the homogenization procedure, 2 mL of 0.12 M sulfuric acid was added, the sonication processes were carried out for 1 min with the help of ionic liquid, and then, 1.5 g of maleic acid anhydride was added. The reaction mixture was kept at room temperature for 90 min. After the completion of this reaction, the maleic anhydride functionalized cellulose nanomaterial suspension was sequentially washed and centrifuged with toluene, methanol, and dichloromethane solvents. The purpose of solvent exchange during the preparation of MA-CNC is to remove nonpolar liquid wastes and polar liquid wastes using these nonpolar and polar solvents, respectively. Using toluene and dichloromethane solvents, the nonpolar wastes are removed, and using methanol and water solvents, the polar wastes are removed from the MA-CNC adsorbents. The sequentially washed maleic anhydride functionalized cellulose nanomaterial suspension was filtered and dried to form maleic anhydride functionalized cellulose nanocrystalline (MA-CNC). The esterification reaction of CNC with maleic anhydride (MA) is given in Figure 2.Figure 2
Esterification of cellulose nanocrystalline (CNC) by using maleic anhydride (MA).


## 2.3.1. Preparation of Chemically Modified (Maleic Anhydride) Cellulose Nanocrystalline (CNC): Esterification

About 50% of the world’s maleic anhydride yield is used in the manufacture of unsaturated polyester resins (UPR), and here, it was used as esterification processes by combining with CNC. CNC properties were improved by the esterification process with maleic anhydride by modification of the method reported in the literature [39]. Firstly, the obtained CNC was washed with the help of glacial acetic acid in order to make the chemical modification of CNC easy and to exchange the solvent. For this purpose, 15 g of previously prepared CNC was mixed with maleic anhydride by consecutively washing and centrifuging with glacial acetic acid four times for the purposes of solvent exchange. Then, this mixture was placed in a 500 mL beaker containing 170 mL of acetic acid and 210 mL of toluene and homogenized in a magnetic stirrer at 50°C for 2 hrs. Next to the homogenization procedure, 2 mL of 0.12 M sulfuric acid was added, the sonication processes were carried out for 1 min with the help of ionic liquid, and then, 1.5 g of maleic acid anhydride was added. The reaction mixture was kept at room temperature for 90 min. After the completion of this reaction, the maleic anhydride functionalized cellulose nanomaterial suspension was sequentially washed and centrifuged with toluene, methanol, and dichloromethane solvents. The purpose of solvent exchange during the preparation of MA-CNC is to remove nonpolar liquid wastes and polar liquid wastes using these nonpolar and polar solvents, respectively. Using toluene and dichloromethane solvents, the nonpolar wastes are removed, and using methanol and water solvents, the polar wastes are removed from the MA-CNC adsorbents. The sequentially washed maleic anhydride functionalized cellulose nanomaterial suspension was filtered and dried to form maleic anhydride functionalized cellulose nanocrystalline (MA-CNC). The esterification reaction of CNC with maleic anhydride (MA) is given in Figure 2.Figure 2
Esterification of cellulose nanocrystalline (CNC) by using maleic anhydride (MA).


## 2.4. Characterization

The crystallite size of both CNC and MA-CNC adsorbents was characterized by using XRD (XRD-7000 X-ray diffractometer, Shimadzu Co., Japan) with Cu-Kα radiation (λ = 0.154 nm) at 40 kV and 40 mA under a 2θ diffraction angle from 0° to 80° at a scan rate of 2°/min. The functional group of the as-synthesized CNC and MA-CNC sorbent materials were identified using the Fourier-transform infrared spectroscopy (FTIR) (Perkin Elmer65, PerkinElmer, Inc., Waltham, USA). The surface morphology of the different treatment phases of both CNC and MA-CNC adsorbents was examined using a Hitachi S-4100 scanning electron microscope (SEM). The specific surface area measurement was determined by the Brunauer–Emmett–Teller (BET) analysis.


## 2.5. Adsorption Experiments

To determine the Cd(II) ion adsorption efficiency of CNC and MA-CNC adsorbents, batch experiments were conducted. In this experiment, each experimental parameter such as the initial concentration of Cd(II) ions ranged from 5 to 40 mg/L, the adsorbent dosage ranged from 0.04 to 1.5 g, the contact time ranged from 30 to 180 min, solution pH ranged from 2 to 12, and the temperature ranged from 20 to 45°C by making the rest parameters at fixed manner. Each of these parameters was accomplished in 100 mL flasks at the temperature of 20°C through shaking by an orbital shaker. Initially, the pH value of each solution was calibrated by the addition of 0.1 M HCl or 0.1 M NaOH solution, and the pH change was measured using a PH meter (pH 21 Hanna instrument). Then, each flask containing these solutions was covered with aluminum foil in all experiments to prevent any contaminant reactions with this solution, and after the reaction completion, it was carefully filtered with filtrate paper No. 42. After this, the measurement of this solution was done by an Atomic Absorption Spectrophotometer (Shimadzu, USA).


### 2.5.1. Adsorption Isotherms

Here, measuring the adsorption isotherms helps to quantify the affinity of the removal of Cd(II) ions from wastewater by CNC and MA-CNC adsorbents. Mathematically, the affinity of the Cd(II) ion uptake for CNC and MA-CNC adsorbents was measured using adsorption isotherms. Thus, the adsorption of Cd(II) ions by using CNC and MA-CNC sorbents was done by using equations (1) and (2). From this equation, one can understand that the amount of Cd(II) ions adsorbed onto the CNC and MA-CNC adsorbents is equal to the amount of Cd(II) ions that were removed from the WW.(1)qe=CiCdII−CeCdIIS,(2)qt=CiCdII−CtCdIIS,where qe and qt represent the amount of heavy metal adsorbed on the adsorbent surface at equilibrium and at any specific time (mg g−1), respectively. Ci, Cd(II) and Ce, Cd(II) represent the initial and equilibrium concentration of the heavy metal in the WW sample (mg L−1), respectively, and Ct is the concentration of Cd(II) ions in wastewater samples (mgL−1) at a specific time. S represents the slurry dosage defined as the ratio between the mass of adsorbent CNC and MA-CNC adsorbents (g) to the initial volume of the water sample (L). Both the initial and the optimum amounts of Cd(II) ions were used to measure the percentage of Cd(II) ions removal as follows:(3)%CdIIion removal=CiCdII−CeCdIICiCdII×100%.The thermodynamic study of the adsorption process was studied by considering the fundamental thermodynamic parameters such as a change in Gibbs free energy (∆G), change in enthalpy (∆H), and change in entropy (∆S) values [34, 35]. Therefore, the thermodynamics of the removal of Cd(II) ions was performed by using all the optimum values of predetermined parameters, such as solution pH, sorbent dosage, Cd(II) ions initial concentration, and agitation speed by varying the temperature range from 20 to 45°C.


### 2.5.2. Adsorption Kinetics

The Cd(II) ion remediation kinetic process from WW was performed using the contact time ranging from 30 to 180 min by making all parameters (solution pH, sorbent dose, shaking speed, and Cd(II) ions initial concentration) at optimum value.


## 2.5.1. Adsorption Isotherms

Here, measuring the adsorption isotherms helps to quantify the affinity of the removal of Cd(II) ions from wastewater by CNC and MA-CNC adsorbents. Mathematically, the affinity of the Cd(II) ion uptake for CNC and MA-CNC adsorbents was measured using adsorption isotherms. Thus, the adsorption of Cd(II) ions by using CNC and MA-CNC sorbents was done by using equations (1) and (2). From this equation, one can understand that the amount of Cd(II) ions adsorbed onto the CNC and MA-CNC adsorbents is equal to the amount of Cd(II) ions that were removed from the WW.(1)qe=CiCdII−CeCdIIS,(2)qt=CiCdII−CtCdIIS,where qe and qt represent the amount of heavy metal adsorbed on the adsorbent surface at equilibrium and at any specific time (mg g−1), respectively. Ci, Cd(II) and Ce, Cd(II) represent the initial and equilibrium concentration of the heavy metal in the WW sample (mg L−1), respectively, and Ct is the concentration of Cd(II) ions in wastewater samples (mgL−1) at a specific time. S represents the slurry dosage defined as the ratio between the mass of adsorbent CNC and MA-CNC adsorbents (g) to the initial volume of the water sample (L). Both the initial and the optimum amounts of Cd(II) ions were used to measure the percentage of Cd(II) ions removal as follows:(3)%CdIIion removal=CiCdII−CeCdIICiCdII×100%.The thermodynamic study of the adsorption process was studied by considering the fundamental thermodynamic parameters such as a change in Gibbs free energy (∆G), change in enthalpy (∆H), and change in entropy (∆S) values [34, 35]. Therefore, the thermodynamics of the removal of Cd(II) ions was performed by using all the optimum values of predetermined parameters, such as solution pH, sorbent dosage, Cd(II) ions initial concentration, and agitation speed by varying the temperature range from 20 to 45°C.


## 2.5.2. Adsorption Kinetics

The Cd(II) ion remediation kinetic process from WW was performed using the contact time ranging from 30 to 180 min by making all parameters (solution pH, sorbent dose, shaking speed, and Cd(II) ions initial concentration) at optimum value.


## 2.6. Regeneration Experiment

For regeneration experiments, the modified (MA-CNC) sorbent was selected because of the high removal efficiency of Cd(II) ions from WW. The experiments were conducted after desorption of Cd(II) ions by the addition of 0.5 g MA-CNC adsorbent to a flask containing 10 mL of 0.1 M HCl solution. Then, this mixture was sonicated and centrifuged to separate the adsorbent from the mixture. The separated MA-CNC sorbent was then washed with deionized water four times, filtered, and dried. The regenerated adsorbent was reused for at least 13th frequent sequences as adsorbent without any significant efficient loss.


## 3. Results and Discussion

### 3.1. Characterization

Both the CNC and MA-CNC sorbents were characterized by using modern instrumental techniques, such as FTIR, XRD, and SEM. The identification of functional groups and surface characteristics of the as-prepared CNM and MA-CNC sorbents were carried out by using FTIR spectroscopy. The spectra of CNC and MA-CNC sorbents prepared with the help of sulfuric acid hydrolysis obtained from the FTIR spectroscopy are shown in Figure3(a). The results revealed that both CNC and MA-CNC have representative broadband around 3355 cm−1 which corresponds to O-H free stretching vibration of the CH2-OH structure on cellulose I and OH groups [40]. The spectra located at 2925 cm−1 are as a result of C-H stretching vibration in cellulose I, and the spectra found in zone four at 1735 cm−1 are recognized to the carbonyl functional groups of cellulose I. The peaks detected at 1458 cm−1 are correlated to the C-C stretching and/or CH2 symmetric bending in aromatic groups of cellulose I. The peak located at 1058 cm−1 is connected to the C-O-C stretching of cellulose I [41]. Compared with the spectrum of raw CNC, additional peaks observed in the oxidized cellulose nanomaterial (MA-CNC) at 1428 cm−1, referring to the stretching vibration of the ionic carboxylic groups, confirmed the insertion of carboxylic groups on the surface of CNC sorbent. Also, the spectra at 1265–1325 cm−1 are indications of the presence of C-O-C groups on the sorbent. This makes maleic anhydride efficaciously oxidize the adjacent hydroxyl groups of cellulose at locations of carbon numbers 2 and 3 into aldehyde groups, concurrently breaking the corresponding carbon-carbon bond of the glucopyranose ring in order to obtain DACNC.Figure 3
(a) FTIR spectra, (b) XRD pattern, and (c, d) SEM images of CNC and MA-CNC sorbents, respectively.
(a)(b)(c)(d)The CNC and MA-CNC sorbent crystalline particle size was determined by using the XRD diffractogram (Figure3(b)). The crystallographic planes of cellulose I structure were certainly fixed to the peaks attributed at 2θ = 15.87°, 22.50°, and 34.82° are (110), (110), and (004), respectively [42]. From the XRD patterns, the pristine CNM sorbent has the same peaks as that of the esterified (MA-CNC) except for the increased degree of crystallinity for the CNC sorbent (Figure 3(b)). Despite the increased degree of crystallinity for the CNC sorbent, both sorbents undoubtedly displayed the amorphous nature in contrast to 100% crystallinity because of the polymeric nature of Eichhornia crassipes. The diffractogram of CNC and MA-CNC sorbents has an obvious sharp band focused at 22.50° attributed to the semicrystalline structure of the cellulose-based sorbents. The functionalized nanocellulose exhibited a reduced percent of crystallinity and broad peak than the raw CNM because of the oxidation of the crystalline region by the addition of maleic anhydride into the raw nanocellulose suspension [43].Both CNC and MA-CNC sorbent microstructures and surface morphologies were done using SEM instruments (Figures3(c) and 3(d)). The image from the SEM micrograph shows that both CNM and MA-CNM sorbents were cylindrical rod-like shapes. From the SEM image, MA-CNC sorbent was probable to agglomerate in comparison with CNC after drying. In MA-CNC adsorbents, the produced carbonyl groups might also encourage the presence of hydrogen bond structures in the MA-CNC sorbents. These variations in biochemical arrangements also caused the variations in surfaces of DACNC [44, 45].Brunauer–Emmett–Teller (BET) data investigation is accomplished according to the BET adsorption isotherm linear equation (4) to determine the specific surface area of CNC and MA-CNC adsorbents. Its measurement was carried out using N2 gas as an adsorbate at a temperature of 77 K.(4)p/pon1−p/po=C−1XmCp/po+1XmC,where Po and P are saturated and partial vapor pressure of N2 gas at equilibrium in Pa, respectively; n is the volume of N2 gas adsorbed at STP in mL; Xm is BET monolayer capacity; C is a dimensionless constant associated with the enthalpy of N2 gas adsorption on the adsorbent.For the well-defined BET monolayer capacity of the nanoparticle materials, the value of C should be ≥80 [46]. Thus, from the given equation (4), it is possible to obtain the C value of NaIO4-NC (188.3 and 190.2) which is ≥80. Figure 4(a) indicates the linear plots of [(P/Po)/(n(1 − P/Po))] versus P/Po and provides a straight line with the approximate relative pressure ranging from 0.05 to 0.3. The linear regression value (R2) obtained from this plot was 0.9985, which is greater than 0.995. This result confirms the acceptability level of the R2 value. The specific surface area (SSA) in m2·g−1 is calculated according to(5)as=XmLσmm×22400,where as is the BET specific surface area of the NaIO4-NC of mass m in grams, L is the Avogadro constant (6.022 × 1023 mol−1), σm is the molecular adsorptive cross-sectional area occupied by N2 gas molecule in the complete monolayer (equal to 0.162 nm2 for N2 gas), and 22400 is the volume occupied by 1 mole of N2 gas at STP, in mL.Figure 4
(a) The linear plot of CNC and MA-CNC and (b) the BET plot of CNC and MA-CNC adsorbents.
(a)(b)The BET plot of CNC and MA-CNC sorbents, respectively, in Figure4(b) has indicated the cylindrical shape model. The symbols used were those given in the 2007 edition of the IUPAC manual [47]. Results indicated that the as-prepared CNC and MA-CNC adsorbents have a higher SSA of 108.2 and 123.9 m2g−1, respectively. Therefore, CNC and MA-CNC adsorbents have shown higher Cd(II) ion adsorption efficiency due to the decrease of the particle size, an increase of specific surface area, and the increase of surface roughness.


### 3.2. Physicochemical Properties of the WW

The collected WW physicochemical property measurements are performed within 24 hours after collection and given in Table1. Values for pH and electrical conductivity were determined in different series and reported as average values of 7.5 ± 0.05 and 265 ± 0.3, respectively. These results have shown that WW taken from the run of Modjo Rivers was nearly neutral. Furthermore, the average concentrations of COD, BOD, TP, TIN, nitrate (NO3−), (NH4+), Mg2+, Cu2+, and Cd2+ in the WW were 51.4 ± 0.2, 36.75 ± 0.02, 11.44 ± 0.3, 43.05 ± 0.02, 5.04 ± 0.05, 29.5 ± 0.02, 50.9 ± 0.6, 0.43 ± 0.03, and 0.12 ± 0.04, respectively.Table 1
Physicochemical properties of the SERWW used in the study.
ParameterLowest valueMaximum valueAveragepH6.9 ± 0.058.3 ± 0.057.5 ± 0.05EC(μS cm−1)260 ± 0.3270 ± 0.3265 ± 0.3COD (mg/L)42.25 ± 0.260.5 ± 0.251.4 ± 0.2BOD (mg/L)30.4 ± 0.0242.8 ± 0.0236.75 ± 0.02TIN (mg/L)31.5 ± 0.0254.6 ± 0.0243.05 ± 0.02NO3− (mg.N/L)4.3 ± 0.055.8 ± 0.055.04 ± 0.05NH4+ (mg.N/L)26.7 ± 0.0232.3 ± 0.0229.5 ± 0.02TP (mg/L)10.2 ± 0.312.6 ± 0.311.44 ± 0.3Mg2+ (mg/L)41.5 ± 0.660.3 ± 0.650.9 ± 0.6Cu2+ (mg/L)0.30 ± 0.030.56 ± 0.030.43 ± 0.03Cd2+ (mg/L)0.08 ± 0.040.16 ± 0.040.12 ± 0.04TP: total phosphorus; TIN: total inorganic nitrogen; BOD: biological oxygen demand; COD: chemical oxygen demand.


### 3.3. Adsorption Studies

#### 3.3.1. Effects of Contact times

Experiments for contact time effects on the removal of Cd(II) ions from wastewater were conducted by using the contact times ranging from 30 to 180 min at optimum CNC and MA-CNC dose of 0.5 g, temperature (T) of 20°C, and initial Cd(II) ions concentration of 20 mg L−1 (Figure 5(b)). The results have shown that the Cd(II) ion removal capacity increases by increasing the contact time from 30 to 120 min for both CNC and MA-CNC sorbents because of the increased number of active sites available on the surfaces of CNC and MA-CNC sorbents. The maximum % removal (%R) of Cd(II) ions of 67.80 and 88.84% was observed at the optimum contact time of 120 min for CNC and MA-CNC adsorbents, respectively. After 120 min., the Cd(II) ions %R remains unchanged because, with the increased contact time, the ratio of surface active sites to the total metal ions in the solution was low, and hence, all active sites had metal ions in solution and were occupied [48, 49]. In comparison to MA-CNC sorbent with CNC, the maximum Cd(II) ion uptake capabilities were observed for MA-CNC sorbent than CNC because of the increased number of active sites resulting from the esterification reaction of maleic anhydride. This result was in agreement with research reported by Madivoli et al. [49].Figure 5
The effect of initial concentration (a) and contact time (b) for the removal of Cd(II) ions from wastewater, respectively, at an optimum temperature of 20°C, adsorbent dosage of 0.5, solution pH of 8, and agitation speed of 250 rpm.
(a)(b)


#### 3.3.2. Effects of Initial Concentration

The effect of the initial concentration of Cd(II) ions against quantity adsorbed was conducted by using the optimum quantity of CNC and MA-CNC sorbents of 0.5 g, pH of 8, and the contact time of 120 min (Figure5(a)). At the starting point, the Cd(II) ion removal process was very rapid until the optimum value of 20 mg/L. At this stage, the ratio of surface active sites to the total metal ions in the solution was high, and hence, all Cd(II) ions are attracted to the surfaces of CNC and MA-CNC adsorbents [50]. At the optimum initial Cd(II) ion concentration of 20 mg L−1, both adsorbents clearly have shown higher Cd(II) ions %R of 64.91 and 88.44 from WW by CNC and MA-CNC adsorbents, respectively. Additionally, the higher %R of Cd(II) ions is evidently detected for MA-CNC sorbent relative to CNC adsorbent. This is because the presence of extra active sites on the MA-CNC adsorbent resulted from the esterification reaction of CNC [51, 52].


#### 3.3.3. Effects of Adsorbent Dose and Temperature

The effects of CNC and MA-CNC dose on the %R of Cd(II) ions from WW at different temperatures,T = 20, 30, and 45°C, were investigated, and the results are shown in Figure 5. Results have indicated that Cd(II) ion uptake ability was increased by increasing the CNC and MA-CNC adsorbent dose. This publicized that the uptake sites become unsaturated during the adsorption reaction, whereas the number of active surface areas available for the adsorption site increased by increasing the CNC and MA-CNC adsorbent dose. The maximum %R of 70.3 and 90.4 was observed at optimum CNC and MA-CNC adsorbent dose of 0.5 g and optimum temperature of 20°C, respectively. After this dose value, the %R becomes unchanged because of the particle aggregation, which would lead to a decrease in the total surface area of the adsorbent [53]. A higher %R of 90.4% was observed by using functionalized adsorbent than CNC because the esterification reaction provides the extra-functional groups on the adsorbent surface that make the functionalized adsorbent most active to adsorb Cd(II) ions onto the surface than a pristine one.Figures6(a) and 6(b) show the temperature effects on the %R of Cd(II) ions from WW by CNC and MA-CNC sorbents. Results have shown that the decreased %R of Cd(II) ions was observed at the higher temperature of 45°C. This is because, at increased temperature, the slow rate of the chemisorption processes prevents the Cd(II) ions to react with the active sites of the sorbent surface for increased %R of Cd(II) ions from wastewater [54]. For both CNC and MA-CNC adsorbents, the maximum %R of 70.3% and 90.4% was detected at the optimum dose and temperature of 0.5 g and 20°C, respectively. Furthermore, the higher %R of Cd(II) ions was observed by using MA-CNC sorbents than CNC sorbents due to the presence of extra-functional groups on the modified one [55].Figure 6
(a, b) Effects of adsorbent dose at different temperatures (20, 30, and 45°C) for Cd(II) ions’ remediation using CNC and MA-CNC adsorbents, respectively, at an optimum contact time of 120 min, agitation speed of 250 rpm, pH of 8, and initial concentration of 20 mg/L.
(a)(b)


#### 3.3.4. Effects of Solution pH

The effect of solution pH on Cd(II) ions removal from WW was performed by using pH values ranging from 2 to 12. As shown in Figure7(b), both CNC and MA-CNC adsorbents show the increasing removal abilities in the solution pH ranging from 2 to 8. The maximum %R for both CNC and MA-CNC adsorbents was 70.3 and 89.9%, respectively. At decreased solution pH amounts, the interaction of Cd(II) ions with adsorbents is declined because of the competition of H+ ions on the surfaces of the adsorbents [50]. Conversely, at the increased solution pH, Cd(II) ions binding to the CNC and MA-CNC adsorbents surfaces rise until the equilibrium pH of 8. After the optimum pH value of 8, the %R becomes declined due to the presence of increased amounts of OH− ions in WW. The increased OH− ions depict the formation of soluble hydroxyl complexes. Furthermore, at a higher alkaline pH value, the Cd(II) ions precipitate as Cd(OH)2. Figure 7(a) also shows that the higher %R of Cd(II) ions was observed by MA-CNC adsorbent than CNC sorbents at the optimum solution pH value of 8. The differences in the reported %R for the Cd(II) ions were related to the occurrence of additional functional groups in the structure of MA-CNC adsorbents with different affinity to Cd(II) ions than CNC sorbent [56].Figure 7
The effect of pH (a) and agitation speed (b) for the removal of Cd(II) ions from wastewater at an optimum initial concentration of 2 mg/L, contact time of 120 min, temperature of 20°C, and adsorbent dosage of 0.5 g, respectively.
(a)(b)


#### 3.3.5. Effects of Agitation Speed

The effect of agitation speed on the removal of Cd(II) ions is shown in Figure7(b). Initially, the agitation speed was slow, but as the agitation speed was increased subsequently, a rapid increase in the removal capability of Cd(II) ions was observed. This is due to the presence of more active sites existing on the binding surface of the adsorbent that is ready to adsorb Cd(II) ions [57]. Thus, the %R capacity of Cd(II) ions by MA-CNC adsorbent was increased from 72.2 to 88.55% as the agitation speed was increased from 100 to 250 rpm. In the same way, the Cd(II) ion %R capability of the CNC sorbent was increased from 34.65 to 67.17% as the agitation speed was increased from 100 to 250 rpm (Figure 7(b)). From this point of view, the %R capability of CNC adsorbent was low compared to MA-CNC adsorbent removal capability. This higher %R capability observed by MA-CNC adsorbent is due to the presence of more accessible surfaces resulting from the addition of maleic anhydride into the CNC. For both sorbents, the maximum Cd(II) ion %R capability was obtained at the optimum agitation speed of 250 rpm. This result was in agreement with the study reported by Mahmood et al. [58]. Generally, an increase in the speed of agitation speed resulted in outstanding pollutant uptake capabilities and the agitation helps in overcoming the resistance of external mass transfer.


### 3.4. The Chemistry of Wastewater

Table1 indicates the summary of the assessment carried out to determine the consequences of wastewater chemistry on the %R of Cd(II) ions. Experiments were performed using wastewater samples containing both synthetic and real wastewater at variable levels. Trials were performed in triplicate and reported as average values. From the experiments, the values for pH, COD, BOD, Cl−, SO4−, Fe2+, Ca2+, Mg2+, and (Cu2+) present in WW were determined using replicate of experiments and reported as the average values. The %R of the Cd(II) ions from both synthetic and real wastewater is represented in Figure 8. From the findings, it was possible to see that the removal processes were negatively affected by the presence of cations and anions in real wastewater. The lowering of the %R of Cd(II) ions in the real wastewater has resulted from the competition of cations and anions for the active sites in the real wastewater. The consequence of competing ions diminishes the interaction of fresh surfaces on MA-CNM adsorbent and the decreased %R of Cd(II) ions was observed [59]. Results indicated that the %R Cd(II) ions from WW were found to be 99.9 and 89.5% for the synthetic and real wastewater, respectively, by MA-CNC adsorbent.Figure 8
The effects of wastewater chemistry for both synthetic and real wastewater on the percent removal of Cd(II) ions at 20 mg/L and 20°C by using MA-CNC adsorbent.


### 3.5. Adsorption Isotherms

To appreciate the mechanism of Cd(II) ions uptake by CNC and MA-CNC adsorbents, Langmuir (equation (7)) and Freundlich (equation (8)) adsorption isotherms are investigated and presented in Figures 9(a) and 9(b), respectively. Table 2 shows the corresponding parameter values and the correlation coefficient (R2) values, obtained from each plot. Higher R2 values for both Langmuir and Freundlich isotherms have shown that both Langmuir and Freundlich isotherm models better fit the isothermal uptake data. That means, evidently, both of these isotherms describe the distribution of the Cd(II) ions between the liquid and solid stages conferring to prospects connected to the heterogeneity or homogeneity of the adsorbent surface, the category of coverage, and the prospect of contact between the Cd(II) ions. This suggested that the surface of CNC and MA-CNC adsorbents was heterogeneous and physically compatible with monolayer adsorption and the adsorption process was favorable. Moreover, strong electrostatic interactions were formed between the Cd(II) ions and the surfaces of adsorbents [60]. The favorability of the uptake process was due to the n value that lies between 1 and 10, and the strong interactions between the adsorbates and surfaces of the adsorbents were due to the fact that 1/n < 1. The fundamental nature of the Langmuir model could be also determined by a dimensionless equilibrium parameter (RL), and its value was calculated by using equation (6). The values (0.104 and 0.602) of RL < 1 suggested that the uptake process of Cd(II) ions by both CNC and MA-CNC was a favorable process. Moreover, Table 2 shows that the maximum uptake capacity of both CNC and MA-CNC adsorbents was 75.76 and 215.52 mg/g, respectively.where qmax is the maximum removal capability of Cd(II) ions per unit mass of adsorbent (mg g−1), kf is the adsorption capability of the CNC and MA-CNC sorbents (Lmg−1), b is the Langmuir constant (Lmg−1), and n is the binding intensity. T is the absolute temperature in Kelvin, R is the ideal gas constant (8.314 J mol−1 K−1), and kC is the equilibrium constant calculated by multiplying the Cd(II) molar weight with Langmuir constant (b).Figure 9
Langmuir (a) and Freundlich (b) adsorption isotherm for the removal of Cd(II) ions, respectively, atCi = 30 mg/L, pH = 6, adsorbent dose = 1 g, contact time = 120 min, and agitation speed = 250 rpm.
(a)(b)Table 2
Langmuir and Freundlich isotherm constants for Cd(II) ion adsorption by CNC and MA-CNC sorbent at 25°C.
Adsorption isothermLangmuir modelFreundlich modelAdsorbentsQmax (mg/g)bRLR2kfnR2(ΔG°)CNC75.760.430.1040.9770.933.570.936−1.576MA-CNC215.520.0830.6020.9770.911.970.932−0272(6)CeQe=1bQmax+CeQmax,(7)RL=11+bC0,(8)logqe=logkf+1nlogCe,(9)ΔGo=−RTlnkC,The thermodynamic study of the Cd(II) ion removal process was conducted using the standard thermodynamic parameter, such as Gibbs free energy (ΔG°). The Gibbs free energy (ΔG°) of the Cd(II) ion adsorption by CNC and MA-CNC was calculated using equation (9). Table 2 presents the calculated Gibbs free energy values of Cd(II) ions. The values of this thermodynamic parameter were determined at temperatures of 20, 30, and 45°C; the optimum temperature was found to be 20°C. The higher value of ΔG° change occurred at the operational temperature of 25°C. This suggests that the adsorption efficiency increases by decreasing the temperature, and the negative value for ΔG° confirms that the removal process of Cd(II) ions was spontaneous and feasible.


### 3.6. Uptake Kinetics

The kinetics of Cd(II) ion removal by CNC and MA-CNC sorbents is established using linearized pseudo-first-order (PFO) (equation (10)) and pseudo-second-order (PSO) (equation (11)), respectively, and given in Figure 10.(10)logqe−qt=logqe−K1t2.303,(11)tqt=1K2qe2+tqe.Figure 10
Plot of the PFO (a) and PSO (b) model (atC0 = 30 mg/L, pH = 6, adsorbent dose = 1 g, contact time = 120 min, and agitation speed = 250 rpm) for Cd(II) ion removal, respectively.
(a)(b)TheR2 value obtained using the PFO kinetic model was too poor at both the initial removal stage and final removal stage because the experimental qe value is much different from the calculated qe value for both sorbents. This phenomenon indicates that the adsorption kinetics does not follow this model. Therefore, Figures 10(a) and 10(b) designate a representative fitness of the data corresponding to PSO for Cd(II) ion adsorption by CNC and MA-CNC sorbents, and this suggests that the adsorption process was more chemisorption. This result was in agreement with the research reported by Priyadarshini et al. [60] on kinetics, thermodynamics, and isotherm studies on adsorption of eriochrome black-T from aqueous solution using Rutile TiO2. Furthermore, this result was in agreement with the research reported by Tsade et al. [61] on Pb(II) ion remediation using Fe–Al-MC nanocomposite. The kinetic data are provided in Figures 7(a) and 7(b) and presented in Table 3. The kinetic model provides maximum correlation coefficient value (R2 = 0.998 and 0.995, for PSO) and below satisfactory correlation coefficient value (R2 = 0.576 and 0.830, for PFO) in CNC and MA-CNC sorbents for Cd(II) ion removal, respectively. Therefore, the study indicated that the PSO model better represents the Cd(II) ion adsorption kinetics, suggesting that more of the removal processes are chemisorption.Table 3
The values of parameters and correlation coefficients of pseudo-second-order (PFO) and pseudo-second-order (PSO) kinetics.
KineticsPFOPSOqe. cal. (mg/g)qe. exp. (mg/g)K1R2qe. cal. (mg/g)qe. exp. (mg/g)K2R2CNC1.042.060.160.5789.939.370.0740.998MA-CNM1.293.230.3400.83014.6814.960.0300.995


### 3.7. Adsorption Mechanism

The probable mechanism of Cd(II) ion uptake by CNCs is schematically represented in equation (12) and Figure 11. Results from this figure have presented that the hydroxyl, carbonyl, and carboxyl groups are principally accountable for the uptake of Cd(II) ions:(12)Cd2+aq+ROH,CO,COOH⟶CdROH,CO,COOH2+.Figure 11
Adsorption mechanism of Cd(II) ion removal by CNCs.This adsorption mechanism was performed via electrostatic interactions between the Cd(II) ions and the hydroxyl, carbonyl, and carboxyl groups, and the chemical activity of these functional groups on the surface of CNCs contributes to the uptake process.


### 3.8. Recycling Test

As a result of cost-effectiveness, the recycling of a provided adsorbent is considered the best skill for the applications of industrial and commercial cases. For this purpose, a series of recycling experiments were conducted after the removal processes to convince the regenerated adsorbent for numerous use. Thus, due to the high adsorption capability of the sorbent materials, the MA-CNC sorbent was nominated for regeneration study. The desorption and regeneration experiments are done by evaluating the %R of Cd(II) ions after the 1st, 4th, and 13th cycles and presented in Figure 12. Regeneration assessments were performed to validate the reusability of the material for real-world applications. Before the regeneration study, the desorption study of the Cd(II) ions for the sorbents with 0.1 M HCl solution was performed using batch experiments. It is found that the sorption capability of Cd(II) ions for MA-CNC sorbent gradually reduced with increasing the cycles of reusable tests. The decrease in adsorption ability of the sorbent with increased regularity of reusability times is normal, because of the loss of fresh active surface areas on the MA-CNC sorbent [62]. However, it was found that the removal ability of the MA-CNC sorbent did not expressively change after the 13th cycle of experiments as the %R was yet pronounced. The decreases in %R for the 13th consecutive cycle were no more than 5%. From this, it is possible to deduce that MA-CNC can be used for heavy metal removal for a long time with an outstanding possibility. The results were in agreement with the review study conducted by Liu et al. and Chu et al. [10, 63] on the removals of heavy metals from wastewater by using molybdenum disulfide sorbent.Figure 12
Percentage of Cd(II) ions’ removal after different cycles (1st, 4th, and 13th) by MA-CNC sorbent.


## 3.1. Characterization

Both the CNC and MA-CNC sorbents were characterized by using modern instrumental techniques, such as FTIR, XRD, and SEM. The identification of functional groups and surface characteristics of the as-prepared CNM and MA-CNC sorbents were carried out by using FTIR spectroscopy. The spectra of CNC and MA-CNC sorbents prepared with the help of sulfuric acid hydrolysis obtained from the FTIR spectroscopy are shown in Figure3(a). The results revealed that both CNC and MA-CNC have representative broadband around 3355 cm−1 which corresponds to O-H free stretching vibration of the CH2-OH structure on cellulose I and OH groups [40]. The spectra located at 2925 cm−1 are as a result of C-H stretching vibration in cellulose I, and the spectra found in zone four at 1735 cm−1 are recognized to the carbonyl functional groups of cellulose I. The peaks detected at 1458 cm−1 are correlated to the C-C stretching and/or CH2 symmetric bending in aromatic groups of cellulose I. The peak located at 1058 cm−1 is connected to the C-O-C stretching of cellulose I [41]. Compared with the spectrum of raw CNC, additional peaks observed in the oxidized cellulose nanomaterial (MA-CNC) at 1428 cm−1, referring to the stretching vibration of the ionic carboxylic groups, confirmed the insertion of carboxylic groups on the surface of CNC sorbent. Also, the spectra at 1265–1325 cm−1 are indications of the presence of C-O-C groups on the sorbent. This makes maleic anhydride efficaciously oxidize the adjacent hydroxyl groups of cellulose at locations of carbon numbers 2 and 3 into aldehyde groups, concurrently breaking the corresponding carbon-carbon bond of the glucopyranose ring in order to obtain DACNC.Figure 3
(a) FTIR spectra, (b) XRD pattern, and (c, d) SEM images of CNC and MA-CNC sorbents, respectively.
(a)(b)(c)(d)The CNC and MA-CNC sorbent crystalline particle size was determined by using the XRD diffractogram (Figure3(b)). The crystallographic planes of cellulose I structure were certainly fixed to the peaks attributed at 2θ = 15.87°, 22.50°, and 34.82° are (110), (110), and (004), respectively [42]. From the XRD patterns, the pristine CNM sorbent has the same peaks as that of the esterified (MA-CNC) except for the increased degree of crystallinity for the CNC sorbent (Figure 3(b)). Despite the increased degree of crystallinity for the CNC sorbent, both sorbents undoubtedly displayed the amorphous nature in contrast to 100% crystallinity because of the polymeric nature of Eichhornia crassipes. The diffractogram of CNC and MA-CNC sorbents has an obvious sharp band focused at 22.50° attributed to the semicrystalline structure of the cellulose-based sorbents. The functionalized nanocellulose exhibited a reduced percent of crystallinity and broad peak than the raw CNM because of the oxidation of the crystalline region by the addition of maleic anhydride into the raw nanocellulose suspension [43].Both CNC and MA-CNC sorbent microstructures and surface morphologies were done using SEM instruments (Figures3(c) and 3(d)). The image from the SEM micrograph shows that both CNM and MA-CNM sorbents were cylindrical rod-like shapes. From the SEM image, MA-CNC sorbent was probable to agglomerate in comparison with CNC after drying. In MA-CNC adsorbents, the produced carbonyl groups might also encourage the presence of hydrogen bond structures in the MA-CNC sorbents. These variations in biochemical arrangements also caused the variations in surfaces of DACNC [44, 45].Brunauer–Emmett–Teller (BET) data investigation is accomplished according to the BET adsorption isotherm linear equation (4) to determine the specific surface area of CNC and MA-CNC adsorbents. Its measurement was carried out using N2 gas as an adsorbate at a temperature of 77 K.(4)p/pon1−p/po=C−1XmCp/po+1XmC,where Po and P are saturated and partial vapor pressure of N2 gas at equilibrium in Pa, respectively; n is the volume of N2 gas adsorbed at STP in mL; Xm is BET monolayer capacity; C is a dimensionless constant associated with the enthalpy of N2 gas adsorption on the adsorbent.For the well-defined BET monolayer capacity of the nanoparticle materials, the value of C should be ≥80 [46]. Thus, from the given equation (4), it is possible to obtain the C value of NaIO4-NC (188.3 and 190.2) which is ≥80. Figure 4(a) indicates the linear plots of [(P/Po)/(n(1 − P/Po))] versus P/Po and provides a straight line with the approximate relative pressure ranging from 0.05 to 0.3. The linear regression value (R2) obtained from this plot was 0.9985, which is greater than 0.995. This result confirms the acceptability level of the R2 value. The specific surface area (SSA) in m2·g−1 is calculated according to(5)as=XmLσmm×22400,where as is the BET specific surface area of the NaIO4-NC of mass m in grams, L is the Avogadro constant (6.022 × 1023 mol−1), σm is the molecular adsorptive cross-sectional area occupied by N2 gas molecule in the complete monolayer (equal to 0.162 nm2 for N2 gas), and 22400 is the volume occupied by 1 mole of N2 gas at STP, in mL.Figure 4
(a) The linear plot of CNC and MA-CNC and (b) the BET plot of CNC and MA-CNC adsorbents.
(a)(b)The BET plot of CNC and MA-CNC sorbents, respectively, in Figure4(b) has indicated the cylindrical shape model. The symbols used were those given in the 2007 edition of the IUPAC manual [47]. Results indicated that the as-prepared CNC and MA-CNC adsorbents have a higher SSA of 108.2 and 123.9 m2g−1, respectively. Therefore, CNC and MA-CNC adsorbents have shown higher Cd(II) ion adsorption efficiency due to the decrease of the particle size, an increase of specific surface area, and the increase of surface roughness.


## 3.2. Physicochemical Properties of the WW

The collected WW physicochemical property measurements are performed within 24 hours after collection and given in Table1. Values for pH and electrical conductivity were determined in different series and reported as average values of 7.5 ± 0.05 and 265 ± 0.3, respectively. These results have shown that WW taken from the run of Modjo Rivers was nearly neutral. Furthermore, the average concentrations of COD, BOD, TP, TIN, nitrate (NO3−), (NH4+), Mg2+, Cu2+, and Cd2+ in the WW were 51.4 ± 0.2, 36.75 ± 0.02, 11.44 ± 0.3, 43.05 ± 0.02, 5.04 ± 0.05, 29.5 ± 0.02, 50.9 ± 0.6, 0.43 ± 0.03, and 0.12 ± 0.04, respectively.Table 1
Physicochemical properties of the SERWW used in the study.
ParameterLowest valueMaximum valueAveragepH6.9 ± 0.058.3 ± 0.057.5 ± 0.05EC(μS cm−1)260 ± 0.3270 ± 0.3265 ± 0.3COD (mg/L)42.25 ± 0.260.5 ± 0.251.4 ± 0.2BOD (mg/L)30.4 ± 0.0242.8 ± 0.0236.75 ± 0.02TIN (mg/L)31.5 ± 0.0254.6 ± 0.0243.05 ± 0.02NO3− (mg.N/L)4.3 ± 0.055.8 ± 0.055.04 ± 0.05NH4+ (mg.N/L)26.7 ± 0.0232.3 ± 0.0229.5 ± 0.02TP (mg/L)10.2 ± 0.312.6 ± 0.311.44 ± 0.3Mg2+ (mg/L)41.5 ± 0.660.3 ± 0.650.9 ± 0.6Cu2+ (mg/L)0.30 ± 0.030.56 ± 0.030.43 ± 0.03Cd2+ (mg/L)0.08 ± 0.040.16 ± 0.040.12 ± 0.04TP: total phosphorus; TIN: total inorganic nitrogen; BOD: biological oxygen demand; COD: chemical oxygen demand.


## 3.3. Adsorption Studies

### 3.3.1. Effects of Contact times

Experiments for contact time effects on the removal of Cd(II) ions from wastewater were conducted by using the contact times ranging from 30 to 180 min at optimum CNC and MA-CNC dose of 0.5 g, temperature (T) of 20°C, and initial Cd(II) ions concentration of 20 mg L−1 (Figure 5(b)). The results have shown that the Cd(II) ion removal capacity increases by increasing the contact time from 30 to 120 min for both CNC and MA-CNC sorbents because of the increased number of active sites available on the surfaces of CNC and MA-CNC sorbents. The maximum % removal (%R) of Cd(II) ions of 67.80 and 88.84% was observed at the optimum contact time of 120 min for CNC and MA-CNC adsorbents, respectively. After 120 min., the Cd(II) ions %R remains unchanged because, with the increased contact time, the ratio of surface active sites to the total metal ions in the solution was low, and hence, all active sites had metal ions in solution and were occupied [48, 49]. In comparison to MA-CNC sorbent with CNC, the maximum Cd(II) ion uptake capabilities were observed for MA-CNC sorbent than CNC because of the increased number of active sites resulting from the esterification reaction of maleic anhydride. This result was in agreement with research reported by Madivoli et al. [49].Figure 5
The effect of initial concentration (a) and contact time (b) for the removal of Cd(II) ions from wastewater, respectively, at an optimum temperature of 20°C, adsorbent dosage of 0.5, solution pH of 8, and agitation speed of 250 rpm.
(a)(b)


### 3.3.2. Effects of Initial Concentration

The effect of the initial concentration of Cd(II) ions against quantity adsorbed was conducted by using the optimum quantity of CNC and MA-CNC sorbents of 0.5 g, pH of 8, and the contact time of 120 min (Figure5(a)). At the starting point, the Cd(II) ion removal process was very rapid until the optimum value of 20 mg/L. At this stage, the ratio of surface active sites to the total metal ions in the solution was high, and hence, all Cd(II) ions are attracted to the surfaces of CNC and MA-CNC adsorbents [50]. At the optimum initial Cd(II) ion concentration of 20 mg L−1, both adsorbents clearly have shown higher Cd(II) ions %R of 64.91 and 88.44 from WW by CNC and MA-CNC adsorbents, respectively. Additionally, the higher %R of Cd(II) ions is evidently detected for MA-CNC sorbent relative to CNC adsorbent. This is because the presence of extra active sites on the MA-CNC adsorbent resulted from the esterification reaction of CNC [51, 52].


### 3.3.3. Effects of Adsorbent Dose and Temperature

The effects of CNC and MA-CNC dose on the %R of Cd(II) ions from WW at different temperatures,T = 20, 30, and 45°C, were investigated, and the results are shown in Figure 5. Results have indicated that Cd(II) ion uptake ability was increased by increasing the CNC and MA-CNC adsorbent dose. This publicized that the uptake sites become unsaturated during the adsorption reaction, whereas the number of active surface areas available for the adsorption site increased by increasing the CNC and MA-CNC adsorbent dose. The maximum %R of 70.3 and 90.4 was observed at optimum CNC and MA-CNC adsorbent dose of 0.5 g and optimum temperature of 20°C, respectively. After this dose value, the %R becomes unchanged because of the particle aggregation, which would lead to a decrease in the total surface area of the adsorbent [53]. A higher %R of 90.4% was observed by using functionalized adsorbent than CNC because the esterification reaction provides the extra-functional groups on the adsorbent surface that make the functionalized adsorbent most active to adsorb Cd(II) ions onto the surface than a pristine one.Figures6(a) and 6(b) show the temperature effects on the %R of Cd(II) ions from WW by CNC and MA-CNC sorbents. Results have shown that the decreased %R of Cd(II) ions was observed at the higher temperature of 45°C. This is because, at increased temperature, the slow rate of the chemisorption processes prevents the Cd(II) ions to react with the active sites of the sorbent surface for increased %R of Cd(II) ions from wastewater [54]. For both CNC and MA-CNC adsorbents, the maximum %R of 70.3% and 90.4% was detected at the optimum dose and temperature of 0.5 g and 20°C, respectively. Furthermore, the higher %R of Cd(II) ions was observed by using MA-CNC sorbents than CNC sorbents due to the presence of extra-functional groups on the modified one [55].Figure 6
(a, b) Effects of adsorbent dose at different temperatures (20, 30, and 45°C) for Cd(II) ions’ remediation using CNC and MA-CNC adsorbents, respectively, at an optimum contact time of 120 min, agitation speed of 250 rpm, pH of 8, and initial concentration of 20 mg/L.
(a)(b)


### 3.3.4. Effects of Solution pH

The effect of solution pH on Cd(II) ions removal from WW was performed by using pH values ranging from 2 to 12. As shown in Figure7(b), both CNC and MA-CNC adsorbents show the increasing removal abilities in the solution pH ranging from 2 to 8. The maximum %R for both CNC and MA-CNC adsorbents was 70.3 and 89.9%, respectively. At decreased solution pH amounts, the interaction of Cd(II) ions with adsorbents is declined because of the competition of H+ ions on the surfaces of the adsorbents [50]. Conversely, at the increased solution pH, Cd(II) ions binding to the CNC and MA-CNC adsorbents surfaces rise until the equilibrium pH of 8. After the optimum pH value of 8, the %R becomes declined due to the presence of increased amounts of OH− ions in WW. The increased OH− ions depict the formation of soluble hydroxyl complexes. Furthermore, at a higher alkaline pH value, the Cd(II) ions precipitate as Cd(OH)2. Figure 7(a) also shows that the higher %R of Cd(II) ions was observed by MA-CNC adsorbent than CNC sorbents at the optimum solution pH value of 8. The differences in the reported %R for the Cd(II) ions were related to the occurrence of additional functional groups in the structure of MA-CNC adsorbents with different affinity to Cd(II) ions than CNC sorbent [56].Figure 7
The effect of pH (a) and agitation speed (b) for the removal of Cd(II) ions from wastewater at an optimum initial concentration of 2 mg/L, contact time of 120 min, temperature of 20°C, and adsorbent dosage of 0.5 g, respectively.
(a)(b)


### 3.3.5. Effects of Agitation Speed

The effect of agitation speed on the removal of Cd(II) ions is shown in Figure7(b). Initially, the agitation speed was slow, but as the agitation speed was increased subsequently, a rapid increase in the removal capability of Cd(II) ions was observed. This is due to the presence of more active sites existing on the binding surface of the adsorbent that is ready to adsorb Cd(II) ions [57]. Thus, the %R capacity of Cd(II) ions by MA-CNC adsorbent was increased from 72.2 to 88.55% as the agitation speed was increased from 100 to 250 rpm. In the same way, the Cd(II) ion %R capability of the CNC sorbent was increased from 34.65 to 67.17% as the agitation speed was increased from 100 to 250 rpm (Figure 7(b)). From this point of view, the %R capability of CNC adsorbent was low compared to MA-CNC adsorbent removal capability. This higher %R capability observed by MA-CNC adsorbent is due to the presence of more accessible surfaces resulting from the addition of maleic anhydride into the CNC. For both sorbents, the maximum Cd(II) ion %R capability was obtained at the optimum agitation speed of 250 rpm. This result was in agreement with the study reported by Mahmood et al. [58]. Generally, an increase in the speed of agitation speed resulted in outstanding pollutant uptake capabilities and the agitation helps in overcoming the resistance of external mass transfer.


## 3.3.1. Effects of Contact times

Experiments for contact time effects on the removal of Cd(II) ions from wastewater were conducted by using the contact times ranging from 30 to 180 min at optimum CNC and MA-CNC dose of 0.5 g, temperature (T) of 20°C, and initial Cd(II) ions concentration of 20 mg L−1 (Figure 5(b)). The results have shown that the Cd(II) ion removal capacity increases by increasing the contact time from 30 to 120 min for both CNC and MA-CNC sorbents because of the increased number of active sites available on the surfaces of CNC and MA-CNC sorbents. The maximum % removal (%R) of Cd(II) ions of 67.80 and 88.84% was observed at the optimum contact time of 120 min for CNC and MA-CNC adsorbents, respectively. After 120 min., the Cd(II) ions %R remains unchanged because, with the increased contact time, the ratio of surface active sites to the total metal ions in the solution was low, and hence, all active sites had metal ions in solution and were occupied [48, 49]. In comparison to MA-CNC sorbent with CNC, the maximum Cd(II) ion uptake capabilities were observed for MA-CNC sorbent than CNC because of the increased number of active sites resulting from the esterification reaction of maleic anhydride. This result was in agreement with research reported by Madivoli et al. [49].Figure 5
The effect of initial concentration (a) and contact time (b) for the removal of Cd(II) ions from wastewater, respectively, at an optimum temperature of 20°C, adsorbent dosage of 0.5, solution pH of 8, and agitation speed of 250 rpm.
(a)(b)


## 3.3.2. Effects of Initial Concentration

The effect of the initial concentration of Cd(II) ions against quantity adsorbed was conducted by using the optimum quantity of CNC and MA-CNC sorbents of 0.5 g, pH of 8, and the contact time of 120 min (Figure5(a)). At the starting point, the Cd(II) ion removal process was very rapid until the optimum value of 20 mg/L. At this stage, the ratio of surface active sites to the total metal ions in the solution was high, and hence, all Cd(II) ions are attracted to the surfaces of CNC and MA-CNC adsorbents [50]. At the optimum initial Cd(II) ion concentration of 20 mg L−1, both adsorbents clearly have shown higher Cd(II) ions %R of 64.91 and 88.44 from WW by CNC and MA-CNC adsorbents, respectively. Additionally, the higher %R of Cd(II) ions is evidently detected for MA-CNC sorbent relative to CNC adsorbent. This is because the presence of extra active sites on the MA-CNC adsorbent resulted from the esterification reaction of CNC [51, 52].


## 3.3.3. Effects of Adsorbent Dose and Temperature

The effects of CNC and MA-CNC dose on the %R of Cd(II) ions from WW at different temperatures,T = 20, 30, and 45°C, were investigated, and the results are shown in Figure 5. Results have indicated that Cd(II) ion uptake ability was increased by increasing the CNC and MA-CNC adsorbent dose. This publicized that the uptake sites become unsaturated during the adsorption reaction, whereas the number of active surface areas available for the adsorption site increased by increasing the CNC and MA-CNC adsorbent dose. The maximum %R of 70.3 and 90.4 was observed at optimum CNC and MA-CNC adsorbent dose of 0.5 g and optimum temperature of 20°C, respectively. After this dose value, the %R becomes unchanged because of the particle aggregation, which would lead to a decrease in the total surface area of the adsorbent [53]. A higher %R of 90.4% was observed by using functionalized adsorbent than CNC because the esterification reaction provides the extra-functional groups on the adsorbent surface that make the functionalized adsorbent most active to adsorb Cd(II) ions onto the surface than a pristine one.Figures6(a) and 6(b) show the temperature effects on the %R of Cd(II) ions from WW by CNC and MA-CNC sorbents. Results have shown that the decreased %R of Cd(II) ions was observed at the higher temperature of 45°C. This is because, at increased temperature, the slow rate of the chemisorption processes prevents the Cd(II) ions to react with the active sites of the sorbent surface for increased %R of Cd(II) ions from wastewater [54]. For both CNC and MA-CNC adsorbents, the maximum %R of 70.3% and 90.4% was detected at the optimum dose and temperature of 0.5 g and 20°C, respectively. Furthermore, the higher %R of Cd(II) ions was observed by using MA-CNC sorbents than CNC sorbents due to the presence of extra-functional groups on the modified one [55].Figure 6
(a, b) Effects of adsorbent dose at different temperatures (20, 30, and 45°C) for Cd(II) ions’ remediation using CNC and MA-CNC adsorbents, respectively, at an optimum contact time of 120 min, agitation speed of 250 rpm, pH of 8, and initial concentration of 20 mg/L.
(a)(b)


## 3.3.4. Effects of Solution pH

The effect of solution pH on Cd(II) ions removal from WW was performed by using pH values ranging from 2 to 12. As shown in Figure7(b), both CNC and MA-CNC adsorbents show the increasing removal abilities in the solution pH ranging from 2 to 8. The maximum %R for both CNC and MA-CNC adsorbents was 70.3 and 89.9%, respectively. At decreased solution pH amounts, the interaction of Cd(II) ions with adsorbents is declined because of the competition of H+ ions on the surfaces of the adsorbents [50]. Conversely, at the increased solution pH, Cd(II) ions binding to the CNC and MA-CNC adsorbents surfaces rise until the equilibrium pH of 8. After the optimum pH value of 8, the %R becomes declined due to the presence of increased amounts of OH− ions in WW. The increased OH− ions depict the formation of soluble hydroxyl complexes. Furthermore, at a higher alkaline pH value, the Cd(II) ions precipitate as Cd(OH)2. Figure 7(a) also shows that the higher %R of Cd(II) ions was observed by MA-CNC adsorbent than CNC sorbents at the optimum solution pH value of 8. The differences in the reported %R for the Cd(II) ions were related to the occurrence of additional functional groups in the structure of MA-CNC adsorbents with different affinity to Cd(II) ions than CNC sorbent [56].Figure 7
The effect of pH (a) and agitation speed (b) for the removal of Cd(II) ions from wastewater at an optimum initial concentration of 2 mg/L, contact time of 120 min, temperature of 20°C, and adsorbent dosage of 0.5 g, respectively.
(a)(b)


## 3.3.5. Effects of Agitation Speed

The effect of agitation speed on the removal of Cd(II) ions is shown in Figure7(b). Initially, the agitation speed was slow, but as the agitation speed was increased subsequently, a rapid increase in the removal capability of Cd(II) ions was observed. This is due to the presence of more active sites existing on the binding surface of the adsorbent that is ready to adsorb Cd(II) ions [57]. Thus, the %R capacity of Cd(II) ions by MA-CNC adsorbent was increased from 72.2 to 88.55% as the agitation speed was increased from 100 to 250 rpm. In the same way, the Cd(II) ion %R capability of the CNC sorbent was increased from 34.65 to 67.17% as the agitation speed was increased from 100 to 250 rpm (Figure 7(b)). From this point of view, the %R capability of CNC adsorbent was low compared to MA-CNC adsorbent removal capability. This higher %R capability observed by MA-CNC adsorbent is due to the presence of more accessible surfaces resulting from the addition of maleic anhydride into the CNC. For both sorbents, the maximum Cd(II) ion %R capability was obtained at the optimum agitation speed of 250 rpm. This result was in agreement with the study reported by Mahmood et al. [58]. Generally, an increase in the speed of agitation speed resulted in outstanding pollutant uptake capabilities and the agitation helps in overcoming the resistance of external mass transfer.


## 3.4. The Chemistry of Wastewater

Table1 indicates the summary of the assessment carried out to determine the consequences of wastewater chemistry on the %R of Cd(II) ions. Experiments were performed using wastewater samples containing both synthetic and real wastewater at variable levels. Trials were performed in triplicate and reported as average values. From the experiments, the values for pH, COD, BOD, Cl−, SO4−, Fe2+, Ca2+, Mg2+, and (Cu2+) present in WW were determined using replicate of experiments and reported as the average values. The %R of the Cd(II) ions from both synthetic and real wastewater is represented in Figure 8. From the findings, it was possible to see that the removal processes were negatively affected by the presence of cations and anions in real wastewater. The lowering of the %R of Cd(II) ions in the real wastewater has resulted from the competition of cations and anions for the active sites in the real wastewater. The consequence of competing ions diminishes the interaction of fresh surfaces on MA-CNM adsorbent and the decreased %R of Cd(II) ions was observed [59]. Results indicated that the %R Cd(II) ions from WW were found to be 99.9 and 89.5% for the synthetic and real wastewater, respectively, by MA-CNC adsorbent.Figure 8
The effects of wastewater chemistry for both synthetic and real wastewater on the percent removal of Cd(II) ions at 20 mg/L and 20°C by using MA-CNC adsorbent.


## 3.5. Adsorption Isotherms

To appreciate the mechanism of Cd(II) ions uptake by CNC and MA-CNC adsorbents, Langmuir (equation (7)) and Freundlich (equation (8)) adsorption isotherms are investigated and presented in Figures 9(a) and 9(b), respectively. Table 2 shows the corresponding parameter values and the correlation coefficient (R2) values, obtained from each plot. Higher R2 values for both Langmuir and Freundlich isotherms have shown that both Langmuir and Freundlich isotherm models better fit the isothermal uptake data. That means, evidently, both of these isotherms describe the distribution of the Cd(II) ions between the liquid and solid stages conferring to prospects connected to the heterogeneity or homogeneity of the adsorbent surface, the category of coverage, and the prospect of contact between the Cd(II) ions. This suggested that the surface of CNC and MA-CNC adsorbents was heterogeneous and physically compatible with monolayer adsorption and the adsorption process was favorable. Moreover, strong electrostatic interactions were formed between the Cd(II) ions and the surfaces of adsorbents [60]. The favorability of the uptake process was due to the n value that lies between 1 and 10, and the strong interactions between the adsorbates and surfaces of the adsorbents were due to the fact that 1/n < 1. The fundamental nature of the Langmuir model could be also determined by a dimensionless equilibrium parameter (RL), and its value was calculated by using equation (6). The values (0.104 and 0.602) of RL < 1 suggested that the uptake process of Cd(II) ions by both CNC and MA-CNC was a favorable process. Moreover, Table 2 shows that the maximum uptake capacity of both CNC and MA-CNC adsorbents was 75.76 and 215.52 mg/g, respectively.where qmax is the maximum removal capability of Cd(II) ions per unit mass of adsorbent (mg g−1), kf is the adsorption capability of the CNC and MA-CNC sorbents (Lmg−1), b is the Langmuir constant (Lmg−1), and n is the binding intensity. T is the absolute temperature in Kelvin, R is the ideal gas constant (8.314 J mol−1 K−1), and kC is the equilibrium constant calculated by multiplying the Cd(II) molar weight with Langmuir constant (b).Figure 9
Langmuir (a) and Freundlich (b) adsorption isotherm for the removal of Cd(II) ions, respectively, atCi = 30 mg/L, pH = 6, adsorbent dose = 1 g, contact time = 120 min, and agitation speed = 250 rpm.
(a)(b)Table 2
Langmuir and Freundlich isotherm constants for Cd(II) ion adsorption by CNC and MA-CNC sorbent at 25°C.
Adsorption isothermLangmuir modelFreundlich modelAdsorbentsQmax (mg/g)bRLR2kfnR2(ΔG°)CNC75.760.430.1040.9770.933.570.936−1.576MA-CNC215.520.0830.6020.9770.911.970.932−0272(6)CeQe=1bQmax+CeQmax,(7)RL=11+bC0,(8)logqe=logkf+1nlogCe,(9)ΔGo=−RTlnkC,The thermodynamic study of the Cd(II) ion removal process was conducted using the standard thermodynamic parameter, such as Gibbs free energy (ΔG°). The Gibbs free energy (ΔG°) of the Cd(II) ion adsorption by CNC and MA-CNC was calculated using equation (9). Table 2 presents the calculated Gibbs free energy values of Cd(II) ions. The values of this thermodynamic parameter were determined at temperatures of 20, 30, and 45°C; the optimum temperature was found to be 20°C. The higher value of ΔG° change occurred at the operational temperature of 25°C. This suggests that the adsorption efficiency increases by decreasing the temperature, and the negative value for ΔG° confirms that the removal process of Cd(II) ions was spontaneous and feasible.


## 3.6. Uptake Kinetics

The kinetics of Cd(II) ion removal by CNC and MA-CNC sorbents is established using linearized pseudo-first-order (PFO) (equation (10)) and pseudo-second-order (PSO) (equation (11)), respectively, and given in Figure 10.(10)logqe−qt=logqe−K1t2.303,(11)tqt=1K2qe2+tqe.Figure 10
Plot of the PFO (a) and PSO (b) model (atC0 = 30 mg/L, pH = 6, adsorbent dose = 1 g, contact time = 120 min, and agitation speed = 250 rpm) for Cd(II) ion removal, respectively.
(a)(b)TheR2 value obtained using the PFO kinetic model was too poor at both the initial removal stage and final removal stage because the experimental qe value is much different from the calculated qe value for both sorbents. This phenomenon indicates that the adsorption kinetics does not follow this model. Therefore, Figures 10(a) and 10(b) designate a representative fitness of the data corresponding to PSO for Cd(II) ion adsorption by CNC and MA-CNC sorbents, and this suggests that the adsorption process was more chemisorption. This result was in agreement with the research reported by Priyadarshini et al. [60] on kinetics, thermodynamics, and isotherm studies on adsorption of eriochrome black-T from aqueous solution using Rutile TiO2. Furthermore, this result was in agreement with the research reported by Tsade et al. [61] on Pb(II) ion remediation using Fe–Al-MC nanocomposite. The kinetic data are provided in Figures 7(a) and 7(b) and presented in Table 3. The kinetic model provides maximum correlation coefficient value (R2 = 0.998 and 0.995, for PSO) and below satisfactory correlation coefficient value (R2 = 0.576 and 0.830, for PFO) in CNC and MA-CNC sorbents for Cd(II) ion removal, respectively. Therefore, the study indicated that the PSO model better represents the Cd(II) ion adsorption kinetics, suggesting that more of the removal processes are chemisorption.Table 3
The values of parameters and correlation coefficients of pseudo-second-order (PFO) and pseudo-second-order (PSO) kinetics.
KineticsPFOPSOqe. cal. (mg/g)qe. exp. (mg/g)K1R2qe. cal. (mg/g)qe. exp. (mg/g)K2R2CNC1.042.060.160.5789.939.370.0740.998MA-CNM1.293.230.3400.83014.6814.960.0300.995


## 3.7. Adsorption Mechanism

The probable mechanism of Cd(II) ion uptake by CNCs is schematically represented in equation (12) and Figure 11. Results from this figure have presented that the hydroxyl, carbonyl, and carboxyl groups are principally accountable for the uptake of Cd(II) ions:(12)Cd2+aq+ROH,CO,COOH⟶CdROH,CO,COOH2+.Figure 11
Adsorption mechanism of Cd(II) ion removal by CNCs.This adsorption mechanism was performed via electrostatic interactions between the Cd(II) ions and the hydroxyl, carbonyl, and carboxyl groups, and the chemical activity of these functional groups on the surface of CNCs contributes to the uptake process.


## 3.8. Recycling Test

As a result of cost-effectiveness, the recycling of a provided adsorbent is considered the best skill for the applications of industrial and commercial cases. For this purpose, a series of recycling experiments were conducted after the removal processes to convince the regenerated adsorbent for numerous use. Thus, due to the high adsorption capability of the sorbent materials, the MA-CNC sorbent was nominated for regeneration study. The desorption and regeneration experiments are done by evaluating the %R of Cd(II) ions after the 1st, 4th, and 13th cycles and presented in Figure 12. Regeneration assessments were performed to validate the reusability of the material for real-world applications. Before the regeneration study, the desorption study of the Cd(II) ions for the sorbents with 0.1 M HCl solution was performed using batch experiments. It is found that the sorption capability of Cd(II) ions for MA-CNC sorbent gradually reduced with increasing the cycles of reusable tests. The decrease in adsorption ability of the sorbent with increased regularity of reusability times is normal, because of the loss of fresh active surface areas on the MA-CNC sorbent [62]. However, it was found that the removal ability of the MA-CNC sorbent did not expressively change after the 13th cycle of experiments as the %R was yet pronounced. The decreases in %R for the 13th consecutive cycle were no more than 5%. From this, it is possible to deduce that MA-CNC can be used for heavy metal removal for a long time with an outstanding possibility. The results were in agreement with the review study conducted by Liu et al. and Chu et al. [10, 63] on the removals of heavy metals from wastewater by using molybdenum disulfide sorbent.Figure 12
Percentage of Cd(II) ions’ removal after different cycles (1st, 4th, and 13th) by MA-CNC sorbent.


## 4. Conclusion

The present work has shown that both CNC and MA-CNC as a cheap adsorbent have a significant adsorption capability toward Cd(II) ions from WW. The achieved results indicate that %R by CNC and MA-CNC adsorbent is affected by the adsorption parameters such as solution pH, contact time, agitation speed, initial Cd(II) ions concentration, and temperature. The maximum adsorption capacities of 75.76 and 215.52 mg L−1 by using both CNC and MA-CNC adsorbents, respectively, were obtained at optimum pH of 8, an adsorbent dose of 0.5 g, agitation speed of 250 rpm initial concentration of 20 mg L−1, and contact time of 150 min. In addition to this, the %R ability of the MA-CNC sorbents toward Cd(II) ions in comparison with the CNC was remarkably enhanced after a maleic reaction with CNC. This is because the proposed mechanisms for the removal process under the optimum condition of MA-CNC sorbent mainly involve the interaction of ester, carboxyl, and hydroxyl groups of cellulose and Cd(II) ions. The Cd(II) ion uptake process for both CNC and MA-CNC sorbent systems was fitted with both Langmuir and Freundlich isotherm models. The rate of the interaction between the Cd(II) ions and CNC and MA-CNC sorbents was described by the PSO kinetic model. The recycling experiment results indicated that the used sorbent was recyclable and economically friendly used for the 13th successive cycle as an adsorbent for contaminant removals. Therefore, on the whole, the obtained results suggested that MA-CNC sorbent is considered as an effective adsorbent for the removal of Cd(II) ions in particular and contaminants in general from the aqueous system.



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