# Utilization of Superparamagnetic Iron Oxide Nanoparticles (SPIONs) Impregnated Activated Carbon for Removal of Hexavalent Chromium

Authors: Aisha Farhana; A. Jenifer Selvarani; Antony V. Samrot; Abdullah Alsrhani; P. Raji; Chamarthy Sai Sahithya; P. J. Jane Cypriyana; P. Senthilkumar; Mok Pooi Ling; Simon Yishak
Journal: Journal of Nanomaterials
 (2022)

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## Abstract

Chromium (Cr) is a toxic heavy metal present in industrial effluent which could cause degenerative diseases on ingestion. Therefore, elimination of Cr from contaminated water becomes essential to preserve and sustain the quality of life. In this study, superparamagnetic iron oxide nanoparticles (SPIONs) were impregnated on activated carbon and checked for enhanced removal of Cr(VI). Thus, granular activated carbon (N-GAC) of mesh size8∗20 was impregnated with SPIONs to produce SPIONs impregnated activated carbon (Sp-GAC) and characterized using UV-VIS spectrophotometer, FT-IR, SEM-EDX, XRD, and VSM. Sp-GAC was found to be possessing superparamagnetic behavior, and it was used in batch adsorption study where the adsorption parameters like pH, concentration of adsorbent, and adsorbent-adsorbate were optimized. It was found that Cr(VI) adsorption was predominant at acidic pH (pH 3) for both cases; moreover, N-GAC showed better adsorption comparatively. Both the N-GAC and Sp-GAC adsorption were found to be obeying to Langmuir.


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## Body

## 1. Introduction

Chromium heavy metal ions are reported as one of the common environmental contaminants of land and natural water bodies [1, 2]. Over the past decades of rapid industrialization, the level of chromium heavy metal ion in environment has increased to an alarming rate, effectively penetrating the lower aquifers [3, 4]. Chromium salts are used by various industries for paints production, wood preservation, cement processing, metallurgy, electroplating, paper production, and majorly for leather tanning [5, 6]. In most cases, the effluents are directly or indirectly discharged into natural water bodies. Chromium heavy metal exists in varied valence or oxidation states such as Cr(0), Cr(III), and Cr(VI) [7], of which hexavalent chromium Cr(VI) are more noxious and causes mutagenesis in plant, animals, and humans [8–10]. Stohs and Bagchi [11] have reported that Cr(VI) formed reactive oxygen species such as superoxide ion, hydrogen peroxide, and hydroxyl radical on reacting with biological reductant like thiols and ascorbate, eventually causing cellular DNA damage due to oxidative stress. And also, Cr(VI) is found to easily enter the cellular membrane by mimicking the isoelectric and isostructural passages of SO42– and HPO42– [12]. Hence, chromium removal from contaminated waters must be resolved with deep concern. Chemical precipitation, adsorption, electrochemical precipitation, ion exchange, and reverse osmosis are the widely followed techniques in industries to eliminate Cr from treated waters [13–17]. Of them, the most easy and feasible technique is adsorption, where the adsorbate (Cr) is confined over the adsorbent by electrostatic or ionic interaction [18]. The other techniques have few limitations such as need of auxiliary chemical agents, expensive installation, energy demands, and management of reduced waste and byproducts [19].Recent efforts in nanotechnology have proved that nanomaterials can also serve as good adsorbents for Cr(VI). The nanostructure offers increased interaction due to increased surface area. Silver nanoparticles are also not much effective when they are used for removal of heavy metals [20]. Parlayici et al. [21] produced nanocarbon tubes (CNTs) installed with activated carbon to remove Cr(VI). According to their report, activated carbon-based nanocarbon tubes showed highest adsorption capacity to 113.29 mg/g than all sphere forms and the adsorption was described with Langmuir isotherm. Iron oxide nanoparticles like SPIONs (superparamagnetic iron oxide nanoparticles) have drawn the attention of many researchers as they can be easily manipulated by externally applied magnetic field. Apart from their wide-ranging applications in targeted drug delivery [22, 23], hyperthermia [24], theragnostic [25, 26], and imaging [27], SPIONs are also employed for removal of heavy metal ions [28]. CNTs impregnated with 10% of iron oxide and aluminium oxides were found to remove Cr(VI) to 100% when the treating solution was maintained at pH 6. It was found that the performance of impregnated CNTs was significantly higher than the raw CNTs. The adsorption under parameters like pH, agitation time, absorbent concentration, and contact time was also checked [29]. Likewise Jain and his coworkers [30] came up with a nanocomposite of activated carbon and Fe3O4. Its adsorption capacity was checked against Cr(VI), Cu(II), and Cd(II) ions where the nanocomposite showed better Cr(VI) removal at acidic pH 2 and pH 6 as the optimal pH for Cu(II) and Cd(II) ions. They further explained the adsorption by Langmuir isotherm as the best fit model and stated that the materials possessed reusability to four adsorption-desorption cycles.According to our earlier report [31], chitosan-coated SPIONs at 10 g/L were found to remove Cr(VI) of 50 ppm to 95% at acidic pH. It was also observed that adsorption of Cr(VI) was greatly influenced by adsorbent concentration, interaction time, and pH. Here, the concept of impregnating SPIONs onto activated carbon was based on the fact that activated carbon is the most commonly used adsorbent material to remove pollutants from water in both industrial and domestic water purifiers. Therefore, commercially available activated carbon was used for impregnation. SPIONs impregnated activated carbon were synthesized by coprecipitation method and characterized by Fourier Transform-Infrared Spectroscopy (FT-IR), Scanning Electron Microscopy–Energy Dispersive X-ray (SEM-EDX), X-ray Diffraction (XRD), and Vibrating Sample Magnetometer (VSM). These impregnated carbon were subjugated for Cr(VI) adsorption, and it was finally evaluated using adsorption isotherms like Langmuir, Freundlich, and Temkin.


## 2. Materials and Methods

### 2.1. Materials and Reagents

The following chemicals and reagents were purchased at analytical grade quality—ferrous chloride (LOBACHEMIE), anhydrous ferric chloride (LOBACHEMIE), ammonium solution (SRL), sodium hydroxide (SRL), hydrochloric acid, acetic acid (RAMKEM), ammonium ferrous sulphate (NH4)2.Fe(SO4)2.6H2O (SRL), diphenyl carbazide (SRL), potassium dichromate (SRL), ascorbic acid (SRL), sodium acetate (anhydrous), and methanol (SRL). The entire study was carried out using nitrogen purged Millipore water.


### 2.2. Synthesis of SPIONs

Iron oxide nanoparticles were synthesized by chemical coprecipitation. 100 mL of 1 M ferric chloride solution and 100 mL of 3 M ferrous chloride solution were prepared separately in nitrogen purged Millipore water. Equal volumes (50 mL) of the prepared precursor solutions were brought into suspension by magnetic agitation for 20 min. Then, the precursor suspension was heated to 60°C. This heat energy is assumed to accelerate the reduction of Fe ions. While heating the precursor solution at 60°C, 75 mL of freshly prepared 8 M NaOH and 25 mL of ammonia solution were added in alternative drops with vigorous mechanical stirring. The addition of reducing agent turned the precursor solution into black precipitate and increased the pH of the mixture. The high alkali pH was neutralized to pH 7 with 1 N HCl washing. Later, the black precipitate which is superparamagnetic iron oxide nanoparticle (SPION) was settled down and collected by applying magnetic field. It was then washed with nitrogen purged Millipore water for several times to remove impurities and then lyophilized [31].


### 2.3. Preparation of SPIONs Impregnated Activated Carbon

Granular activated carbon (N-GAC) of mesh size8∗20 was bought commercially and rinsed for multiple times with distilled water until the spent water becomes clear. This removed the carbon dust and impurities present. The washed activated carbon was dried on a filter paper and then heated to 80°C to remove moisture. 40 g activated carbon (N-GAC) was added with the iron precursor solution and subjected for SPION production as described above in the way to incorporate SPIONs. Then, it was heated to 60°C and stirred by magnetic agitation for 20 min. By doing so, the carbon and the pores within would get completely wet with the iron ions. Then, the reducing agents NaOH and ammonia were added simultaneously in drops with vigorous mechanical stirring. This leads to formation of SPIONs onto the surface as well as within the pore of the activated carbon. Thus, the carbon was impregnated with SPIONs. Finally, the carbon was filtered out using a nylon mesh filter and washed with Millipore water until the filtrate becomes clear and neutral (pH 7). The granular activated carbon impregnated with SPIONs (Sp-GAC) was used after freeze drying.


### 2.4. Characterization of SPIONs and SPIONs Impregnated Activated Carbon

SPIONs, N-GAC, and Sp-GAC were characterized by performing the following analysis: FT-IR (IR affinity-1S, Shimadzu, Japan), Scanning Electron Microscopy (SEM) (Carl Zeiss, Germany), Energy Dispersive X-ray (EDX) analysis, and XRD (Rigaku, Tokyo), where the SPIONs and Sp-GAC were subjected for Vibrating Sample Magnetometer (VSM) with a maximum magnetic field of 2.5 T and dynamic moment range of1×10e−6 emu-10e3 emu (Lakeshore, USA, Model 7407).


### 2.5. Quantification of Iron Impregnated onto Activated Carbon

#### 2.5.1. Establishment of Standard Iron Curve

3.511 g of ammonium ferrous sulphate (NH4)2.Fe(SO4)2.6H2O (which contains 500 mg of Fe) in 1 L of nitrogen purged Millipore water was used as standard iron stock solution for 500 ppm. On diluting the stock, different parts per million (ppm) of iron solution was prepared and photometrically detected the total iron in accordance with Changzhao et al. [32]. Standard was prepared and made up to 0.5 mL with water and then with 6.8 mL of Millipore water, 0.2 mL of ascorbic acid (5 g in 50 mL), and 2 mL of sodium acetate buffer (16.4 g of sodium acetate in 24% acetic acid). Then, the reaction mixture was pipetted with 1 ml of 1,4 phenanthroline reagent (0.1%) and vortexed. The absorbance was photometrically read at 510 nm. A graph was plotted having the concentration in ppm as X-axis and absorbance as Y-axis.


#### 2.5.2. Estimation of Total Iron Impregnated on activated carbon Using 1,4 Phenanthroline

To detect total iron impregnated on activated carbon, different concentrations of each sample (N-GAC and Sp-GAC) such as 10 mg, 30 mg, and 50 mg were treated with 10 mL of 10% H2SO4 for 24 h. After acid digestion, 0.5 mL of solution from each sample was processed (as prescribed above) for photometric detection with 1,4 phenanthroline at 510 nm and concentration was calculated from standard graph.


### 2.6. Preparation of Cr(VI) Solution

For the study, different ppm concentrations of chromium were prepared using potassium dichromate as the chromium salt. 0.14 g of potassium dichromate (K2Cr2O7) in 100 mL of Millipore water corresponds to 500 ppm; further dilution was done to obtain 5 ppm of chromium solution (adsorbate).


#### 2.6.1. Establishment of Standard Cr(VI) Curve

Different ppm concentrations of chromium solution were prepared by diluting the stock solution. Diphenyl carbazide (DPC) is a compound that binds exclusively to hexavalent chromium ions; and therefore, it acts as an indicator of hexavalent chromium. On binding with hexavalent chromium ions, the reacting mixture turns reddish violet colour [33, 34]. An aliquot of Cr solution from each dilution was reacted with DPC reagent for colour development. Then, it was spectrophotometrically read at 540 nm. A graph was plotted having ppm in X-axis vs. OD at 540 nm in Y-axis.


### 2.7. Adsorption Study in Batch Experimental System

Chromium removal by different adsorbents was studied in batch system, and the parameters like concentration of adsorbent, concentration of adsorbate, and pH were optimized. Here, the adsorption study was considered for a particular period, i.e., 0th min to 120th min. All the batch setups were placed on rotatory shaker at 200 rpm in room temperature.


#### 2.7.1. Effect of pH

To identify the activity of adsorbents against Cr ions at different pH, the adsorption was checked at a pH range of 3, 5, 7, 9, 11, and 13. 1 M HCl and 1 M NaOH prepared in Millipore water were used to adjust the pH of the Cr(VI) solution to a respective range. To each flask with 100 ml of 5 ppm Cr(VI) at different pH, 10 g/L of N-GAC and Sp-GAC was added separately and placed in shaker at 200 rpm for 2 h. After incubation, the supernatant from each setup was spectrophotometrically read at 540 nm. The final concentration of Cr in the solution was calibrated from the standard curve. % removal was calculated from the below formula:(1)%removal=initialconcentration−finalconcentrationinitialconcentration×100.To check the concentration of iron leached out from the adsorbent material, 0.5 mL of the supernatant was acid digested with 0.2 ml of H2SO4 and later, it was tagged with the reagent 1,4 phenanthroline by following the above described method in Section 2.5.1. The iron released was estimated from the standard. The final data were made into a graph with X-axis as pH, primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm).


#### 2.7.2. Optimization of Adsorbent Concentration

Different concentrations (1 g/L to 10 g/L) of the adsorbents N-GAC and Sp-GAC were added to 100 ml of 5 ppm Cr(VI) solution at optimal pH (from above results). It was allowed to react for 2 h by constantly shaking at 200 rpm. Later, an aliquot of treated solution from each set was processed for DPC tagging and read at 540 nm. % removal of Cr and iron leached into the reaction mixture was also estimated from standard curve. A graph was plotted with adsorbate concentration asX-axis, % removal as primary Y-axis, and iron leached as secondary Y-axis.


#### 2.7.3. Optimization of Adsorbate-Adsorbent Concentration

Here, the efficiency of the adsorbents N-GAC and Sp-GAC at 10 g/L in removal of maximum concentration of adsorbate was determined. It was performed with a fixed concentration of adsorbent against varied concentration of adsorbate. 10 g/L of N-GAC was added to each of 100 mL of Cr(VI) solution at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. All the different concentrations of adsorbate were prepared at the optimal pH. Similar reaction setup was made for the adsorbent, Sp-GAC. They were kept on shaker at 200 rpm for 2 h. After treatment, the % removal of Cr was estimated spectrophotometrically by the DPC method (540 nm). Parallelly, 0.5 ml of each of the supernatant was reacted with 1,4 phenanthroline after acid digestion to quantify (in ppm) the concentration of iron leached from the adsorbents. The graph was plotted between % removal (X-axis), adsorbate concentration (primary Y-axis), and iron leached (secondary Y-axis).


### 2.8. Adsorption Isotherm of Batch System

The mechanism of adsorption of adsorbate onto the adsorbent can be understood from adsorption isotherms. Having all the parameters optimized, the resultant data was used to bring up the following isotherm models, namely, Langmuir (1/qe vs. 1/Ce), Freundlich (ln qe vs. ln Ce), and Temkin (qe vs. ln Ce). The isotherms were plotted by calculating Ce, qe, 1/Ce, ln Ce, 1/qe, and ln qe values [35].
(2)qe=Ci−CeVmwhere qe is the adsorption capacity at equilibrium, Ci is the initial concentration, Ce is the final concentration, V is volume of the adsorbate, and m is mass of the adsorbent.


## 2.1. Materials and Reagents

The following chemicals and reagents were purchased at analytical grade quality—ferrous chloride (LOBACHEMIE), anhydrous ferric chloride (LOBACHEMIE), ammonium solution (SRL), sodium hydroxide (SRL), hydrochloric acid, acetic acid (RAMKEM), ammonium ferrous sulphate (NH4)2.Fe(SO4)2.6H2O (SRL), diphenyl carbazide (SRL), potassium dichromate (SRL), ascorbic acid (SRL), sodium acetate (anhydrous), and methanol (SRL). The entire study was carried out using nitrogen purged Millipore water.


## 2.2. Synthesis of SPIONs

Iron oxide nanoparticles were synthesized by chemical coprecipitation. 100 mL of 1 M ferric chloride solution and 100 mL of 3 M ferrous chloride solution were prepared separately in nitrogen purged Millipore water. Equal volumes (50 mL) of the prepared precursor solutions were brought into suspension by magnetic agitation for 20 min. Then, the precursor suspension was heated to 60°C. This heat energy is assumed to accelerate the reduction of Fe ions. While heating the precursor solution at 60°C, 75 mL of freshly prepared 8 M NaOH and 25 mL of ammonia solution were added in alternative drops with vigorous mechanical stirring. The addition of reducing agent turned the precursor solution into black precipitate and increased the pH of the mixture. The high alkali pH was neutralized to pH 7 with 1 N HCl washing. Later, the black precipitate which is superparamagnetic iron oxide nanoparticle (SPION) was settled down and collected by applying magnetic field. It was then washed with nitrogen purged Millipore water for several times to remove impurities and then lyophilized [31].


## 2.3. Preparation of SPIONs Impregnated Activated Carbon

Granular activated carbon (N-GAC) of mesh size8∗20 was bought commercially and rinsed for multiple times with distilled water until the spent water becomes clear. This removed the carbon dust and impurities present. The washed activated carbon was dried on a filter paper and then heated to 80°C to remove moisture. 40 g activated carbon (N-GAC) was added with the iron precursor solution and subjected for SPION production as described above in the way to incorporate SPIONs. Then, it was heated to 60°C and stirred by magnetic agitation for 20 min. By doing so, the carbon and the pores within would get completely wet with the iron ions. Then, the reducing agents NaOH and ammonia were added simultaneously in drops with vigorous mechanical stirring. This leads to formation of SPIONs onto the surface as well as within the pore of the activated carbon. Thus, the carbon was impregnated with SPIONs. Finally, the carbon was filtered out using a nylon mesh filter and washed with Millipore water until the filtrate becomes clear and neutral (pH 7). The granular activated carbon impregnated with SPIONs (Sp-GAC) was used after freeze drying.


## 2.4. Characterization of SPIONs and SPIONs Impregnated Activated Carbon

SPIONs, N-GAC, and Sp-GAC were characterized by performing the following analysis: FT-IR (IR affinity-1S, Shimadzu, Japan), Scanning Electron Microscopy (SEM) (Carl Zeiss, Germany), Energy Dispersive X-ray (EDX) analysis, and XRD (Rigaku, Tokyo), where the SPIONs and Sp-GAC were subjected for Vibrating Sample Magnetometer (VSM) with a maximum magnetic field of 2.5 T and dynamic moment range of1×10e−6 emu-10e3 emu (Lakeshore, USA, Model 7407).


## 2.5. Quantification of Iron Impregnated onto Activated Carbon

### 2.5.1. Establishment of Standard Iron Curve

3.511 g of ammonium ferrous sulphate (NH4)2.Fe(SO4)2.6H2O (which contains 500 mg of Fe) in 1 L of nitrogen purged Millipore water was used as standard iron stock solution for 500 ppm. On diluting the stock, different parts per million (ppm) of iron solution was prepared and photometrically detected the total iron in accordance with Changzhao et al. [32]. Standard was prepared and made up to 0.5 mL with water and then with 6.8 mL of Millipore water, 0.2 mL of ascorbic acid (5 g in 50 mL), and 2 mL of sodium acetate buffer (16.4 g of sodium acetate in 24% acetic acid). Then, the reaction mixture was pipetted with 1 ml of 1,4 phenanthroline reagent (0.1%) and vortexed. The absorbance was photometrically read at 510 nm. A graph was plotted having the concentration in ppm as X-axis and absorbance as Y-axis.


### 2.5.2. Estimation of Total Iron Impregnated on activated carbon Using 1,4 Phenanthroline

To detect total iron impregnated on activated carbon, different concentrations of each sample (N-GAC and Sp-GAC) such as 10 mg, 30 mg, and 50 mg were treated with 10 mL of 10% H2SO4 for 24 h. After acid digestion, 0.5 mL of solution from each sample was processed (as prescribed above) for photometric detection with 1,4 phenanthroline at 510 nm and concentration was calculated from standard graph.


## 2.5.1. Establishment of Standard Iron Curve

3.511 g of ammonium ferrous sulphate (NH4)2.Fe(SO4)2.6H2O (which contains 500 mg of Fe) in 1 L of nitrogen purged Millipore water was used as standard iron stock solution for 500 ppm. On diluting the stock, different parts per million (ppm) of iron solution was prepared and photometrically detected the total iron in accordance with Changzhao et al. [32]. Standard was prepared and made up to 0.5 mL with water and then with 6.8 mL of Millipore water, 0.2 mL of ascorbic acid (5 g in 50 mL), and 2 mL of sodium acetate buffer (16.4 g of sodium acetate in 24% acetic acid). Then, the reaction mixture was pipetted with 1 ml of 1,4 phenanthroline reagent (0.1%) and vortexed. The absorbance was photometrically read at 510 nm. A graph was plotted having the concentration in ppm as X-axis and absorbance as Y-axis.


## 2.5.2. Estimation of Total Iron Impregnated on activated carbon Using 1,4 Phenanthroline

To detect total iron impregnated on activated carbon, different concentrations of each sample (N-GAC and Sp-GAC) such as 10 mg, 30 mg, and 50 mg were treated with 10 mL of 10% H2SO4 for 24 h. After acid digestion, 0.5 mL of solution from each sample was processed (as prescribed above) for photometric detection with 1,4 phenanthroline at 510 nm and concentration was calculated from standard graph.


## 2.6. Preparation of Cr(VI) Solution

For the study, different ppm concentrations of chromium were prepared using potassium dichromate as the chromium salt. 0.14 g of potassium dichromate (K2Cr2O7) in 100 mL of Millipore water corresponds to 500 ppm; further dilution was done to obtain 5 ppm of chromium solution (adsorbate).


### 2.6.1. Establishment of Standard Cr(VI) Curve

Different ppm concentrations of chromium solution were prepared by diluting the stock solution. Diphenyl carbazide (DPC) is a compound that binds exclusively to hexavalent chromium ions; and therefore, it acts as an indicator of hexavalent chromium. On binding with hexavalent chromium ions, the reacting mixture turns reddish violet colour [33, 34]. An aliquot of Cr solution from each dilution was reacted with DPC reagent for colour development. Then, it was spectrophotometrically read at 540 nm. A graph was plotted having ppm in X-axis vs. OD at 540 nm in Y-axis.


## 2.6.1. Establishment of Standard Cr(VI) Curve

Different ppm concentrations of chromium solution were prepared by diluting the stock solution. Diphenyl carbazide (DPC) is a compound that binds exclusively to hexavalent chromium ions; and therefore, it acts as an indicator of hexavalent chromium. On binding with hexavalent chromium ions, the reacting mixture turns reddish violet colour [33, 34]. An aliquot of Cr solution from each dilution was reacted with DPC reagent for colour development. Then, it was spectrophotometrically read at 540 nm. A graph was plotted having ppm in X-axis vs. OD at 540 nm in Y-axis.


## 2.7. Adsorption Study in Batch Experimental System

Chromium removal by different adsorbents was studied in batch system, and the parameters like concentration of adsorbent, concentration of adsorbate, and pH were optimized. Here, the adsorption study was considered for a particular period, i.e., 0th min to 120th min. All the batch setups were placed on rotatory shaker at 200 rpm in room temperature.


### 2.7.1. Effect of pH

To identify the activity of adsorbents against Cr ions at different pH, the adsorption was checked at a pH range of 3, 5, 7, 9, 11, and 13. 1 M HCl and 1 M NaOH prepared in Millipore water were used to adjust the pH of the Cr(VI) solution to a respective range. To each flask with 100 ml of 5 ppm Cr(VI) at different pH, 10 g/L of N-GAC and Sp-GAC was added separately and placed in shaker at 200 rpm for 2 h. After incubation, the supernatant from each setup was spectrophotometrically read at 540 nm. The final concentration of Cr in the solution was calibrated from the standard curve. % removal was calculated from the below formula:(1)%removal=initialconcentration−finalconcentrationinitialconcentration×100.To check the concentration of iron leached out from the adsorbent material, 0.5 mL of the supernatant was acid digested with 0.2 ml of H2SO4 and later, it was tagged with the reagent 1,4 phenanthroline by following the above described method in Section 2.5.1. The iron released was estimated from the standard. The final data were made into a graph with X-axis as pH, primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm).


### 2.7.2. Optimization of Adsorbent Concentration

Different concentrations (1 g/L to 10 g/L) of the adsorbents N-GAC and Sp-GAC were added to 100 ml of 5 ppm Cr(VI) solution at optimal pH (from above results). It was allowed to react for 2 h by constantly shaking at 200 rpm. Later, an aliquot of treated solution from each set was processed for DPC tagging and read at 540 nm. % removal of Cr and iron leached into the reaction mixture was also estimated from standard curve. A graph was plotted with adsorbate concentration asX-axis, % removal as primary Y-axis, and iron leached as secondary Y-axis.


### 2.7.3. Optimization of Adsorbate-Adsorbent Concentration

Here, the efficiency of the adsorbents N-GAC and Sp-GAC at 10 g/L in removal of maximum concentration of adsorbate was determined. It was performed with a fixed concentration of adsorbent against varied concentration of adsorbate. 10 g/L of N-GAC was added to each of 100 mL of Cr(VI) solution at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. All the different concentrations of adsorbate were prepared at the optimal pH. Similar reaction setup was made for the adsorbent, Sp-GAC. They were kept on shaker at 200 rpm for 2 h. After treatment, the % removal of Cr was estimated spectrophotometrically by the DPC method (540 nm). Parallelly, 0.5 ml of each of the supernatant was reacted with 1,4 phenanthroline after acid digestion to quantify (in ppm) the concentration of iron leached from the adsorbents. The graph was plotted between % removal (X-axis), adsorbate concentration (primary Y-axis), and iron leached (secondary Y-axis).


## 2.7.1. Effect of pH

To identify the activity of adsorbents against Cr ions at different pH, the adsorption was checked at a pH range of 3, 5, 7, 9, 11, and 13. 1 M HCl and 1 M NaOH prepared in Millipore water were used to adjust the pH of the Cr(VI) solution to a respective range. To each flask with 100 ml of 5 ppm Cr(VI) at different pH, 10 g/L of N-GAC and Sp-GAC was added separately and placed in shaker at 200 rpm for 2 h. After incubation, the supernatant from each setup was spectrophotometrically read at 540 nm. The final concentration of Cr in the solution was calibrated from the standard curve. % removal was calculated from the below formula:(1)%removal=initialconcentration−finalconcentrationinitialconcentration×100.To check the concentration of iron leached out from the adsorbent material, 0.5 mL of the supernatant was acid digested with 0.2 ml of H2SO4 and later, it was tagged with the reagent 1,4 phenanthroline by following the above described method in Section 2.5.1. The iron released was estimated from the standard. The final data were made into a graph with X-axis as pH, primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm).


## 2.7.2. Optimization of Adsorbent Concentration

Different concentrations (1 g/L to 10 g/L) of the adsorbents N-GAC and Sp-GAC were added to 100 ml of 5 ppm Cr(VI) solution at optimal pH (from above results). It was allowed to react for 2 h by constantly shaking at 200 rpm. Later, an aliquot of treated solution from each set was processed for DPC tagging and read at 540 nm. % removal of Cr and iron leached into the reaction mixture was also estimated from standard curve. A graph was plotted with adsorbate concentration asX-axis, % removal as primary Y-axis, and iron leached as secondary Y-axis.


## 2.7.3. Optimization of Adsorbate-Adsorbent Concentration

Here, the efficiency of the adsorbents N-GAC and Sp-GAC at 10 g/L in removal of maximum concentration of adsorbate was determined. It was performed with a fixed concentration of adsorbent against varied concentration of adsorbate. 10 g/L of N-GAC was added to each of 100 mL of Cr(VI) solution at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. All the different concentrations of adsorbate were prepared at the optimal pH. Similar reaction setup was made for the adsorbent, Sp-GAC. They were kept on shaker at 200 rpm for 2 h. After treatment, the % removal of Cr was estimated spectrophotometrically by the DPC method (540 nm). Parallelly, 0.5 ml of each of the supernatant was reacted with 1,4 phenanthroline after acid digestion to quantify (in ppm) the concentration of iron leached from the adsorbents. The graph was plotted between % removal (X-axis), adsorbate concentration (primary Y-axis), and iron leached (secondary Y-axis).


## 2.8. Adsorption Isotherm of Batch System

The mechanism of adsorption of adsorbate onto the adsorbent can be understood from adsorption isotherms. Having all the parameters optimized, the resultant data was used to bring up the following isotherm models, namely, Langmuir (1/qe vs. 1/Ce), Freundlich (ln qe vs. ln Ce), and Temkin (qe vs. ln Ce). The isotherms were plotted by calculating Ce, qe, 1/Ce, ln Ce, 1/qe, and ln qe values [35].
(2)qe=Ci−CeVmwhere qe is the adsorption capacity at equilibrium, Ci is the initial concentration, Ce is the final concentration, V is volume of the adsorbate, and m is mass of the adsorbent.


## 3. Results and Discussions

### 3.1. Characterization of SPIONs

#### 3.1.1. UV-VIS Spectroscopy

The optical property of the synthesized SPIONs can be described from UV-VIS spectroscopy. Figure1 shows the optical adsorption spectra of synthesized iron oxide nanoparticles at neutral pH. The surface plasmon resonance (SPR) of SPIONs was observed as a broad peak in the UV region (250 nm–300 nm) which signifies the characteristic adsorption spectral range of iron oxide nanoparticles [36]. The adsorption maxima for the synthesized particles were recorded at 294 nm. The spectra were more analogous to previous reports [31, 37]. Samrot et al. [38] reported SPIONs to show absorption maxima from 420 nm, where here too an absorption maxima was found around 490 nm.Figure 1
UV-VIS spectroscopy of SPIONs.


#### 3.1.2. Fourier Transform-Infrared Spectroscopy

The FT-IR spectrum of SPIONs is shown in Figure2. The spectra clearly show IR adsorption bands in the low-frequency regions in the range of 487 cm-1 and 569 cm-1 which represents the stretching vibrations of Fe-O-Fe bond stretching vibration of tetrahedral sites of spinel structure of the synthesis magnetic nanoparticles [39–42]. Presence of other minor bands may be attributed to adsorbed organic molecules. Thus, the synthesized SPIONs are affirmed to contain Fe-O bond from infrared adsorption spectra.Figure 2
Fourier Transform-Infrared Spectroscopy (FT-IR) of SPIONs.


#### 3.1.3. Scanning Electron Microscopy-Energy Dispersive X-Ray

From Figure3(a), the particle size was between 23 nm and 35 nm. The overall morphology of the particles was observed to be uniform and spherical with slight aggregation. As pristine samples, iron oxide nanoparticles tend to aggregate due to its high magnetic moment. Here, the slight aggregation may be because of the prevailing magnetic moment within the particle [43]. This can be prevented by coating SPIONs with detergents, biopolymer, and other materials [44]. In EDX (Figure 3(b) and Table 1), the presence of Fe and O was spotted with intense high peaks. Furthermore, this confirmed the presence of elementary components Fe and O in the prepared iron oxide nanoparticles.Figure 3
(a) Scanning Electron Microscopy. (b) Energy Dispersive X-ray (SEM-EDX) of SPIONs.
(a)(b)Table 1
Atomic percentage and weight percentage of the elemental composition present in SPIONs.
ElementWeight%Atomic%O K36.7166.94Fe K63.2933.06Totals100.00


#### 3.1.4. X-Ray Diffraction Spectroscopy

X-ray diffractogram of synthesized iron oxide nanoparticles produced sharp characteristic peaks for magnetite nanoparticles with high degree crystallinity (Figure4). The recorded 2ѳ peaks at corresponding degrees 30.47°, 35.81°, 57.35°, and 62.97° corresponded to planes (220), (311), (511), and (440) referred to magnetite nanoparticle (JCPDS card no. 85-1436) [45]. Comparable XRD pattern was stated by Sruthi et al. [44]. By applying the below Scherer equation, the crystallite size was calculated from the diffraction peak with highest intensity.
(3)D=KλβCosΘ,where variable D is crystal size (nm), K is lattice constant (0.98), λ is wavelength (0.154 nm), β is Full Width at Half Maximum (FWHM) of the sharp peaks, and ѳ is the Bragg angle. The high intensity peak at 35.81° was a retort to crystallite of size 16.43 nm, and the average crystallite size was determined as 14.22 nm.Figure 4
X-ray Diffraction (XRD) of SPIONs.


#### 3.1.5. Vibrating Sample Magnetometer

VSM was recorded under applied magnetic field between ±15 kOe at room temperature (RT). This technique helps in deducing the magnetization power of the synthesized iron oxide nanoparticles. The magnetization power was found to increase sharply around the origin, and this was typical of superparamagnetism (Figure5). Chellappan et al. [46] reported 2.4 emu/g for magnetite produced using 5 M NaOH as reducing agent. The produced iron oxide nanoparticles responded with maximum magnetization (Ms) of 88.22 emu/g at 15 kOe. Coercivity field value and remnant magnetization (Mr) were recorded at negligible magnitudes as 124.51 Oe and 12.7 emu/g, respectively. Presence of hysteresis in SPIONs was found by Prijic et al. [47] with zero coercivity, and it was used to treat malignant cells [47]. Hysteresis loop forms when the sample retained a residual magnetic moment in the absence of externally applied field [48]. Baykal et al. [49] produced iron oxide nanoparticles of size 12 nm by chemical method using the same reducing agent (NaOH) and reported the superparamagnetic behaviour of his nanoparticles via VSM spectra with no hysteresis loop.Figure 5
Vibrating Sample Magnetometer (VSM) of SPIONs.


### 3.2. Characterization of SPIONs Impregnated Activated Carbon

#### 3.2.1. Fourier Transform-Infrared Spectroscopy

Figure6 depicts the FT-IR spectra of N-GAC and Sp-GAC. The IR spectra of N-GAC showed peaks at 2883 cm-1 and 1570 cm-1 and Sp-GAC at 1571 cm-1, 1211 cm-1, and near 550 cm-1. The peak at 1570 cm-1 corresponds C=O stretching [50]. Sp-GAC showed a major IR shift in the low-frequency region around 510 cm-1-570 cm-1. This is the characteristic vibration of Fe-O-Fe from iron oxide nanoparticles [51]. Therefore, this stated the successful impregnation of iron oxide onto Sp-GAC.Figure 6
FT-IR. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).


#### 3.2.2. Scanning Electron Microscopy-Energy Dispersive X-Ray

Though granular size of carbon was already known, SEM revealed the surface topography of the naked activated carbon (N-GAC) as well as the SPIONs impregnated activated carbon (Sp-GAC). Figure7(a) shows the SEM micrograph of N-GAC. By observing N-GAC under SEM, it was found that the surface of the granules was nonuniform where each granule possessed irregular frame. SEM micrograph showed the porous structure of carbon. After impregnating (Sp-GAC), the surface was evenly distributed with SPIONs (Figure 7(b)). SPIONs formed on the surface of Sp-GAC were spherical with similar in morphology to SPIONs in Figure 3. This expresses that iron ion enriched surfaces of carbon act as nucleation site for iron oxide formation. However, the impregnated SPION size was bigger comparatively in the range of 50 nm - 70 nm, might because of agglomeration of nanoparticles. EDX results confirmed the elemental source of each adsorbents. N-GAC produced high intense carbon peaks (Figure 7(a)). Sp-GAC responded with peaks of C, Fe, and O which further confirms the presence of iron oxide (Figure 7(b)). The intensity of C peak was much reduced in Sp-GAC since the surface of carbon was concealed by iron oxides. Samrot et al. [38] reported SPIONs produced using NaOH and ammonia solution as reducing agent to show size around 41 nm.Figure 7
SEM-EDX. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


#### 3.2.3. X-Ray Diffraction Spectroscopy

N-GAC showed peaks at2ѳ=25, 45 corresponding to the planes (002) and (100) of graphitic crystallites of carbon (Figures 8(a) and 8(b)). In terms of structure, the activated carbon can be termed as more amorphous from XRD spectra. Rajendran et al. [52] also reported similar XRD records for the activated carbon produced from agricultural waste. Activated carbon produced from cocoa shell were also reported to be amorphous in nature by Tejada et al. [53]. The XRD pattern of activated carbon after impregnation (Sp-GAC) was found to have peaks at 30.47°, 35.81°, and 62.97° which are characteristics of SPIONs and looked to be amorphic in structure as carbon was there (Figure 4).Figure 8
XRD. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


#### 3.2.4. Vibrating Sample Magnetometer

The M-H at RT spectra revealed the superparamagnetic behaviour of Sp-GAC (Figure9). Sp-GAC showed saturation magnetization (Ms) of about 53.22 emu/g with coercivity at 144.18 Oe and remnant magnetization (Mr) at 9.04 emu/g. Although Sp-GAC expressed less magnetization (Ms) compared to SPIONs (Figure 5), it maintained reduced remanence effect throughout the analysis. This was apparent with absence of hysteresis loop. Hence, this proves that activated carbon possess superparamagnetism on impregnating with iron oxide nanoparticles. Gallios and his coworkers [54] produced magnetic activated carbon for arsenic removal and checked its magnetic behaviour in VSM. Magnetization (Ms=0.35 emu g −1) of impregnated carbon was higher than the unimpregnated carbon (Ms=0.1 emu g −1) (result not shown here)", and its superparamagnetic magnetization curve was more analogous to the VSM of SPIONs.Figure 9
VSM of SPIONs impregnated granular activated carbon (Sp-GAC).


### 3.3. Quantification of Iron Impregnated onto Activated Carbon

A standard graph of Fe withR2=0.988 was established for ammonium ferrous sulphate salt following the abovesaid method. The acid digested samples (obtained from N-GAC and Sp-GAC) were treated with 1,4 phenanthroline as stated in the above method, and the concentration of iron was identified against the standard graph (Figure 10). It showed that the concentration of iron was directly proportional to concentration of adsorbents, even the commercial activated carbon (N-GAC) contained iron within it which should be the iron contamination from carbon processing or in the source itself. 10 mg, 20 mg, and 30 mg of Sp-GAC contained 0.052 μg/mg, 0.073 μg/mg, and 0.143 μg/mg of iron, respectively. Szpak et al. [55] have also employed the above method (using 1,4 phenanthroline) to quantify the iron concentration in SPIONs for relaxometry analysis. Likewise, Górka et al. [56] also estimated the total iron content of his SPIONs as 0.871 mg/ml using 1,4 phenanthroline reagent.Figure 10
Quantification of iron. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


### 3.4. Batch Adsorption Studies

#### 3.4.1. Adsorption at various pH

Identification of optimal pH is important for adsorption study because ionic charge of the absorbents in most cases relies on the pH of the reacting solution. This trial was carried out by treating fixed concentration of adsorbent with adsorbate solution at varied pH (Figure11). Adsorption was significantly higher in the acidic pH range with maximal Cr removal at pH 3. Despite a metal ion, chromium will exist as anionic chromates (oxidation states) in aqueous solution. Cr(VI) takes the anionic form as hydrogen chromate (HCrO4-) and dichromate ions (Cr2O72-) of which dichromate ions are the predominant ratio of chromic anionic at low pH (as per the speciation report) [57]. And at acidic condition, the surface of adsorbent gets enriched with hydrogen ion, thereby acts as active positive charge site. This promotes electrostatic interaction between the adsorbent surface and anionic chromates which eventually turn out as the driving force for adsorption. This electrostatic force and the charge of the reacting components explained the principle of adsorption. As a contrary, in alkali pH, the absorbent possesses negative charge due to abundant -OH which creates electric repulsion towards Cr(VI) anions. Here, at pH 3, the adsorbents N-GAC and Sp-GAC are offered with more of H+ ions which have supported the adsorption of anionic chromates. However, SPIONs are known to disintegrate at acidic pH. pH was reduced, leading to increased iron discharge in high acidic pH (pH 1).Figure 11
Adsorption of N-GAC and Sp-GAC at various pH. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


#### 3.4.2. Adsorption at different Adsorbent Concentration

Here, a fixed concentration of adsorbate (Cr(VI) at 5 ppm) is allowed to react with varied concentration of adsorbents N-GAC and Sp-GAC. Doing so, the maximum adsorbents required for complete removal are known. In each case, the iron leached was also estimated. The adsorption result is represented as a graph (Figure12) with X-axis as adsorbent concentration (g/L), primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm). The resultant data clearly explained that the adsorption (% removal of Cr(VI)) increased with increase in concentration of the absorbent). This proved that efficiency of adsorption was dependent on the dosage of adsorbent used. Adsorption activity of N-GAC and Sp-GAC was found to be similar which achieved 100% removal of 5 ppm Cr(VI) when 10 g/L of each adsorbent was used. Therefore, the optimal concentration of adsorbent was fixed as 10 g/L. The better removal was shown by N-GAC due to the increased surface area but in case of Sp-GAC, availability of active sites might be low as SPIONs occupied the active sites of the granular activated carbon which did not allow way for the effective binding of chromium. Qureshi et al. [29] explained the adsorption of Cr(VI) by aluminium oxide and iron oxide impregnated carbon nanotubes. It was found that adsorption improved as the dosage of adsorbent was increased.Figure 12
Determination of adsorbate-adsorbent concentration. (a) N-GAC: naked granular activated carbon and (b) Sp-GAC: SPIONs impregnated granular activated carbon.
(a)(b)


#### 3.4.3. Adsorbate-Adsorbent Concentration

Here, a fixed concentration of adsorbent (10 g/L) is allowed to react with varied concentration of adsorbate — 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. Through this trial, the maximum efficiency of the adsorbent against the heavy metal Cr was identified. Also, the iron leached in each case was assessed. It was found that 10 g/L of N-GAC showed 95.9%, 99.9%, 99.9%, 99.45%, 99.32%, 98%, 87.02%, and 69.8% of Cr(VI) removal at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm whereas Sp-GAC removed maximum chromium of 99.7, 89.6%, 84.6%, 74.11%, 74.37%, 62.8%, and 40.09% and 23% at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm, respectively (Figure13). The performance of Sp-GAC greatly declined when Cr(VI) of high concentration was used. This manifested N-GAC as a better adsorbent material than Sp-GAC. This might be due to the increased surface area of the N-GAC and active sites available for binding of chromium to its surface. In Sp-GAC, the surface area is comparatively less due to which iron leach was high when higher concentration of chromium was used since there is no active site readily available for the adsorption reaction to take place. Also, N-GAC-treated samples showed total iron leach to 1.5 ppm but Sp-GAC was found to leach more iron (2 ppm). Iron leaching could be ruled out by suitable functionalization or biopolymer coating. Under coexistent batch experiment [58], Cu(II) showed better affinity towards the magnetite (Fe3O4) nanoparticles than Cr(VI). It was also noticed that the removal rates of both the metal ions (Cr(VI) and Cu(II)) depreciated when the initial concentration of the adsorbates was increased.Figure 13
Adsorption as a function of adsorbate-adsorbent concentration. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


### 3.5. Adsorption Isotherm

The adsorption of Cr(VI) in the batch system was analysed by applying the adsorption isotherm models like Langmuir, Freundlich, and Temkin. The correlation coefficient (R2) from each case were compared, and the isotherm with highest R2 value was considered as the best fit model. N-GAC responded to Langmuir, Freundlich, and Temkin isotherms with R2=0.37, 0.70, and 0.44, respectively (Figure 14). Likewise, Sp-GAC showed R2 values as 0.57, 0.64, and 0.44 correspondingly (Figure 14). In both cases, R2 of Freundlich isotherm were greater than 0.6. Therefore, it can be assumed that adsorption reaction between the adsorbent and adsorbate abide by the Freundlich isotherm model. This described the adsorption mechanism as multilayered and homogenous. Cr(VI) adsorption by differently processed activated carbon from Tuncbilek lignite was reported to be influenced by factors like pH, temperature, and initial adsorbate concentration [59]. The activated carbon produced by physical methods showed better adsorption (95 % of Cr removal at 563 ppm), and it followed Langmuir adsorption principle.Figure 14
Adsorption isotherm. (a) Langmuir isotherm, (b) Freundlich isotherm, and (c) Temkin isotherm.
(a)(b)(c)


## 3.1. Characterization of SPIONs

### 3.1.1. UV-VIS Spectroscopy

The optical property of the synthesized SPIONs can be described from UV-VIS spectroscopy. Figure1 shows the optical adsorption spectra of synthesized iron oxide nanoparticles at neutral pH. The surface plasmon resonance (SPR) of SPIONs was observed as a broad peak in the UV region (250 nm–300 nm) which signifies the characteristic adsorption spectral range of iron oxide nanoparticles [36]. The adsorption maxima for the synthesized particles were recorded at 294 nm. The spectra were more analogous to previous reports [31, 37]. Samrot et al. [38] reported SPIONs to show absorption maxima from 420 nm, where here too an absorption maxima was found around 490 nm.Figure 1
UV-VIS spectroscopy of SPIONs.


### 3.1.2. Fourier Transform-Infrared Spectroscopy

The FT-IR spectrum of SPIONs is shown in Figure2. The spectra clearly show IR adsorption bands in the low-frequency regions in the range of 487 cm-1 and 569 cm-1 which represents the stretching vibrations of Fe-O-Fe bond stretching vibration of tetrahedral sites of spinel structure of the synthesis magnetic nanoparticles [39–42]. Presence of other minor bands may be attributed to adsorbed organic molecules. Thus, the synthesized SPIONs are affirmed to contain Fe-O bond from infrared adsorption spectra.Figure 2
Fourier Transform-Infrared Spectroscopy (FT-IR) of SPIONs.


### 3.1.3. Scanning Electron Microscopy-Energy Dispersive X-Ray

From Figure3(a), the particle size was between 23 nm and 35 nm. The overall morphology of the particles was observed to be uniform and spherical with slight aggregation. As pristine samples, iron oxide nanoparticles tend to aggregate due to its high magnetic moment. Here, the slight aggregation may be because of the prevailing magnetic moment within the particle [43]. This can be prevented by coating SPIONs with detergents, biopolymer, and other materials [44]. In EDX (Figure 3(b) and Table 1), the presence of Fe and O was spotted with intense high peaks. Furthermore, this confirmed the presence of elementary components Fe and O in the prepared iron oxide nanoparticles.Figure 3
(a) Scanning Electron Microscopy. (b) Energy Dispersive X-ray (SEM-EDX) of SPIONs.
(a)(b)Table 1
Atomic percentage and weight percentage of the elemental composition present in SPIONs.
ElementWeight%Atomic%O K36.7166.94Fe K63.2933.06Totals100.00


### 3.1.4. X-Ray Diffraction Spectroscopy

X-ray diffractogram of synthesized iron oxide nanoparticles produced sharp characteristic peaks for magnetite nanoparticles with high degree crystallinity (Figure4). The recorded 2ѳ peaks at corresponding degrees 30.47°, 35.81°, 57.35°, and 62.97° corresponded to planes (220), (311), (511), and (440) referred to magnetite nanoparticle (JCPDS card no. 85-1436) [45]. Comparable XRD pattern was stated by Sruthi et al. [44]. By applying the below Scherer equation, the crystallite size was calculated from the diffraction peak with highest intensity.
(3)D=KλβCosΘ,where variable D is crystal size (nm), K is lattice constant (0.98), λ is wavelength (0.154 nm), β is Full Width at Half Maximum (FWHM) of the sharp peaks, and ѳ is the Bragg angle. The high intensity peak at 35.81° was a retort to crystallite of size 16.43 nm, and the average crystallite size was determined as 14.22 nm.Figure 4
X-ray Diffraction (XRD) of SPIONs.


### 3.1.5. Vibrating Sample Magnetometer

VSM was recorded under applied magnetic field between ±15 kOe at room temperature (RT). This technique helps in deducing the magnetization power of the synthesized iron oxide nanoparticles. The magnetization power was found to increase sharply around the origin, and this was typical of superparamagnetism (Figure5). Chellappan et al. [46] reported 2.4 emu/g for magnetite produced using 5 M NaOH as reducing agent. The produced iron oxide nanoparticles responded with maximum magnetization (Ms) of 88.22 emu/g at 15 kOe. Coercivity field value and remnant magnetization (Mr) were recorded at negligible magnitudes as 124.51 Oe and 12.7 emu/g, respectively. Presence of hysteresis in SPIONs was found by Prijic et al. [47] with zero coercivity, and it was used to treat malignant cells [47]. Hysteresis loop forms when the sample retained a residual magnetic moment in the absence of externally applied field [48]. Baykal et al. [49] produced iron oxide nanoparticles of size 12 nm by chemical method using the same reducing agent (NaOH) and reported the superparamagnetic behaviour of his nanoparticles via VSM spectra with no hysteresis loop.Figure 5
Vibrating Sample Magnetometer (VSM) of SPIONs.


## 3.1.1. UV-VIS Spectroscopy

The optical property of the synthesized SPIONs can be described from UV-VIS spectroscopy. Figure1 shows the optical adsorption spectra of synthesized iron oxide nanoparticles at neutral pH. The surface plasmon resonance (SPR) of SPIONs was observed as a broad peak in the UV region (250 nm–300 nm) which signifies the characteristic adsorption spectral range of iron oxide nanoparticles [36]. The adsorption maxima for the synthesized particles were recorded at 294 nm. The spectra were more analogous to previous reports [31, 37]. Samrot et al. [38] reported SPIONs to show absorption maxima from 420 nm, where here too an absorption maxima was found around 490 nm.Figure 1
UV-VIS spectroscopy of SPIONs.


## 3.1.2. Fourier Transform-Infrared Spectroscopy

The FT-IR spectrum of SPIONs is shown in Figure2. The spectra clearly show IR adsorption bands in the low-frequency regions in the range of 487 cm-1 and 569 cm-1 which represents the stretching vibrations of Fe-O-Fe bond stretching vibration of tetrahedral sites of spinel structure of the synthesis magnetic nanoparticles [39–42]. Presence of other minor bands may be attributed to adsorbed organic molecules. Thus, the synthesized SPIONs are affirmed to contain Fe-O bond from infrared adsorption spectra.Figure 2
Fourier Transform-Infrared Spectroscopy (FT-IR) of SPIONs.


## 3.1.3. Scanning Electron Microscopy-Energy Dispersive X-Ray

From Figure3(a), the particle size was between 23 nm and 35 nm. The overall morphology of the particles was observed to be uniform and spherical with slight aggregation. As pristine samples, iron oxide nanoparticles tend to aggregate due to its high magnetic moment. Here, the slight aggregation may be because of the prevailing magnetic moment within the particle [43]. This can be prevented by coating SPIONs with detergents, biopolymer, and other materials [44]. In EDX (Figure 3(b) and Table 1), the presence of Fe and O was spotted with intense high peaks. Furthermore, this confirmed the presence of elementary components Fe and O in the prepared iron oxide nanoparticles.Figure 3
(a) Scanning Electron Microscopy. (b) Energy Dispersive X-ray (SEM-EDX) of SPIONs.
(a)(b)Table 1
Atomic percentage and weight percentage of the elemental composition present in SPIONs.
ElementWeight%Atomic%O K36.7166.94Fe K63.2933.06Totals100.00


## 3.1.4. X-Ray Diffraction Spectroscopy

X-ray diffractogram of synthesized iron oxide nanoparticles produced sharp characteristic peaks for magnetite nanoparticles with high degree crystallinity (Figure4). The recorded 2ѳ peaks at corresponding degrees 30.47°, 35.81°, 57.35°, and 62.97° corresponded to planes (220), (311), (511), and (440) referred to magnetite nanoparticle (JCPDS card no. 85-1436) [45]. Comparable XRD pattern was stated by Sruthi et al. [44]. By applying the below Scherer equation, the crystallite size was calculated from the diffraction peak with highest intensity.
(3)D=KλβCosΘ,where variable D is crystal size (nm), K is lattice constant (0.98), λ is wavelength (0.154 nm), β is Full Width at Half Maximum (FWHM) of the sharp peaks, and ѳ is the Bragg angle. The high intensity peak at 35.81° was a retort to crystallite of size 16.43 nm, and the average crystallite size was determined as 14.22 nm.Figure 4
X-ray Diffraction (XRD) of SPIONs.


## 3.1.5. Vibrating Sample Magnetometer

VSM was recorded under applied magnetic field between ±15 kOe at room temperature (RT). This technique helps in deducing the magnetization power of the synthesized iron oxide nanoparticles. The magnetization power was found to increase sharply around the origin, and this was typical of superparamagnetism (Figure5). Chellappan et al. [46] reported 2.4 emu/g for magnetite produced using 5 M NaOH as reducing agent. The produced iron oxide nanoparticles responded with maximum magnetization (Ms) of 88.22 emu/g at 15 kOe. Coercivity field value and remnant magnetization (Mr) were recorded at negligible magnitudes as 124.51 Oe and 12.7 emu/g, respectively. Presence of hysteresis in SPIONs was found by Prijic et al. [47] with zero coercivity, and it was used to treat malignant cells [47]. Hysteresis loop forms when the sample retained a residual magnetic moment in the absence of externally applied field [48]. Baykal et al. [49] produced iron oxide nanoparticles of size 12 nm by chemical method using the same reducing agent (NaOH) and reported the superparamagnetic behaviour of his nanoparticles via VSM spectra with no hysteresis loop.Figure 5
Vibrating Sample Magnetometer (VSM) of SPIONs.


## 3.2. Characterization of SPIONs Impregnated Activated Carbon

### 3.2.1. Fourier Transform-Infrared Spectroscopy

Figure6 depicts the FT-IR spectra of N-GAC and Sp-GAC. The IR spectra of N-GAC showed peaks at 2883 cm-1 and 1570 cm-1 and Sp-GAC at 1571 cm-1, 1211 cm-1, and near 550 cm-1. The peak at 1570 cm-1 corresponds C=O stretching [50]. Sp-GAC showed a major IR shift in the low-frequency region around 510 cm-1-570 cm-1. This is the characteristic vibration of Fe-O-Fe from iron oxide nanoparticles [51]. Therefore, this stated the successful impregnation of iron oxide onto Sp-GAC.Figure 6
FT-IR. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).


### 3.2.2. Scanning Electron Microscopy-Energy Dispersive X-Ray

Though granular size of carbon was already known, SEM revealed the surface topography of the naked activated carbon (N-GAC) as well as the SPIONs impregnated activated carbon (Sp-GAC). Figure7(a) shows the SEM micrograph of N-GAC. By observing N-GAC under SEM, it was found that the surface of the granules was nonuniform where each granule possessed irregular frame. SEM micrograph showed the porous structure of carbon. After impregnating (Sp-GAC), the surface was evenly distributed with SPIONs (Figure 7(b)). SPIONs formed on the surface of Sp-GAC were spherical with similar in morphology to SPIONs in Figure 3. This expresses that iron ion enriched surfaces of carbon act as nucleation site for iron oxide formation. However, the impregnated SPION size was bigger comparatively in the range of 50 nm - 70 nm, might because of agglomeration of nanoparticles. EDX results confirmed the elemental source of each adsorbents. N-GAC produced high intense carbon peaks (Figure 7(a)). Sp-GAC responded with peaks of C, Fe, and O which further confirms the presence of iron oxide (Figure 7(b)). The intensity of C peak was much reduced in Sp-GAC since the surface of carbon was concealed by iron oxides. Samrot et al. [38] reported SPIONs produced using NaOH and ammonia solution as reducing agent to show size around 41 nm.Figure 7
SEM-EDX. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


### 3.2.3. X-Ray Diffraction Spectroscopy

N-GAC showed peaks at2ѳ=25, 45 corresponding to the planes (002) and (100) of graphitic crystallites of carbon (Figures 8(a) and 8(b)). In terms of structure, the activated carbon can be termed as more amorphous from XRD spectra. Rajendran et al. [52] also reported similar XRD records for the activated carbon produced from agricultural waste. Activated carbon produced from cocoa shell were also reported to be amorphous in nature by Tejada et al. [53]. The XRD pattern of activated carbon after impregnation (Sp-GAC) was found to have peaks at 30.47°, 35.81°, and 62.97° which are characteristics of SPIONs and looked to be amorphic in structure as carbon was there (Figure 4).Figure 8
XRD. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


### 3.2.4. Vibrating Sample Magnetometer

The M-H at RT spectra revealed the superparamagnetic behaviour of Sp-GAC (Figure9). Sp-GAC showed saturation magnetization (Ms) of about 53.22 emu/g with coercivity at 144.18 Oe and remnant magnetization (Mr) at 9.04 emu/g. Although Sp-GAC expressed less magnetization (Ms) compared to SPIONs (Figure 5), it maintained reduced remanence effect throughout the analysis. This was apparent with absence of hysteresis loop. Hence, this proves that activated carbon possess superparamagnetism on impregnating with iron oxide nanoparticles. Gallios and his coworkers [54] produced magnetic activated carbon for arsenic removal and checked its magnetic behaviour in VSM. Magnetization (Ms=0.35 emu g −1) of impregnated carbon was higher than the unimpregnated carbon (Ms=0.1 emu g −1) (result not shown here)", and its superparamagnetic magnetization curve was more analogous to the VSM of SPIONs.Figure 9
VSM of SPIONs impregnated granular activated carbon (Sp-GAC).


## 3.2.1. Fourier Transform-Infrared Spectroscopy

Figure6 depicts the FT-IR spectra of N-GAC and Sp-GAC. The IR spectra of N-GAC showed peaks at 2883 cm-1 and 1570 cm-1 and Sp-GAC at 1571 cm-1, 1211 cm-1, and near 550 cm-1. The peak at 1570 cm-1 corresponds C=O stretching [50]. Sp-GAC showed a major IR shift in the low-frequency region around 510 cm-1-570 cm-1. This is the characteristic vibration of Fe-O-Fe from iron oxide nanoparticles [51]. Therefore, this stated the successful impregnation of iron oxide onto Sp-GAC.Figure 6
FT-IR. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).


## 3.2.2. Scanning Electron Microscopy-Energy Dispersive X-Ray

Though granular size of carbon was already known, SEM revealed the surface topography of the naked activated carbon (N-GAC) as well as the SPIONs impregnated activated carbon (Sp-GAC). Figure7(a) shows the SEM micrograph of N-GAC. By observing N-GAC under SEM, it was found that the surface of the granules was nonuniform where each granule possessed irregular frame. SEM micrograph showed the porous structure of carbon. After impregnating (Sp-GAC), the surface was evenly distributed with SPIONs (Figure 7(b)). SPIONs formed on the surface of Sp-GAC were spherical with similar in morphology to SPIONs in Figure 3. This expresses that iron ion enriched surfaces of carbon act as nucleation site for iron oxide formation. However, the impregnated SPION size was bigger comparatively in the range of 50 nm - 70 nm, might because of agglomeration of nanoparticles. EDX results confirmed the elemental source of each adsorbents. N-GAC produced high intense carbon peaks (Figure 7(a)). Sp-GAC responded with peaks of C, Fe, and O which further confirms the presence of iron oxide (Figure 7(b)). The intensity of C peak was much reduced in Sp-GAC since the surface of carbon was concealed by iron oxides. Samrot et al. [38] reported SPIONs produced using NaOH and ammonia solution as reducing agent to show size around 41 nm.Figure 7
SEM-EDX. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


## 3.2.3. X-Ray Diffraction Spectroscopy

N-GAC showed peaks at2ѳ=25, 45 corresponding to the planes (002) and (100) of graphitic crystallites of carbon (Figures 8(a) and 8(b)). In terms of structure, the activated carbon can be termed as more amorphous from XRD spectra. Rajendran et al. [52] also reported similar XRD records for the activated carbon produced from agricultural waste. Activated carbon produced from cocoa shell were also reported to be amorphous in nature by Tejada et al. [53]. The XRD pattern of activated carbon after impregnation (Sp-GAC) was found to have peaks at 30.47°, 35.81°, and 62.97° which are characteristics of SPIONs and looked to be amorphic in structure as carbon was there (Figure 4).Figure 8
XRD. (a) Naked granular activated carbon (N-GAC) and (b) SPIONs impregnated granular activated carbon (Sp-GAC).
(a)(b)


## 3.2.4. Vibrating Sample Magnetometer

The M-H at RT spectra revealed the superparamagnetic behaviour of Sp-GAC (Figure9). Sp-GAC showed saturation magnetization (Ms) of about 53.22 emu/g with coercivity at 144.18 Oe and remnant magnetization (Mr) at 9.04 emu/g. Although Sp-GAC expressed less magnetization (Ms) compared to SPIONs (Figure 5), it maintained reduced remanence effect throughout the analysis. This was apparent with absence of hysteresis loop. Hence, this proves that activated carbon possess superparamagnetism on impregnating with iron oxide nanoparticles. Gallios and his coworkers [54] produced magnetic activated carbon for arsenic removal and checked its magnetic behaviour in VSM. Magnetization (Ms=0.35 emu g −1) of impregnated carbon was higher than the unimpregnated carbon (Ms=0.1 emu g −1) (result not shown here)", and its superparamagnetic magnetization curve was more analogous to the VSM of SPIONs.Figure 9
VSM of SPIONs impregnated granular activated carbon (Sp-GAC).


## 3.3. Quantification of Iron Impregnated onto Activated Carbon

A standard graph of Fe withR2=0.988 was established for ammonium ferrous sulphate salt following the abovesaid method. The acid digested samples (obtained from N-GAC and Sp-GAC) were treated with 1,4 phenanthroline as stated in the above method, and the concentration of iron was identified against the standard graph (Figure 10). It showed that the concentration of iron was directly proportional to concentration of adsorbents, even the commercial activated carbon (N-GAC) contained iron within it which should be the iron contamination from carbon processing or in the source itself. 10 mg, 20 mg, and 30 mg of Sp-GAC contained 0.052 μg/mg, 0.073 μg/mg, and 0.143 μg/mg of iron, respectively. Szpak et al. [55] have also employed the above method (using 1,4 phenanthroline) to quantify the iron concentration in SPIONs for relaxometry analysis. Likewise, Górka et al. [56] also estimated the total iron content of his SPIONs as 0.871 mg/ml using 1,4 phenanthroline reagent.Figure 10
Quantification of iron. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


## 3.4. Batch Adsorption Studies

### 3.4.1. Adsorption at various pH

Identification of optimal pH is important for adsorption study because ionic charge of the absorbents in most cases relies on the pH of the reacting solution. This trial was carried out by treating fixed concentration of adsorbent with adsorbate solution at varied pH (Figure11). Adsorption was significantly higher in the acidic pH range with maximal Cr removal at pH 3. Despite a metal ion, chromium will exist as anionic chromates (oxidation states) in aqueous solution. Cr(VI) takes the anionic form as hydrogen chromate (HCrO4-) and dichromate ions (Cr2O72-) of which dichromate ions are the predominant ratio of chromic anionic at low pH (as per the speciation report) [57]. And at acidic condition, the surface of adsorbent gets enriched with hydrogen ion, thereby acts as active positive charge site. This promotes electrostatic interaction between the adsorbent surface and anionic chromates which eventually turn out as the driving force for adsorption. This electrostatic force and the charge of the reacting components explained the principle of adsorption. As a contrary, in alkali pH, the absorbent possesses negative charge due to abundant -OH which creates electric repulsion towards Cr(VI) anions. Here, at pH 3, the adsorbents N-GAC and Sp-GAC are offered with more of H+ ions which have supported the adsorption of anionic chromates. However, SPIONs are known to disintegrate at acidic pH. pH was reduced, leading to increased iron discharge in high acidic pH (pH 1).Figure 11
Adsorption of N-GAC and Sp-GAC at various pH. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


### 3.4.2. Adsorption at different Adsorbent Concentration

Here, a fixed concentration of adsorbate (Cr(VI) at 5 ppm) is allowed to react with varied concentration of adsorbents N-GAC and Sp-GAC. Doing so, the maximum adsorbents required for complete removal are known. In each case, the iron leached was also estimated. The adsorption result is represented as a graph (Figure12) with X-axis as adsorbent concentration (g/L), primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm). The resultant data clearly explained that the adsorption (% removal of Cr(VI)) increased with increase in concentration of the absorbent). This proved that efficiency of adsorption was dependent on the dosage of adsorbent used. Adsorption activity of N-GAC and Sp-GAC was found to be similar which achieved 100% removal of 5 ppm Cr(VI) when 10 g/L of each adsorbent was used. Therefore, the optimal concentration of adsorbent was fixed as 10 g/L. The better removal was shown by N-GAC due to the increased surface area but in case of Sp-GAC, availability of active sites might be low as SPIONs occupied the active sites of the granular activated carbon which did not allow way for the effective binding of chromium. Qureshi et al. [29] explained the adsorption of Cr(VI) by aluminium oxide and iron oxide impregnated carbon nanotubes. It was found that adsorption improved as the dosage of adsorbent was increased.Figure 12
Determination of adsorbate-adsorbent concentration. (a) N-GAC: naked granular activated carbon and (b) Sp-GAC: SPIONs impregnated granular activated carbon.
(a)(b)


### 3.4.3. Adsorbate-Adsorbent Concentration

Here, a fixed concentration of adsorbent (10 g/L) is allowed to react with varied concentration of adsorbate — 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. Through this trial, the maximum efficiency of the adsorbent against the heavy metal Cr was identified. Also, the iron leached in each case was assessed. It was found that 10 g/L of N-GAC showed 95.9%, 99.9%, 99.9%, 99.45%, 99.32%, 98%, 87.02%, and 69.8% of Cr(VI) removal at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm whereas Sp-GAC removed maximum chromium of 99.7, 89.6%, 84.6%, 74.11%, 74.37%, 62.8%, and 40.09% and 23% at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm, respectively (Figure13). The performance of Sp-GAC greatly declined when Cr(VI) of high concentration was used. This manifested N-GAC as a better adsorbent material than Sp-GAC. This might be due to the increased surface area of the N-GAC and active sites available for binding of chromium to its surface. In Sp-GAC, the surface area is comparatively less due to which iron leach was high when higher concentration of chromium was used since there is no active site readily available for the adsorption reaction to take place. Also, N-GAC-treated samples showed total iron leach to 1.5 ppm but Sp-GAC was found to leach more iron (2 ppm). Iron leaching could be ruled out by suitable functionalization or biopolymer coating. Under coexistent batch experiment [58], Cu(II) showed better affinity towards the magnetite (Fe3O4) nanoparticles than Cr(VI). It was also noticed that the removal rates of both the metal ions (Cr(VI) and Cu(II)) depreciated when the initial concentration of the adsorbates was increased.Figure 13
Adsorption as a function of adsorbate-adsorbent concentration. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


## 3.4.1. Adsorption at various pH

Identification of optimal pH is important for adsorption study because ionic charge of the absorbents in most cases relies on the pH of the reacting solution. This trial was carried out by treating fixed concentration of adsorbent with adsorbate solution at varied pH (Figure11). Adsorption was significantly higher in the acidic pH range with maximal Cr removal at pH 3. Despite a metal ion, chromium will exist as anionic chromates (oxidation states) in aqueous solution. Cr(VI) takes the anionic form as hydrogen chromate (HCrO4-) and dichromate ions (Cr2O72-) of which dichromate ions are the predominant ratio of chromic anionic at low pH (as per the speciation report) [57]. And at acidic condition, the surface of adsorbent gets enriched with hydrogen ion, thereby acts as active positive charge site. This promotes electrostatic interaction between the adsorbent surface and anionic chromates which eventually turn out as the driving force for adsorption. This electrostatic force and the charge of the reacting components explained the principle of adsorption. As a contrary, in alkali pH, the absorbent possesses negative charge due to abundant -OH which creates electric repulsion towards Cr(VI) anions. Here, at pH 3, the adsorbents N-GAC and Sp-GAC are offered with more of H+ ions which have supported the adsorption of anionic chromates. However, SPIONs are known to disintegrate at acidic pH. pH was reduced, leading to increased iron discharge in high acidic pH (pH 1).Figure 11
Adsorption of N-GAC and Sp-GAC at various pH. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


## 3.4.2. Adsorption at different Adsorbent Concentration

Here, a fixed concentration of adsorbate (Cr(VI) at 5 ppm) is allowed to react with varied concentration of adsorbents N-GAC and Sp-GAC. Doing so, the maximum adsorbents required for complete removal are known. In each case, the iron leached was also estimated. The adsorption result is represented as a graph (Figure12) with X-axis as adsorbent concentration (g/L), primary Y-axis as % removal, and secondary Y-axis as iron leached (ppm). The resultant data clearly explained that the adsorption (% removal of Cr(VI)) increased with increase in concentration of the absorbent). This proved that efficiency of adsorption was dependent on the dosage of adsorbent used. Adsorption activity of N-GAC and Sp-GAC was found to be similar which achieved 100% removal of 5 ppm Cr(VI) when 10 g/L of each adsorbent was used. Therefore, the optimal concentration of adsorbent was fixed as 10 g/L. The better removal was shown by N-GAC due to the increased surface area but in case of Sp-GAC, availability of active sites might be low as SPIONs occupied the active sites of the granular activated carbon which did not allow way for the effective binding of chromium. Qureshi et al. [29] explained the adsorption of Cr(VI) by aluminium oxide and iron oxide impregnated carbon nanotubes. It was found that adsorption improved as the dosage of adsorbent was increased.Figure 12
Determination of adsorbate-adsorbent concentration. (a) N-GAC: naked granular activated carbon and (b) Sp-GAC: SPIONs impregnated granular activated carbon.
(a)(b)


## 3.4.3. Adsorbate-Adsorbent Concentration

Here, a fixed concentration of adsorbent (10 g/L) is allowed to react with varied concentration of adsorbate — 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm. Through this trial, the maximum efficiency of the adsorbent against the heavy metal Cr was identified. Also, the iron leached in each case was assessed. It was found that 10 g/L of N-GAC showed 95.9%, 99.9%, 99.9%, 99.45%, 99.32%, 98%, 87.02%, and 69.8% of Cr(VI) removal at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm whereas Sp-GAC removed maximum chromium of 99.7, 89.6%, 84.6%, 74.11%, 74.37%, 62.8%, and 40.09% and 23% at 1 ppm, 5 ppm, 10 ppm, 20 ppm, 40 ppm, 80 ppm, 160 ppm, and 320 ppm, respectively (Figure13). The performance of Sp-GAC greatly declined when Cr(VI) of high concentration was used. This manifested N-GAC as a better adsorbent material than Sp-GAC. This might be due to the increased surface area of the N-GAC and active sites available for binding of chromium to its surface. In Sp-GAC, the surface area is comparatively less due to which iron leach was high when higher concentration of chromium was used since there is no active site readily available for the adsorption reaction to take place. Also, N-GAC-treated samples showed total iron leach to 1.5 ppm but Sp-GAC was found to leach more iron (2 ppm). Iron leaching could be ruled out by suitable functionalization or biopolymer coating. Under coexistent batch experiment [58], Cu(II) showed better affinity towards the magnetite (Fe3O4) nanoparticles than Cr(VI). It was also noticed that the removal rates of both the metal ions (Cr(VI) and Cu(II)) depreciated when the initial concentration of the adsorbates was increased.Figure 13
Adsorption as a function of adsorbate-adsorbent concentration. N-GAC: naked granular activated carbon; Sp-GAC: SPIONs impregnated granular activated carbon.


## 3.5. Adsorption Isotherm

The adsorption of Cr(VI) in the batch system was analysed by applying the adsorption isotherm models like Langmuir, Freundlich, and Temkin. The correlation coefficient (R2) from each case were compared, and the isotherm with highest R2 value was considered as the best fit model. N-GAC responded to Langmuir, Freundlich, and Temkin isotherms with R2=0.37, 0.70, and 0.44, respectively (Figure 14). Likewise, Sp-GAC showed R2 values as 0.57, 0.64, and 0.44 correspondingly (Figure 14). In both cases, R2 of Freundlich isotherm were greater than 0.6. Therefore, it can be assumed that adsorption reaction between the adsorbent and adsorbate abide by the Freundlich isotherm model. This described the adsorption mechanism as multilayered and homogenous. Cr(VI) adsorption by differently processed activated carbon from Tuncbilek lignite was reported to be influenced by factors like pH, temperature, and initial adsorbate concentration [59]. The activated carbon produced by physical methods showed better adsorption (95 % of Cr removal at 563 ppm), and it followed Langmuir adsorption principle.Figure 14
Adsorption isotherm. (a) Langmuir isotherm, (b) Freundlich isotherm, and (c) Temkin isotherm.
(a)(b)(c)


## 4. Conclusion

By following chemical coprecipitation method, SPIONs impregnated activated carbon (Sp-GAC) were produced and characterized. SEM micrograph portrayed the pattern of impregnation in Sp-GAC, where the surface of activated carbon was found to be covered with SPIONs. FT-IR and EDX confirmed the impregnation of SPIONs on activated carbon whose superparamagnetic property was identified through VSM. XRD spectra confirmed the amorphic nature of carbon (N-GAC) whereas impregnated carbon (Sp-GAC) was found to be slightly crystalline. On utilizing N-GAC and Sp-GAC in adsorption of Cr(VI), it was found that the adsorption was phenomenally influenced by the pH of the treating solution. Better adsorption was noticed at pH 3. Further adsorption study revealed that N-GAC showed better adsorption to Sp-GAC at increased Cr(VI) concentration. Hence, it can be concluded that the SPION impregnation on to carbon has not much influence on Cr(VI) removal in batch system.



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*Source: 4326939-2022-01-18.xml*