# Removal of Safranin-T and Toluidine from Water through Gum Arabic/Acrylamide Hydrogel

Authors: Salma Jabeen; Sultan Alam; Luqman Ali Shah; Muhammad Zahoor; Najeeb Ur Rahman; Farhat Ali Khan; Riaz Ullah; Essam A. Ali; H. C. Ananda Murthy; Aamir Sohail
Journal: Adsorption Science & Technology
 (2022)

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## Abstract

Hydrogels as “smart sorbents” for wastewater treatment have attracted much attention due to their facile fabrication, rapid regeneration, environment friendly nature, and strong interaction with pollutants. In this study, gum arabic/acrylamide (GA/AM) hydrogel was developed via the free radical polymerization method by employing acrylamide (AM) (monomer), gum arabic (GA) (grafting backbone), N,N-methylenebisacrylamide (MBA) (chemical crosslinker), and tetramethylethylenediamine (TEMED) (accelerator). The fabricated adsorbent was characterized by scanning electron microscopy (SEM), Fourier transform infrared (FTIR) spectroscopy, and surface area analyzer. The adsorption properties of the subject hydrogel were explored against cationic safranin and toluidine dyes in aqueous media. The point of zero charge (PZC) for the GA/AM sorbent was found to bepHPZC=7.1 whereas maximum sorption occurred at pH 11. Different kinetic and isotherm models were applied to evaluate the adsorption mechanism and estimate values of different adsorption parameters. The adsorption isotherm and kinetics were better explained by the Langmuir isotherm and pseudo-second-order kinetic model whereas the adsorption thermodynamics depicted the endothermic, spontaneous, and favorable nature of the process. The adsorbent was regenerated with acetone and reused for the selected dyes for many cycles. After the 5th cycle, the hydrogel retained safranin/toluidine removal capacity≥60% which pointed toward the reusability of the prepared adsorbent for cycles without appreciable reduction in its adsorption capacity. Hence, the GA/AM sorbent can be applied as an alternative of activated carbon to treat dye-contaminated waters.


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## Body

## 1. Introduction

Different industries such as textile [1], paint [2], food [3], and pharmaceutics [4] are the direct emitters of different pollutants [5] including dyes [6] and heavy metal ions [7, 8] into water. The presence of these toxic pollutants can cause severe environmental problems that can adversely affect the biotic components of the ecosystem as well [9, 10]. Apart from it, they also affect the human health by causing problems such as skin irritation, cancer, and allergic dermatitis [11]. Therefore, it is important to remove dyes from contaminated water before their discharge into main sewerage lines.Currently, numerous techniques are in use for the reclamation of dye-contaminated water which are broadly classified into physical, chemical, and biological methods. Among them, the most frequently used techniques are degradation, ion exchange, coagulation, oxidation, photocatalysis, and adsorption [12–14]. Out of them, adsorption is the best and most efficient technique used for the dye’s removal from wastewater due to its low cost, reasonably greater efficiency, and easy availability. A large number of materials have been tested as adsorbents (like zeolites, activated carbon, and synthetic polymers) for the removal of dyes and heavy metals from water. It has been observed that hydrogels have exhibited superior efficiencies towards the adsorptive removal of various dyes and inorganic pollutants [15–19]. The crosslinked polymeric networks of hydrogel make it a superior material which can imbibe a lot of water inside its network. The swelling behavior and active charges on the hydrogel network are responsible for dyes and other pollutant’s effective removal from contaminated water. Therefore, the hydrogel modifications require a key consideration to use them in an effective way in water reclamation from contaminants [20, 21]. Superabsorbent polymer hydrogels represent the most important class of the polymeric hydrogels which are porous and have an immensely crosslinked three-dimensional skeleton. Simple preparation, easy separation, high efficiency, and low cost are some of the distinctive properties of these hydrogels. These hydrogels have the unique ability to bind or dissolve water hundred times more than other adsorbents because of their hydrophilicity and swelling potential [22, 23]. Gum arabic is a high-molecular weight natural polysaccharide obtained from the tree of Acacia. It is composed of 1,3-linked β-D-galactopyranosyl units. The side chains are made of two to five 1,3-related β-D-galactopyranosyl units, combined with the core chain by 1,6-connections. Both the side and the core chains contain units of α-L-arabinofuranos, α-L-rhamnopyranosyl, β-D-glucopyranosyl, and 4-O-methyl-β-D-glucopyranosyl [24, 25]. According to recent literature, the gum Arabic nanohydrogel and polyacrylamide (PAM) nanohydrogel have been fabricated by the microwave-assisted technique. Such hydrogels have been used as adsorbent for removal of crystal violet dye from water [26]. Similarly, GA/poly (acrylic acid) hydrogel has been developed and applied as adsorbent for the removal of methylene blue dye from wastewater [27]. Another study about the fabrication of GA/poly(acrylamide)/Ni(OH)2/FeOOH hydrogel and its subsequent use as adsorbent for the dye removal from wastewater has also been reported [28]. Moreover, hydrogel synthesized from gum arabic, polyacrylate, and polyacrylamide has also been documented in literature which has displayed good adsorption properties toward eradication of methylene blue from wastewater [29]. So far, the use gum arabic/acrylamide hydrogel for adsorption of safranin and toluidine has not been documented in literature which promoted us to fabricate and apply gum arabic/acrylamide hydrogel for adsorption of the mentioned cationic dyes.In this study, the gum arabic/acrylamide (GA/AM) hydrogel was fabricated from gum arabic and acrylamide in the presence of N, N-methylenebisacrylamide (MBA) (chemical cross-linker) and tetra-methyl ethylene diamine (TEMED) (accelerator). The fabricated adsorbent was used for the removal of safranin and toluidine stains/dyes from water. Since the dyes have received a plethora of applications in industries like paper, textile, and silk, the dyes are also used as redox initiators and photosensitizers and for staining cell organelles. Despite their numerous applications, there are meagre reports regarding their removal from wastewater by using hydrogels which promoted us to utilize safranin and toluidine as model pollutants in the present study.


## 2. Materials and Method

### 2.1. Chemicals

All the chemicals used in the experiments were of analytical grade and were used without further purification. Safranin and toluidine dyes/stains were purchased from Sigma-Aldrich (Germany). The physicochemical properties of the selected dyes are given in Table1. Other chemicals used in this study include acrylamide (AM) (CH2=CHC(O)NH2) obtained from FLUKA (Switzerland), gum arabic (GA) (C15H20NNaO4) obtained from Merck (USA), N-N-methylenebisacrylamide (MBA) bought from FLUKA (Switzerland), and ammonium persulphate (APS, NH4)2S2O8 from FLUKA (Switzerland) used as an initiator while tetramethylethylenediamine (TEMED) was obtained from FLUKA Switzerland.Table 1
Physiochemical properties of safranin and toluidine dyes [48, 49].
Name of dyeSafranin TToluidine blueChemical formulaMolecular formulaC20H19N4 + Cl−C15H16CIN3SMolecular weight350.85 g/mol270.374 g/molλ max554 nm625 nmWater solubility0.05 g/mL38.2 g/100 mLSolubility in other solventsSoluble in alcoholSlightly soluble in alcohol: ethanol, methanol


### 2.2. Instrumentation

The prepared hydrogel (GA/AM) was characterized by scanning electron microscopy (SEM) (JSM5910, JEOL Tokyo, Japan). The surface area of the hydrogel was determined by Quantachrome (NOVA2200e, Quantachrome, Boynton Beach, Florida, USA) while the functionalities on the surface of the adsorbent were determined using Fourier transform infrared spectroscopy (FTIR) (Thermo Fisher Nicoletis50). The sample in form of a KBr pellet was scanned from 4000 to 500 cm−1. The dye concentration was determined calorimetrically by measuring absorbance using a double-beam ultraviolet-visible (UV–vis) spectrophotometer (UV-1800, Shimadzu Scientific Instruments Inc., Kyoto, Japan) at a specified wavelength mentioned in Table 1. All the adsorption experiments were conducted in the thermostated water bath shaker.


### 2.3. Synthesis of Polymeric Hydrogel

The polymeric sorbent was prepared using a free radical polymerization approach in which AM was used as a monomer and GA as the backbone onto which the acrylamide chains were grafted. Briefly, 1 gram each of AM and GA was charged to 200 mL water in a beaker followed by stirring the mixture (500 rpm) at 333 K which resulted into the formation of a homogenous mixture. Dropwise 20μL tetramethyl ethylene diamine (TEMED) was then added followed by 5% ammonium persulphate (APS) solution. This resulted into the development of polymeric GA/AM hydrogel which was washed with water and dried for 420 min in an oven at 338 K. Finally, the dried hydrogel (GA/AM) was grinded with a hammer-type minigrinder and stored till the commencement of adsorption experiments.


### 2.4. Point of Zero Charge of the Prepared Adsorbent

Point zero charge abbreviated as PZC is the characteristic pH value at which the surface charge of a material becomes zero, i.e., all its active sites are neutral. The PZC of the GA/AM hydrogel was calculated by placing 0.01 g hydrogel in 30 mL of 0.1 N NaNO3 solution. Each solution was divided in 11 bottles having different pH ranges from 2 to 11, monitored by a pH meter (Ph-2106). The pH of solutions was adjusted by 0.1 M NaOH and 0.1 M HNO3 solution. The bottles were then kept in a shaker 24 h. The resultant final pH of the bottles was noted where the difference in pH values of the sample was calculated using the equation ΔpH=pHi−pHf [30] with pHi denoting the initial pH and pHf the final pH of the given solution.


### 2.5. Adsorption Experiments

The adsorption performance of prepared adsorbent towards safranin and toluidine dyes in aqueous solution was measured using the batch experimental approach, such as 0.01 g polymeric hydrogel which was stirred with 10 mL dye solution in distilled water (0.001 M). In the kinetic study, a series of reagent bottles containing the same volume (10 mL) and concentration 0.001 M of selected dyes were mixed with 0.01 g of prepared adsorbent and then shaken on a thermostated shaker for 30 min at 293, 313, and 333 K. A specified volume of the sample was filtered and analyzed by a UV-visible spectrophotometer at 554 and 625 nm, respectively, for the remaining concentration of safranin and toluidine. All the experiments were performed in triplicate. Different kinetics models (given in equations (1) to (4)) were used to explain the kinetics of the adsorption process [31].The pseudo-1st-order equation is expressed as equation (1) as follows:
(1)logqe−qt=logqe−k1t2.303.The pseudo-2nd-order equation is expressed as equation (2) as follows:
(2)tqt=tqe+1k2qe2.The Elovich equation is expressed as equation (3) as follows:
(3)qt=lnβαα+lntβ.The intraparticle diffusion model is expressed as equation (4) as follows:
(4)qt=Kit1/2+C.In these equations,qe and qt are the adsorption capacities at equilibrium and at any time t in mol/g, k1 is the rate constant of the pseudo-1st-order model (1/min), k2 is the rate constant of the pseudo-2nd-order equation (g/mg/min), α is the initial adsorption rate (mg/g·min), β is the desorption constant (mg/g min), and C is the intercept in equation (4) whereas, kid is the intraparticle diffusion constant (mg/g·min1/2).In the isotherm studies, a series of reagent bottles containing 10 mL of different concentrations (0.0005–0.003) of selected dyes were mixed with 0.01 g of the prepared adsorbent and then shaken on a thermostated shaker for 30 min at 293, 313, and 333 K. Specific amounts of sample were filtered and analyzed for the remaining concentration of selected dyes using a UV-visible spectrophotometer. For the determination of different isotherm parameters, Langmuir, Freundlich, and Temkin models were used. Such types of studies are important to evaluate how the adsorbate interacts with the adsorbent and also gives information about adsorption capacities. Isotherm parameters also give information on the formation of a monolayer or multilayer over the adsorbent surface by the adsorbate [32, 33].The Langmuir isotherm model defines the sorption of adsorbate at homogenous sites on the adsorbent surface where the adsorbate only forms a monolayer on the surface of the adsorbent. The linear form of this model can be given as equation (5) as follows:
(5)CoC=Cec∞+1KadC∞,where C, Co, Kad, and C∞ are the adsorbed amount of dye at equilibrium (mg/g), the concentration of dye solution at equilibrium (mg/L), Langmuir constant (L/mol), and the maximum adsorption capacity (mg/g), respectively, [34].The Freundlich isotherm model describes the nonideal behavior and reversibility of the adsorption process being nonrestricted to the monolayer formation which can be applied to the adsorption on heterogeneous surfaces (multilayer adsorption) with nonuniform distribution of adsorption heat and affinities of the sites over the adsorbent surface. Mathematically, this model can be given as equation (6) as follows:
(6)lnqe=lnKf+1nlnCe,where qe, Ce, Kf, and 1/n represent the quantity of adsorbate adsorbed at equilibrium, the equilibrium concentration of dye solution, adsorption capacity at unit concentration, and adsorption intensity. It should be noted that if 1/n=0, the adsorption process will be irreversible while favorable when 0<1/n<1 and, if 1/n>1, the process will be unfavorable [35].The Temkin model in the linear form can be given as equation (7) as follows:
(7)qe+B1lnkT+B1lnCe,where B1 and KT are the constant of adsorption and equilibrium binding, respectively [36].The whole process carried out can be represented as follows (Scheme1):Scheme 1
Schematic representation of the adsorption process.Furthermore, the effect of pH on adsorption was investigated using a series of reagent bottles at different pH ranging from 3 to 11 in which pH values were adjusted using dilute solutions of HCl or NaOH (0.1 mol·L−1); then, the same volume and concentration of selected dyes were mixed with 0.01 g of the prepared hydrogel and shaken on a thermostatic shaker for 60 min.The effect of temperature on the selected dye adsorption was evaluated at 293, 313, and 333 K where the same concentration solutions were contacted with the fixed amount of adsorbent for 60 min. The Van’t Hoff plot was drawn to estimate values of enthalpy and entropy changes whereas Gibbs free energy values were estimated from the enthalpy and entropy values at respective temperatures.The polymeric hydrogel was recycled for 5 cycles where the dye-loaded hydrogel was washed with acetone using the solvent extraction method. The recycled hydrogel was dried in an oven at 373 K and reused for 5 cycles to estimate the reduction in adsorption capacity values and consequently the possibility of regeneration of hydrogel.


## 2.1. Chemicals

All the chemicals used in the experiments were of analytical grade and were used without further purification. Safranin and toluidine dyes/stains were purchased from Sigma-Aldrich (Germany). The physicochemical properties of the selected dyes are given in Table1. Other chemicals used in this study include acrylamide (AM) (CH2=CHC(O)NH2) obtained from FLUKA (Switzerland), gum arabic (GA) (C15H20NNaO4) obtained from Merck (USA), N-N-methylenebisacrylamide (MBA) bought from FLUKA (Switzerland), and ammonium persulphate (APS, NH4)2S2O8 from FLUKA (Switzerland) used as an initiator while tetramethylethylenediamine (TEMED) was obtained from FLUKA Switzerland.Table 1
Physiochemical properties of safranin and toluidine dyes [48, 49].
Name of dyeSafranin TToluidine blueChemical formulaMolecular formulaC20H19N4 + Cl−C15H16CIN3SMolecular weight350.85 g/mol270.374 g/molλ max554 nm625 nmWater solubility0.05 g/mL38.2 g/100 mLSolubility in other solventsSoluble in alcoholSlightly soluble in alcohol: ethanol, methanol


## 2.2. Instrumentation

The prepared hydrogel (GA/AM) was characterized by scanning electron microscopy (SEM) (JSM5910, JEOL Tokyo, Japan). The surface area of the hydrogel was determined by Quantachrome (NOVA2200e, Quantachrome, Boynton Beach, Florida, USA) while the functionalities on the surface of the adsorbent were determined using Fourier transform infrared spectroscopy (FTIR) (Thermo Fisher Nicoletis50). The sample in form of a KBr pellet was scanned from 4000 to 500 cm−1. The dye concentration was determined calorimetrically by measuring absorbance using a double-beam ultraviolet-visible (UV–vis) spectrophotometer (UV-1800, Shimadzu Scientific Instruments Inc., Kyoto, Japan) at a specified wavelength mentioned in Table 1. All the adsorption experiments were conducted in the thermostated water bath shaker.


## 2.3. Synthesis of Polymeric Hydrogel

The polymeric sorbent was prepared using a free radical polymerization approach in which AM was used as a monomer and GA as the backbone onto which the acrylamide chains were grafted. Briefly, 1 gram each of AM and GA was charged to 200 mL water in a beaker followed by stirring the mixture (500 rpm) at 333 K which resulted into the formation of a homogenous mixture. Dropwise 20μL tetramethyl ethylene diamine (TEMED) was then added followed by 5% ammonium persulphate (APS) solution. This resulted into the development of polymeric GA/AM hydrogel which was washed with water and dried for 420 min in an oven at 338 K. Finally, the dried hydrogel (GA/AM) was grinded with a hammer-type minigrinder and stored till the commencement of adsorption experiments.


## 2.4. Point of Zero Charge of the Prepared Adsorbent

Point zero charge abbreviated as PZC is the characteristic pH value at which the surface charge of a material becomes zero, i.e., all its active sites are neutral. The PZC of the GA/AM hydrogel was calculated by placing 0.01 g hydrogel in 30 mL of 0.1 N NaNO3 solution. Each solution was divided in 11 bottles having different pH ranges from 2 to 11, monitored by a pH meter (Ph-2106). The pH of solutions was adjusted by 0.1 M NaOH and 0.1 M HNO3 solution. The bottles were then kept in a shaker 24 h. The resultant final pH of the bottles was noted where the difference in pH values of the sample was calculated using the equation ΔpH=pHi−pHf [30] with pHi denoting the initial pH and pHf the final pH of the given solution.


## 2.5. Adsorption Experiments

The adsorption performance of prepared adsorbent towards safranin and toluidine dyes in aqueous solution was measured using the batch experimental approach, such as 0.01 g polymeric hydrogel which was stirred with 10 mL dye solution in distilled water (0.001 M). In the kinetic study, a series of reagent bottles containing the same volume (10 mL) and concentration 0.001 M of selected dyes were mixed with 0.01 g of prepared adsorbent and then shaken on a thermostated shaker for 30 min at 293, 313, and 333 K. A specified volume of the sample was filtered and analyzed by a UV-visible spectrophotometer at 554 and 625 nm, respectively, for the remaining concentration of safranin and toluidine. All the experiments were performed in triplicate. Different kinetics models (given in equations (1) to (4)) were used to explain the kinetics of the adsorption process [31].The pseudo-1st-order equation is expressed as equation (1) as follows:
(1)logqe−qt=logqe−k1t2.303.The pseudo-2nd-order equation is expressed as equation (2) as follows:
(2)tqt=tqe+1k2qe2.The Elovich equation is expressed as equation (3) as follows:
(3)qt=lnβαα+lntβ.The intraparticle diffusion model is expressed as equation (4) as follows:
(4)qt=Kit1/2+C.In these equations,qe and qt are the adsorption capacities at equilibrium and at any time t in mol/g, k1 is the rate constant of the pseudo-1st-order model (1/min), k2 is the rate constant of the pseudo-2nd-order equation (g/mg/min), α is the initial adsorption rate (mg/g·min), β is the desorption constant (mg/g min), and C is the intercept in equation (4) whereas, kid is the intraparticle diffusion constant (mg/g·min1/2).In the isotherm studies, a series of reagent bottles containing 10 mL of different concentrations (0.0005–0.003) of selected dyes were mixed with 0.01 g of the prepared adsorbent and then shaken on a thermostated shaker for 30 min at 293, 313, and 333 K. Specific amounts of sample were filtered and analyzed for the remaining concentration of selected dyes using a UV-visible spectrophotometer. For the determination of different isotherm parameters, Langmuir, Freundlich, and Temkin models were used. Such types of studies are important to evaluate how the adsorbate interacts with the adsorbent and also gives information about adsorption capacities. Isotherm parameters also give information on the formation of a monolayer or multilayer over the adsorbent surface by the adsorbate [32, 33].The Langmuir isotherm model defines the sorption of adsorbate at homogenous sites on the adsorbent surface where the adsorbate only forms a monolayer on the surface of the adsorbent. The linear form of this model can be given as equation (5) as follows:
(5)CoC=Cec∞+1KadC∞,where C, Co, Kad, and C∞ are the adsorbed amount of dye at equilibrium (mg/g), the concentration of dye solution at equilibrium (mg/L), Langmuir constant (L/mol), and the maximum adsorption capacity (mg/g), respectively, [34].The Freundlich isotherm model describes the nonideal behavior and reversibility of the adsorption process being nonrestricted to the monolayer formation which can be applied to the adsorption on heterogeneous surfaces (multilayer adsorption) with nonuniform distribution of adsorption heat and affinities of the sites over the adsorbent surface. Mathematically, this model can be given as equation (6) as follows:
(6)lnqe=lnKf+1nlnCe,where qe, Ce, Kf, and 1/n represent the quantity of adsorbate adsorbed at equilibrium, the equilibrium concentration of dye solution, adsorption capacity at unit concentration, and adsorption intensity. It should be noted that if 1/n=0, the adsorption process will be irreversible while favorable when 0<1/n<1 and, if 1/n>1, the process will be unfavorable [35].The Temkin model in the linear form can be given as equation (7) as follows:
(7)qe+B1lnkT+B1lnCe,where B1 and KT are the constant of adsorption and equilibrium binding, respectively [36].The whole process carried out can be represented as follows (Scheme1):Scheme 1
Schematic representation of the adsorption process.Furthermore, the effect of pH on adsorption was investigated using a series of reagent bottles at different pH ranging from 3 to 11 in which pH values were adjusted using dilute solutions of HCl or NaOH (0.1 mol·L−1); then, the same volume and concentration of selected dyes were mixed with 0.01 g of the prepared hydrogel and shaken on a thermostatic shaker for 60 min.The effect of temperature on the selected dye adsorption was evaluated at 293, 313, and 333 K where the same concentration solutions were contacted with the fixed amount of adsorbent for 60 min. The Van’t Hoff plot was drawn to estimate values of enthalpy and entropy changes whereas Gibbs free energy values were estimated from the enthalpy and entropy values at respective temperatures.The polymeric hydrogel was recycled for 5 cycles where the dye-loaded hydrogel was washed with acetone using the solvent extraction method. The recycled hydrogel was dried in an oven at 373 K and reused for 5 cycles to estimate the reduction in adsorption capacity values and consequently the possibility of regeneration of hydrogel.


## 3. Results and Discussion

### 3.1. Surface Morphology

The morphology of polymer hydrogel was studied using SEM analysis. The SEM images are shown in Figure1. The micrographs show rough interfaces along with many cavities with characteristic irregular channels of hydrogel that would probably be responsible for the enhanced adsorption of the selected dyes [26, 28].Figure 1
SEM images of hydrogel at various magnifications: (a) 1.00μm and (b) 500 nm.
(a)(b)


### 3.2. Surface Functionalities

FTIR spectroscopy was used to identify the surface functional groups on polymeric hydrogel as shown in Figure2. Both characteristic bands of the acrylamide and gum arabic are present in the synthesized hydrogel. The broad and strong peak at 3428 cm−1 is related to the NH or OH stretching of the carboxylic and hydroxyl groups of acrylamide [26, 28, 29]. The medium peaks at 1067–1090 cm−1 represent the stretching vibration of C−O−C and C−O−H bonds. The sharpest peak at 1669 cm−1 is related to C=O stretching. The amide bond presence was confirmed from a weak and obvious band at 1456 cm−1, which is due to the C−N bending vibration. The two strong peaks at 1565–1648 cm−1 shows the C=O stretching [37, 38]. The presence of peaks for both of hydrogel and acryl amide in FTIR spectra confirm the formation of the polymeric hydrogel network that was attempted to be prepared through a free radical polymerization reaction in this study.Figure 2
FTIR spectrum of polymeric GA/AM hydrogel.


### 3.3. Surface Area and Thermal Properties of the Hydrogel

Various models like Brunauer-Emmett-Teller (BET), Brookhurst Junior High (BJH), Langmuir, and Dubinin-Radushkevitch (DR) are used to find out the surface area of the adsorbents. Among the abovementioned methods, the commonly used method is BET surface area (m2/g) analysis that is frequently used to determine the specific surface area, pore size, and pore distribution of the adsorbents. This method involves the nitrogen adsorption and desorption processes (Table 2). The isotherm of the adsorption-desorption of hydrogel refers to the type IV isotherm as shown in Figure 3. The increase in pore size distribution can be confirmed from increase in area under the hysteresis loops with increase in temperature. The BET equation is expressed as equation (8)) as follows [39].
(8)1WP0/P−1=1WmC+C−1WmCPp0,where W is the weight of gas adsorbed, P/P0 is relative pressure, Wm is the weight of adsorbate constituting a monolayer coverage, and C is related to the energy of adsorption in the first adsorbed layer.Table 2
Surface area and pore size distribution of hydrogel GA/AM.
Surface area (m2/g)Pore size distributionBJH methodsDR methodBETPore volume (cm3/g)Pore diameter (A°)Micropore volume (cm3/g)Average pore width (A°)Ads. Energy (kJ/mol)26.73500.06810.4530.06811.1793.853Figure 3
Characterization of hydrogel: (a) BET surface area and (b) thermogram.
(a)(b)The thermogram of GA/AM sorption as presented in Figure3(b) displays three phases of mass loss corresponding to different temperature domains. The first phase with 5% (40–130°C) mass loss is due to the elimination of water molecules and dehydration of neighboring –COOH functionalities [40, 41]. The second (130–250°C) mass loss can be attributed to decarboxylation of the remaining –COOH groups. The final-phase (250–500°C) mass loss is most probably due to the degradation of polymeric chains and breakage of the 3D polymeric network of the hydrogel.


### 3.4. Point of Zero Charge (PZC) and pH Effect on the Absorption of Safranin and Toluidine

The PZC of GA/AM was noted as 7.1 in Figure4(a). The surface was positively charged at acidic pH whereas at basic pH, it was negatively charged. As both the dyes are cationic, therefore, the favorable interaction was observed at 11 pH and high adsorption was observed at this pH as shown in Figure 4(b).Figure 4
(a) Point of zero charge (conditions: temp 313 K, dose 0.01–0.005, time 24 h, pH range (2–11) adjusted by 0.1 M HNO3 and NaOH, using NaNO3 0.1 N solution and volume 30 mL) and (b) effect of pH on the % removal of safranin and toluidine by hydrogel.
(a)(b)The process of adsorption of the dyes (safranin, toluidine) from the solution by superabsorbent hydrogel takes place under the influence of two types of driving forces in which the first one is diffusion of dyes in the network of hydrogel that occurs whereas the second deriving force is electrostatic interactions between adsorbent and adsorbate. The pH of media markedly affects the process of adsorption [26, 28, 29]. Figure 4(b) explains the effect of pH on the selected dye adsorption. The rate of adsorption increases with the increase in pH of the medium. At PZC, the percentage removal of dyes decreases slightly as the isoelectric point is lying there. The percentage removal then abruptly increases after PZC as the pores became negatively charged; thus, maximum adsorption of the dyes occurred [26, 28, 29]. The hydrogel showed a %removal of 78 to 73 for safranin and toluidine at highest pH tested whereas the % removal was 56 and 55% for safranin toluidine, respectively, at PZC (pH 7.08). The % removal of the selected dyes was calculated using equation (9).
(9)%removal=Co−CeCo×100.


### 3.5. Effect of Contact Time on Adsorption

The effect of contact time on the absorption of dyes, safranin and toluidine, was investigated in the abovementioned fed-batch experiment described in detail. The results are graphically shown in Figures5 and 6 for safranin and toluidine, respectively. Initially, the rate of adsorption is high as there is no competition for adsorption sites being free. Up to 60 min, the rate of adsorption increases proportionately, and then, equilibrium is reached where adsorption and desorption rates are equal; thus, the curve has become parallel up to 480 min. The adsorption rate in the beginning is high because of the availability of a larger number of active sites on the surface of hydrogel. Such types of behavior have been observed in other studies as well [42]. Thus, 60 min time was noted as equilibrium time for the 0.01 g hydrogel used.Figure 5
Effect of time on the adsorption of safranin on polymeric hydrogel (adsorbent dosage 0.01 g, dye solution 10 mL, time 30–480 min,pH=11, temperature 313 K).Figure 6
Effect of time on the adsorption of toluidine on polymeric hydrogel (adsorbent dosage 0.01 g, dye solution 10 mL, time 30–480 min,pH=11, temperature 313 K).


### 3.6. Adsorption Kinetics

Adsorption kinetics are important while evaluating the adsorption processes, and one can get insight into the adsorption mechanism and adsorbate-adsorbent interaction [43]. From an economical point of view in the industries, it is important to have information about kinetics of a given process.The experimental data of the kinetics study were fitted into different models which are graphically shown in Figures7(a)–7(d) (safranin) and Figures 8(a)–8(d) (toluidine). The slope and intercept values in the case of each model were calculated and interpreted as valuable adsorption parameters listed in Tables 3(a) and 3(b). The R2 (linear correlation coefficients) values (0.99) of pseudo-second-order plots (Figures 7(b) and 8(b)) are significantly higher than that of pseudo-first-order plots (Figures 7(a) and 8(a); R2=0.82–0.96) indicating the chemical nature of the sorption process [44, 45]. Also, the Qe experimental and calculated values in the case of the pseudo-second-order model are close to each other, clearly indicating that the best fit of the kinetics data can be achieved with this model. Moreover, the k2 values increase with the rise in temperature which indicates a high adsorption rate at elevated temperature.Figure 7
Kinetics of safranin adsorption on GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, temp 313 K, time 60 min): (a) pseudo-1st-order plot and (b) pseudo-2nd-order plot.
(a)(b)Figure 8
Kinetics of toluidine adsorption on the GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, temp 313 K, time 60 min): (a) pseudo-1st-order plot and (b) pseudo-2nd-order plot.
(a)(b)Table 3(a)
Kinetics parameters estimated from the kinetics model for safranin adsorption on the prepared adsorbent
Parameter293 K313 K333 KPseudofirst orderK1 (min−1)0.570.0530.072Qe (mg/g; calculated)66.6961.0377.52Qe (mg/g; experimental)249268295R20.95220.95720.9603Pseudosecond orderQe (mg/g; calculated)256.4277.7303.1Qe (mg/g; experimental)249268295K2 (g/mg/min)1.49×10−31.59×10−31.67×10−3R20.99980.99980.9999(b)
Kinetics parameters estimated from the kinetics model for toluidine adsorption on the prepared adsorbent
Parameter293 K313 K333 KPseudofirst orderK1 (min−1)0.0610.0580.063Qe (mg/g; calculated)59.7153.2546.62Qe (mg/g; experimental)217.4232.12249.77R20.92990.9440.9022Pseudosecond orderQe (mg/g; calculated)227.27238.09256.41Qe (mg/g; experimental)217.4232.12249.77K2 (g/mg/min)0.001650.001940.00231R20.99960.99980.9998TheR2 values of the intraparticle diffusion plots depicted in Figure 1(a) (safranin) and Figure S2a (toluidine) are less than those of Elovich plots displayed in Figure S1b (safranin) and Figure S2b (toluidine). Thus, the Elovich model appropriately describes the data where electrostatic bond formation between the cationic sites of safranin/toluidine and anionic carboxylate groups of the hydrogel is predominant [46].


### 3.7. Isotherm Studies

To determine the surface properties and affinity of the adsorbent towards various environmental contaminants, various isotherm models like Langmuir, Freundlich, and Temkin models were used. Their theoretical and mathematical backgrounds have been described in the experimental section. The estimated parameters calculated are described as follows:The Langmuir isotherm plots,Ce/qe versus Ce, are given in Figures 9(a)–9(c) for safranin and Figures 10(a)–10(c) for toluidine. From the slope and intercept of these plots, the values of KL and Qm were estimated. The values of these constants along with the correlation coefficient R2 are given in Tables 4(a) and 4(b).Figure 9
Adsorption isotherms for safranin adsorption on the GA/AM (adsorbent 0.01 g, time 60 min, dye solution 10 mL, pH 11, temp 293,313, 333 K). Langmuir isotherm at (a) 293 K, (b) 313 K, and (c) 333 K; Freundlich isotherm at (d) 293 K, (e) 313 K, and (f) 333 K; and Temkin isotherm at (g) 293 K, (h) 313 K, and (i) 333 K.
(a)(b)(c)(d)(e)(f)(g)(h)(i)Figure 10
Adsorption isotherms for the toluidine adsorption on the GA/AM (adsorbent 0.01 g, dye solution 10 mL, time 60 min, pH 11, temp 293, 313, 333 K). Langmuir isotherm at (a) 293 K, (b) 313 K, and (c) 333 K; Freundlich isotherm at (d) 293 K, (e) 313 K, and (f) 333 K; and Temkin isotherm at (g) 293 K, (h) 313 K, and (i) 333 K.
(a)(b)(c)(d)(e)(f)(g)(h)(i)Table 4(a)
Isothermal parameters for the adsorption of safranin dye on the prepared adsorbent
Parameter293 K313 K333 KLangmuir isotherm modelQm (mg/g)833769769Ka6.14×10−30.010.02R20.99150.99740.9939Freundlich isotherm model1/n0.56870.50590.3752Kf20.6533.7280.31R20.95770.95080.9823Temkin isotherm modelB1183.38175.03138.49KT0.0580.0940.349R20.98790.99220.9739(b)
Isothermal parameters for the adsorption of toluidine dye on the prepared adsorbent
Parameter293 K313 K333 KLangmuir isotherm modelQm (mg/g)526500592Ka0.01060.0210.051R20.91470.98020.9992Freundlich isotherm model1/n0.52590.43080.3256Kf22.141.6581.73R20.7310.76480.8392Temkin isotherm modelB1125.79111.8790.278KT0.0940.1950.724R20.84530.86990.925The Freundlich isotherm plots,lnqe versus Ce, are shown in Figures 9(d)–9(f) (safranin) and Figures 10(d)–10(f) (toluidine). Drawing such plots makes it possible to estimate values of constants: n and Kf (from the slope and intercept).The Temkin isotherm plots,qe versus lnCe, that give us the values of the constants of the model are shown in Figures 9(g)–9(i) (for safranin) and Figures 10(g)–10(i) (for toluidine) while the respective values of the constants are shown in Tables 4(a) and 4(b). According to Tables 4(a) and 4(b), the regression values are higher for the Freundlich as compared with those of the Langmuir and Temkin models.


### 3.8. Thermodynamics of the Process

The thermodynamic parameters for the adsorption of dyes on the polymeric hydrogel were calculated using the following equations (10) and (11):
(10)∆G°=−RTlnKd,where Kd=qe/Ce,
(11)lnlnKd=∆S°R−∆H°RT.In these equations,ΔG°, ΔH°, and ΔS° are the changes in the Gibbs free energy, enthalpy, and entropy, respectively. A plot lnKd versus 1/T defines the parameters: ΔH° and ΔS° that are usually obtained from the slope and intercept of the given plot (Figures 11 and 12). Their values are given in Table 5(a) (safranin) and Table 5(b) (toluidine). The values of Gibbs free energy (ΔG°) were negative at all temperatures indicating a spontaneous nature and feasibility of the process at high temperature. The observed increase in ΔG° values with an increase in temperature suggests that a higher temperature would result in the faster absorption of the dye. The positive value of the ΔH° indicates the endothermic nature of the process and the positive value of entropy show the increase in randomness at the dye/adsorbent interfaces. [47]Figure 11
Effect of temperature on adsorption of safranin on GA/AM (adsorbent 0.01, dye solution 10 mL, time 60 min, pH 11, temp 293, 313, 333 K).Figure 12
Effect of temperature on adsorption of toluidine on GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, time 60 min, temp 293,313, 333 K).Table 5(a)
Thermodynamic parameters for the adsorption of safranin on polymeric hydrogel
∆G° (kJ·mol−1)∆H° (kJ·mol−1)∆S° (kJ·mol−1·K−1)293 K313 K333 K6876.5125.189−503.845−1007.647−1511.427(b)
Thermodynamic parameters for the adsorption of toluidine on polymeric hydrogel
∆G° (kJ·mol−1)∆H° (kJ·mol−1)∆S° (kJ·mol−1·K−1)293 K313 K333 K5324.95118.247−21.42−386.36−751.3


### 3.9. Compression of Adsorption Capacity of Prepared Hydrogel with Those Reported in Literature

The adsorption capacity of the present adsorbent under study was compared with the adsorbent reported in literature as given in Table6. Despite of the polymeric nature, the hydrogel has exhibited high adsorption capacity as compared with few of those adsorbents reported in literature.Table 6
Comparison of the hydrogel adsorption capacity with the activated carbon adsorption capacity.
S. no.AdsorbentAdsorption capacityReferences1Wood ofPaulownia tomentosa238.44 (mg/g)[10]2Pd–Ni/AC333.3 (mg/g)[15]3Magnetic activated carbon149.2 (mg/g)[21]4ActivatedAilanthus altissima sawdust11.46 (mg/g)[50]5Hydrogel gum arabic/acrylamide526 (mg/g) for toluidine and 833 (mg/g) for safraninPresent study


### 3.10. Reusability and Regeneration of Polymeric Hydrogel

The beauty of the prepared hydrogel adsorbent is reusing by a simple and easy method to remove the entrapped dyes in the hydrogel network structure via the solvent extraction method. This method is good as compared with others because the dye molecules do not decompose in this method and are recycled its initial state. The regeneration experiment of the hydrogel was investigated in 5 cycles, and the results are as shown in Figure13 [44, 45].Figure 13
Reusability and regeneration of polymeric hydrogel (GA/AM) toward safranin and toluidine dyes.


## 3.1. Surface Morphology

The morphology of polymer hydrogel was studied using SEM analysis. The SEM images are shown in Figure1. The micrographs show rough interfaces along with many cavities with characteristic irregular channels of hydrogel that would probably be responsible for the enhanced adsorption of the selected dyes [26, 28].Figure 1
SEM images of hydrogel at various magnifications: (a) 1.00μm and (b) 500 nm.
(a)(b)


## 3.2. Surface Functionalities

FTIR spectroscopy was used to identify the surface functional groups on polymeric hydrogel as shown in Figure2. Both characteristic bands of the acrylamide and gum arabic are present in the synthesized hydrogel. The broad and strong peak at 3428 cm−1 is related to the NH or OH stretching of the carboxylic and hydroxyl groups of acrylamide [26, 28, 29]. The medium peaks at 1067–1090 cm−1 represent the stretching vibration of C−O−C and C−O−H bonds. The sharpest peak at 1669 cm−1 is related to C=O stretching. The amide bond presence was confirmed from a weak and obvious band at 1456 cm−1, which is due to the C−N bending vibration. The two strong peaks at 1565–1648 cm−1 shows the C=O stretching [37, 38]. The presence of peaks for both of hydrogel and acryl amide in FTIR spectra confirm the formation of the polymeric hydrogel network that was attempted to be prepared through a free radical polymerization reaction in this study.Figure 2
FTIR spectrum of polymeric GA/AM hydrogel.


## 3.3. Surface Area and Thermal Properties of the Hydrogel

Various models like Brunauer-Emmett-Teller (BET), Brookhurst Junior High (BJH), Langmuir, and Dubinin-Radushkevitch (DR) are used to find out the surface area of the adsorbents. Among the abovementioned methods, the commonly used method is BET surface area (m2/g) analysis that is frequently used to determine the specific surface area, pore size, and pore distribution of the adsorbents. This method involves the nitrogen adsorption and desorption processes (Table 2). The isotherm of the adsorption-desorption of hydrogel refers to the type IV isotherm as shown in Figure 3. The increase in pore size distribution can be confirmed from increase in area under the hysteresis loops with increase in temperature. The BET equation is expressed as equation (8)) as follows [39].
(8)1WP0/P−1=1WmC+C−1WmCPp0,where W is the weight of gas adsorbed, P/P0 is relative pressure, Wm is the weight of adsorbate constituting a monolayer coverage, and C is related to the energy of adsorption in the first adsorbed layer.Table 2
Surface area and pore size distribution of hydrogel GA/AM.
Surface area (m2/g)Pore size distributionBJH methodsDR methodBETPore volume (cm3/g)Pore diameter (A°)Micropore volume (cm3/g)Average pore width (A°)Ads. Energy (kJ/mol)26.73500.06810.4530.06811.1793.853Figure 3
Characterization of hydrogel: (a) BET surface area and (b) thermogram.
(a)(b)The thermogram of GA/AM sorption as presented in Figure3(b) displays three phases of mass loss corresponding to different temperature domains. The first phase with 5% (40–130°C) mass loss is due to the elimination of water molecules and dehydration of neighboring –COOH functionalities [40, 41]. The second (130–250°C) mass loss can be attributed to decarboxylation of the remaining –COOH groups. The final-phase (250–500°C) mass loss is most probably due to the degradation of polymeric chains and breakage of the 3D polymeric network of the hydrogel.


## 3.4. Point of Zero Charge (PZC) and pH Effect on the Absorption of Safranin and Toluidine

The PZC of GA/AM was noted as 7.1 in Figure4(a). The surface was positively charged at acidic pH whereas at basic pH, it was negatively charged. As both the dyes are cationic, therefore, the favorable interaction was observed at 11 pH and high adsorption was observed at this pH as shown in Figure 4(b).Figure 4
(a) Point of zero charge (conditions: temp 313 K, dose 0.01–0.005, time 24 h, pH range (2–11) adjusted by 0.1 M HNO3 and NaOH, using NaNO3 0.1 N solution and volume 30 mL) and (b) effect of pH on the % removal of safranin and toluidine by hydrogel.
(a)(b)The process of adsorption of the dyes (safranin, toluidine) from the solution by superabsorbent hydrogel takes place under the influence of two types of driving forces in which the first one is diffusion of dyes in the network of hydrogel that occurs whereas the second deriving force is electrostatic interactions between adsorbent and adsorbate. The pH of media markedly affects the process of adsorption [26, 28, 29]. Figure 4(b) explains the effect of pH on the selected dye adsorption. The rate of adsorption increases with the increase in pH of the medium. At PZC, the percentage removal of dyes decreases slightly as the isoelectric point is lying there. The percentage removal then abruptly increases after PZC as the pores became negatively charged; thus, maximum adsorption of the dyes occurred [26, 28, 29]. The hydrogel showed a %removal of 78 to 73 for safranin and toluidine at highest pH tested whereas the % removal was 56 and 55% for safranin toluidine, respectively, at PZC (pH 7.08). The % removal of the selected dyes was calculated using equation (9).
(9)%removal=Co−CeCo×100.


## 3.5. Effect of Contact Time on Adsorption

The effect of contact time on the absorption of dyes, safranin and toluidine, was investigated in the abovementioned fed-batch experiment described in detail. The results are graphically shown in Figures5 and 6 for safranin and toluidine, respectively. Initially, the rate of adsorption is high as there is no competition for adsorption sites being free. Up to 60 min, the rate of adsorption increases proportionately, and then, equilibrium is reached where adsorption and desorption rates are equal; thus, the curve has become parallel up to 480 min. The adsorption rate in the beginning is high because of the availability of a larger number of active sites on the surface of hydrogel. Such types of behavior have been observed in other studies as well [42]. Thus, 60 min time was noted as equilibrium time for the 0.01 g hydrogel used.Figure 5
Effect of time on the adsorption of safranin on polymeric hydrogel (adsorbent dosage 0.01 g, dye solution 10 mL, time 30–480 min,pH=11, temperature 313 K).Figure 6
Effect of time on the adsorption of toluidine on polymeric hydrogel (adsorbent dosage 0.01 g, dye solution 10 mL, time 30–480 min,pH=11, temperature 313 K).


## 3.6. Adsorption Kinetics

Adsorption kinetics are important while evaluating the adsorption processes, and one can get insight into the adsorption mechanism and adsorbate-adsorbent interaction [43]. From an economical point of view in the industries, it is important to have information about kinetics of a given process.The experimental data of the kinetics study were fitted into different models which are graphically shown in Figures7(a)–7(d) (safranin) and Figures 8(a)–8(d) (toluidine). The slope and intercept values in the case of each model were calculated and interpreted as valuable adsorption parameters listed in Tables 3(a) and 3(b). The R2 (linear correlation coefficients) values (0.99) of pseudo-second-order plots (Figures 7(b) and 8(b)) are significantly higher than that of pseudo-first-order plots (Figures 7(a) and 8(a); R2=0.82–0.96) indicating the chemical nature of the sorption process [44, 45]. Also, the Qe experimental and calculated values in the case of the pseudo-second-order model are close to each other, clearly indicating that the best fit of the kinetics data can be achieved with this model. Moreover, the k2 values increase with the rise in temperature which indicates a high adsorption rate at elevated temperature.Figure 7
Kinetics of safranin adsorption on GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, temp 313 K, time 60 min): (a) pseudo-1st-order plot and (b) pseudo-2nd-order plot.
(a)(b)Figure 8
Kinetics of toluidine adsorption on the GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, temp 313 K, time 60 min): (a) pseudo-1st-order plot and (b) pseudo-2nd-order plot.
(a)(b)Table 3(a)
Kinetics parameters estimated from the kinetics model for safranin adsorption on the prepared adsorbent
Parameter293 K313 K333 KPseudofirst orderK1 (min−1)0.570.0530.072Qe (mg/g; calculated)66.6961.0377.52Qe (mg/g; experimental)249268295R20.95220.95720.9603Pseudosecond orderQe (mg/g; calculated)256.4277.7303.1Qe (mg/g; experimental)249268295K2 (g/mg/min)1.49×10−31.59×10−31.67×10−3R20.99980.99980.9999(b)
Kinetics parameters estimated from the kinetics model for toluidine adsorption on the prepared adsorbent
Parameter293 K313 K333 KPseudofirst orderK1 (min−1)0.0610.0580.063Qe (mg/g; calculated)59.7153.2546.62Qe (mg/g; experimental)217.4232.12249.77R20.92990.9440.9022Pseudosecond orderQe (mg/g; calculated)227.27238.09256.41Qe (mg/g; experimental)217.4232.12249.77K2 (g/mg/min)0.001650.001940.00231R20.99960.99980.9998TheR2 values of the intraparticle diffusion plots depicted in Figure 1(a) (safranin) and Figure S2a (toluidine) are less than those of Elovich plots displayed in Figure S1b (safranin) and Figure S2b (toluidine). Thus, the Elovich model appropriately describes the data where electrostatic bond formation between the cationic sites of safranin/toluidine and anionic carboxylate groups of the hydrogel is predominant [46].


## 3.7. Isotherm Studies

To determine the surface properties and affinity of the adsorbent towards various environmental contaminants, various isotherm models like Langmuir, Freundlich, and Temkin models were used. Their theoretical and mathematical backgrounds have been described in the experimental section. The estimated parameters calculated are described as follows:The Langmuir isotherm plots,Ce/qe versus Ce, are given in Figures 9(a)–9(c) for safranin and Figures 10(a)–10(c) for toluidine. From the slope and intercept of these plots, the values of KL and Qm were estimated. The values of these constants along with the correlation coefficient R2 are given in Tables 4(a) and 4(b).Figure 9
Adsorption isotherms for safranin adsorption on the GA/AM (adsorbent 0.01 g, time 60 min, dye solution 10 mL, pH 11, temp 293,313, 333 K). Langmuir isotherm at (a) 293 K, (b) 313 K, and (c) 333 K; Freundlich isotherm at (d) 293 K, (e) 313 K, and (f) 333 K; and Temkin isotherm at (g) 293 K, (h) 313 K, and (i) 333 K.
(a)(b)(c)(d)(e)(f)(g)(h)(i)Figure 10
Adsorption isotherms for the toluidine adsorption on the GA/AM (adsorbent 0.01 g, dye solution 10 mL, time 60 min, pH 11, temp 293, 313, 333 K). Langmuir isotherm at (a) 293 K, (b) 313 K, and (c) 333 K; Freundlich isotherm at (d) 293 K, (e) 313 K, and (f) 333 K; and Temkin isotherm at (g) 293 K, (h) 313 K, and (i) 333 K.
(a)(b)(c)(d)(e)(f)(g)(h)(i)Table 4(a)
Isothermal parameters for the adsorption of safranin dye on the prepared adsorbent
Parameter293 K313 K333 KLangmuir isotherm modelQm (mg/g)833769769Ka6.14×10−30.010.02R20.99150.99740.9939Freundlich isotherm model1/n0.56870.50590.3752Kf20.6533.7280.31R20.95770.95080.9823Temkin isotherm modelB1183.38175.03138.49KT0.0580.0940.349R20.98790.99220.9739(b)
Isothermal parameters for the adsorption of toluidine dye on the prepared adsorbent
Parameter293 K313 K333 KLangmuir isotherm modelQm (mg/g)526500592Ka0.01060.0210.051R20.91470.98020.9992Freundlich isotherm model1/n0.52590.43080.3256Kf22.141.6581.73R20.7310.76480.8392Temkin isotherm modelB1125.79111.8790.278KT0.0940.1950.724R20.84530.86990.925The Freundlich isotherm plots,lnqe versus Ce, are shown in Figures 9(d)–9(f) (safranin) and Figures 10(d)–10(f) (toluidine). Drawing such plots makes it possible to estimate values of constants: n and Kf (from the slope and intercept).The Temkin isotherm plots,qe versus lnCe, that give us the values of the constants of the model are shown in Figures 9(g)–9(i) (for safranin) and Figures 10(g)–10(i) (for toluidine) while the respective values of the constants are shown in Tables 4(a) and 4(b). According to Tables 4(a) and 4(b), the regression values are higher for the Freundlich as compared with those of the Langmuir and Temkin models.


## 3.8. Thermodynamics of the Process

The thermodynamic parameters for the adsorption of dyes on the polymeric hydrogel were calculated using the following equations (10) and (11):
(10)∆G°=−RTlnKd,where Kd=qe/Ce,
(11)lnlnKd=∆S°R−∆H°RT.In these equations,ΔG°, ΔH°, and ΔS° are the changes in the Gibbs free energy, enthalpy, and entropy, respectively. A plot lnKd versus 1/T defines the parameters: ΔH° and ΔS° that are usually obtained from the slope and intercept of the given plot (Figures 11 and 12). Their values are given in Table 5(a) (safranin) and Table 5(b) (toluidine). The values of Gibbs free energy (ΔG°) were negative at all temperatures indicating a spontaneous nature and feasibility of the process at high temperature. The observed increase in ΔG° values with an increase in temperature suggests that a higher temperature would result in the faster absorption of the dye. The positive value of the ΔH° indicates the endothermic nature of the process and the positive value of entropy show the increase in randomness at the dye/adsorbent interfaces. [47]Figure 11
Effect of temperature on adsorption of safranin on GA/AM (adsorbent 0.01, dye solution 10 mL, time 60 min, pH 11, temp 293, 313, 333 K).Figure 12
Effect of temperature on adsorption of toluidine on GA/AM (adsorbent 0.01, dye solution 10 mL, pH 11, time 60 min, temp 293,313, 333 K).Table 5(a)
Thermodynamic parameters for the adsorption of safranin on polymeric hydrogel
∆G° (kJ·mol−1)∆H° (kJ·mol−1)∆S° (kJ·mol−1·K−1)293 K313 K333 K6876.5125.189−503.845−1007.647−1511.427(b)
Thermodynamic parameters for the adsorption of toluidine on polymeric hydrogel
∆G° (kJ·mol−1)∆H° (kJ·mol−1)∆S° (kJ·mol−1·K−1)293 K313 K333 K5324.95118.247−21.42−386.36−751.3


## 3.9. Compression of Adsorption Capacity of Prepared Hydrogel with Those Reported in Literature

The adsorption capacity of the present adsorbent under study was compared with the adsorbent reported in literature as given in Table6. Despite of the polymeric nature, the hydrogel has exhibited high adsorption capacity as compared with few of those adsorbents reported in literature.Table 6
Comparison of the hydrogel adsorption capacity with the activated carbon adsorption capacity.
S. no.AdsorbentAdsorption capacityReferences1Wood ofPaulownia tomentosa238.44 (mg/g)[10]2Pd–Ni/AC333.3 (mg/g)[15]3Magnetic activated carbon149.2 (mg/g)[21]4ActivatedAilanthus altissima sawdust11.46 (mg/g)[50]5Hydrogel gum arabic/acrylamide526 (mg/g) for toluidine and 833 (mg/g) for safraninPresent study


## 3.10. Reusability and Regeneration of Polymeric Hydrogel

The beauty of the prepared hydrogel adsorbent is reusing by a simple and easy method to remove the entrapped dyes in the hydrogel network structure via the solvent extraction method. This method is good as compared with others because the dye molecules do not decompose in this method and are recycled its initial state. The regeneration experiment of the hydrogel was investigated in 5 cycles, and the results are as shown in Figure13 [44, 45].Figure 13
Reusability and regeneration of polymeric hydrogel (GA/AM) toward safranin and toluidine dyes.


## 4. Conclusions

In this study, polymeric hydrogel GA/AM (that has not been used as adsorbent for the selected dyes previously) was prepared by grafting acrylamide on gum arabic with a crosslinker and initiator. The surface morphology and physicochemical properties of the prepared hydrogel were studied by the SEM, FTIR, and BET surface area analyzer. The point of zero charge was also determined in order to explain the effect of pH on the adsorption of selected dyes. Electrostatic interactions between the negatively charged adsorbent surface and positively charged at pH 11 are the responsible factor for high absorption values at the mentioned pH. The adsorption capacities of the prepared adsorbent were 833 mgg−1 and 526 mgg−1 mgg−1 for safranin and toluidine, respectively, showing that the adsorbent is quite efficient in removing the selected dyes. The adsorption phenomena and kinetics were better explained by the Langmuir isotherm and pseudo-second-order kinetic model whereas the thermodynamic aspects of the adsorption process were endothermic, spontaneous, and favorable at high temperature. After the 5th cycle, an appreciable dye removal ability of more than 60% was still retained showing the reusability of the prepared adsorbent for many times. From the results, it can be concluded that this hydrogel can be used as an alternative of activated carbon to treat water contaminated with toxic dyes.



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*Source: 6100791-2022-05-10.xml*