# Sorption Efficiency of a New Sorbent towards Cadmium(II): Methylphosphonic Acid Grafted Polystyrene Resin

Authors: Nacer Ferrah; Omar Abderrahim; Mohamed Amine Didi; Didier Villemin
Journal: Journal of Chemistry
 (2013)

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## Abstract

A new chelating polymeric sorbent has been developed using polystyrene resin grafted with phosphonic acid. After characterization by FTIR and elementary analysis, the new resin has been investigated in liquid-solid extraction of cadmium(II). The results indicated that phosphonic resin could adsorb Cd(II) ion effectively from aqueous solution. The adsorption was strongly dependent on the pH of the medium and the optimum pH value level for better sorption was between 3.2 and 5.2. The influence of other analytical parameters including contact time, amount of resin, metal ion concentration, and the presence of some electrolytes was investigated. The maximum uptake capacity of Cd(II) ions was 37,9 mg·g−1 grafted resin at ambient temperature, at an initial pH value of 5.0. The overall adsorption process was best described by pseudo second-order kinetic. When Freundlich and Langmuir isotherms were tested, the latter had a better fit with the experimental data. Furthermore, more than 92% of Cd(II) could be eluted by using 1.0 mol·L−1 HCl in one cycle.


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## Body

## 1. Introduction

Some heavy metals like Cd, Hg, As, Pb, and so forth have no biological function and are detrimental to the organisms even at a very low concentration [1]. They originate from natural sources such as rocks, metalliferous minerals, and anthropogenic inputs from agriculture, metallurgy, energy production, microelectronics, mining, sewage sludge, and waste disposal [2, 3]. A concentration higher than the prescribed limit may lead to the formation of nonspecific complex compounds in the cell, which leads to toxic effects. The major sources of cadmium release into the environment are electroplating, smelting, plastics, batteries, paint pigments, and mining and refining processes [4].In this industrialized era, the presence of cadmium ions in aqueous water ways has become a serious environmental problem, and many methods such as ion exchange, surface complexation, diffusion through the solid, reverse osmosis, membrane separation, chemical oxidation or reduction, co-precipitation, and control of sample-specific surface area have been employed to remove it from wastewater [5–8]. It reveals that surface complexation is the most important mechanism with possibly ion exchange and solid diffusion also contributing to the overall sorption process [9]. The use of solid phase extraction has been proved to be more advantageous in the view of their total insolubility in aqueous phase, low rate of physical degradation, high sorption capacity for metal ions, low organic solvent inventory, and good flexibility in working conditions [9].In the present work, we described the synthesis and characterization of polystyrene resin grafted with phosphonic acid. This resin was applied as a new sorption material for cadmium(II) extraction in batch process. The effects of analytical parameters, adsorption kinetic, isotherm studies, and desorption process were investigated.


## 2. Experimental

### 2.1. Instrumentation

Infrared spectra were recorded on a Perkin-Elmer ATR spectrometer. A Bruker Advance 400 spectrometer was used for13C and 31P MAS NMR analysis. Elemental analyses were carried out on a Thermoquest CHP analyzer. Visible spectra were measured using Perkin-Elmer-Lambda 800 UV-Vis spectrophotometer. pH measurements were taken on a potentiometer Consort C831.


### 2.2. Reagents

Chloromethyl styrene-divinylbenzene copolymer (S-3% DVB) was precursor of Amberlite resin, gifted by Rohm and Haas Company. Triethylphosphite, hydrobromic acid, acetic acid, oxalic acid, sodium acetate, sodium sulphate, sodium hydroxide (80%), dichloromethane, sulphuric acid 95–97%, acetone, and 4-(2-pyridylazo)resorcinol (PAR) were provided from Fluka. Cadmium sulphate (99%), sodium nitrate, sodium acetate, ethylenediaminetetraacetic acid (EDTA), ammonium carbonate, and sodium chloride were obtained from Merck. Hydrochloride acid (36%) and nitric acid (65%) were purchased from Reidel-de-Haen.Stock solution (1.0 mol·L−1) of cadmium(II) was prepared by dissolving her sulphate salt in distilled water. Solutions of lower concentrations were prepared by the dilution of stock solution.


### 2.3. Synthesis of Polystyrene Resin Anchored with Phosphonic Acid

The sorbent, phosphonic acid grafted polystyrene resin beads, was synthesized using the Arbuzov reaction [10–13] (Figure 1). In the first step, after washing the Merrifield resin beads with acetone and dried under vacuum, Merrifield resin 3% (20.34 g) was reacted with 35 mL of triethylphosphite (excess). The reaction mixture was refluxed for 4 hours (hrs). The phosphonate grafted polystyrene resin beads obtained were purified from the excess of reactants by washing repeatedly with water and acetone. The resin beads were dried under vacuum (14.26 g). In the second step, a bromide hydrogen acid (33 mL) was added on the phosphonate grafted polystyrene resin beads (10.00 g) and vigorously shaken on a vibrating table under reflux for 3 hrs. In order to remove unreacted reagents, the resulting resin beads were filtered, washed repeatedly with distilled water and dichloromethane, and dried in vacuum (8.62 g).Figure 1
Scheme for synthesis of methylene phosphonic acid grafted polystyrene resin beads.


### 2.4. Characterization Studies

The structure and purity of the final complexing agent were identified and characterized by MAS NMR of31P and 13C spectroscopy, FTIR measurement, and elemental microanalysis. The MAS NMR spectra showed the expected signals due to the polystyrene skeleton and phosphonic units as matched to the proposed structure (Figure 1).31P MAS NMR is 17.8 ppm, 13C MAS is 36.4 ppm (CH2–P), 127.75, 130.1, 137.1, and 138.5 (CH–CH) ppm. The presence of phosphonic acid was confirmed by the appearance of absorption at 3000–2850 cm−1 (OH), 1124 cm−1 (P=O), 1037 cm−1 (νas P–OH), and 941 cm−1 (νs P–OH) and by the disappearance of P-OEt band at 1023 cm−1 [14]. The experimental CHP analysis data (%) of phosphonic acid grafted polystyrene resin is C, 85.31; H, 9.34; P, 2.35.


### 2.5. Adsorption Technique

Batch technique was applied to investigate the different parametric effects on the sorption process, where a certain weight 0.030 g (m) of the grafted resin was mixed with a certain volume 5 mL (V) of Cd(II) aqueous solutions and equilibrated by shaking in a shaker with speed 250 round per minute (rpm) at room temperature. The ratio of m/V (6.0 g·L−1) was kept constant for all the experiments. The solutions were separated after a certain time (t) and the concentrations of Cd(II) in the aqueous phase were determined, before and after extraction spectrophotometrically with PAR at pH 5.5 [15]. The absorbance of PAR-cadmium(II) complex was measured at 520 nm. The extraction yield (%) was determined using the following equation:
(1)Extractionyield(%)=(C0-CeC0)100%,
where C0 and Ce denote the initial and equilibrium concentrations of Cd(II) in the aqueous phase (mol·L−1).


### 2.6. Kinetic and Sorption Isotherms

In order to quantify the extent of uptake in adsorption kinetics three simple kinetic models were tested [16].(1)
Lagergren’s pseudo first-order rate equation expressed as follows:(2)log(qe-qt)=logqe-k12.303t,
where k1 (min−1) is the equilibrium rate constant of the pseudo first-order adsorption, qt and qe are the amount of Cd(II) adsorbed (mg·g−1) at time t and equilibrium time (180 min), respectively. The values of k1 and qe can be obtained from the intercept and slope of the plot of (log(qe-qt)) versus (t/2.303).(2)
A pseudo second-order adsorption kinetic rate equation is(3)tqt=1k2qe2+tqe,
where k2 (g·mg−1·min−1) is the rate constant of the pseudo second-order adsorption. The values of  k2 and qe were obtained from the intercept and slope of the plot of (t/qt) versus t.(3)
A second-order adsorption kinetic rate equation is(4)1qe-qt=1qe+k3t,
where k3 (g·mg−1·min−1) is the rate constant of the second-order adsorption. The values of k3 and qe can be obtained from the intercept and slope of the plot of (1/(qe-qt)) versus t.Sorption isotherms for Cd(II) were determined over the concentration range of 10−3 to 10−2mol·L−1. The amount of ions sorbed by phosphonic resin, qt (mg·g−1) was calculated by the following relationship:
(5)qt(mgg)=(C0-Ct)·V·Mm,
where Ct is the final concentrations at certain time t of the ions in the liquid phase (mol·L−1), V is the volume of the aqueous phase (5 mL), m is the weight of grafted resin (0.030 g), and M (112.411 g·mol−1) is the atomic weight of cadmium.


## 2.1. Instrumentation

Infrared spectra were recorded on a Perkin-Elmer ATR spectrometer. A Bruker Advance 400 spectrometer was used for13C and 31P MAS NMR analysis. Elemental analyses were carried out on a Thermoquest CHP analyzer. Visible spectra were measured using Perkin-Elmer-Lambda 800 UV-Vis spectrophotometer. pH measurements were taken on a potentiometer Consort C831.


## 2.2. Reagents

Chloromethyl styrene-divinylbenzene copolymer (S-3% DVB) was precursor of Amberlite resin, gifted by Rohm and Haas Company. Triethylphosphite, hydrobromic acid, acetic acid, oxalic acid, sodium acetate, sodium sulphate, sodium hydroxide (80%), dichloromethane, sulphuric acid 95–97%, acetone, and 4-(2-pyridylazo)resorcinol (PAR) were provided from Fluka. Cadmium sulphate (99%), sodium nitrate, sodium acetate, ethylenediaminetetraacetic acid (EDTA), ammonium carbonate, and sodium chloride were obtained from Merck. Hydrochloride acid (36%) and nitric acid (65%) were purchased from Reidel-de-Haen.Stock solution (1.0 mol·L−1) of cadmium(II) was prepared by dissolving her sulphate salt in distilled water. Solutions of lower concentrations were prepared by the dilution of stock solution.


## 2.3. Synthesis of Polystyrene Resin Anchored with Phosphonic Acid

The sorbent, phosphonic acid grafted polystyrene resin beads, was synthesized using the Arbuzov reaction [10–13] (Figure 1). In the first step, after washing the Merrifield resin beads with acetone and dried under vacuum, Merrifield resin 3% (20.34 g) was reacted with 35 mL of triethylphosphite (excess). The reaction mixture was refluxed for 4 hours (hrs). The phosphonate grafted polystyrene resin beads obtained were purified from the excess of reactants by washing repeatedly with water and acetone. The resin beads were dried under vacuum (14.26 g). In the second step, a bromide hydrogen acid (33 mL) was added on the phosphonate grafted polystyrene resin beads (10.00 g) and vigorously shaken on a vibrating table under reflux for 3 hrs. In order to remove unreacted reagents, the resulting resin beads were filtered, washed repeatedly with distilled water and dichloromethane, and dried in vacuum (8.62 g).Figure 1
Scheme for synthesis of methylene phosphonic acid grafted polystyrene resin beads.


## 2.4. Characterization Studies

The structure and purity of the final complexing agent were identified and characterized by MAS NMR of31P and 13C spectroscopy, FTIR measurement, and elemental microanalysis. The MAS NMR spectra showed the expected signals due to the polystyrene skeleton and phosphonic units as matched to the proposed structure (Figure 1).31P MAS NMR is 17.8 ppm, 13C MAS is 36.4 ppm (CH2–P), 127.75, 130.1, 137.1, and 138.5 (CH–CH) ppm. The presence of phosphonic acid was confirmed by the appearance of absorption at 3000–2850 cm−1 (OH), 1124 cm−1 (P=O), 1037 cm−1 (νas P–OH), and 941 cm−1 (νs P–OH) and by the disappearance of P-OEt band at 1023 cm−1 [14]. The experimental CHP analysis data (%) of phosphonic acid grafted polystyrene resin is C, 85.31; H, 9.34; P, 2.35.


## 2.5. Adsorption Technique

Batch technique was applied to investigate the different parametric effects on the sorption process, where a certain weight 0.030 g (m) of the grafted resin was mixed with a certain volume 5 mL (V) of Cd(II) aqueous solutions and equilibrated by shaking in a shaker with speed 250 round per minute (rpm) at room temperature. The ratio of m/V (6.0 g·L−1) was kept constant for all the experiments. The solutions were separated after a certain time (t) and the concentrations of Cd(II) in the aqueous phase were determined, before and after extraction spectrophotometrically with PAR at pH 5.5 [15]. The absorbance of PAR-cadmium(II) complex was measured at 520 nm. The extraction yield (%) was determined using the following equation:
(1)Extractionyield(%)=(C0-CeC0)100%,
where C0 and Ce denote the initial and equilibrium concentrations of Cd(II) in the aqueous phase (mol·L−1).


## 2.6. Kinetic and Sorption Isotherms

In order to quantify the extent of uptake in adsorption kinetics three simple kinetic models were tested [16].(1)
Lagergren’s pseudo first-order rate equation expressed as follows:(2)log(qe-qt)=logqe-k12.303t,
where k1 (min−1) is the equilibrium rate constant of the pseudo first-order adsorption, qt and qe are the amount of Cd(II) adsorbed (mg·g−1) at time t and equilibrium time (180 min), respectively. The values of k1 and qe can be obtained from the intercept and slope of the plot of (log(qe-qt)) versus (t/2.303).(2)
A pseudo second-order adsorption kinetic rate equation is(3)tqt=1k2qe2+tqe,
where k2 (g·mg−1·min−1) is the rate constant of the pseudo second-order adsorption. The values of  k2 and qe were obtained from the intercept and slope of the plot of (t/qt) versus t.(3)
A second-order adsorption kinetic rate equation is(4)1qe-qt=1qe+k3t,
where k3 (g·mg−1·min−1) is the rate constant of the second-order adsorption. The values of k3 and qe can be obtained from the intercept and slope of the plot of (1/(qe-qt)) versus t.Sorption isotherms for Cd(II) were determined over the concentration range of 10−3 to 10−2mol·L−1. The amount of ions sorbed by phosphonic resin, qt (mg·g−1) was calculated by the following relationship:
(5)qt(mgg)=(C0-Ct)·V·Mm,
where Ct is the final concentrations at certain time t of the ions in the liquid phase (mol·L−1), V is the volume of the aqueous phase (5 mL), m is the weight of grafted resin (0.030 g), and M (112.411 g·mol−1) is the atomic weight of cadmium.


## 3. Results and Discussion

### 3.1. Effect of pH

Changes in the pH of the medium are one of the most important factors affecting the concentration and metal recovery procedure, which is related to the formation of soluble metal complexes and subsequently their stabilities in aqueous solutions. It is well known that surface charge of adsorbent can be modified by changing the pH of the solution and the chemical species in the solution depends on this parameter [17]. According to the chemical equilibrium diagram for cadmium in aqueous solution obtained by the MEDUSA program, the species Cd(OH)2 precipitates at pH higher than 8 and the concentration of Cd2+ ions in solution decreases. (Program MEDUSA, Make Equilibrium Diagrams Using Sophisticated Algorithms. http://home.telfort.nl/cheaqs/). Under the experimental conditions of the present paper, Cd2+ was the major species present in solution.In order to optimize the pH for maximum removal, experiments were conducted in the pH range from 1.77 to 5.15 at ambient temperature, 4 hrs equilibration time, and 1.0 mmol·L−1 metal ion concentration. Figure 2 shows the influence of pH in sorption process of Cd(II) by modified resin. As can be seen from Figure 2 the sorption increases quickly with increasing pH values from 1.8 to 3.2. The progressive decrease in the retention of metal ions at low pH is due to [17] the following: (i) the competition of the hydrogen ion with the metal ions for binding to the phosphonic acid group (P–OH); (ii) the oxygen atoms (P=O) are more protonated, and hence, they are less available to coordinate with the cadmium; (iii) the competition between the excess of H+ ions in the medium and positively charged cationic species present in solution; (iv) as pH is increased there is a decrease of positive surface charge, which results in the lower coulombic repulsion of the adsorbing metal ions. Consequently the number of moles of Cd(II) removal may decrease at low pH [18]. The observed reduction in the level of metal ion removal from solution by the sorbent indicates that the interaction between the Cd(II) ions and the sorbent is an ion exchange process.Figure 2
Effect of the initial pH of the aqueous solution on the retention of Cd(II) by the functionalized resin.C0=1.0 mmol·L−1, m=0.030 g, V=5 mL, and contact time = 4 hrs.The data reveals that the highest extraction yield value is recorded at the pH range 3.2–5.2. This is attributed to the presence of free lone pair of electrons on the oxygen of phosphoryl (P=O) group and deprotonated oxygen atoms, which are suitable ligands for coordination with the cadmium ions [19, 20]. This cation exchange process can be represented by the following general reaction [6]:
(6)Resin–P–OH+Cd2+→Resin–P–O–Cd++H+.In order to make further approaching of the functional group of resin and Cd(II), the spectra of resin, before and after Cd(II) is sorbed, are compared. It is found that the characteristic sorption peak of the bond P=0 (at 1124 cm−1) disappears on the whole, which shows that the formation of the coordination bond between oxygen atom and Cd(II) weakens the stretch vibration and causes the peak to shift to the lower frequency. The characteristic sorption peak of P–OH (941 cm−1) is weakened and the new characteristic sorption peak of (-PO32-) is formed [21], which shows that H+ and Cd2+ has been exchanged. All those changes result from the formation of a complex compound.


### 3.2. Effect of Contact Time

The rate of loading of Cd(II) onto the grafted polystyrene resin was determined for two concentrations of Cd(II) 0.5 and 1.0 mmol·L−1, by shaking 5 mL of Cd(II) with 0.030 g of resin in an Erlenmayer flask at ambient temperature for 2, 4, 10, 15, 30, 60, 120, 180, and 200 min. Figure 3 shows that the initial concentration of Cd(II) has an important effect on the rate of sorption. For all the sorption experiments, the amount of cadmium ions sorbed onto the grafted resin increased quickly with time and then slowly reached equilibrium after 180 min. The equilibrium times in which the polymer attains 50% saturation with Cd(II) (half time t1/2) are <2.4 min and <13.0 min for initial Cd(II) concentration = 0.5 mmol·L−1 and 1.0 mmol·L−1, respectively. The amounts of cadmium metal ions sorbed at equilibrium (qe) at [Cd(II)] = 0.5 mmol·L−1 and 1.0 mmol·L−1, respectively, are 9.02 and 17.93 mg·g−1.Figure 3
Effect of contact time on the sorption of Cd(II) on the functionalized resin from aqueous Cd(II) solutions at two different concentrations (C0 and C0′); C0=0.5 mmol·L−1: ■-percent Cd(II) removal, (%), □-uptake (q), mg·g−1; C0′=1.0 mmol·L−1: ★-percent Cd(II) removal, (%), ☆-uptake (q), mg·g−1; V=5 mL; m=0.030 g; initial pH = 5.0.


### 3.3. Rate of Kinetics Adsorption

In this study, batch sorption kinetics of Cd(II) ions at two different concentrations,C0=0.5 and C0′=1.0 mmol·L−1, with the functionalized polymer have been studied. The different values of constants from the slopes and intercepts of linear plots of (2) (figure not shown), (3) (shown in Figure 4), and (4) (figure not showed) are summarized in Table 1. As seen from Table 1, the obtained correlation coefficient for the pseudo second-order model (>0.99) was better than those of the first-order and second-order models for the adsorption of Cd(II) at the two considered concentrations, suggesting that the pseudo second-order model was more suitable to describe the adsorption kinetics of phosphonic acid grafted on polystyrene resin for Cd(II), especially at the lower concentration (0.5 mmol·L−1). This suggests that the rate limiting step may be chemical sorption or chemisorption involving valency forces through sharing or exchange of electrons between sorbent (containing O atoms) and sorbate [16]. Similar results have been observed in the adsorption of Cd(II) by lignocellulosic sorbent [22] and onto kraft and organosolv lignins [23]. The values of the second-order rate constants (k2) were found to decrease from 1.6442 to 0.00262 g·mg−1·min−1 as the initial concentration increased from 0.5 to 1.0 mmol·L−1, showing the process to be highly concentration dependent, which is consistent with studies reported [24].Table 1
Models rate constants for Cd(II) sorption kinetics by the functionalized resin.
Models
Parameters
[Cd(II)]0 = 0.5 mmol·L−1
[Cd(II)]0 = 1.0 mmol·L−1
First-order rate
q
cal. (mg·g−1)
2.20
12.43
q
exp
. (mg·g−1)
9.02
17.93
k
1 (min−1)
0.050
0.020
r
0.800
0.880
Pseudo second-order rate
q
cal. (mg·g−1)
9.09
20.0
q
exp
. (mg·g−1)
9.02
17.93
k
2 (g·mg−1·min−1)
1.6442
0.00262
r
0.999
0.991
Second-order rate
q
cal. (mg·g−1)
0.67
14.37
q
exp
. (mg·g−1)
9.02
17.93
k
3 (g·mg−1·min−1)
0.8052
0.05599
r
0.928
0.901Figure 4
Plots for the adsorption of Cd(II),m=0.030 g, V=5 mL, and initial pH = 5.0.


### 3.4. Sorption Capacity

The retention capacity of functionalized resin was determined by equilibrating 0.030 g of the resin with 5 mL of cadmium(II) ion solutions at different concentrations (0.1.10−2–1.0.10-2mol·L−1), under optimum pH. The experimental capacity obtained is 37.9 mg·g−1 of polymer (Figure 5). At similar conditions, this sorbent possesses very high extraction ability towards Eu(III) and UO22+ cations metals; the extraction capacities are 122.5 and 152.2 mg g−1, respectively [25, 26]. This result is attributed to that phosphonic acid derivatives are more selective towards lanthanides elements [27].Figure 5
Effect of the initial concentration of Cd(II) on the uptake and the extraction yield.m=0.030 g, V=5 mL, equilibrium time = 180 min, and initial pH = 5.0.


### 3.5. Adsorption Isotherm

The adsorbed amounts of Cd(II) on resin have been determined as a function of the metal concentration in the supernatant at the equilibrium state and ambient temperature. The Langmuir treatment (7) is based on the assumption that [28] (i) maximum adsorption corresponds to saturated monolayer of adsorbate molecules on the adsorbent surface, (ii) the energy of adsorption is constant, and (iii) there is no transmigration of adsorbate in the plane of the surface. One has
(7)Ceqe=Ceqm+1qmKL,
where qm and KL are Langmuir constants related to adsorption capacity and energy of adsorption, respectively. The linear plot of Ce/qe versus Ce shows that adsorption obeys Langmuir adsorption model (Figure 6). The correlation coefficient for the linear regression fits of the Langmuir plot was found to be 0.995. qm and KL determined from the Langmuir plot were found to be 38.2 mg·g−1 and 0,0441 L·mol−1, respectively. We note that the capacity of sorption deducted after Langmuir model application is similar to this calculated experimentally (37.9 mg·g−1).Figure 6
Langmuir plot for the adsorption of Cd(II),m=0.030 g, V=5 mL, initial pH = 5.0, and equilibrium time = 180 min.The essential characteristics of Langmuir isotherm can be expressed in terms of a dimensionless constant, separation factor or equilibrium parameter,RL which is defined by
(8)RL=11+KLC0.The value ofRL indicates the type of the isotherm to be either unfavorable (RL>1), linear (RL=1), favorable (0<RL<1), or irreversible (RL=0). As shown in Table 2, the values of RL are ranged from 0.9999 to 0.9995 in the initial Cd(II) ions concentrations 0.01–0.001 mol·L−1. These values indicated that the adsorption process is favorable [29, 30].Table 2
Equilibrium parameter,RL.
C
0, mol·L−1
0.001
0.002
0.004
0.005
0.006
0.008
0.01
R
L
0.99995
0.99991
0.99982
0.99977
0.99973
0.99964
0.99955The Freundlich equation was also applied to the adsorption. The Freundlich equation is basically empirical but is often useful as a means of data description. It generally agrees quite well compared to Langmuir equation and experimental data over a moderate range of adsorbate concentrations [28]. The linearized Freundlich isotherm is represented by
(9)logqe=logKF+1nlogCe.A plot oflog(qe) versus logCe (figure not shown) is linear at only low concentrations of Cd(II) and the constants KF and n were found to be 154.74 mg·g−1and 0.266, respectively. The correlation coefficient for the linear regression fits of the Freundlich plot was found to be 0.830.


### 3.6. Diffusion Study

The adsorption of cadmium(II) on the grafted resin from cadmium sulphate solutions at two different initial metal concentrations was studied as a function of time at ambient temperature. The adsorption onto ion exchange resin must be considered as a liquid-solid phase reaction which includes several steps [31]: (i) The diffusion of ions from the solution to the resin surface, (ii) the diffusion of ions within the solid resin, and (iii) the chemical reaction between ions and functional groups of the resin.The adsorption of the metal is governed by the slowest of these processes. The kinetic models and the rate equations for the above three cases have been established. The exchange of ions can be described by the Nernst-Planck equations which apply to counter diffusion of two species in an almost homogeneous media [17, 31].If the liquid film diffusion controls the rate of exchange, the following relation can be used:(10)-ln(1-F)=kt.If the cases of the diffusion of ions in the resin phase controlling process, the equation used is:(11)-ln(1-F2)=kt.After testing both mathematical models proposed for homogeneous diffusion in the adsorption of Cd(II) onto the resin, this is best fitted when the metal uptake is the particle diffusion controlled and at time contact ≤30 min (Figure7). Thus, the values of the adsorption rate constant, regression equations, and regression coefficients of the diffusion of Cd(II) in the resin phase calculated from the slope of the straight lines (Figure 7) are summarized in Table 3.Table 3
The regression equations (y), regression coefficients (r), and diffusion coefficients (Dr).
[Cd(II)], mmol·L−1
Eq. (10)
Eq. (11)
Eq. (13)
0.5
Y
0.106
t
0.098
t
0.024
t
r
0.925
0.932
0.900
D
r, 10−5, cm²·min−1
—
2.485
—
1.0
Y
0.062
t
0.040
t
0.015
t
r
0.941
0.951
0.945
D
r, 10−5, cm²·min−1
—
1.014
—Figure 7
Plot of (11) for Cd(II) adsorption on grafted resin, m=0.030 g, V=5 mL, and initial pH = 5.0.In both (10) and (11), k is the kinetic coefficient or rate constant. k is defined by expression (12):
(12)k=Drπ2r02,
where Dr is the diffusion coefficient in the resin phase and r0 is the average radius of resin particle. The values of the diffusion coefficient in the resin phase calculated from (12) are also given in Table 3.When the adsorption of metal ion involves mass transfer accompanied by chemical reaction the process can be explained by the moving boundary model [32]. This model assumes a sharp boundary that separates a completely reacted shell from an unreacted core and that advances from the surface toward the center of the solid with the progression of adsorption. In this case, the rate equation is given by
(13)3-3(1-F)2/3-2F=kt.The graphical correlation in Figure8 of (13) shows that the moving boundary particle diffusion model fits only the initial adsorption on the grafted resin. The linear regression analyses of (13) are also given in Table 3.Figure 8
Plot of the moving boundary particle diffusion model for the Cd(II) adsorption on grafted resin,m=0.030 g, V=5 mL, and initial pH = 5.0.


### 3.7. Effect of Electrolytes on Cd(II) Extraction

As the sulphates, chlorides, and acetate of alkali ions (Na+) frequently accompany cadmium ions in industrial solutions, it is worthwhile to know if they affect the extraction process efficiency. The influence on the extraction of Cd(II) was studied at the varying concentrations of NaCl, Na2SO4, and CH3COONa, in aqueous solution, from 0.1 to 0.7 mol·L−1. The influence of the concentration of those salts is shown in Figure 9.Figure 9
Effect of Na2SO4, CH3COONa, and NaCl salts concentrations on the extraction of Cd(II) with grafted resin, m=0.030 g, V=5 mL, initial pH = 5.0, C0=1.0 mmol/L, and equilibrium time = 180 min.At Na2SO4 and NaCl concentrations between 0.1 and 0.7 mol·L−1 there is a negative trend on increasing electrolytes concentrations. The decrease in the extraction of Cd(II) may be due to the formation of more stable metal sulphate or chloride complexes, which were nonextractable by the grafted resin [33, 34].The presence of CH3COONa does not become annoying until a concentration of 0.4 mol·L−1. At high concentration, it was found that the extraction yield drop from 100% to 75% when the acetate concentration increases from 0.4 mol·L−1 to 0.7 mol·L−1. This effect is attributed to a competition between Na+ cations of added salt and Cd(II) in the formation of bonds with the active sites of the resin [34].


### 3.8. Effect of Temperature on Sorption

Temperature has two major effects on the sorption process. Increasing the temperature is known to increase the rate of the diffusion of the sorbate molecule across the external boundary layer and in the internal pores of the sorbent particle, owing to a decrease in the velocity of the solution. In addition, changing the temperature will change the equilibrium capacity of the sorbent for the particle sorbate. The influence of temperature variation was examined on the sorption of Cd(II) of fixed concentration 1.0 mmol L−1 onto grafted resin using 180 min of equilibration time and sorbent to aqueous phase ratio of 0.030 g : 5 mL from 293 K to 333 K.Experimental results (yield extraction) concerning the effect of temperature on the Cd(II) sorption are shown in Figure10. An increase in temperature results is an increase in metal ion sorption. There is about 15% increase in the yield sorption of Cd(II) sorbed on grafted resin when the temperature is raised from 293 to 333 K. Better sorption at higher temperatures may be either due to acceleration of some originally slow sorption steps or due to the enhanced mobility of Cd(II) ions from the solution to the functionalized resin surface.Figure 10
Effect of temperature on the yield extraction of Cd(II) by the functionalized resin.C0=1.0 mmol·L−1, m=0.030 g, V=5 mL, initial pH = 5.0, and equilibrium time = 180 min.


### 3.9. Thermodynamic Parameters

In environmental engineering practice, both energy and entropy factors must be considered in order to determine which process will occur spontaneously. The Gibbs free energy change,ΔG0, is the fundamental criterion of spontaneity [35].The apparent thermodynamic parametersΔH and ΔS for the sorption process were calculated from the slopes and intercepts of the linear variation of lnKd versus 1/T  in Figure 11 by:
(14)LnKd=ΔSR-ΔHRT,
where R is the gas constant, 8.314 J·mol−1·K−1 and T is the absolute temperature in Kelvin. The free energy (ΔG) for the sorption was calculated by
(15)ΔG=ΔH-TΔS.Figure 11
Variation oflogKd with 1/T for the sorption of cadmium(II) onto the grafted resin, m=0.030 g, [Cd(II)]0 = 1.0 mmol·L−1, V=5 mL, initial pH = 5.0, and contact time = 180 min.Further, the thermodynamic equilibrium constant,Kd in mL·g−1 (16), obtained from the distribution constant was used to compute the apparent thermodynamic parameters
(16)Kd=(C0-Ce)VCem.The calculated apparent thermodynamic parameters for sorption of Cd(II) onto functionalized resin are summarized in Table4.Table 4
Thermodynamics parameters for sorption process of Cd(II) on functionalized resin.
ΔH, (kJ·mol−1)
ΔS, (J·mol−1·K−1)
ΔG, (kJ·mol−1)
—
—
293 K
303 K
313 K
323 K
333 K
+35.53
+133.34
−3.57
−4.90
−6.24
−7.57
−8.90In the present work, the Gibbs energy decrease in each case was responsible for imparting stability to the cadmium ions-functionalized resin sorption complexes. The negative values ofΔG are due to the fact that the sorption process is spontaneous with high affinity of Cd(II) ions to the derivative of phosphonic acids. However, the negative values of ΔG decrease indicating that the spontaneous nature of the sorption of metal ions is inversely proportional to the temperature; higher temperature favours the sorption process. The positive value of ΔH confirms the endothermic nature of the sorption process. Hence, by increasing temperature, the degree of sorption/exchange will increase. Increased temperature will cause a rupturing of the hydration zone formed around Cd(II) in mother liquid to a great extent and direct interaction of metal ions with functional group of resin (decreasing in hydrated diameter), increasing diffusion force by supplying partial ion-exchange activation energy, increasing diffusion into the inner sections of the grafted resin, and subsequently an increase in the degree of sorption/exchange. The positive value of ΔS reflected the affinity of the sorbent for Cd(II) ions and confirms the increased randomness at the solid-solution interface during sorption [36].


### 3.10. Elution Studies

Adsorption and elution processes depend on the solution pH. Therefore, elution is possible by controlling the pH/acid concentration of the solution. Elution of Cd(II) from loaded grafted resin was carried out using HCl solution at different concentrations (0.0 to 2.5 mol·L−1). The contact time was maintained at 120 min. The results in Figure 12 show that percentage elution increased with increasing acid concentration and a hydrochloric acid concentration of 1.0 mol·L−1 was found suitable to elute more than 92% of the Cd(II) from the functionalized resin in one cycle.Figure 12
Effect of HCl concentration on the desorption of Cd(II) loaded on grafted resin. Loaded resin quantity: 0.030 g, acid volume: 5 mL, and time contact: 120 min.


## 3.1. Effect of pH

Changes in the pH of the medium are one of the most important factors affecting the concentration and metal recovery procedure, which is related to the formation of soluble metal complexes and subsequently their stabilities in aqueous solutions. It is well known that surface charge of adsorbent can be modified by changing the pH of the solution and the chemical species in the solution depends on this parameter [17]. According to the chemical equilibrium diagram for cadmium in aqueous solution obtained by the MEDUSA program, the species Cd(OH)2 precipitates at pH higher than 8 and the concentration of Cd2+ ions in solution decreases. (Program MEDUSA, Make Equilibrium Diagrams Using Sophisticated Algorithms. http://home.telfort.nl/cheaqs/). Under the experimental conditions of the present paper, Cd2+ was the major species present in solution.In order to optimize the pH for maximum removal, experiments were conducted in the pH range from 1.77 to 5.15 at ambient temperature, 4 hrs equilibration time, and 1.0 mmol·L−1 metal ion concentration. Figure 2 shows the influence of pH in sorption process of Cd(II) by modified resin. As can be seen from Figure 2 the sorption increases quickly with increasing pH values from 1.8 to 3.2. The progressive decrease in the retention of metal ions at low pH is due to [17] the following: (i) the competition of the hydrogen ion with the metal ions for binding to the phosphonic acid group (P–OH); (ii) the oxygen atoms (P=O) are more protonated, and hence, they are less available to coordinate with the cadmium; (iii) the competition between the excess of H+ ions in the medium and positively charged cationic species present in solution; (iv) as pH is increased there is a decrease of positive surface charge, which results in the lower coulombic repulsion of the adsorbing metal ions. Consequently the number of moles of Cd(II) removal may decrease at low pH [18]. The observed reduction in the level of metal ion removal from solution by the sorbent indicates that the interaction between the Cd(II) ions and the sorbent is an ion exchange process.Figure 2
Effect of the initial pH of the aqueous solution on the retention of Cd(II) by the functionalized resin.C0=1.0 mmol·L−1, m=0.030 g, V=5 mL, and contact time = 4 hrs.The data reveals that the highest extraction yield value is recorded at the pH range 3.2–5.2. This is attributed to the presence of free lone pair of electrons on the oxygen of phosphoryl (P=O) group and deprotonated oxygen atoms, which are suitable ligands for coordination with the cadmium ions [19, 20]. This cation exchange process can be represented by the following general reaction [6]:
(6)Resin–P–OH+Cd2+→Resin–P–O–Cd++H+.In order to make further approaching of the functional group of resin and Cd(II), the spectra of resin, before and after Cd(II) is sorbed, are compared. It is found that the characteristic sorption peak of the bond P=0 (at 1124 cm−1) disappears on the whole, which shows that the formation of the coordination bond between oxygen atom and Cd(II) weakens the stretch vibration and causes the peak to shift to the lower frequency. The characteristic sorption peak of P–OH (941 cm−1) is weakened and the new characteristic sorption peak of (-PO32-) is formed [21], which shows that H+ and Cd2+ has been exchanged. All those changes result from the formation of a complex compound.


## 3.2. Effect of Contact Time

The rate of loading of Cd(II) onto the grafted polystyrene resin was determined for two concentrations of Cd(II) 0.5 and 1.0 mmol·L−1, by shaking 5 mL of Cd(II) with 0.030 g of resin in an Erlenmayer flask at ambient temperature for 2, 4, 10, 15, 30, 60, 120, 180, and 200 min. Figure 3 shows that the initial concentration of Cd(II) has an important effect on the rate of sorption. For all the sorption experiments, the amount of cadmium ions sorbed onto the grafted resin increased quickly with time and then slowly reached equilibrium after 180 min. The equilibrium times in which the polymer attains 50% saturation with Cd(II) (half time t1/2) are <2.4 min and <13.0 min for initial Cd(II) concentration = 0.5 mmol·L−1 and 1.0 mmol·L−1, respectively. The amounts of cadmium metal ions sorbed at equilibrium (qe) at [Cd(II)] = 0.5 mmol·L−1 and 1.0 mmol·L−1, respectively, are 9.02 and 17.93 mg·g−1.Figure 3
Effect of contact time on the sorption of Cd(II) on the functionalized resin from aqueous Cd(II) solutions at two different concentrations (C0 and C0′); C0=0.5 mmol·L−1: ■-percent Cd(II) removal, (%), □-uptake (q), mg·g−1; C0′=1.0 mmol·L−1: ★-percent Cd(II) removal, (%), ☆-uptake (q), mg·g−1; V=5 mL; m=0.030 g; initial pH = 5.0.


## 3.3. Rate of Kinetics Adsorption

In this study, batch sorption kinetics of Cd(II) ions at two different concentrations,C0=0.5 and C0′=1.0 mmol·L−1, with the functionalized polymer have been studied. The different values of constants from the slopes and intercepts of linear plots of (2) (figure not shown), (3) (shown in Figure 4), and (4) (figure not showed) are summarized in Table 1. As seen from Table 1, the obtained correlation coefficient for the pseudo second-order model (>0.99) was better than those of the first-order and second-order models for the adsorption of Cd(II) at the two considered concentrations, suggesting that the pseudo second-order model was more suitable to describe the adsorption kinetics of phosphonic acid grafted on polystyrene resin for Cd(II), especially at the lower concentration (0.5 mmol·L−1). This suggests that the rate limiting step may be chemical sorption or chemisorption involving valency forces through sharing or exchange of electrons between sorbent (containing O atoms) and sorbate [16]. Similar results have been observed in the adsorption of Cd(II) by lignocellulosic sorbent [22] and onto kraft and organosolv lignins [23]. The values of the second-order rate constants (k2) were found to decrease from 1.6442 to 0.00262 g·mg−1·min−1 as the initial concentration increased from 0.5 to 1.0 mmol·L−1, showing the process to be highly concentration dependent, which is consistent with studies reported [24].Table 1
Models rate constants for Cd(II) sorption kinetics by the functionalized resin.
Models
Parameters
[Cd(II)]0 = 0.5 mmol·L−1
[Cd(II)]0 = 1.0 mmol·L−1
First-order rate
q
cal. (mg·g−1)
2.20
12.43
q
exp
. (mg·g−1)
9.02
17.93
k
1 (min−1)
0.050
0.020
r
0.800
0.880
Pseudo second-order rate
q
cal. (mg·g−1)
9.09
20.0
q
exp
. (mg·g−1)
9.02
17.93
k
2 (g·mg−1·min−1)
1.6442
0.00262
r
0.999
0.991
Second-order rate
q
cal. (mg·g−1)
0.67
14.37
q
exp
. (mg·g−1)
9.02
17.93
k
3 (g·mg−1·min−1)
0.8052
0.05599
r
0.928
0.901Figure 4
Plots for the adsorption of Cd(II),m=0.030 g, V=5 mL, and initial pH = 5.0.


## 3.4. Sorption Capacity

The retention capacity of functionalized resin was determined by equilibrating 0.030 g of the resin with 5 mL of cadmium(II) ion solutions at different concentrations (0.1.10−2–1.0.10-2mol·L−1), under optimum pH. The experimental capacity obtained is 37.9 mg·g−1 of polymer (Figure 5). At similar conditions, this sorbent possesses very high extraction ability towards Eu(III) and UO22+ cations metals; the extraction capacities are 122.5 and 152.2 mg g−1, respectively [25, 26]. This result is attributed to that phosphonic acid derivatives are more selective towards lanthanides elements [27].Figure 5
Effect of the initial concentration of Cd(II) on the uptake and the extraction yield.m=0.030 g, V=5 mL, equilibrium time = 180 min, and initial pH = 5.0.


## 3.5. Adsorption Isotherm

The adsorbed amounts of Cd(II) on resin have been determined as a function of the metal concentration in the supernatant at the equilibrium state and ambient temperature. The Langmuir treatment (7) is based on the assumption that [28] (i) maximum adsorption corresponds to saturated monolayer of adsorbate molecules on the adsorbent surface, (ii) the energy of adsorption is constant, and (iii) there is no transmigration of adsorbate in the plane of the surface. One has
(7)Ceqe=Ceqm+1qmKL,
where qm and KL are Langmuir constants related to adsorption capacity and energy of adsorption, respectively. The linear plot of Ce/qe versus Ce shows that adsorption obeys Langmuir adsorption model (Figure 6). The correlation coefficient for the linear regression fits of the Langmuir plot was found to be 0.995. qm and KL determined from the Langmuir plot were found to be 38.2 mg·g−1 and 0,0441 L·mol−1, respectively. We note that the capacity of sorption deducted after Langmuir model application is similar to this calculated experimentally (37.9 mg·g−1).Figure 6
Langmuir plot for the adsorption of Cd(II),m=0.030 g, V=5 mL, initial pH = 5.0, and equilibrium time = 180 min.The essential characteristics of Langmuir isotherm can be expressed in terms of a dimensionless constant, separation factor or equilibrium parameter,RL which is defined by
(8)RL=11+KLC0.The value ofRL indicates the type of the isotherm to be either unfavorable (RL>1), linear (RL=1), favorable (0<RL<1), or irreversible (RL=0). As shown in Table 2, the values of RL are ranged from 0.9999 to 0.9995 in the initial Cd(II) ions concentrations 0.01–0.001 mol·L−1. These values indicated that the adsorption process is favorable [29, 30].Table 2
Equilibrium parameter,RL.
C
0, mol·L−1
0.001
0.002
0.004
0.005
0.006
0.008
0.01
R
L
0.99995
0.99991
0.99982
0.99977
0.99973
0.99964
0.99955The Freundlich equation was also applied to the adsorption. The Freundlich equation is basically empirical but is often useful as a means of data description. It generally agrees quite well compared to Langmuir equation and experimental data over a moderate range of adsorbate concentrations [28]. The linearized Freundlich isotherm is represented by
(9)logqe=logKF+1nlogCe.A plot oflog(qe) versus logCe (figure not shown) is linear at only low concentrations of Cd(II) and the constants KF and n were found to be 154.74 mg·g−1and 0.266, respectively. The correlation coefficient for the linear regression fits of the Freundlich plot was found to be 0.830.


## 3.6. Diffusion Study

The adsorption of cadmium(II) on the grafted resin from cadmium sulphate solutions at two different initial metal concentrations was studied as a function of time at ambient temperature. The adsorption onto ion exchange resin must be considered as a liquid-solid phase reaction which includes several steps [31]: (i) The diffusion of ions from the solution to the resin surface, (ii) the diffusion of ions within the solid resin, and (iii) the chemical reaction between ions and functional groups of the resin.The adsorption of the metal is governed by the slowest of these processes. The kinetic models and the rate equations for the above three cases have been established. The exchange of ions can be described by the Nernst-Planck equations which apply to counter diffusion of two species in an almost homogeneous media [17, 31].If the liquid film diffusion controls the rate of exchange, the following relation can be used:(10)-ln(1-F)=kt.If the cases of the diffusion of ions in the resin phase controlling process, the equation used is:(11)-ln(1-F2)=kt.After testing both mathematical models proposed for homogeneous diffusion in the adsorption of Cd(II) onto the resin, this is best fitted when the metal uptake is the particle diffusion controlled and at time contact ≤30 min (Figure7). Thus, the values of the adsorption rate constant, regression equations, and regression coefficients of the diffusion of Cd(II) in the resin phase calculated from the slope of the straight lines (Figure 7) are summarized in Table 3.Table 3
The regression equations (y), regression coefficients (r), and diffusion coefficients (Dr).
[Cd(II)], mmol·L−1
Eq. (10)
Eq. (11)
Eq. (13)
0.5
Y
0.106
t
0.098
t
0.024
t
r
0.925
0.932
0.900
D
r, 10−5, cm²·min−1
—
2.485
—
1.0
Y
0.062
t
0.040
t
0.015
t
r
0.941
0.951
0.945
D
r, 10−5, cm²·min−1
—
1.014
—Figure 7
Plot of (11) for Cd(II) adsorption on grafted resin, m=0.030 g, V=5 mL, and initial pH = 5.0.In both (10) and (11), k is the kinetic coefficient or rate constant. k is defined by expression (12):
(12)k=Drπ2r02,
where Dr is the diffusion coefficient in the resin phase and r0 is the average radius of resin particle. The values of the diffusion coefficient in the resin phase calculated from (12) are also given in Table 3.When the adsorption of metal ion involves mass transfer accompanied by chemical reaction the process can be explained by the moving boundary model [32]. This model assumes a sharp boundary that separates a completely reacted shell from an unreacted core and that advances from the surface toward the center of the solid with the progression of adsorption. In this case, the rate equation is given by
(13)3-3(1-F)2/3-2F=kt.The graphical correlation in Figure8 of (13) shows that the moving boundary particle diffusion model fits only the initial adsorption on the grafted resin. The linear regression analyses of (13) are also given in Table 3.Figure 8
Plot of the moving boundary particle diffusion model for the Cd(II) adsorption on grafted resin,m=0.030 g, V=5 mL, and initial pH = 5.0.


## 3.7. Effect of Electrolytes on Cd(II) Extraction

As the sulphates, chlorides, and acetate of alkali ions (Na+) frequently accompany cadmium ions in industrial solutions, it is worthwhile to know if they affect the extraction process efficiency. The influence on the extraction of Cd(II) was studied at the varying concentrations of NaCl, Na2SO4, and CH3COONa, in aqueous solution, from 0.1 to 0.7 mol·L−1. The influence of the concentration of those salts is shown in Figure 9.Figure 9
Effect of Na2SO4, CH3COONa, and NaCl salts concentrations on the extraction of Cd(II) with grafted resin, m=0.030 g, V=5 mL, initial pH = 5.0, C0=1.0 mmol/L, and equilibrium time = 180 min.At Na2SO4 and NaCl concentrations between 0.1 and 0.7 mol·L−1 there is a negative trend on increasing electrolytes concentrations. The decrease in the extraction of Cd(II) may be due to the formation of more stable metal sulphate or chloride complexes, which were nonextractable by the grafted resin [33, 34].The presence of CH3COONa does not become annoying until a concentration of 0.4 mol·L−1. At high concentration, it was found that the extraction yield drop from 100% to 75% when the acetate concentration increases from 0.4 mol·L−1 to 0.7 mol·L−1. This effect is attributed to a competition between Na+ cations of added salt and Cd(II) in the formation of bonds with the active sites of the resin [34].


## 3.8. Effect of Temperature on Sorption

Temperature has two major effects on the sorption process. Increasing the temperature is known to increase the rate of the diffusion of the sorbate molecule across the external boundary layer and in the internal pores of the sorbent particle, owing to a decrease in the velocity of the solution. In addition, changing the temperature will change the equilibrium capacity of the sorbent for the particle sorbate. The influence of temperature variation was examined on the sorption of Cd(II) of fixed concentration 1.0 mmol L−1 onto grafted resin using 180 min of equilibration time and sorbent to aqueous phase ratio of 0.030 g : 5 mL from 293 K to 333 K.Experimental results (yield extraction) concerning the effect of temperature on the Cd(II) sorption are shown in Figure10. An increase in temperature results is an increase in metal ion sorption. There is about 15% increase in the yield sorption of Cd(II) sorbed on grafted resin when the temperature is raised from 293 to 333 K. Better sorption at higher temperatures may be either due to acceleration of some originally slow sorption steps or due to the enhanced mobility of Cd(II) ions from the solution to the functionalized resin surface.Figure 10
Effect of temperature on the yield extraction of Cd(II) by the functionalized resin.C0=1.0 mmol·L−1, m=0.030 g, V=5 mL, initial pH = 5.0, and equilibrium time = 180 min.


## 3.9. Thermodynamic Parameters

In environmental engineering practice, both energy and entropy factors must be considered in order to determine which process will occur spontaneously. The Gibbs free energy change,ΔG0, is the fundamental criterion of spontaneity [35].The apparent thermodynamic parametersΔH and ΔS for the sorption process were calculated from the slopes and intercepts of the linear variation of lnKd versus 1/T  in Figure 11 by:
(14)LnKd=ΔSR-ΔHRT,
where R is the gas constant, 8.314 J·mol−1·K−1 and T is the absolute temperature in Kelvin. The free energy (ΔG) for the sorption was calculated by
(15)ΔG=ΔH-TΔS.Figure 11
Variation oflogKd with 1/T for the sorption of cadmium(II) onto the grafted resin, m=0.030 g, [Cd(II)]0 = 1.0 mmol·L−1, V=5 mL, initial pH = 5.0, and contact time = 180 min.Further, the thermodynamic equilibrium constant,Kd in mL·g−1 (16), obtained from the distribution constant was used to compute the apparent thermodynamic parameters
(16)Kd=(C0-Ce)VCem.The calculated apparent thermodynamic parameters for sorption of Cd(II) onto functionalized resin are summarized in Table4.Table 4
Thermodynamics parameters for sorption process of Cd(II) on functionalized resin.
ΔH, (kJ·mol−1)
ΔS, (J·mol−1·K−1)
ΔG, (kJ·mol−1)
—
—
293 K
303 K
313 K
323 K
333 K
+35.53
+133.34
−3.57
−4.90
−6.24
−7.57
−8.90In the present work, the Gibbs energy decrease in each case was responsible for imparting stability to the cadmium ions-functionalized resin sorption complexes. The negative values ofΔG are due to the fact that the sorption process is spontaneous with high affinity of Cd(II) ions to the derivative of phosphonic acids. However, the negative values of ΔG decrease indicating that the spontaneous nature of the sorption of metal ions is inversely proportional to the temperature; higher temperature favours the sorption process. The positive value of ΔH confirms the endothermic nature of the sorption process. Hence, by increasing temperature, the degree of sorption/exchange will increase. Increased temperature will cause a rupturing of the hydration zone formed around Cd(II) in mother liquid to a great extent and direct interaction of metal ions with functional group of resin (decreasing in hydrated diameter), increasing diffusion force by supplying partial ion-exchange activation energy, increasing diffusion into the inner sections of the grafted resin, and subsequently an increase in the degree of sorption/exchange. The positive value of ΔS reflected the affinity of the sorbent for Cd(II) ions and confirms the increased randomness at the solid-solution interface during sorption [36].


## 3.10. Elution Studies

Adsorption and elution processes depend on the solution pH. Therefore, elution is possible by controlling the pH/acid concentration of the solution. Elution of Cd(II) from loaded grafted resin was carried out using HCl solution at different concentrations (0.0 to 2.5 mol·L−1). The contact time was maintained at 120 min. The results in Figure 12 show that percentage elution increased with increasing acid concentration and a hydrochloric acid concentration of 1.0 mol·L−1 was found suitable to elute more than 92% of the Cd(II) from the functionalized resin in one cycle.Figure 12
Effect of HCl concentration on the desorption of Cd(II) loaded on grafted resin. Loaded resin quantity: 0.030 g, acid volume: 5 mL, and time contact: 120 min.


## 4. Conclusion

The phosphonic acid grafted on polystyrene resin was synthesized using the Arbuzov reaction and used as a support material for Cd(II) sorption, in batch process. The extraction efficiency was determined as a function of various parameters such as time, pH, cadmium concentration, and electrolytes effect. The experimental capacity obtained is 37.9 mg·g−1. The kinetics of Cd(II) adsorption on functionalyzed resin follows the Pseudo second-order rate. The equilibrium isotherm for sorption of the investigated metal ions has been modelled successfully using the Langmuir isotherm. The Cd(II) uptake is best explained by a particle diffusion controlled process, whereas the moving boundary model only fits the initial adsorption on the phosphonic resin. Various thermodynamic parameters, such as ΔG, ΔH, and ΔS, were calculated from the data. The thermodynamics of Cd(II) ions/functionalized resin system indicate a spontaneous and endothermic nature of the process.More than 92% of loaded Cd(II) on the grafted resin can be eluted with HCl 1.0 mol·L−1 after 120 minutes of shaking in one cycle.The results presented in this work reveal that polystyrene resin functionalized with phosphonic group is feasible for the removal of cadmium cations from wastewater.



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*Source: 980825-2012-11-08.xml*