# Solid-Phase Extraction of Trace Amounts of Uranium(VI) in Environmental Water Samples Using an Extractant-Impregnated Resin Followed by Detection with UV-Vis Spectrophotometry

Authors: Ahmad Hosseini-Bandegharaei; Masoud Sarwghadi; Aliasghar Heydarbeigi; Seyyed Hossein Hosseini; Mehdi Nedaie
Journal: Journal of Chemistry
 (2013)

---

## Abstract

A stable extractant-impregnated resin (EIR) containing Chrome Azurol B was prepared using Amberlite XAD-2010 as a porous polymeric support. The new EIR was employed for trace separation and preconcentration of U(VI) ion followed by spectrophotometric determination with the arsenazo III procedure. CAB/XAD-2010 exhibited excellent selectivity for U(VI) ion over coexisting ions. Experimental parameters including pH, contact time, shaking speed, and ionic strength were investigated by batch extraction methods. Maximum sorption of U(VI) ions occurred at pH 4.3–6.9. The capacity of EIR was found to be 0.632 mmol·g−1. Equilibrium was reached in 25 min and the loading half-time, t1/2, was less than 6 min. The equilibrium adsorption isotherm of U(VI) was fitted with the Langmuir adsorption model. In addition, a column packed with CAB/XAD-2010 was used for column-mode separation and preconcentration of U(VI) ion. For the optimization of the dynamic procedure, effects of sample volume, sample and eluent flow rate, eluent concentration, and its volume were investigated. The preconcentration factors for U(VI) were found out to be 160. But, for convenience, a preconcentration factor of 150 was utilized for the column-mode preconcentration. The dynamic procedure gave a detection limit of 5.0×10-10 mol·L−1 (0.12 μg·L−1) for U(VI) ion. The proposed dynamic method showed good performance in analyzing environmental water samples.


---

## Body

## 1. Introduction

Nowadays, a great attention is paid to the analytical monitoring of uranium in environmental samples due to its serious toxic effects even at low concentrations [1, 2]. Among the eminent techniques developed for the determination of uranium in environmental samples [3–7], preconcentrative separation of trace amounts of uranium from these samples followed by spectrophotometric determination, using arsenazo III procedure, has attracted much attention in the last decades [8–13]. This fact is due to availability, easy operation, and relative low operational and instrumental costs.Solid-phase extraction (SPE) has come to the forefront compared with other preconcentration techniques because of the development of solid adsorbents, including chelating polymeric supports, and the advantages in the use of these adsorbents in metal ions preconcentration. SPE offers several important advantages such as [12–18] the following:(i)
higher enrichment factors,(ii)
absence of emulsion,(iii)
safety with respect to hazardous samples,(iv)
minimal costs due to low consumption of reagents,(v)
flexibility,(vi)
ease of automation.In addition, several properties such as selectivity, simplicity of equipment, ease of operation, and the possibility of using adsorbents for many separation and preconcentration cycles without losses in the metal ion sorption capacity have made their use popular.Extractant-impregnated resins, EIRs, have recently been developed for designing chelating polymeric supports and separating transition metal ions from aqueous media, because the preparation of chelating polymeric ion exchangers with chelating ligand connected to the polymer matrix by chemical bonds is usually very complex, time consuming, and costly. The preparation of chelating polymeric ion exchangers by the impregnation methods is exceedingly easy to perform, merely requiring stirring of an adequate extractant and the polymeric support. In addition, there is a wide choice of reagents for desired selectivity [19–26]. Therefore, by preparing a stable impregnated resin, one can combine the specific properties of an extractant, such as its selectivity, with the advantages of solid-ion-exchange technology for processing highly diluted solutions. Consequently, the extractant-impregnated resins (EIRs) are more suitable than conventional solvent extraction for recovering a specified metal ion with high selectivity. Among the studies concerning EIRs, several studies have been reported for polymeric supports in which an inert support is impregnated with a selective organic extractant to produce a solid sorbent used to separate and preconcentrate U(VI) from various analytical matrices [12, 13, 23–26].In the followup of our group researches on the EIRs applications [12, 13, 27–31], this work focuses on the selective separation and preconcentration of trace amounts of uranium in various environmental water samples using a new EIR containing Amberlite XAD-2010 resin beads impregnated with Chrome Azurol B. Our new EIR sorbent showed excellent selectivity for U(VI) sorption from aqueous solutions. The adsorbed U(VI) ions stripped easily with 0.50 M HCl solution and the regenerated EIR could be used in subsequent cycles for U(VI) separation and preconcentration. In this paper, performance testing of the new EIR for solid-phase extraction of uranium is discussed.


## 2. Experimental

### 2.1. Reagents and Apparatus

Deionized water was used to prepare all solutions. Unless stated, all solvents and reagents used were analytical reagent grade and purchased from Merck (Darmstadt, Germany). Stock standard solution of U(VI) was prepared by dissolving the appropriate amounts of uranyl nitrate in deionized water, acidified with a small amount of HNO3. The solutions of uranium(VI) were standardized gravimetrically (as U3O8). Buffer solutions of pH 1–3, 4–6, and 7–9 were prepared by mixing appropriate ratios of 0.1 M HCl and KCl, 0.5 M acetic acid and ammonium acetate, and 0.5 M ammonia and NH4Cl solutions, respectively. Chrome Azurol B (Chromazurol B; Mordant Blue 1; CI Mordant Blue 1; CI Mordant Blue 1, free acid; Eriochrome Blue SBB; Eriochrome Azurol B free form; Eriochrome Azurol 6B free form; EINECS 239-098-7), CAB (4-[(3-Carboxy-5-methyl-4-oxo-1-cyclohexa-2,5-dienylidene)(2,6-dichlorophenyl)methyl]-2-hydroxy-3-ethylbenzoic acid), and Amberlite XAD-2010 (surface area of 660 m2 g−1, pore diameter 28.0 nm, and bead size 20–60 mesh) were obtained from Sigma Chem. Co., St. Louis. The surface area, pore diameter, and mesh size of the resin were quoted by the supplier.For the determination of U(VI) in solutions using arsenazo III procedure, adsorption measurements were recorded on a Shimadzu double-beams UV-Vis (2150-PC, Japan) spectrophotometer equipped with quartz cuvettes of 1 cm thickness. The pH measurements were made on a model PHS-3BW pH-meter (Bel, Italy). A Fine PCR automatic shaker model SH30L-t, Korea, was used for the batch experiments. The flow of sample and eluent solutions through the short column was controlled with a BT100-1L peristaltic pump and a DG-2 head pump (Longer pump, China). A Sartorius membrane filter of pore size 0.45μm was used to remove particles in analysis of real samples.


### 2.2. Preparation of the EIR

The dry procedure was used for preparing CAB-impregnated XAD-2010 resin beads [29]. Before the impregnation process, Amberlite XAD-2010 resin beads were treated with 1 : 1 methanol-water solution containing 6 M HCl for 12 h in order to remove remaining monomers and other types of impurities which may be found with the fabricated beads. The resin was thoroughly rinsed with doubly-distilled water and placed into a drying oven at 323 K for 30 min. To prepare the impregnated resin, portions of Amberlite XAD-2010 resin (1 g of dry resin) were transferred into a series of glass stoppered bottles containing different concentrations of CAB in 200 mL methanol, which was used as the solvent. The mixtures were slowly shaken for 10 h to complete the impregnation process and then heated at 333 K in a drying oven to remove the solvent. Each EIR sample was then transferred to a porous filter and washed successively with HCl (3 M) solution and large amounts of distilled water until no CAB was found in the filtrate, spectrophotometrically. Finally, the impregnated resins were dried at 323 K and weighed. The amount of CAB impregnated on/in the resin beads was determined from the weight change of polymeric resin. To avoid surface peeling and cracking, which cause the leaching of some extractant molecules from the resin beads, the prepared EIR beads were stored under deionized water in a stoppered glass bottle.


### 2.3. Sorption Procedures

#### 2.3.1. Static Sorption of U(VI) Ions

A batch technique was used to sorb the U(VI) ions at298±1 K. The 100 mL aliquots of aqueous solution containing suitable concentrations of U(VI) were taken in glass-stoppered bottles and adjusted to a known pH. The CAB-impregnated XAD-2010 resin beads (0.150 g) were added to each bottle and the mixtures were equilibrated for a fixed period of time. The EIR beads were filtered and the sorbed U(VI) ions were desorbed by shaking with 5 mL of 0.50 M HCl. The desorbed U(VI) ions were measured spectrophotometrically by the arsenazo III procedure described in Section 2.4. For adsorption equilibrium studies, the mixtures were shaken at a fixed temperature using a temperature controlled shaker set at 180 rpm for a period of desired time at the optimum pH value and desired ionic strength. After that, the suspensions were filtered and the filtrates were analyzed spectrophotometrically by the arsenazo III procedure described in Section 2.4. The amounts of uranium adsorbed per gram of the EIR beads were calculated at various time “t” (qt) and at equilibrium (qe) by the mass balance equations:
(1)qt=(C0-Ct)Vm,qe=(C0-Ce)Vm,
where qt is the amount of the uranium adsorbed onto the EIR beads at time “t” (mg·g−1), qe, the amount of the uranium adsorbed onto the EIR beads at equilibrium (mg·g−1), C0, the initial concentration of U(VI) in the aqueous solutions (mg·L−1), Ct, the U(VI) concentration remaining in the solutions at time “t” (mg·L−1), Ce, the equilibrium concentration of U(VI) in the solutions (mg·L−1), V, the volume of the solutions used (L), and m, the weight of the EIR beads used in g.


#### 2.3.2. Dynamic Sorption of U(VI) Ions

Five hundred milligrams of new EIR was slurried in water and then packed into a polyethylene column with an internal diameter of 0.4 cm. The ends were fitted with a small amount of glass wool to keep the EIR beads inside of the column and to prevent any loss of the EIR beads during the sample running. The bed length of EIR in the column was about 32 mm. Working solutions containing U(VI) metal ion, with the concentration exceeding the detection limit, prepared in which the pH and ionic strength were, respectively, adjusted to 4.5 and 0.1 M, using the acetic acid and ammonium acetate solutions, and passed through the column at a known flow rate. After this step, stripping experiments were performed. For this purpose, the column was washed with distilled water (5 mL), and then, 5 mL of 0.50 mol L−1 HCl was used to strip U(VI) ions. The desorbed metal ions were analyzed spectrophotometrically by arsenazo III procedure described in Section 2.4.


### 2.4. Spectrophotometric Arsenazo III Method for the Determination of U(VI)

The arsenazo III procedure was utilized for the determination of U(VI) in solutions [32]. A pH 2.0 buffer solution of KCl/HCl was prepared by mixing 8.1 mL of 0.20 mol L−1 HCl and 41.9 mL of 0.2 mol L−1 KCl solutions and diluting to 100 mL with doubly-distilled water. A reagent blank solution containing arsenazo III 1% (w/v) and buffer solution was freshly prepared before each measurement. Working solutions (2.5 mL) containing U(VI) + 0.2 mL of arsenazo III solution + 2.0 mL of buffer solution were diluted to 5.0 mL with distilled water and measured at 653.0 nm.


## 2.1. Reagents and Apparatus

Deionized water was used to prepare all solutions. Unless stated, all solvents and reagents used were analytical reagent grade and purchased from Merck (Darmstadt, Germany). Stock standard solution of U(VI) was prepared by dissolving the appropriate amounts of uranyl nitrate in deionized water, acidified with a small amount of HNO3. The solutions of uranium(VI) were standardized gravimetrically (as U3O8). Buffer solutions of pH 1–3, 4–6, and 7–9 were prepared by mixing appropriate ratios of 0.1 M HCl and KCl, 0.5 M acetic acid and ammonium acetate, and 0.5 M ammonia and NH4Cl solutions, respectively. Chrome Azurol B (Chromazurol B; Mordant Blue 1; CI Mordant Blue 1; CI Mordant Blue 1, free acid; Eriochrome Blue SBB; Eriochrome Azurol B free form; Eriochrome Azurol 6B free form; EINECS 239-098-7), CAB (4-[(3-Carboxy-5-methyl-4-oxo-1-cyclohexa-2,5-dienylidene)(2,6-dichlorophenyl)methyl]-2-hydroxy-3-ethylbenzoic acid), and Amberlite XAD-2010 (surface area of 660 m2 g−1, pore diameter 28.0 nm, and bead size 20–60 mesh) were obtained from Sigma Chem. Co., St. Louis. The surface area, pore diameter, and mesh size of the resin were quoted by the supplier.For the determination of U(VI) in solutions using arsenazo III procedure, adsorption measurements were recorded on a Shimadzu double-beams UV-Vis (2150-PC, Japan) spectrophotometer equipped with quartz cuvettes of 1 cm thickness. The pH measurements were made on a model PHS-3BW pH-meter (Bel, Italy). A Fine PCR automatic shaker model SH30L-t, Korea, was used for the batch experiments. The flow of sample and eluent solutions through the short column was controlled with a BT100-1L peristaltic pump and a DG-2 head pump (Longer pump, China). A Sartorius membrane filter of pore size 0.45μm was used to remove particles in analysis of real samples.


## 2.2. Preparation of the EIR

The dry procedure was used for preparing CAB-impregnated XAD-2010 resin beads [29]. Before the impregnation process, Amberlite XAD-2010 resin beads were treated with 1 : 1 methanol-water solution containing 6 M HCl for 12 h in order to remove remaining monomers and other types of impurities which may be found with the fabricated beads. The resin was thoroughly rinsed with doubly-distilled water and placed into a drying oven at 323 K for 30 min. To prepare the impregnated resin, portions of Amberlite XAD-2010 resin (1 g of dry resin) were transferred into a series of glass stoppered bottles containing different concentrations of CAB in 200 mL methanol, which was used as the solvent. The mixtures were slowly shaken for 10 h to complete the impregnation process and then heated at 333 K in a drying oven to remove the solvent. Each EIR sample was then transferred to a porous filter and washed successively with HCl (3 M) solution and large amounts of distilled water until no CAB was found in the filtrate, spectrophotometrically. Finally, the impregnated resins were dried at 323 K and weighed. The amount of CAB impregnated on/in the resin beads was determined from the weight change of polymeric resin. To avoid surface peeling and cracking, which cause the leaching of some extractant molecules from the resin beads, the prepared EIR beads were stored under deionized water in a stoppered glass bottle.


## 2.3. Sorption Procedures

### 2.3.1. Static Sorption of U(VI) Ions

A batch technique was used to sorb the U(VI) ions at298±1 K. The 100 mL aliquots of aqueous solution containing suitable concentrations of U(VI) were taken in glass-stoppered bottles and adjusted to a known pH. The CAB-impregnated XAD-2010 resin beads (0.150 g) were added to each bottle and the mixtures were equilibrated for a fixed period of time. The EIR beads were filtered and the sorbed U(VI) ions were desorbed by shaking with 5 mL of 0.50 M HCl. The desorbed U(VI) ions were measured spectrophotometrically by the arsenazo III procedure described in Section 2.4. For adsorption equilibrium studies, the mixtures were shaken at a fixed temperature using a temperature controlled shaker set at 180 rpm for a period of desired time at the optimum pH value and desired ionic strength. After that, the suspensions were filtered and the filtrates were analyzed spectrophotometrically by the arsenazo III procedure described in Section 2.4. The amounts of uranium adsorbed per gram of the EIR beads were calculated at various time “t” (qt) and at equilibrium (qe) by the mass balance equations:
(1)qt=(C0-Ct)Vm,qe=(C0-Ce)Vm,
where qt is the amount of the uranium adsorbed onto the EIR beads at time “t” (mg·g−1), qe, the amount of the uranium adsorbed onto the EIR beads at equilibrium (mg·g−1), C0, the initial concentration of U(VI) in the aqueous solutions (mg·L−1), Ct, the U(VI) concentration remaining in the solutions at time “t” (mg·L−1), Ce, the equilibrium concentration of U(VI) in the solutions (mg·L−1), V, the volume of the solutions used (L), and m, the weight of the EIR beads used in g.


### 2.3.2. Dynamic Sorption of U(VI) Ions

Five hundred milligrams of new EIR was slurried in water and then packed into a polyethylene column with an internal diameter of 0.4 cm. The ends were fitted with a small amount of glass wool to keep the EIR beads inside of the column and to prevent any loss of the EIR beads during the sample running. The bed length of EIR in the column was about 32 mm. Working solutions containing U(VI) metal ion, with the concentration exceeding the detection limit, prepared in which the pH and ionic strength were, respectively, adjusted to 4.5 and 0.1 M, using the acetic acid and ammonium acetate solutions, and passed through the column at a known flow rate. After this step, stripping experiments were performed. For this purpose, the column was washed with distilled water (5 mL), and then, 5 mL of 0.50 mol L−1 HCl was used to strip U(VI) ions. The desorbed metal ions were analyzed spectrophotometrically by arsenazo III procedure described in Section 2.4.


## 2.3.1. Static Sorption of U(VI) Ions

A batch technique was used to sorb the U(VI) ions at298±1 K. The 100 mL aliquots of aqueous solution containing suitable concentrations of U(VI) were taken in glass-stoppered bottles and adjusted to a known pH. The CAB-impregnated XAD-2010 resin beads (0.150 g) were added to each bottle and the mixtures were equilibrated for a fixed period of time. The EIR beads were filtered and the sorbed U(VI) ions were desorbed by shaking with 5 mL of 0.50 M HCl. The desorbed U(VI) ions were measured spectrophotometrically by the arsenazo III procedure described in Section 2.4. For adsorption equilibrium studies, the mixtures were shaken at a fixed temperature using a temperature controlled shaker set at 180 rpm for a period of desired time at the optimum pH value and desired ionic strength. After that, the suspensions were filtered and the filtrates were analyzed spectrophotometrically by the arsenazo III procedure described in Section 2.4. The amounts of uranium adsorbed per gram of the EIR beads were calculated at various time “t” (qt) and at equilibrium (qe) by the mass balance equations:
(1)qt=(C0-Ct)Vm,qe=(C0-Ce)Vm,
where qt is the amount of the uranium adsorbed onto the EIR beads at time “t” (mg·g−1), qe, the amount of the uranium adsorbed onto the EIR beads at equilibrium (mg·g−1), C0, the initial concentration of U(VI) in the aqueous solutions (mg·L−1), Ct, the U(VI) concentration remaining in the solutions at time “t” (mg·L−1), Ce, the equilibrium concentration of U(VI) in the solutions (mg·L−1), V, the volume of the solutions used (L), and m, the weight of the EIR beads used in g.


## 2.3.2. Dynamic Sorption of U(VI) Ions

Five hundred milligrams of new EIR was slurried in water and then packed into a polyethylene column with an internal diameter of 0.4 cm. The ends were fitted with a small amount of glass wool to keep the EIR beads inside of the column and to prevent any loss of the EIR beads during the sample running. The bed length of EIR in the column was about 32 mm. Working solutions containing U(VI) metal ion, with the concentration exceeding the detection limit, prepared in which the pH and ionic strength were, respectively, adjusted to 4.5 and 0.1 M, using the acetic acid and ammonium acetate solutions, and passed through the column at a known flow rate. After this step, stripping experiments were performed. For this purpose, the column was washed with distilled water (5 mL), and then, 5 mL of 0.50 mol L−1 HCl was used to strip U(VI) ions. The desorbed metal ions were analyzed spectrophotometrically by arsenazo III procedure described in Section 2.4.


## 2.4. Spectrophotometric Arsenazo III Method for the Determination of U(VI)

The arsenazo III procedure was utilized for the determination of U(VI) in solutions [32]. A pH 2.0 buffer solution of KCl/HCl was prepared by mixing 8.1 mL of 0.20 mol L−1 HCl and 41.9 mL of 0.2 mol L−1 KCl solutions and diluting to 100 mL with doubly-distilled water. A reagent blank solution containing arsenazo III 1% (w/v) and buffer solution was freshly prepared before each measurement. Working solutions (2.5 mL) containing U(VI) + 0.2 mL of arsenazo III solution + 2.0 mL of buffer solution were diluted to 5.0 mL with distilled water and measured at 653.0 nm.


## 3. Results and Discussion

### 3.1. Preparation of CAB-Impregnated Resin

Chrome Azurol B (CAB) is one of the triphenylmethane dyes. It is a dicarboxylic acid with molecular formula of C23H16Cl2O6 (structure is shown in Figure 1). It is slightly soluble in alcohol, soluble in water and gives a reddish orange color solution. This solution turns blue violet at pH 13 (595 nm). It is a highly sensitive colorimetric reagent for Fe(III) and is utilized for the determination of the iron content in blood serum at pH 4.4–5.5 in the presence of cetyltrimethylammonium bromide [33, 34]. The dye has been utilized for spectrophotometric determination of protein (human serum albumin) using Chrom Azurol B-beryllium(II) complex by manual and flow-injection methods [35]. Also, it has been used as a precipitating reagent, in the presence of a nonionic surfactant (Triton X-100), for preparing a membrane and its application to effective collection of iron(III) from homogeneous aqueous solutions [36].Figure 1
Molecular structure of CAB.In the current study, CAB was impregnated onto/into Amberlite XAD-2010 which is used for the preconcentration and isolation of organic materials at trace levels. The resin also has been used as a polymeric support for solid-phase extraction and preconcentration of certain metal ions [37–39].To prepare the appropriate form of the EIR, the impregnation process was carried out at various impregnation ratios (g CAB/g dry polymer adsorbent). Figure2 depicts the weight change obtained against the CAB concentration after washing the EIR with HCl and distilled water. A maximum weight change (150.8%) was found at the concentrations more than 2.50 g CAB per 200 mL methanol, which was used for the EIR preparation.Figure 2
Effect of CAB/resin ratio (g CAB/g dry resin) on the EIR preparation at the conditions in which portions of 1 g of the dry polymer beads of Amberlite XAD-2010 were subjected to the impregnation process in 200 mL methanol.


### 3.2. Stabilizing Extractant Capacity Impregnated on the Polymer

The impregnation of porous matrices leads to the immobilization of the extractant both in pores and in the gel regions of the polymer beads. The impregnating extractant located in the pore volume is weakly retained by the polymer (mainly due to the capillary forces) and can be easily leached out from the freshly prepared EIR samples during the first days of its use (unstable part of EIR capacity). The impregnating extractant taken up by the gel regions of the matrix represents the most stable part of the EIR capacity, which remains practically constant for a long period [40, 41]. Thus, for stabilizing the EIR capacity (the amount of extractant impregnated on the resin), several sorption-desorption cycles were carried out by treating the EIR samples obtained in Figure 2 (EIR sample with maximum impregnated extractant, 1.51 g CAB per 1 g XAD-2010 resin beads) with 100 mL aliquots of U(VI) solution having high concentration (0.01 M at the optimum pH and ionic strength) and 10 mL aliquots of HCl 2 mol L−1 solution as eluent. The sorption-desorption cycles lead to the gradual removal of the extractant molecules from the pore volume of the polymer matrix. The experiments showed that after 13 sorption-desorption cycles the impregnated extractant capacity of EIR was constant. Figure 3 shows the decreasing impregnating extractant capacity (decreasing extractant weight percent impregnated onto 1 g XAD-2010 resin) on the resin against the number of sorption-desorption cycles. In addition, Figure 3 shows that the impregnating extractant molecules, which were mainly retained due to the capillary forces on the EIR samples, were leached out after 13 cycles of U(VI) sorption-desorption and, final washing, the EIR samples with HCl 4 mol·L−1 and distilled water. Also, Figure 3 depicts that almost 36.9% of impregnating extractant capacity immobilized on the untreated EIR, prepared at the maximum impregnating ratio, leach out from the EIR beads by 13 cycles of sorption and desorption. Hence, the maximum weight change is 95.1% (150.8% in untreated EIR) which can obtain at the concentrations more than 6.25 g CAB per 1 L methanol.Figure 3
Stabilizing impregnating extractant capacity on the resin weight change after stabilizing extractant content of EIR beads by carrying out sorption-desorption cycles.The chemical stability of the EIR was examined by sequentially suspending a 0.150-g portion of the EIR in different pHs and shaking for 10 h. After filtering the solutions and rinsing the EIR with distilled water, the released amount of CAB in solution was examined, spectrophotometrically. The EIR demonstrated high chemical stability since no quantity of CAB was released into the solutions.


### 3.3. Effect of pH and Ionic Strength on U(VI) Sorption onto/into New EIR

Initially, these experiments were carried out to select the optimum sorption medium. Buffer solutions of pH 1–8 were used to measure the pH effect on the sorption of U(VI) ions. The concentration and volume of U(VI) solutions used for this study were 100μg L−1 and 100 mL at 298±1 K. The adsorbent dosage was 0.150 g of dry EIR at maximum impregnation ratio (0.95 g CAB/g dry XAD-2010). The shaker speed was 180 rpm and time contact was about 30 min. The results are shown in Figure 4. The sorption increases with increasing pH of sorptive solution and attains a maximum value at pH 4.2–4.7. This indicates that the sorption process involves the release of H+ ions to allow the firm complexation of U(VI) ions to CAB/XAD-2010 at the optimum pH. At the low pHs, the release of H+ ions was not efficient because of the low acidic dissociation constant of Chrome Azurol B. However, the amount of metal ions sorbed decreased when pH was very high. This may be due to the hydrolysis of the U(VI) metal ions in high pH solutions [25]. Because of these considerations, the buffer pH of 4.5 was selected for subsequent investigations.Figure 4
Effect of pH on the recovery percent of U(VI) using 100 mL of model solutions of 100μg L−1 U(VI) containing 0.150 g of the EIR at 298±1 K.The effect of ionic strength on the sorption process was also studied at the presence of sodium nitrate within the concentration range 0.01–0.40 mol·L−1. For this purpose, 100 mL aliquots of U(VI) solution (pH 4.5) having concentration of 100 μg L−1 U(VI) were treated with 0.150-g portions of EIR at 298±1 K and different ionic strengths. It was found that the sorption efficiencies were diminished at the ionic strength values greater than 0.3 mol L−1. This behavior is almost predictable since by increasing the ionic strength the salt effect is enhanced and, consequently, the sorption process is inhibited. Hence, the ionic strength did not exceed 0.3 mol·L−1 at subsequent investigations.


### 3.4. Effect of Shaking Speed on U(VI) Ions Sorption

Sorption of metal ions as a function of shaking speed was studied in the range of 30–200 rpm. The aliquots of 100 mL of U(VI) solution having concentration of 100μg L−1 were treated with 0.150-g portions of EIR at the optimum conditions. It was found that percent sorption increases with increasing shaking speed and attains a maximum sorption at 180 rpm. For further studies, shaking speed of 180 rpm was employed for U(VI) ions sorption in batch experiments.


### 3.5. Effect of Contact Time on U(VI) Ions Sorption

The sorption of U(VI) ions onto/into EIR was studied as a function of shaking time. Sorption process was very rapid andt1/2 is smaller than 6 min. Also, 25 min was found to be sufficient time to attain maximum sorption of U(VI) ions onto/into new EIR. The fast kinetics of resin-metal interaction at optimum pH (4.5) may be attributed to better accessibility of the chelating sites of the modified resin for metal ions. Beyond 25 min, no increase in percent sorption was observed; therefore, for further investigations 25 min agitation time was applied. Also, this fast equilibration rate may be related to the large surface area and pore size of Amberlite XAD-2010. Accordingly, the EIR can be applied to column separation and preconcentration of U(VI) ions.


### 3.6. Sorption Capacity

The sorption capacity of the Amberlite XAD-2010 resin impregnated with CAB for the extraction of uranium was also determined. Increasing amounts of uranium were added to 0.150 g of impregnated resin. The sorption curve (not shown) appears to be linear in the range of 1.5 × 10−6–1.5 × 10−4 mol of U(VI) per 150.0 mL and it reaches a plateau at maximum sorption capacity, that is, 0.632 mmol Uranium/g EIR at pH 4.5. To compare the sorption capacity of the EIR with that of nonimpregnated Amberlite XAD-2010, the sorption capacity of the nonimpregnated Amberlite XAD-2010 resin, also, was determined at the above mentioned concentrations. The results showed that the sorption capacity of the nonimpregnated Amberlite XAD-2010 resin was negligible. This indicates that CAB/XAD-2010 resin could be used as a good sorbent for preconcentration of uranium in the trace concentration range.


### 3.7. Desorption Studies

Various mineral acids were studied as eluent to investigate their efficiency for desorbing and separating U(VI) ions from the EIR, using different volumes and concentrations of each eluent. The results were summarized in Table1. It was found that 5 mL of 0.50 mol·L−1 HCl was sufficient for quantitative recovery of U(VI) ions. Therefore, 5 mL of 0.50 mol·L−1 HCl specified as the eluent for desorption of metal U(VI) ions from EIR and was used for the subsequent studies.Table 1
Effect of type and concentration of eluting acid on recovery of U(VI) ions (n=3).
Eluent
Volume (mL)
Concentration (M)
Recovery (%)
HNO3
10
0.5
83.1
HNO3
10
1.0
87.5
HCl
10
1.0
98.9
HCl
10
0.5
98.9
HCl
5
1.0
98.8
HCl
5
0.5
98.9
HCl
5
0.4
94.6
H2SO4
10
0.5
92.3
H2SO4
5
1.0
94.0
H2SO4
5
2.0
93.8
HAC
10
0.5
38.1
HAC
10
1.0
40.8


### 3.8. Adsorption Equilibrium Studies

Equilibrium properties of adsorption systems are usually expressed as adsorption isotherms. Adsorption isotherm is a function that correlates the amount of metal ion adsorbed per unit weight of the adsorbent,qe (mg·g−1), and the equilibrium concentration of metal ion in bulk solution, Ce (mg·L−1), at a given temperature. The isotherm function deals with the adsorption model, which is an important physicochemical feature for the description of how metal ions interact with active sites in the adsorbent surface. The adsorption model is critical in evaluating the basic characteristics of a good adsorbent. In an EIR system, the adsorption process results in the sorption of metal ions from the solution onto the polymeric matrix until the remaining metal ions in the solution are in dynamic equilibrium with metal ions on the EIR surface. At equilibrium there is a finite distribution of the metal ion between the solution and EIR phase, which can be described by many isotherms and adsorption models that can be used to fit the observed experimental data and determining the model parameters. Three isotherm equations have been tested in the present study, namely, Langmuir [42], Tempkin and Pyzhev [43], and Freundlich [44]. These isotherm equations are represented by the following.Langmuir isotherm:(2)qe=qmaxbCe1+bCe,
freundlich isotherm:
(3)qe=KFCe1/n,
tempkin isotherm:
(4)qe=RTb(lnKTCe).The linear form of the Langmuir, Freundlich and Tempkin isotherms can be expressed by (5)–(7), respectively. Consider
(5)Ceqe=Ceqmax+1bqmax,(6)logqe=logKf+1nlogCe,(7)qe=BlnKT+BlnCe,
where Ce is the equilibrium concentration (mg·L−1), qe is the adsorption capacity at equilibrium (mg·g−1), qmax (mg·g−1) represents the maximum adsorption capacity, b (L·mg−1) relates the energy of adsorption, Kf indicates relative adsorption capacity (mg1−(1/n) ·L1/n·g−1), n is an empirical parameter related to the intensity of adsorption, B is the Tempkin constant related to the heat of adsorption (B=RT/b), and KT is the equilibrium binding constant (L·g−1) corresponding to the maximum binding energy.The isotherm plots were drawn using (5)–(7) and the resulted plots are depicted in Figure 5. The values of isotherms parameters are presented in Table 2. As seen from Table 2 and Figure 5, the Langmuir isotherm shows a higher correlation coefficient, and a better fit, to adsorption data than the other isotherm equations. This explains the suitability of Langmuir model for describing the adsorption equilibrium of U(VI) onto CAB/XAD-2010.Table 2
Parameters of the Langmuir and Freundlich isotherm models for the adsorption of U(II) ion by CAB-impregnated XAD-2010.
Isotherm model
Magnitude
Langmuir
qmax (mg·g−1)
156.2
b (L·mg−1)
48.85
×
10
-
2
R2
0.9998
Freundlich
KF (mg1-(1/n)·L1/n·g−1)
51.02
n
3.323
R2
0.8181
Tempkin
B
22.41
KT (L·g−1)
16.013
R2
0.9641Langmuir (a), Freundlich (b), and Tempkin (c) adsorption isotherms for U(VI) adsorption by EIR (pH 4.5 and temperature 298 K).
(a)
(b)
(c)The Langmuir adsorption isotherm is based on the assumption that all adsorption sites are equivalent and that adsorption in an active site is independent of whether the adjacent sites are occupied or not. The fact that the Langmuir isotherm fits the experimental data very well may be due to homogenous distribution of extractant molecules, or active chelating sites, on the polymeric surface, since the Langmuir equation assumes that the adsorbent surface is homogenous [28].


### 3.9. Dynamic Sorption

#### 3.9.1. Effect of Column Flow Rate on Sorption and Desorption

The effect of column flow rate on the sorption of U(VI) was separately studied in the range of 1–18 mL min−1 using 1 L of solution with U(VI) concentration of 10 μg L−1 at the pH chosen for maximum sorption for both metal ions. The optimum flow rates for U(VI) absorption were 11 mL min−1 (Figure 6). Therefore, a flow rate of 11 mL min−1 was selected for further studies in the preconcentration of U(VI) ions.  Optimum column desorption flow rates were investigated using 5 mL of the recommended eluent solution, 0.50 mol·L−1 HCl, after loading the column with 1 L of sample solutions with concentration of 10 μg L−1 with respect to U(VI) followed by rinsing the column with 5 mL double-distilled water. Figure 6 shows that optimum flow rate for desorpting U(VI) is 0.5 mL min−1.Figure 6
Effect of sample and eluent flow rates on the recovery of U(VI) using 1 L of model solution of 10μg L−1 U(VI), eluting with 5 mL eluent solution of 0.50 M HCl. The data presented are the average of five experiments.


#### 3.9.2. Effect of Sample Volume and Preconcentration Factor

Since the concentrations of uranium in real samples are low, the amounts of uranium in these samples should be taken into smaller volumes for high preconcentration factor. Therefore, the limit of preconcentration was determined by increasing the dilution of the U(VI) ion in solution keeping the total amount of loaded U(VI) ion at 10μg. Adsorbed metal ions were stripped (desorbed) with the optimum concentration and volume of specified eluent. Complete recovery can be carried out from solutions with volumes up to 1600 mL with a recovery of >98%, yielding in the preconcentration factor of 160. Thus, for convenience, the sample volume of 1500 mL (the preconcentration factor of 150) was chosen for the column-mode separation and preconcentration of U(VI) ions.In order to determine the detection limit of the proposed dynamic method, 1500 mL aliquots of blank solutions were adjusted to optimized conditions and passed through the column. After eluting the column and determining uranium, the detection limit of the procedure (based on3δ of the blank solution, n=8) was found to be 5.0 × 10−10 mol·L−1 (0.12 μg·L−1).


### 3.10. Effect of Foreign Ions

The performance of the technique for the quantitative separation and preconcentration of U(VI) ions in the presence of foreign cations and anions was investigated by measuring the recovery (%) of U(VI) under optimized conditions. For this purpose, 1500 mL aliquots of U(VI) solution with concentration of 7.0μg L−1 were taken with different amounts of foreign ions and the recommended column-mode procedure was followed. The tolerance limit was defined as the highest ratio of foreign ions that produced an error not exceeding ±5% in the determination of U(VI) ions by the combination of the column solid-phase extraction and arsenazo III method, as described above. The serious interference from Ni(II) and Cu(II) was avoided by masking with potassium cyanide [45], whereas the interference due to Th(VI) was removed by adding EDTA [46]. The tolerated amounts of the foreign ions are given in Table 3. The results show that the proposed method can be adequately applied for the selective determination of U(VI) in the aqueous samples.Table 3
Effect of foreign ions on the determination of 7.0μg of U(VI) in 1,500-mL aliquots of the solution.
Foreign ion
Tolerance ratio
Na+, K+, Mg2+, Ca2+, Ba2+, Zn2+, NH4+, Cl−, I−, Co2+, Sr2+
5000
S
O
4
2
-, Pb2+, CrO42-, Mn2+, Cd2+
3000
Mo
O
4
2
-, Citrate
1000
Ag+
500
Ni2+
300a
Ce3+
200
Th4+
200b
Cu2+
150a
Zr4+, La3+
100
Fe3+
80
Ni2+
5
Cu2+
2
Th4+
1
aIn the presence of potassium cyanide (1×10-3 M).
bIn the presence of EDTA (1×10-3 M).


### 3.11. Application of Proposed Method for Natural Water Samples

The proposed method was applied to the determination of U(VI) in natural water samples including spring, well, and river water samples that they were isokinetically collected in polyethylene bottles from different areas of Kashmar, a city in Iran, Khorasan Razavi province. These water samples were passed through a membrane filter with a pore size of 0.45 mm to remove their particulates and then pH was brought to 4.5. By adding sufficient amounts of potassium cyanide and EDTA, as masking agents, their concentration reached up to 1.0 × 10−3 M. Then, 1500 mL aliquots of the samples were subjected to the recommended dynamic procedure. A recovery test was also performed by determining the spiked amounts of U(VI) to the samples. The obtained results are summarized in Table 4. As observed from the results, the recoveries for the various amounts spiked to the sample solutions were in the range 96.1–101.3%, which reflect the suitability of the present EIR as a preconcentration tool before actual measurement of U(VI) in contaminated water samples using arsenazo III method.Table 4
Application of the proposed method for the determination of U(VI) in 1500 aliquots of environmental water samples.
Sample
Added (μg L−1)
Found (μg L−1)
Recovery (%)
0.0
1.4 (2.9)a
—
Spring water
2.0
3.3 (2.6)
97.0
(Ghazi Spring)
5.0
6.2 (2.7)
96.9
10.0
11.0 (2.6)
96.5
20.0
20.7 (2.6)
96.7
0.0
5.7 (2.3)
—
River water
2.0
7.8 (2.2)
101.3
(Shesh-Taraz)
10.0
15.8 (2.2)
100.6
20.0
25.9 (1.9)
100.7
30.0
35.6 (2.0)
99.7
0.00
—
—
Well water
10.00
9.8 (1.9)
98.0
(Argha)
20.00
19.6 (1.7)
98.0
30.00
29.3 (1.3)
97.7
40.00
39.1 (1.2)
97.8
aRSD of five replicate measurements.


### 3.12. Application of Proposed Method for Standard Geological Samples

For testing the accuracy of the measurements, two model solutions were prepared just according to the composition of JG-1a and JR-1 (Geological Survey of Japan reference samples) by precisely following the literature considerations [47]. The results of the expected and found values are detailed in Table 5. The agreement between found and expected values demonstrated that the described method was accurate for trace analysis of U(VI) in the complex matrices.Table 5
Results of the accuracy test of proposed method for U(VI) determination in two geological standard reference materials.
Samples
U(VI) content (μg g−1)
Found (μg g−1)
Recovery (%)
JG-1aa
4.7
4.63 (3.1)b
98.6
JR-1a
8.9
8.81 (3.0)b
99.0
aThe treatments were carried out on 0.5 g of the sample.
bRSD of five replicate measurements.


## 3.1. Preparation of CAB-Impregnated Resin

Chrome Azurol B (CAB) is one of the triphenylmethane dyes. It is a dicarboxylic acid with molecular formula of C23H16Cl2O6 (structure is shown in Figure 1). It is slightly soluble in alcohol, soluble in water and gives a reddish orange color solution. This solution turns blue violet at pH 13 (595 nm). It is a highly sensitive colorimetric reagent for Fe(III) and is utilized for the determination of the iron content in blood serum at pH 4.4–5.5 in the presence of cetyltrimethylammonium bromide [33, 34]. The dye has been utilized for spectrophotometric determination of protein (human serum albumin) using Chrom Azurol B-beryllium(II) complex by manual and flow-injection methods [35]. Also, it has been used as a precipitating reagent, in the presence of a nonionic surfactant (Triton X-100), for preparing a membrane and its application to effective collection of iron(III) from homogeneous aqueous solutions [36].Figure 1
Molecular structure of CAB.In the current study, CAB was impregnated onto/into Amberlite XAD-2010 which is used for the preconcentration and isolation of organic materials at trace levels. The resin also has been used as a polymeric support for solid-phase extraction and preconcentration of certain metal ions [37–39].To prepare the appropriate form of the EIR, the impregnation process was carried out at various impregnation ratios (g CAB/g dry polymer adsorbent). Figure2 depicts the weight change obtained against the CAB concentration after washing the EIR with HCl and distilled water. A maximum weight change (150.8%) was found at the concentrations more than 2.50 g CAB per 200 mL methanol, which was used for the EIR preparation.Figure 2
Effect of CAB/resin ratio (g CAB/g dry resin) on the EIR preparation at the conditions in which portions of 1 g of the dry polymer beads of Amberlite XAD-2010 were subjected to the impregnation process in 200 mL methanol.


## 3.2. Stabilizing Extractant Capacity Impregnated on the Polymer

The impregnation of porous matrices leads to the immobilization of the extractant both in pores and in the gel regions of the polymer beads. The impregnating extractant located in the pore volume is weakly retained by the polymer (mainly due to the capillary forces) and can be easily leached out from the freshly prepared EIR samples during the first days of its use (unstable part of EIR capacity). The impregnating extractant taken up by the gel regions of the matrix represents the most stable part of the EIR capacity, which remains practically constant for a long period [40, 41]. Thus, for stabilizing the EIR capacity (the amount of extractant impregnated on the resin), several sorption-desorption cycles were carried out by treating the EIR samples obtained in Figure 2 (EIR sample with maximum impregnated extractant, 1.51 g CAB per 1 g XAD-2010 resin beads) with 100 mL aliquots of U(VI) solution having high concentration (0.01 M at the optimum pH and ionic strength) and 10 mL aliquots of HCl 2 mol L−1 solution as eluent. The sorption-desorption cycles lead to the gradual removal of the extractant molecules from the pore volume of the polymer matrix. The experiments showed that after 13 sorption-desorption cycles the impregnated extractant capacity of EIR was constant. Figure 3 shows the decreasing impregnating extractant capacity (decreasing extractant weight percent impregnated onto 1 g XAD-2010 resin) on the resin against the number of sorption-desorption cycles. In addition, Figure 3 shows that the impregnating extractant molecules, which were mainly retained due to the capillary forces on the EIR samples, were leached out after 13 cycles of U(VI) sorption-desorption and, final washing, the EIR samples with HCl 4 mol·L−1 and distilled water. Also, Figure 3 depicts that almost 36.9% of impregnating extractant capacity immobilized on the untreated EIR, prepared at the maximum impregnating ratio, leach out from the EIR beads by 13 cycles of sorption and desorption. Hence, the maximum weight change is 95.1% (150.8% in untreated EIR) which can obtain at the concentrations more than 6.25 g CAB per 1 L methanol.Figure 3
Stabilizing impregnating extractant capacity on the resin weight change after stabilizing extractant content of EIR beads by carrying out sorption-desorption cycles.The chemical stability of the EIR was examined by sequentially suspending a 0.150-g portion of the EIR in different pHs and shaking for 10 h. After filtering the solutions and rinsing the EIR with distilled water, the released amount of CAB in solution was examined, spectrophotometrically. The EIR demonstrated high chemical stability since no quantity of CAB was released into the solutions.


## 3.3. Effect of pH and Ionic Strength on U(VI) Sorption onto/into New EIR

Initially, these experiments were carried out to select the optimum sorption medium. Buffer solutions of pH 1–8 were used to measure the pH effect on the sorption of U(VI) ions. The concentration and volume of U(VI) solutions used for this study were 100μg L−1 and 100 mL at 298±1 K. The adsorbent dosage was 0.150 g of dry EIR at maximum impregnation ratio (0.95 g CAB/g dry XAD-2010). The shaker speed was 180 rpm and time contact was about 30 min. The results are shown in Figure 4. The sorption increases with increasing pH of sorptive solution and attains a maximum value at pH 4.2–4.7. This indicates that the sorption process involves the release of H+ ions to allow the firm complexation of U(VI) ions to CAB/XAD-2010 at the optimum pH. At the low pHs, the release of H+ ions was not efficient because of the low acidic dissociation constant of Chrome Azurol B. However, the amount of metal ions sorbed decreased when pH was very high. This may be due to the hydrolysis of the U(VI) metal ions in high pH solutions [25]. Because of these considerations, the buffer pH of 4.5 was selected for subsequent investigations.Figure 4
Effect of pH on the recovery percent of U(VI) using 100 mL of model solutions of 100μg L−1 U(VI) containing 0.150 g of the EIR at 298±1 K.The effect of ionic strength on the sorption process was also studied at the presence of sodium nitrate within the concentration range 0.01–0.40 mol·L−1. For this purpose, 100 mL aliquots of U(VI) solution (pH 4.5) having concentration of 100 μg L−1 U(VI) were treated with 0.150-g portions of EIR at 298±1 K and different ionic strengths. It was found that the sorption efficiencies were diminished at the ionic strength values greater than 0.3 mol L−1. This behavior is almost predictable since by increasing the ionic strength the salt effect is enhanced and, consequently, the sorption process is inhibited. Hence, the ionic strength did not exceed 0.3 mol·L−1 at subsequent investigations.


## 3.4. Effect of Shaking Speed on U(VI) Ions Sorption

Sorption of metal ions as a function of shaking speed was studied in the range of 30–200 rpm. The aliquots of 100 mL of U(VI) solution having concentration of 100μg L−1 were treated with 0.150-g portions of EIR at the optimum conditions. It was found that percent sorption increases with increasing shaking speed and attains a maximum sorption at 180 rpm. For further studies, shaking speed of 180 rpm was employed for U(VI) ions sorption in batch experiments.


## 3.5. Effect of Contact Time on U(VI) Ions Sorption

The sorption of U(VI) ions onto/into EIR was studied as a function of shaking time. Sorption process was very rapid andt1/2 is smaller than 6 min. Also, 25 min was found to be sufficient time to attain maximum sorption of U(VI) ions onto/into new EIR. The fast kinetics of resin-metal interaction at optimum pH (4.5) may be attributed to better accessibility of the chelating sites of the modified resin for metal ions. Beyond 25 min, no increase in percent sorption was observed; therefore, for further investigations 25 min agitation time was applied. Also, this fast equilibration rate may be related to the large surface area and pore size of Amberlite XAD-2010. Accordingly, the EIR can be applied to column separation and preconcentration of U(VI) ions.


## 3.6. Sorption Capacity

The sorption capacity of the Amberlite XAD-2010 resin impregnated with CAB for the extraction of uranium was also determined. Increasing amounts of uranium were added to 0.150 g of impregnated resin. The sorption curve (not shown) appears to be linear in the range of 1.5 × 10−6–1.5 × 10−4 mol of U(VI) per 150.0 mL and it reaches a plateau at maximum sorption capacity, that is, 0.632 mmol Uranium/g EIR at pH 4.5. To compare the sorption capacity of the EIR with that of nonimpregnated Amberlite XAD-2010, the sorption capacity of the nonimpregnated Amberlite XAD-2010 resin, also, was determined at the above mentioned concentrations. The results showed that the sorption capacity of the nonimpregnated Amberlite XAD-2010 resin was negligible. This indicates that CAB/XAD-2010 resin could be used as a good sorbent for preconcentration of uranium in the trace concentration range.


## 3.7. Desorption Studies

Various mineral acids were studied as eluent to investigate their efficiency for desorbing and separating U(VI) ions from the EIR, using different volumes and concentrations of each eluent. The results were summarized in Table1. It was found that 5 mL of 0.50 mol·L−1 HCl was sufficient for quantitative recovery of U(VI) ions. Therefore, 5 mL of 0.50 mol·L−1 HCl specified as the eluent for desorption of metal U(VI) ions from EIR and was used for the subsequent studies.Table 1
Effect of type and concentration of eluting acid on recovery of U(VI) ions (n=3).
Eluent
Volume (mL)
Concentration (M)
Recovery (%)
HNO3
10
0.5
83.1
HNO3
10
1.0
87.5
HCl
10
1.0
98.9
HCl
10
0.5
98.9
HCl
5
1.0
98.8
HCl
5
0.5
98.9
HCl
5
0.4
94.6
H2SO4
10
0.5
92.3
H2SO4
5
1.0
94.0
H2SO4
5
2.0
93.8
HAC
10
0.5
38.1
HAC
10
1.0
40.8


## 3.8. Adsorption Equilibrium Studies

Equilibrium properties of adsorption systems are usually expressed as adsorption isotherms. Adsorption isotherm is a function that correlates the amount of metal ion adsorbed per unit weight of the adsorbent,qe (mg·g−1), and the equilibrium concentration of metal ion in bulk solution, Ce (mg·L−1), at a given temperature. The isotherm function deals with the adsorption model, which is an important physicochemical feature for the description of how metal ions interact with active sites in the adsorbent surface. The adsorption model is critical in evaluating the basic characteristics of a good adsorbent. In an EIR system, the adsorption process results in the sorption of metal ions from the solution onto the polymeric matrix until the remaining metal ions in the solution are in dynamic equilibrium with metal ions on the EIR surface. At equilibrium there is a finite distribution of the metal ion between the solution and EIR phase, which can be described by many isotherms and adsorption models that can be used to fit the observed experimental data and determining the model parameters. Three isotherm equations have been tested in the present study, namely, Langmuir [42], Tempkin and Pyzhev [43], and Freundlich [44]. These isotherm equations are represented by the following.Langmuir isotherm:(2)qe=qmaxbCe1+bCe,
freundlich isotherm:
(3)qe=KFCe1/n,
tempkin isotherm:
(4)qe=RTb(lnKTCe).The linear form of the Langmuir, Freundlich and Tempkin isotherms can be expressed by (5)–(7), respectively. Consider
(5)Ceqe=Ceqmax+1bqmax,(6)logqe=logKf+1nlogCe,(7)qe=BlnKT+BlnCe,
where Ce is the equilibrium concentration (mg·L−1), qe is the adsorption capacity at equilibrium (mg·g−1), qmax (mg·g−1) represents the maximum adsorption capacity, b (L·mg−1) relates the energy of adsorption, Kf indicates relative adsorption capacity (mg1−(1/n) ·L1/n·g−1), n is an empirical parameter related to the intensity of adsorption, B is the Tempkin constant related to the heat of adsorption (B=RT/b), and KT is the equilibrium binding constant (L·g−1) corresponding to the maximum binding energy.The isotherm plots were drawn using (5)–(7) and the resulted plots are depicted in Figure 5. The values of isotherms parameters are presented in Table 2. As seen from Table 2 and Figure 5, the Langmuir isotherm shows a higher correlation coefficient, and a better fit, to adsorption data than the other isotherm equations. This explains the suitability of Langmuir model for describing the adsorption equilibrium of U(VI) onto CAB/XAD-2010.Table 2
Parameters of the Langmuir and Freundlich isotherm models for the adsorption of U(II) ion by CAB-impregnated XAD-2010.
Isotherm model
Magnitude
Langmuir
qmax (mg·g−1)
156.2
b (L·mg−1)
48.85
×
10
-
2
R2
0.9998
Freundlich
KF (mg1-(1/n)·L1/n·g−1)
51.02
n
3.323
R2
0.8181
Tempkin
B
22.41
KT (L·g−1)
16.013
R2
0.9641Langmuir (a), Freundlich (b), and Tempkin (c) adsorption isotherms for U(VI) adsorption by EIR (pH 4.5 and temperature 298 K).
(a)
(b)
(c)The Langmuir adsorption isotherm is based on the assumption that all adsorption sites are equivalent and that adsorption in an active site is independent of whether the adjacent sites are occupied or not. The fact that the Langmuir isotherm fits the experimental data very well may be due to homogenous distribution of extractant molecules, or active chelating sites, on the polymeric surface, since the Langmuir equation assumes that the adsorbent surface is homogenous [28].


## 3.9. Dynamic Sorption

### 3.9.1. Effect of Column Flow Rate on Sorption and Desorption

The effect of column flow rate on the sorption of U(VI) was separately studied in the range of 1–18 mL min−1 using 1 L of solution with U(VI) concentration of 10 μg L−1 at the pH chosen for maximum sorption for both metal ions. The optimum flow rates for U(VI) absorption were 11 mL min−1 (Figure 6). Therefore, a flow rate of 11 mL min−1 was selected for further studies in the preconcentration of U(VI) ions.  Optimum column desorption flow rates were investigated using 5 mL of the recommended eluent solution, 0.50 mol·L−1 HCl, after loading the column with 1 L of sample solutions with concentration of 10 μg L−1 with respect to U(VI) followed by rinsing the column with 5 mL double-distilled water. Figure 6 shows that optimum flow rate for desorpting U(VI) is 0.5 mL min−1.Figure 6
Effect of sample and eluent flow rates on the recovery of U(VI) using 1 L of model solution of 10μg L−1 U(VI), eluting with 5 mL eluent solution of 0.50 M HCl. The data presented are the average of five experiments.


### 3.9.2. Effect of Sample Volume and Preconcentration Factor

Since the concentrations of uranium in real samples are low, the amounts of uranium in these samples should be taken into smaller volumes for high preconcentration factor. Therefore, the limit of preconcentration was determined by increasing the dilution of the U(VI) ion in solution keeping the total amount of loaded U(VI) ion at 10μg. Adsorbed metal ions were stripped (desorbed) with the optimum concentration and volume of specified eluent. Complete recovery can be carried out from solutions with volumes up to 1600 mL with a recovery of >98%, yielding in the preconcentration factor of 160. Thus, for convenience, the sample volume of 1500 mL (the preconcentration factor of 150) was chosen for the column-mode separation and preconcentration of U(VI) ions.In order to determine the detection limit of the proposed dynamic method, 1500 mL aliquots of blank solutions were adjusted to optimized conditions and passed through the column. After eluting the column and determining uranium, the detection limit of the procedure (based on3δ of the blank solution, n=8) was found to be 5.0 × 10−10 mol·L−1 (0.12 μg·L−1).


## 3.9.1. Effect of Column Flow Rate on Sorption and Desorption

The effect of column flow rate on the sorption of U(VI) was separately studied in the range of 1–18 mL min−1 using 1 L of solution with U(VI) concentration of 10 μg L−1 at the pH chosen for maximum sorption for both metal ions. The optimum flow rates for U(VI) absorption were 11 mL min−1 (Figure 6). Therefore, a flow rate of 11 mL min−1 was selected for further studies in the preconcentration of U(VI) ions.  Optimum column desorption flow rates were investigated using 5 mL of the recommended eluent solution, 0.50 mol·L−1 HCl, after loading the column with 1 L of sample solutions with concentration of 10 μg L−1 with respect to U(VI) followed by rinsing the column with 5 mL double-distilled water. Figure 6 shows that optimum flow rate for desorpting U(VI) is 0.5 mL min−1.Figure 6
Effect of sample and eluent flow rates on the recovery of U(VI) using 1 L of model solution of 10μg L−1 U(VI), eluting with 5 mL eluent solution of 0.50 M HCl. The data presented are the average of five experiments.


## 3.9.2. Effect of Sample Volume and Preconcentration Factor

Since the concentrations of uranium in real samples are low, the amounts of uranium in these samples should be taken into smaller volumes for high preconcentration factor. Therefore, the limit of preconcentration was determined by increasing the dilution of the U(VI) ion in solution keeping the total amount of loaded U(VI) ion at 10μg. Adsorbed metal ions were stripped (desorbed) with the optimum concentration and volume of specified eluent. Complete recovery can be carried out from solutions with volumes up to 1600 mL with a recovery of >98%, yielding in the preconcentration factor of 160. Thus, for convenience, the sample volume of 1500 mL (the preconcentration factor of 150) was chosen for the column-mode separation and preconcentration of U(VI) ions.In order to determine the detection limit of the proposed dynamic method, 1500 mL aliquots of blank solutions were adjusted to optimized conditions and passed through the column. After eluting the column and determining uranium, the detection limit of the procedure (based on3δ of the blank solution, n=8) was found to be 5.0 × 10−10 mol·L−1 (0.12 μg·L−1).


## 3.10. Effect of Foreign Ions

The performance of the technique for the quantitative separation and preconcentration of U(VI) ions in the presence of foreign cations and anions was investigated by measuring the recovery (%) of U(VI) under optimized conditions. For this purpose, 1500 mL aliquots of U(VI) solution with concentration of 7.0μg L−1 were taken with different amounts of foreign ions and the recommended column-mode procedure was followed. The tolerance limit was defined as the highest ratio of foreign ions that produced an error not exceeding ±5% in the determination of U(VI) ions by the combination of the column solid-phase extraction and arsenazo III method, as described above. The serious interference from Ni(II) and Cu(II) was avoided by masking with potassium cyanide [45], whereas the interference due to Th(VI) was removed by adding EDTA [46]. The tolerated amounts of the foreign ions are given in Table 3. The results show that the proposed method can be adequately applied for the selective determination of U(VI) in the aqueous samples.Table 3
Effect of foreign ions on the determination of 7.0μg of U(VI) in 1,500-mL aliquots of the solution.
Foreign ion
Tolerance ratio
Na+, K+, Mg2+, Ca2+, Ba2+, Zn2+, NH4+, Cl−, I−, Co2+, Sr2+
5000
S
O
4
2
-, Pb2+, CrO42-, Mn2+, Cd2+
3000
Mo
O
4
2
-, Citrate
1000
Ag+
500
Ni2+
300a
Ce3+
200
Th4+
200b
Cu2+
150a
Zr4+, La3+
100
Fe3+
80
Ni2+
5
Cu2+
2
Th4+
1
aIn the presence of potassium cyanide (1×10-3 M).
bIn the presence of EDTA (1×10-3 M).


## 3.11. Application of Proposed Method for Natural Water Samples

The proposed method was applied to the determination of U(VI) in natural water samples including spring, well, and river water samples that they were isokinetically collected in polyethylene bottles from different areas of Kashmar, a city in Iran, Khorasan Razavi province. These water samples were passed through a membrane filter with a pore size of 0.45 mm to remove their particulates and then pH was brought to 4.5. By adding sufficient amounts of potassium cyanide and EDTA, as masking agents, their concentration reached up to 1.0 × 10−3 M. Then, 1500 mL aliquots of the samples were subjected to the recommended dynamic procedure. A recovery test was also performed by determining the spiked amounts of U(VI) to the samples. The obtained results are summarized in Table 4. As observed from the results, the recoveries for the various amounts spiked to the sample solutions were in the range 96.1–101.3%, which reflect the suitability of the present EIR as a preconcentration tool before actual measurement of U(VI) in contaminated water samples using arsenazo III method.Table 4
Application of the proposed method for the determination of U(VI) in 1500 aliquots of environmental water samples.
Sample
Added (μg L−1)
Found (μg L−1)
Recovery (%)
0.0
1.4 (2.9)a
—
Spring water
2.0
3.3 (2.6)
97.0
(Ghazi Spring)
5.0
6.2 (2.7)
96.9
10.0
11.0 (2.6)
96.5
20.0
20.7 (2.6)
96.7
0.0
5.7 (2.3)
—
River water
2.0
7.8 (2.2)
101.3
(Shesh-Taraz)
10.0
15.8 (2.2)
100.6
20.0
25.9 (1.9)
100.7
30.0
35.6 (2.0)
99.7
0.00
—
—
Well water
10.00
9.8 (1.9)
98.0
(Argha)
20.00
19.6 (1.7)
98.0
30.00
29.3 (1.3)
97.7
40.00
39.1 (1.2)
97.8
aRSD of five replicate measurements.


## 3.12. Application of Proposed Method for Standard Geological Samples

For testing the accuracy of the measurements, two model solutions were prepared just according to the composition of JG-1a and JR-1 (Geological Survey of Japan reference samples) by precisely following the literature considerations [47]. The results of the expected and found values are detailed in Table 5. The agreement between found and expected values demonstrated that the described method was accurate for trace analysis of U(VI) in the complex matrices.Table 5
Results of the accuracy test of proposed method for U(VI) determination in two geological standard reference materials.
Samples
U(VI) content (μg g−1)
Found (μg g−1)
Recovery (%)
JG-1aa
4.7
4.63 (3.1)b
98.6
JR-1a
8.9
8.81 (3.0)b
99.0
aThe treatments were carried out on 0.5 g of the sample.
bRSD of five replicate measurements.


## 4. Conclusions

Chrome Azurol B-impregnated XAD-2010 resin beads were prepared and used for solid-phase extraction and preconcentration of U(VI) in various environmental water samples. The proposed procedure for the determination of trace amounts of U(VI) ions combines preconcentration of the analyte with spectrophotometric measurement with the arsenazo III procedure. The sorption equilibrium data were analyzed using widely used isotherm models. The Langmuir isotherm gave the best fit of the experimental equilibrium data. Thus, the distribution of extractant molecules on the polymeric surface is homogenous, and the adsorption process is monolayer. The optimized experimental parameters for the new solid-phase extraction system have been summarized in Table6. The new EIR benefits from high sorption capacities and excellent selectivity. Also the proposed preconcentration method was simple and rapid, and it is a convenient and low cost one. The new EIR had excellent selectivity for U(VI) in the complex matrixes of geological samples, and the matrix effects with the method were reasonably tolerable. The system was also successful in pre-concentrating metal ions from large sample volume. Overall, some of the practical benefits of the new method include its capacity, selectivity, good detection limit, high preconcentration factor, low cost, speed, convenience, and ease of regeneration of the EIR.Table 6
Optimized experimental parameters for separation and pre-concentration of U(VI) ions by CAB-impregnated XAD-2010.
Experimental parameter
Optimum magnitude
Batch parameters
pH
4.2–4.7
Ionic strength
0.01–0.30 mol·L−1
Shaking speed
180 rpm
Contact time
25 min
t1/2
6 min
Capacity
0.632 mmol·g−1
Concentration of eluent (HCl)
0.50 M
Volume of eluent
5 mL
Dynamic parameters
Sample flow rate
11 mL·min−1
Eluent flow rate
0.5 mL·min−1
Sample volume
1600 mL
LOD
5.0
×
10
-
10 mol·L−1



---

*Source: 671564-2013-11-04.xml*