# The Establishment of Bisphenol A Sensing System Utilizing Molecularly Imprinted Polymer Receptor and Electrochemical Determination

Authors: Izumi Kubo; Nobuyuki Yokota; Yuko Nakane; Yusuke Fuchiwaki
Journal: International Journal of Electrochemistry
 (2011)

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## Abstract

A sensing system of bisphenol A (BPA) based on the electrochemical detection utilizing molecularly imprinted polymer (MIP) as a receptor of BPA was investigated. MIP for BPA was polymerized thermally from 4-vinylpyridine as a functional monomer and ethylene dimethacrylate (EDMA) as a cross-linker and served to prepare an MIP packed column. BPA in an aqueous solution was adsorbed to an MIP packed column and eluted by acetonitrile/phosphate buffer (60/40, v/v). From aqueous solution, BPA was adsorbed to the column and eluted completely in the eluent. The eluted BPA was electrochemically detected by cyclic voltammetry.  Optimum pH and scan rate were 7.0 and 0.1 V/s in phosphate buffer. Electrochemical detection of BPA in acetonitrile/phosphate buffer was performed, and linear relationship between BPA and anodic peak current was observed at the range of 10–100μM. In the eluent, anodic peak current of BPA was observed around 650 mV.


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## Body

## 1. Introduction

Bisphenol A (BPA) is widely used as a material of plastic container, dishes, and milk bottles and distributed almost everywhere on earth. However, it is known to be an endocrine disrupting chemical (EDC) and its toxicity and biological influences have been reported [1, 2].  Detection and removal of bisphenol A are quite important.Conventionally, BPA has been determined with use of GC/MS or HPLC [3]. These apparatuses are expensive and need complicated pretreatment and are not applicable to the on-site monitoring. On the other hand, as electrochemical sensor is simple, inexpensive, and applicable to monitoring.Molecularly imprinted polymers (MIPs) have been utilized as a solid phase extraction in HPLC. Recently MIPs are utilized as a recognition element of chemical sensors.  Chemical sensors to detect triazine moiety such as atrazine and simazine have been reported by coupling of MIP- membrane and electrochemical detection [4–9]. To detect simazine, MIP receptor for simazine was prepared with use of simazine as a template and served to selective binding of simazine in a column [10].  The simazine-imprinted polymer packed column was coupled with the electrochemical determination of simazine and a sensing system of simazine was established by Fuchiwaki et al. [11]. On the other hand, MIP for BPA was extensively studied [12–14] and applied to chromatography in extraction of BPA from environmental water. Electrochemical oxidation of BPA has been studied and applied to its removal from aqueous solution [15].  Sensing system for BPA detection has not been reported based on voltammetry of BPA utilizing MIP as a receptor.In this study we aimed to establish a sensing system of BPA based on its electrochemical detection, utilizing MIP as a receptor of BPA.  To fabricate MIP for BPA, 4-vilylpyridine was used as a functional monomer to recognize BPA by hydrogen bond, which was cross-linked by ethylene dimethacrylate (EDMA). And MIP packed column was coupled with electrochemical detection system. BPA was determined through cyclic voltammetry. This system looked simple, reasonable, and user friendly.


## 2. Experimental

### 2.1. Materials

BPA, which is a standard chemical for environmental analysis, and 4-vinylpyridine were purchased from Kanto Chemicals. Dibutyl phthalate, 2, 2′-azobis(2, 4 dimethylvaleronitril), and Ethylene dimethacrylate (EDMA) were obtained from WAKO Pure Chemicals.  Other reagents were laboratory-grade and used without any purification. 4-vinylpiridine was distilled to remove stabilizer prior to use.


### 2.2. Preparation of Molecularly Imprinted Polymer Receptor for BPA

Molecularly imprinted polymer for BPA was prepared according to the procedure reported previously in [13] and modified. 4-vinyl pyridine was used as a functional monomer to fabricate the recognition site for BPA by the hydrogen bonding and cross-liked by EDMA.  All the reagents were dissolved by toluene and polymerized at 60°C. The obtained polymer was crushed well into particles. The particles were thoroughly washed to remove template molecule by methanol and dried in vacuo. In the preparation of MIP, 1 g of MIP was obtained from 90 mg of BPA, 320 mg of 4-vinylpyridine, and 2.5 mL of EDMA. The dried polymer particles were filtrated and selected, size between 32 and 90 μm mesh. These particles were served as MIP receptor for BPA and 10 mg of them were packed in a glass column.  Absorbance of BPA to the MIP receptor was evaluated by the UV absorbance at 270 nm of the loaded and eluted solution of BPA.


### 2.3. Electrochemical Measurements

A three-electrode cell was used in the electrochemical measurements.  A gold electrode (I.D.=1.6mm) was used as a working electrode. A platinum wire counter and an Ag/AgCl reference electrode were used in the electrochemical experiments. Electrochemical measurements were carried out in a glass vial containing 1 mL of deoxygenated electrolyte solution at room temperature according to the previously reported procedure [15]. Cyclic voltammetry of BPA was measured at a range from 0 V to 0.8 V.   The response to BPA was obtained from the current difference, with and without BPA at around 0.6 V, which was the anodic peak current of BPA oxidation.


### 2.4. BPA Sensing System

BPA sensing system was equipped with an MIP packed column to electrochemical measurement system. An aliquot of sample solution containing BPA was loaded to the MIP column. The bound BPA was eluted by 60% (v/v) acetonitrile/0.1 M phosphate buffer (pH7.0).  The eluent was served to electrochemical measurement.


## 2.1. Materials

BPA, which is a standard chemical for environmental analysis, and 4-vinylpyridine were purchased from Kanto Chemicals. Dibutyl phthalate, 2, 2′-azobis(2, 4 dimethylvaleronitril), and Ethylene dimethacrylate (EDMA) were obtained from WAKO Pure Chemicals.  Other reagents were laboratory-grade and used without any purification. 4-vinylpiridine was distilled to remove stabilizer prior to use.


## 2.2. Preparation of Molecularly Imprinted Polymer Receptor for BPA

Molecularly imprinted polymer for BPA was prepared according to the procedure reported previously in [13] and modified. 4-vinyl pyridine was used as a functional monomer to fabricate the recognition site for BPA by the hydrogen bonding and cross-liked by EDMA.  All the reagents were dissolved by toluene and polymerized at 60°C. The obtained polymer was crushed well into particles. The particles were thoroughly washed to remove template molecule by methanol and dried in vacuo. In the preparation of MIP, 1 g of MIP was obtained from 90 mg of BPA, 320 mg of 4-vinylpyridine, and 2.5 mL of EDMA. The dried polymer particles were filtrated and selected, size between 32 and 90 μm mesh. These particles were served as MIP receptor for BPA and 10 mg of them were packed in a glass column.  Absorbance of BPA to the MIP receptor was evaluated by the UV absorbance at 270 nm of the loaded and eluted solution of BPA.


## 2.3. Electrochemical Measurements

A three-electrode cell was used in the electrochemical measurements.  A gold electrode (I.D.=1.6mm) was used as a working electrode. A platinum wire counter and an Ag/AgCl reference electrode were used in the electrochemical experiments. Electrochemical measurements were carried out in a glass vial containing 1 mL of deoxygenated electrolyte solution at room temperature according to the previously reported procedure [15]. Cyclic voltammetry of BPA was measured at a range from 0 V to 0.8 V.   The response to BPA was obtained from the current difference, with and without BPA at around 0.6 V, which was the anodic peak current of BPA oxidation.


## 2.4. BPA Sensing System

BPA sensing system was equipped with an MIP packed column to electrochemical measurement system. An aliquot of sample solution containing BPA was loaded to the MIP column. The bound BPA was eluted by 60% (v/v) acetonitrile/0.1 M phosphate buffer (pH7.0).  The eluent was served to electrochemical measurement.


## 3. Results and Discussion

### 3.1. Selective Adsorption of BPA to MIP

Aqueous BPA solution (50μM) was loaded to the column and adsorption and elution of BPA were examined by UV spectroscopy. As shown in Figure 1, the loaded BPA was mostly adsorbed to the column, and in the eluent, bound BPA was removed completely.  In order to test the selectivity of the column, bisphenol F (BPF) and nonylphenol were examined. The chemical structures of BPA, BPF, and nonylphenol were shown in Figure 2. Fifty μM of these solutions were loaded to the MIP column and checked.  Table 1 shows the selectivity of the adsorption and elution.  More than 90% of adsorbed BPA was eluted; however, adsorption of BPF was smaller than BPA and elution of nonylphenol was less than half of BPA. Among them, recovery of BPA from the MIP packed column was the largest. It was favorable for the selective determination of BPA.Table 1
Selectivity of MIP packed column to bisphenol A.
Bisphenol ABisphenol FNonylphenolSample Conc. (μM)505050Adsorption efficiency1.00.801.0Elution efficiency0.920.740.43Figure 1
Absorbance of bisphenol A to MIP packed column, and elution from the column◯ loading solution of bisphenol A, ▴ passed through solution, ■ eluent.Figure 2
Chemical structures of bisphenol A, bisphenol F, and nonylphenol.


### 3.2. Electrochemical Determination of BPA

Experimental condition of electrochemical measurement of BPA was optimized first.  As the condition, pH of the electrolyte was examined at 4.0, 5.8, and 7.0. At higher pH than 7.0 electrochemical measurement of BPA was not examined because the hydroxyl group of BPA is reported to be partly dissociated to phenolate ion and oxidation of neutral BPA does not take place. Therefore neutral and acidic pH was examined. Anodic oxidation of BPA was observed as shown in Figure3, and anodic peak potentials of pH 4.0, 5.8, and 7.0 were 0.695, 0.604, and 0.520 mV, respectively. Peak potentials shifted to lower as to the higher pH. The peak current was the highest at pH 7.0.  Thus in this study, 0.1 M phosphate buffer, pH 7.0, was used. As for the mechanism of electrochemical oxidation of BPA, it was known as the generation of the phenoxy radical and quinone [15].Figure 3
Effect of pH to the anodic oxidation of bisphenol A. Cyclic voltammogram of 0.02 mM bisphenol A. scan rate 0.1 V/sec.Next, scan rate was examined (Figure4).  Below the scan rate of 0.1 V/sec, peak current showed the linear relationship to square root of scan rate.  On the other hand, linear relationship was not observed at the scan rate faster than 0.1 V/sec.  These phenomena suggest that at the faster scan rate, electrochemical reaction is not reversible and the side reaction occurs coincidently. In the detection of BPA, cyclic voltammetry was carried out at the scan rate of 0.1 V/sec or 0.05 V/sec to avoid side reaction.Figure 4
Effect of scan rate to the anodic oxidation of bisphenol A. Anodic peak potentials of 0.1 mM bisphenol A at pH 7.0 were plotted.Under the optimum condition, calibration of BPA was performed. In Figure5 anodic peak current was plotted against the concentration of BPA in 0.1 M phosphate buffer, pH 7.0, and 60% (v/v) acetonitrile in phosphate buffer (eluting solution). Linear relationship (y=8.8843x) was observed between 10 μM to 100 μM of BPA in phosphate buffer pH 7.0. In the eluting solution (60% of acetonitrile), linear relationship (y=6.836x+0.149) was observed at almost the same range of concentration, although the slope was slightly smaller than in phosphate buffer. In eluting solution, at lower concentration than 0.02 mM, larger peak current was observed than in phosphate buffer. Electrolyte in acetonitrile worked to help the electrochemical oxidation especially at lower concentration. Then the apparent intercept of the calibration line of BPA in acetonitrile was larger than in phosphate buffer.Figure 5
Calibration plot of bisphenol A. ■ in 0.1 M phosphate buffer, pH 7.0, ◯ in 60% (v/v) acetonitrile/0.1 M phosphate buffer, pH7.0. Scan rate 0.1 V/sec.


### 3.3. Determination of BPA in the Sensing System

As BPA was electrochemically measured in eluting solution, BPA was determined, using the system coupled with the MIP column. One ml of sample solution containing 50μM of BPA was loaded to the column and the path-thorough solution and eluent was electrochemically measured. As shown in Figure 6 distinguished peak to passed-through solution was not observed; however, in the eluent, anodic peak at around 0.6 V was clearly observed, and 10 μM of BPA was detected too.  Observed peak current almost agreed with that observed in 60% acetonitrile solution.  As for the selectivity in anodic response, nonylphenol showed a different response in cyclic voltammetry. BPA would be easily distinguished from other phenols except bisphenols.Figure 6
Response of bisphenol A with this sensing system.


## 3.1. Selective Adsorption of BPA to MIP

Aqueous BPA solution (50μM) was loaded to the column and adsorption and elution of BPA were examined by UV spectroscopy. As shown in Figure 1, the loaded BPA was mostly adsorbed to the column, and in the eluent, bound BPA was removed completely.  In order to test the selectivity of the column, bisphenol F (BPF) and nonylphenol were examined. The chemical structures of BPA, BPF, and nonylphenol were shown in Figure 2. Fifty μM of these solutions were loaded to the MIP column and checked.  Table 1 shows the selectivity of the adsorption and elution.  More than 90% of adsorbed BPA was eluted; however, adsorption of BPF was smaller than BPA and elution of nonylphenol was less than half of BPA. Among them, recovery of BPA from the MIP packed column was the largest. It was favorable for the selective determination of BPA.Table 1
Selectivity of MIP packed column to bisphenol A.
Bisphenol ABisphenol FNonylphenolSample Conc. (μM)505050Adsorption efficiency1.00.801.0Elution efficiency0.920.740.43Figure 1
Absorbance of bisphenol A to MIP packed column, and elution from the column◯ loading solution of bisphenol A, ▴ passed through solution, ■ eluent.Figure 2
Chemical structures of bisphenol A, bisphenol F, and nonylphenol.


## 3.2. Electrochemical Determination of BPA

Experimental condition of electrochemical measurement of BPA was optimized first.  As the condition, pH of the electrolyte was examined at 4.0, 5.8, and 7.0. At higher pH than 7.0 electrochemical measurement of BPA was not examined because the hydroxyl group of BPA is reported to be partly dissociated to phenolate ion and oxidation of neutral BPA does not take place. Therefore neutral and acidic pH was examined. Anodic oxidation of BPA was observed as shown in Figure3, and anodic peak potentials of pH 4.0, 5.8, and 7.0 were 0.695, 0.604, and 0.520 mV, respectively. Peak potentials shifted to lower as to the higher pH. The peak current was the highest at pH 7.0.  Thus in this study, 0.1 M phosphate buffer, pH 7.0, was used. As for the mechanism of electrochemical oxidation of BPA, it was known as the generation of the phenoxy radical and quinone [15].Figure 3
Effect of pH to the anodic oxidation of bisphenol A. Cyclic voltammogram of 0.02 mM bisphenol A. scan rate 0.1 V/sec.Next, scan rate was examined (Figure4).  Below the scan rate of 0.1 V/sec, peak current showed the linear relationship to square root of scan rate.  On the other hand, linear relationship was not observed at the scan rate faster than 0.1 V/sec.  These phenomena suggest that at the faster scan rate, electrochemical reaction is not reversible and the side reaction occurs coincidently. In the detection of BPA, cyclic voltammetry was carried out at the scan rate of 0.1 V/sec or 0.05 V/sec to avoid side reaction.Figure 4
Effect of scan rate to the anodic oxidation of bisphenol A. Anodic peak potentials of 0.1 mM bisphenol A at pH 7.0 were plotted.Under the optimum condition, calibration of BPA was performed. In Figure5 anodic peak current was plotted against the concentration of BPA in 0.1 M phosphate buffer, pH 7.0, and 60% (v/v) acetonitrile in phosphate buffer (eluting solution). Linear relationship (y=8.8843x) was observed between 10 μM to 100 μM of BPA in phosphate buffer pH 7.0. In the eluting solution (60% of acetonitrile), linear relationship (y=6.836x+0.149) was observed at almost the same range of concentration, although the slope was slightly smaller than in phosphate buffer. In eluting solution, at lower concentration than 0.02 mM, larger peak current was observed than in phosphate buffer. Electrolyte in acetonitrile worked to help the electrochemical oxidation especially at lower concentration. Then the apparent intercept of the calibration line of BPA in acetonitrile was larger than in phosphate buffer.Figure 5
Calibration plot of bisphenol A. ■ in 0.1 M phosphate buffer, pH 7.0, ◯ in 60% (v/v) acetonitrile/0.1 M phosphate buffer, pH7.0. Scan rate 0.1 V/sec.


## 3.3. Determination of BPA in the Sensing System

As BPA was electrochemically measured in eluting solution, BPA was determined, using the system coupled with the MIP column. One ml of sample solution containing 50μM of BPA was loaded to the column and the path-thorough solution and eluent was electrochemically measured. As shown in Figure 6 distinguished peak to passed-through solution was not observed; however, in the eluent, anodic peak at around 0.6 V was clearly observed, and 10 μM of BPA was detected too.  Observed peak current almost agreed with that observed in 60% acetonitrile solution.  As for the selectivity in anodic response, nonylphenol showed a different response in cyclic voltammetry. BPA would be easily distinguished from other phenols except bisphenols.Figure 6
Response of bisphenol A with this sensing system.


## 4. Conclusion

With the sensing system composed of the MIP packed column and an electrochemical analyzer, BPA was easily determined at the range of 10–100μM of BPA rapidly.  This system will be applied to the determination of food or biological fluid in the near future.



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*Source: 534936-2010-12-02.xml*