# Micelle-Mediated Extraction Prior to LC-UV for Preconcentration and Determination of Trace Amounts of Bisphenol A in Environmental Samples

Authors: Naghi Saadatjou; Shahab Shariati; Mostafa Golshekan
Journal: ISRN Analytical Chemistry
 (2013)

---

## Abstract

A simple and high sensitive preconcentration method based on micelle-mediated extraction followed by high performance liquid chromatography (LC-UV) was developed for preconcentration and determination of trace amounts of bisphenol A (BPA) in aqueous samples. The BPA was quantitatively extracted from aqueous samples in the presence of Triton X-114 as a nonionic surfactant and preconcentrated into the small volume (about 30μL) of the surfactant-rich phase. Taguchi method, an orthogonal array design (OA16 (45)), was utilized to optimize the various factors affecting the micellar extraction of BPA. The maximum extraction efficiency of BPA was obtained at pH 3, 0.2% (w/v) Triton X-114, and 0.25 mol L−1 sodium acetate. For the preconcentration, the solutions were incubated in a thermostatic water bath at 50°C for 7 min. After centrifuge and separation of aqueous phase, the surfactant-rich phase was diluted with 100 μL acetone and injected in the chromatographic system. Under the optimum conditions, preconcentration factor of  34.9 was achieved for extraction from 10 mL of sample solution and the relative standard deviation (RSD%) of the method was lower than 6.6%. The calibration curve was linear in the range of 0.5–150 μg L−1 with reasonable linearity (r2>0.9987). The limit of detection (LOD) based on S/N = 3 was 0.13 μg L−1 for 10 mL sample volumes. The limit of quantification (LOQ) based on S/N = 10 was 0.43 μg L−1 for 10 mL sample volumes. Finally, the applicability of the proposed method was evaluated by the extraction and determination of BPA in the real samples, and satisfactory results were obtained.


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## Body

## 1. Introduction

The distribution and abundance of plastic particles in the environment have rapidly increased, and the adverse effects of chemicals that leach from the plastic debris on aquatic animals have been of great concern [1, 2]. It is well known that 4,4-(1-methylethylidene) bisphenol or 2,2-(4,4-dihydroxydiphenyl) propane (commonly named bisphenol A; BPA) has estrogenic activity [3, 4]. BPA is a monomer widely used in the manufacture of epoxy and phenolic resins, as stabilizing material or antioxidant for numerous types of plastics including polyvinyl chloride [5, 6]. It is also used in polycarbonates, polyacrylates, and corrosion-resistant unsaturated polyester-styrene resins. BPA has been found to be widely distributed in the environment, because of highly production of plastics [7, 8]. BPA is leached from lacquer-coated cans [4], polycarbonate flasks during autoclaving, and baby feeding bottles [9] due to the hydrolysis of the polymer during thermal treatment [4, 10, 11]. Therefore, highly reliable methods are required for the detection of trace amounts of BPA. Some sample preparation techniques such as liquid-liquid extraction (LLE) [12], dispersive liquid-liquid microextraction (DLLME) [13], solid-phase extraction [14–16], and molecularly imprinted solid-phase extraction [17, 18] have been developed for the extraction of BPA from various matrices.Micelle-mediated extraction is a simple and powerful extraction method that is based on the property of most non-ionic surfactants in the aqueous solutions to form micelles and to separate into a surfactant-rich phase with a small volume. Any component present in the solution that interacts with the micellar aggregates can thus be extracted in the surfactant-rich phase. Small volume of the surfactant-rich phase and its compatibility with hydroorganic mobile phases allow the extraction and preconcentration of organic compounds prior to high-performance liquid chromatography (LC) [19] and capillary electrophoresis (CE) [20]. For LC, the viscosity of the surfactant-rich phase and its adsorption on the analytical columns can be resulted in the broad overlapping peaks when UV detection was employed. A lot of experimental studies were devoted to resolving this problem; one of them was decreasing the viscosity of the surfactant-rich phase by use of organic solvent before its introduction to LC. However, micelle-mediated extraction can easily be adapted for LC. It improves the detection limit and selectivity of determinations. In the present study, the applicability of the micellar extraction prior to LC-UV for the preconcentration and determination of trace amounts of BPA in aqueous samples was investigated using orthogonal array experimental design.


## 2. Experimental

### 2.1. Reagents and Materials

All chemicals used were of analytical reagent grade and were prepared from Merck (Darmstadt, Germany) and Fluka companies (Chemie AG, Switzerland). LC-grade solvents (water, methanol, and acetonitrile) were used throughout the experiments and were obtained from Merck. All solutions were prepared with doubly distilled water. A stock standard solution of BPA at a concentration of 1000 mg L−1 was prepared in methanol. This standard solution was diluted with distilled water to prepare stock solutions with the concentration of 5, 10, and 50 mg L−1 of BPA. The non-ionic surfactant, Triton X-114 from Fluka, was used without further purification. Nitric acid (1.0 mol L−1) and sodium hydroxide (1.0 mol L−1) were used to adjust the pH of solutions.


### 2.2. Apparatus

Chromatographic separations were carried out on a Knauer LC equipped with a K-1001 LC pump (Germany) and a K-2600 UV-Vis detector. Separations were carried out on a Zorbax Extend C18 column (250 mm × 4.6 mm i.d., 5 μm particle diameter). A mixture of deionized water and acetonitrile (55 : 45) at a constant flow rate of 1.0 mL min−1 was used as the mobile phase in isocratic mode. The injection volume was 20 μL for all the solutions, and the detection was performed at the wavelength of 224 nm. A model 3305 digital Jenway pH meter equipped with a combined glass-calomel electrode was used for the pH adjustments. A centrifuge (Model H-108 N, Kokusan, Democrartic People’s Republic of Korea) was applied to accelerate the separation of surfactant-rich phase from aqueous solution.


### 2.3. Extraction Procedure

For the cloud point extraction, aliquots of the solution containing BPA (10 mL) were adjusted to the appropriate ionic strength and pH (sodium acetate: 0.25 mol L−1, pH 3.0). Triton X-114 at 0.2% (w/v) concentration was added to solutions and the solutions were kept at 50°C (the temperature above the cloud point temperature of the system) for 7 min in the thermostatic water bath to become cloudy. Since Triton X-114 is denser than water, the surfactant-rich phase typically settled through the aqueous phase. In order to accelerate the phase separation, the turbid solutions were centrifuged for 8 min at 3000 rpm. After that, the tubes were cooled in an ice bath for 5 min to reach a denser surfactant-rich phase that could facilitate the separation of aqueous phase by means of pipette. After the separation of aqueous phase, 100 μL of pure acetone was added to the surfactant-rich phase to decrease the viscosity of surfactant-rich phase for further measurement by LC-UV.


## 2.1. Reagents and Materials

All chemicals used were of analytical reagent grade and were prepared from Merck (Darmstadt, Germany) and Fluka companies (Chemie AG, Switzerland). LC-grade solvents (water, methanol, and acetonitrile) were used throughout the experiments and were obtained from Merck. All solutions were prepared with doubly distilled water. A stock standard solution of BPA at a concentration of 1000 mg L−1 was prepared in methanol. This standard solution was diluted with distilled water to prepare stock solutions with the concentration of 5, 10, and 50 mg L−1 of BPA. The non-ionic surfactant, Triton X-114 from Fluka, was used without further purification. Nitric acid (1.0 mol L−1) and sodium hydroxide (1.0 mol L−1) were used to adjust the pH of solutions.


## 2.2. Apparatus

Chromatographic separations were carried out on a Knauer LC equipped with a K-1001 LC pump (Germany) and a K-2600 UV-Vis detector. Separations were carried out on a Zorbax Extend C18 column (250 mm × 4.6 mm i.d., 5 μm particle diameter). A mixture of deionized water and acetonitrile (55 : 45) at a constant flow rate of 1.0 mL min−1 was used as the mobile phase in isocratic mode. The injection volume was 20 μL for all the solutions, and the detection was performed at the wavelength of 224 nm. A model 3305 digital Jenway pH meter equipped with a combined glass-calomel electrode was used for the pH adjustments. A centrifuge (Model H-108 N, Kokusan, Democrartic People’s Republic of Korea) was applied to accelerate the separation of surfactant-rich phase from aqueous solution.


## 2.3. Extraction Procedure

For the cloud point extraction, aliquots of the solution containing BPA (10 mL) were adjusted to the appropriate ionic strength and pH (sodium acetate: 0.25 mol L−1, pH 3.0). Triton X-114 at 0.2% (w/v) concentration was added to solutions and the solutions were kept at 50°C (the temperature above the cloud point temperature of the system) for 7 min in the thermostatic water bath to become cloudy. Since Triton X-114 is denser than water, the surfactant-rich phase typically settled through the aqueous phase. In order to accelerate the phase separation, the turbid solutions were centrifuged for 8 min at 3000 rpm. After that, the tubes were cooled in an ice bath for 5 min to reach a denser surfactant-rich phase that could facilitate the separation of aqueous phase by means of pipette. After the separation of aqueous phase, 100 μL of pure acetone was added to the surfactant-rich phase to decrease the viscosity of surfactant-rich phase for further measurement by LC-UV.


## 3. Results and Discussion

### 3.1. Method Development

In the proposed procedure, to achieve maximum extraction efficiency, various parameters affecting the extraction of BPA were studied using the Taguchi orthogonal array design (OAD). Taguchi method is a type of fractional factorial design in which orthogonal array is used to assign the selected factors to a serial of experimental combinations [21]. The results of the orthogonal array design experiments can be treated by the analysis of variance (ANOVA) and/or the direct observation analysis. In ANOVA, the effects of different factors on the response function can be evaluated by computing F-ratio (variances ratio) and percent contribution (PC) values for each factor [22, 23]. All optimization experiments were done at 100 μg L−1 of BPA, and Falcon tubes with 15 mL volumes were used for optimization.


### 3.2. Experimental Design and Data Analysis

In this study, the effect of five experimental factors including solution pH and temperature, surfactant concentration, ionic strength, and organic solvent volume (acetone) on the micelle-mediated extraction of BPA was studied using Taguchi’s OA16 design. The used levels (four levels) of the main factors (A-E) and the OA16 (45) matrix employed to assign the considered factors are shown in Tables 1 and 2, respectively.Table 1
Factors and levels for Taguchi orthogonal array design of proposed method (A–E are the respective codes for each factor).
Levels
Factors
A (pH)
B (surfactant (%))
C (ionic strength (mol L−1))
D (temperature (°C))
E (organic solvent volume (µL))
1
3
0.05
0.01
30
50
2
4
0.1
0.1
40
75
3
5
0.2
0.25
50
100
4
6
0.3
0.5
60
125Table 2
OA16 (45) experimental design for the optimization of CPE of BPA.
Trial no.
pH
% Surfactant
Ionic strength (mol L−1)
Temperature (°C)
Organic solvent volume (µL)
1
6
0.3
0.01
50
75
2
5
0.1
0.5
50
50
3
4
0.05
0.1
50
125
4
3
0.3
0.5
60
125
5
3
0.1
0.1
40
75
6
5
0.3
0.1
30
100
7
3
0.2
0.25
50
100
8
5
0.05
0.25
60
75
9
4
0.2
0.5
30
75
10
5
0.2
0.01
40
125
11
6
0.1
0.25
30
125
12
3
0.05
0.01
30
50
13
4
0.3
0.25
40
50
14
6
0.05
0.5
40
100
15
6
0.2
0.1
60
50
16
4
0.1
0.01
60
100The designing of the table was done via experimental design 7.0 software. For increasing the precision of the optimization process, each trial was repeated twice (n=32). The sequence, in which the experiments were carried out, was randomized to avoid any personal or subjective bias. ANOVA was used to assess the OAD results. For ANOVA calculations, peak area of BPA in the chromatogram was used and the results of the sums of squares (SS) for different variables were calculated.The mean values of the four levels of each factor revealed how the extraction efficiency changes with variation of the level of each factor. Figure1 shows the mean absorbance as a function of the levels of the studied factors.Figure 1
The response graph illustrating the variation of the mean area peak values plotted against various extraction parameters. pH (level 1 = 3.0, level 2 = 4.0, level 3 = 5.0, level 4 = 6.0). Surfactant (%) (level 1 = 0.05, level 2 = 0.1, level 3 = 0.2, level 4 = 0.3). Ionic strength (mol L−1) (level 1 = 0.01, level 2 = 0.1, level 3 = 0.25, level 4 = 0.5). Temperature (°C) (level 1 = 30, level 2 = 40, level 3 = 50, level 4=60). Acetone volume (μL) (level 1 = 50, level 2 = 75, level 3 = 100, level 4 = 125).The ANOVA results (Table3) showed that the most important factor contributing to the extraction efficiency was acetone volume (44.21%). The results also showed that pH had low effect on the extraction.Table 3
ANOVA results for experimental responses in the OA16 (45) matrix.
Factor
DOFa
Sum of squares
Variance
F-ratiob
Pure sum of squares
% PCc
pH (A)
3
1.1107
×
10
12
2.7768
×
10
11
0.21
9.283
×
10
11
5.99
% surfactant (B)
3
2.70846
×
10
12
6.77115
×
10
11
0.514
2.526
×
10
12
16.3
Ionic strength (C)
3
1.80809
×
10
12
4.52022
×
10
11
0.343
1.626
×
10
12
10.49
Temperature (D)
3
1.86311
×
10
12
4.65777
×
10
11
0.353
1.681
×
10
12
10.85
Organic solvent volume (µL)
3
7.03123
×
10
12
1.75781
×
10
11
1.333
6.849
×
10
12
44.21
Error
16
0.729
×
10
11
6.08062
×
10
10
12.16
Total
31
1.54945
×
10
13
100
aDegrees of freedom. bF, critical value is 3.24 (P<0.05).  cPercent of contribution.


### 3.3. Study of Micelle-Mediated Extraction

#### 3.3.1. Influence of pH

BPA withpKa value in the range of 9.6–10.2 should mainly exist as a neutral compound at pHs below 9.0 and it can be extracted to hydrophobic core of micellar aggregates. At pHs higher than 10, BPA exists as an ionic form that has extremely water solubility. Hence, the extraction of BPA was performed at acidic pH. To investigate the effect of pH on the extraction of BPA, pH of the samples was adjusted in the range of 3.0–6.0 using the sodium acetate (0.25 mol L−1) with addition of NaOH (1.0 mol L−1) or HNO3 (1.0 mol L−1), according to the experimental design (Figure 1). The results showed that the maximum extraction efficiency of BPA was obtained at pH 3.


#### 3.3.2. Influence of Triton X-114 Concentration

In CPE, the theoretical preconcentration factors depend on the volume of the surfactant-rich phase, which at the same time varies with the surfactant concentration in the solution [29]. In the present study, Triton X-114 as a non-ionic surfactant was chosen for its low cloud-point temperature, low toxicological properties, and high density [30, 31]. The effect of the surfactant concentration on the extraction efficiency was studied in the range of 0.05–0.3% (w/v). According to Figure 1, at 0.2% (w/v) of Triton X-114, more extraction was occurred. At lower concentrations of the surfactant, the extraction efficiency was low probably due to inadequacy of the assemblies to entrap the BPA quantitatively. At higher concentrations, the signal’s intensity decreased probably due to increase in the viscosity and the volume of the surfactant phase. To obtain maximum preconcentration factor, 0.2% (w/v) of Triton X-114 was selected for further experiments.


#### 3.3.3. Influence of Ionic Strength

The addition of salt to solution can influence the phase separation process. To study the influence of the ionic strength on the extraction performance, the concentration of sodium acetate was changed in the range of 0.01–0.5 mol L−1. The results showed that the addition of the sodium acetate facilitates the phase separation since it increases the density of the aqueous phase [32]. With the increase of the salt concentration, the micellar size and the aggregation number are increased [33]. According to Figure 1, the extraction at 0.25 mol L−1 sodium acetate gives the best results. At very high concentrations of sodium acetate the surfactant-rich phase was located on the surface of the solution, which makes it more difficult to separate the extraction solvent.


#### 3.3.4. Influence of Equilibrium Temperature

It was desirable to employ the lowest possible equilibration temperature, which compromises completion of the reaction and efficient separation of the phases.For Triton X-114, an increase in the cloud point temperature leads to a slight decrease in the volume of the surfactant-rich phase. This can be interpreted in terms of the fact that as temperature increases, hydrogen bonds are disrupted and dehydration occurs. Thus, by increasing of temperature, the amount of water in the surfactant-rich phase and consequently the volume of the surfactant-rich phase decrease [34]. The greatest preconcentration can be obtained when the extraction is conducted at the temperatures well above the cloud point temperature of the surfactant. According to Figure 1, the optimum equilibration temperature was found to be 50°C.


#### 3.3.5. Influence of Organic Solvent Volume

After extraction and separation of the surfactant-rich phase from aqueous phase, it is necessary to decrease its viscosity before injection to LC. Acetone, acetonitrile, and methanol were studied as an organic solvents. In order to investigate the effect of solvent type on extraction performance a series of extracted samples of BPA (100μg L−1) were prepared and 50 μL of each solvent was added into the surfactant-rich phase. Acetone has the best chromatographic results in comparison with other solvent. After selection of acetone as organic solvent, the effect of its volume on the peak area of BPA was investigated in the range of 50–125 μL. According to Figure 1, 100 μL of acetone showed the best results. The viscosity of surfactant-rich phase decreased by increasing of the acetone volume. At higher acetone volumes (above 100 μL), the preconcentration factor decreased because of increase in the volume of extractant.


### 3.4. Evaluation of Method Performance

The quantitative parameters of the proposed method were calculated under the optimized conditions (pH 3, 0.2% (w/v) surfactant, 0.25 mol L−1 ionic strength, temperature 50°C, and 100 μL acetone). The calibration curve was obtained by preconcentration of BPA in 10 mL of spiked standard solutions under the optimum conditions. The calibration line exhibited a good linearity over the concentration range of 0.5–150 μg L−1 with correlation coefficient better than 0.9987. The limit of detection (LOD), calculated as the concentration equivalent to three times of the blank standard deviation (for ten replicates) divided into the slope of calibration curve, was 0.13 μg L−1. The limit of quantification (LOQ) based on S/N=10 was 0.43 μg L−1 for 10 mL sample volumes. The preconcentration factor was calculated as the ratio of concentration of analyte in the surfactant-rich phase to its initial concentration in aqueous solution (100 μg L−1). The preconcentration factor was 34.9 for 10 mL sample. The relative standard deviation (RSD%) resulted from four replicate extractions of BPA from 10 mL solution (100 μg L−1) was lower than 6.6%.A comparison between the figures of merit of the proposed method and some of the recently published methods for extraction and determination of BPA is summarized in Table4.Table 4
Comparison of the characteristic data between recently published extraction methods and the developed method.
Methods
LOD (µg L−1)
LRa (µg L−1)
RSD (%)
SVb (mL)
Reference
LPMEc-GC-MS
5.0
1–1000
15
10
[24]
SBSEd-GC-MS
0.5
2–100
<10
2
[25]
SPMEe-LC
3.25
10–500
4.4
10
[26]
ELISAf
0.3
0.3–100
—
10
[27]
ELISA
0.1
1–10000
—
10
[28]
DLLMEg-LC
0.07
0.5–100
6
10
[13]
CPE-LC
0.13
0.5–150
6.6
10
Proposed method
aLinear range. bSample volume. cLiquid phase microextraction. dStir bar sorptive extraction. eSolid phase microextraction. fEnzyme-linked immunosorbent assay. gDispersive liquid-liquid microextraction.The extraction method applied in the present work has some advantages in comparison with the other extraction methods including low consumption of organic solvents and reagents, ease of operation, simplicity, minimum carry over, and cross-contamination as well as producing a clean extracting phase for the analysis.


### 3.5. Analysis of Real Samples

The applicability of the proposed method to real samples was studied by analyzing the lagoon water collected from Bojagh lagoon (Kiashahr, Gilan, Iran) and the leachate (BPA) from the solution of the baby feeding bottle and transfusion distilled water (preservation in plastic bottle). The leachate of baby feeding bottle was collected from the containers filled with 150 mL of boiling water. A 150 mL of boiling water (100°C) was transferred into a commercially available baby feeding bottle, which was tightly capped and kept in an oven at 95°C for 30 min and cooled to room temperature. Another leachate sample from baby feeding bottle was tested without thermal processing. Figure2 shows the chromatograms obtained for the leachate samples from baby feeding bottle kept in 95°C and without thermal processing.LC chromatograms of BPA leached BPA from baby feeding bottle (a) nonspiked and without being kept in oven, (b) spiked (10μg L−1) and without being kept in oven, (c) nonspiked and kept in oven (at 95°C for 30 min), and (d) spiked (10 μg L−1) and kept in oven.
(a)
(b)
(c)
(d)Results (Table5) showed that BPA leached from baby feeding bottle after thermal processing in oven was more than ones without any thermal processing.Table 5
Analytical results for determination of BPA in real ware samples.
Sample
Concentration (mean,n=3) (µg mL−1)
BPA added
BPA found
Recovery (%)
S1
0.0
1.16
±
0.22
103
10.0
11.53
±
0.66
S2
0.0
1.99
±
0.27
98
10.0
11.84
±
0.35
S3
0.0
4.50
±
0.65
97
10.0
14.14
±
0.71
S4
0.0
2.39
±
0.27
97
10.0
12.05
±
0.3
S1: transfusion distilled water (preservation in plastic bottle).
S2: leachate from baby feeding bottle.
S3: leachate from baby feeding bottle kept in oven (95°C-30 min).
S4: lagoon water collected from Bojagh lagoon (Gilan, Iran).


## 3.1. Method Development

In the proposed procedure, to achieve maximum extraction efficiency, various parameters affecting the extraction of BPA were studied using the Taguchi orthogonal array design (OAD). Taguchi method is a type of fractional factorial design in which orthogonal array is used to assign the selected factors to a serial of experimental combinations [21]. The results of the orthogonal array design experiments can be treated by the analysis of variance (ANOVA) and/or the direct observation analysis. In ANOVA, the effects of different factors on the response function can be evaluated by computing F-ratio (variances ratio) and percent contribution (PC) values for each factor [22, 23]. All optimization experiments were done at 100 μg L−1 of BPA, and Falcon tubes with 15 mL volumes were used for optimization.


## 3.2. Experimental Design and Data Analysis

In this study, the effect of five experimental factors including solution pH and temperature, surfactant concentration, ionic strength, and organic solvent volume (acetone) on the micelle-mediated extraction of BPA was studied using Taguchi’s OA16 design. The used levels (four levels) of the main factors (A-E) and the OA16 (45) matrix employed to assign the considered factors are shown in Tables 1 and 2, respectively.Table 1
Factors and levels for Taguchi orthogonal array design of proposed method (A–E are the respective codes for each factor).
Levels
Factors
A (pH)
B (surfactant (%))
C (ionic strength (mol L−1))
D (temperature (°C))
E (organic solvent volume (µL))
1
3
0.05
0.01
30
50
2
4
0.1
0.1
40
75
3
5
0.2
0.25
50
100
4
6
0.3
0.5
60
125Table 2
OA16 (45) experimental design for the optimization of CPE of BPA.
Trial no.
pH
% Surfactant
Ionic strength (mol L−1)
Temperature (°C)
Organic solvent volume (µL)
1
6
0.3
0.01
50
75
2
5
0.1
0.5
50
50
3
4
0.05
0.1
50
125
4
3
0.3
0.5
60
125
5
3
0.1
0.1
40
75
6
5
0.3
0.1
30
100
7
3
0.2
0.25
50
100
8
5
0.05
0.25
60
75
9
4
0.2
0.5
30
75
10
5
0.2
0.01
40
125
11
6
0.1
0.25
30
125
12
3
0.05
0.01
30
50
13
4
0.3
0.25
40
50
14
6
0.05
0.5
40
100
15
6
0.2
0.1
60
50
16
4
0.1
0.01
60
100The designing of the table was done via experimental design 7.0 software. For increasing the precision of the optimization process, each trial was repeated twice (n=32). The sequence, in which the experiments were carried out, was randomized to avoid any personal or subjective bias. ANOVA was used to assess the OAD results. For ANOVA calculations, peak area of BPA in the chromatogram was used and the results of the sums of squares (SS) for different variables were calculated.The mean values of the four levels of each factor revealed how the extraction efficiency changes with variation of the level of each factor. Figure1 shows the mean absorbance as a function of the levels of the studied factors.Figure 1
The response graph illustrating the variation of the mean area peak values plotted against various extraction parameters. pH (level 1 = 3.0, level 2 = 4.0, level 3 = 5.0, level 4 = 6.0). Surfactant (%) (level 1 = 0.05, level 2 = 0.1, level 3 = 0.2, level 4 = 0.3). Ionic strength (mol L−1) (level 1 = 0.01, level 2 = 0.1, level 3 = 0.25, level 4 = 0.5). Temperature (°C) (level 1 = 30, level 2 = 40, level 3 = 50, level 4=60). Acetone volume (μL) (level 1 = 50, level 2 = 75, level 3 = 100, level 4 = 125).The ANOVA results (Table3) showed that the most important factor contributing to the extraction efficiency was acetone volume (44.21%). The results also showed that pH had low effect on the extraction.Table 3
ANOVA results for experimental responses in the OA16 (45) matrix.
Factor
DOFa
Sum of squares
Variance
F-ratiob
Pure sum of squares
% PCc
pH (A)
3
1.1107
×
10
12
2.7768
×
10
11
0.21
9.283
×
10
11
5.99
% surfactant (B)
3
2.70846
×
10
12
6.77115
×
10
11
0.514
2.526
×
10
12
16.3
Ionic strength (C)
3
1.80809
×
10
12
4.52022
×
10
11
0.343
1.626
×
10
12
10.49
Temperature (D)
3
1.86311
×
10
12
4.65777
×
10
11
0.353
1.681
×
10
12
10.85
Organic solvent volume (µL)
3
7.03123
×
10
12
1.75781
×
10
11
1.333
6.849
×
10
12
44.21
Error
16
0.729
×
10
11
6.08062
×
10
10
12.16
Total
31
1.54945
×
10
13
100
aDegrees of freedom. bF, critical value is 3.24 (P<0.05).  cPercent of contribution.


## 3.3. Study of Micelle-Mediated Extraction

### 3.3.1. Influence of pH

BPA withpKa value in the range of 9.6–10.2 should mainly exist as a neutral compound at pHs below 9.0 and it can be extracted to hydrophobic core of micellar aggregates. At pHs higher than 10, BPA exists as an ionic form that has extremely water solubility. Hence, the extraction of BPA was performed at acidic pH. To investigate the effect of pH on the extraction of BPA, pH of the samples was adjusted in the range of 3.0–6.0 using the sodium acetate (0.25 mol L−1) with addition of NaOH (1.0 mol L−1) or HNO3 (1.0 mol L−1), according to the experimental design (Figure 1). The results showed that the maximum extraction efficiency of BPA was obtained at pH 3.


### 3.3.2. Influence of Triton X-114 Concentration

In CPE, the theoretical preconcentration factors depend on the volume of the surfactant-rich phase, which at the same time varies with the surfactant concentration in the solution [29]. In the present study, Triton X-114 as a non-ionic surfactant was chosen for its low cloud-point temperature, low toxicological properties, and high density [30, 31]. The effect of the surfactant concentration on the extraction efficiency was studied in the range of 0.05–0.3% (w/v). According to Figure 1, at 0.2% (w/v) of Triton X-114, more extraction was occurred. At lower concentrations of the surfactant, the extraction efficiency was low probably due to inadequacy of the assemblies to entrap the BPA quantitatively. At higher concentrations, the signal’s intensity decreased probably due to increase in the viscosity and the volume of the surfactant phase. To obtain maximum preconcentration factor, 0.2% (w/v) of Triton X-114 was selected for further experiments.


### 3.3.3. Influence of Ionic Strength

The addition of salt to solution can influence the phase separation process. To study the influence of the ionic strength on the extraction performance, the concentration of sodium acetate was changed in the range of 0.01–0.5 mol L−1. The results showed that the addition of the sodium acetate facilitates the phase separation since it increases the density of the aqueous phase [32]. With the increase of the salt concentration, the micellar size and the aggregation number are increased [33]. According to Figure 1, the extraction at 0.25 mol L−1 sodium acetate gives the best results. At very high concentrations of sodium acetate the surfactant-rich phase was located on the surface of the solution, which makes it more difficult to separate the extraction solvent.


### 3.3.4. Influence of Equilibrium Temperature

It was desirable to employ the lowest possible equilibration temperature, which compromises completion of the reaction and efficient separation of the phases.For Triton X-114, an increase in the cloud point temperature leads to a slight decrease in the volume of the surfactant-rich phase. This can be interpreted in terms of the fact that as temperature increases, hydrogen bonds are disrupted and dehydration occurs. Thus, by increasing of temperature, the amount of water in the surfactant-rich phase and consequently the volume of the surfactant-rich phase decrease [34]. The greatest preconcentration can be obtained when the extraction is conducted at the temperatures well above the cloud point temperature of the surfactant. According to Figure 1, the optimum equilibration temperature was found to be 50°C.


### 3.3.5. Influence of Organic Solvent Volume

After extraction and separation of the surfactant-rich phase from aqueous phase, it is necessary to decrease its viscosity before injection to LC. Acetone, acetonitrile, and methanol were studied as an organic solvents. In order to investigate the effect of solvent type on extraction performance a series of extracted samples of BPA (100μg L−1) were prepared and 50 μL of each solvent was added into the surfactant-rich phase. Acetone has the best chromatographic results in comparison with other solvent. After selection of acetone as organic solvent, the effect of its volume on the peak area of BPA was investigated in the range of 50–125 μL. According to Figure 1, 100 μL of acetone showed the best results. The viscosity of surfactant-rich phase decreased by increasing of the acetone volume. At higher acetone volumes (above 100 μL), the preconcentration factor decreased because of increase in the volume of extractant.


## 3.3.1. Influence of pH

BPA withpKa value in the range of 9.6–10.2 should mainly exist as a neutral compound at pHs below 9.0 and it can be extracted to hydrophobic core of micellar aggregates. At pHs higher than 10, BPA exists as an ionic form that has extremely water solubility. Hence, the extraction of BPA was performed at acidic pH. To investigate the effect of pH on the extraction of BPA, pH of the samples was adjusted in the range of 3.0–6.0 using the sodium acetate (0.25 mol L−1) with addition of NaOH (1.0 mol L−1) or HNO3 (1.0 mol L−1), according to the experimental design (Figure 1). The results showed that the maximum extraction efficiency of BPA was obtained at pH 3.


## 3.3.2. Influence of Triton X-114 Concentration

In CPE, the theoretical preconcentration factors depend on the volume of the surfactant-rich phase, which at the same time varies with the surfactant concentration in the solution [29]. In the present study, Triton X-114 as a non-ionic surfactant was chosen for its low cloud-point temperature, low toxicological properties, and high density [30, 31]. The effect of the surfactant concentration on the extraction efficiency was studied in the range of 0.05–0.3% (w/v). According to Figure 1, at 0.2% (w/v) of Triton X-114, more extraction was occurred. At lower concentrations of the surfactant, the extraction efficiency was low probably due to inadequacy of the assemblies to entrap the BPA quantitatively. At higher concentrations, the signal’s intensity decreased probably due to increase in the viscosity and the volume of the surfactant phase. To obtain maximum preconcentration factor, 0.2% (w/v) of Triton X-114 was selected for further experiments.


## 3.3.3. Influence of Ionic Strength

The addition of salt to solution can influence the phase separation process. To study the influence of the ionic strength on the extraction performance, the concentration of sodium acetate was changed in the range of 0.01–0.5 mol L−1. The results showed that the addition of the sodium acetate facilitates the phase separation since it increases the density of the aqueous phase [32]. With the increase of the salt concentration, the micellar size and the aggregation number are increased [33]. According to Figure 1, the extraction at 0.25 mol L−1 sodium acetate gives the best results. At very high concentrations of sodium acetate the surfactant-rich phase was located on the surface of the solution, which makes it more difficult to separate the extraction solvent.


## 3.3.4. Influence of Equilibrium Temperature

It was desirable to employ the lowest possible equilibration temperature, which compromises completion of the reaction and efficient separation of the phases.For Triton X-114, an increase in the cloud point temperature leads to a slight decrease in the volume of the surfactant-rich phase. This can be interpreted in terms of the fact that as temperature increases, hydrogen bonds are disrupted and dehydration occurs. Thus, by increasing of temperature, the amount of water in the surfactant-rich phase and consequently the volume of the surfactant-rich phase decrease [34]. The greatest preconcentration can be obtained when the extraction is conducted at the temperatures well above the cloud point temperature of the surfactant. According to Figure 1, the optimum equilibration temperature was found to be 50°C.


## 3.3.5. Influence of Organic Solvent Volume

After extraction and separation of the surfactant-rich phase from aqueous phase, it is necessary to decrease its viscosity before injection to LC. Acetone, acetonitrile, and methanol were studied as an organic solvents. In order to investigate the effect of solvent type on extraction performance a series of extracted samples of BPA (100μg L−1) were prepared and 50 μL of each solvent was added into the surfactant-rich phase. Acetone has the best chromatographic results in comparison with other solvent. After selection of acetone as organic solvent, the effect of its volume on the peak area of BPA was investigated in the range of 50–125 μL. According to Figure 1, 100 μL of acetone showed the best results. The viscosity of surfactant-rich phase decreased by increasing of the acetone volume. At higher acetone volumes (above 100 μL), the preconcentration factor decreased because of increase in the volume of extractant.


## 3.4. Evaluation of Method Performance

The quantitative parameters of the proposed method were calculated under the optimized conditions (pH 3, 0.2% (w/v) surfactant, 0.25 mol L−1 ionic strength, temperature 50°C, and 100 μL acetone). The calibration curve was obtained by preconcentration of BPA in 10 mL of spiked standard solutions under the optimum conditions. The calibration line exhibited a good linearity over the concentration range of 0.5–150 μg L−1 with correlation coefficient better than 0.9987. The limit of detection (LOD), calculated as the concentration equivalent to three times of the blank standard deviation (for ten replicates) divided into the slope of calibration curve, was 0.13 μg L−1. The limit of quantification (LOQ) based on S/N=10 was 0.43 μg L−1 for 10 mL sample volumes. The preconcentration factor was calculated as the ratio of concentration of analyte in the surfactant-rich phase to its initial concentration in aqueous solution (100 μg L−1). The preconcentration factor was 34.9 for 10 mL sample. The relative standard deviation (RSD%) resulted from four replicate extractions of BPA from 10 mL solution (100 μg L−1) was lower than 6.6%.A comparison between the figures of merit of the proposed method and some of the recently published methods for extraction and determination of BPA is summarized in Table4.Table 4
Comparison of the characteristic data between recently published extraction methods and the developed method.
Methods
LOD (µg L−1)
LRa (µg L−1)
RSD (%)
SVb (mL)
Reference
LPMEc-GC-MS
5.0
1–1000
15
10
[24]
SBSEd-GC-MS
0.5
2–100
<10
2
[25]
SPMEe-LC
3.25
10–500
4.4
10
[26]
ELISAf
0.3
0.3–100
—
10
[27]
ELISA
0.1
1–10000
—
10
[28]
DLLMEg-LC
0.07
0.5–100
6
10
[13]
CPE-LC
0.13
0.5–150
6.6
10
Proposed method
aLinear range. bSample volume. cLiquid phase microextraction. dStir bar sorptive extraction. eSolid phase microextraction. fEnzyme-linked immunosorbent assay. gDispersive liquid-liquid microextraction.The extraction method applied in the present work has some advantages in comparison with the other extraction methods including low consumption of organic solvents and reagents, ease of operation, simplicity, minimum carry over, and cross-contamination as well as producing a clean extracting phase for the analysis.


## 3.5. Analysis of Real Samples

The applicability of the proposed method to real samples was studied by analyzing the lagoon water collected from Bojagh lagoon (Kiashahr, Gilan, Iran) and the leachate (BPA) from the solution of the baby feeding bottle and transfusion distilled water (preservation in plastic bottle). The leachate of baby feeding bottle was collected from the containers filled with 150 mL of boiling water. A 150 mL of boiling water (100°C) was transferred into a commercially available baby feeding bottle, which was tightly capped and kept in an oven at 95°C for 30 min and cooled to room temperature. Another leachate sample from baby feeding bottle was tested without thermal processing. Figure2 shows the chromatograms obtained for the leachate samples from baby feeding bottle kept in 95°C and without thermal processing.LC chromatograms of BPA leached BPA from baby feeding bottle (a) nonspiked and without being kept in oven, (b) spiked (10μg L−1) and without being kept in oven, (c) nonspiked and kept in oven (at 95°C for 30 min), and (d) spiked (10 μg L−1) and kept in oven.
(a)
(b)
(c)
(d)Results (Table5) showed that BPA leached from baby feeding bottle after thermal processing in oven was more than ones without any thermal processing.Table 5
Analytical results for determination of BPA in real ware samples.
Sample
Concentration (mean,n=3) (µg mL−1)
BPA added
BPA found
Recovery (%)
S1
0.0
1.16
±
0.22
103
10.0
11.53
±
0.66
S2
0.0
1.99
±
0.27
98
10.0
11.84
±
0.35
S3
0.0
4.50
±
0.65
97
10.0
14.14
±
0.71
S4
0.0
2.39
±
0.27
97
10.0
12.05
±
0.3
S1: transfusion distilled water (preservation in plastic bottle).
S2: leachate from baby feeding bottle.
S3: leachate from baby feeding bottle kept in oven (95°C-30 min).
S4: lagoon water collected from Bojagh lagoon (Gilan, Iran).


## 4. Conclusion

The use of micellar systems as an alternative to other methods of separation and preconcentration offers several advantages including experimental convenience, safety and being an inexpensive method. Also, in this method, the consumption of organic solvent is low. In the present study, the results of ANOVA showed that the pH has low significant effect on the extraction efficiency. The proposed method gives low limit of detection as well as good RSD and linearity that results detection of low concentration of BPA in samples.



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*Source: 357807-2013-05-21.xml*