Single-step extraction and cleanup of bisphenol A in soft drinks by hemimicellar magnetic solid...
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Title: Single-step extraction and cleanup of bisphenol A insoft drinks by hemimicellar magnetic SPE prior to liquidchromatography/tandem mass spectrometry
Author: <ce:author id="aut0005"> Samaneh RaoufYazdinezhad<ce:author id="aut0010"> AnaBallesteros-Gomez<ce:author id="aut0015"> LoretoLunar<ce:author id="aut0020"> Soledad Rubio
PII: S0003-2670(13)00365-6DOI: http://dx.doi.org/doi:10.1016/j.aca.2013.03.025Reference: ACA 232454
To appear in: Analytica Chimica Acta
Received date: 16-1-2013Revised date: 6-3-2013Accepted date: 9-3-2013
Please cite this article as: S.R. Yazdinezhad, A. Ballesteros-Gomez, L. Lunarb, S.Rubio, Single-step extraction and cleanup of bisphenol A in soft drinks by hemimicellarmagnetic SPE prior to liquid chromatography/tandem mass spectrometry, AnalyticaChimica Acta (2013), http://dx.doi.org/10.1016/j.aca.2013.03.025
This is a PDF file of an unedited manuscript that has been accepted for publication.As a service to our customers we are providing this early version of the manuscript.The manuscript will undergo copyediting, typesetting, and review of the resulting proofbefore it is published in its final form. Please note that during the production processerrors may be discovered which could affect the content, and all legal disclaimers thatapply to the journal pertain.
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Title: Single-step extraction and cleanup of bisphenol A in soft drinks by hemimicellar magnetic 9
SPE prior to liquid chromatography/tandem mass spectrometry10
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Authors: Samaneh Raouf Yazdinezhada, Ana Ballesteros-Gómezb, Loreto Lunarb and Soledad 14
Rubiob*15
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Address: a Department of Chemistry, Faculty of Sciences, Ferdowsi University of Mashhad, 19
Mashhad, Iran 20b Department of Analytical Chemistry. Institute of Fine Chemistry and Nanochemistry. 21
Edificio Anexo Marie Curie Campus de Rabanales. University of Córdoba. Spain 22
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*corresponding author26
E-mail: [email protected] ; Phone: 34-957-218644; Fax: 34-957-21864427
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Abstract32
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Hemimicelles of tetradecanoate chemisorbed onto magnetic nanoparticles (MNPs) are here 34
proposed as a sorbent for the single-step extraction and cleanup of bisphenol A (BPA) in soft 35
drinks. The purpose of this work was to develop a simple, rapid and low-cost sample treatment 36
suitable to assess the human exposure to BPA from this type of high consumption food. The 37
nanoparticles were easily coated by mixing commercially available magnetite of 20-30 nm mean 38
particle diameter with tetradecanoate at 85 ºC for 30 min. The extraction/cleanup procedure 39
involved stirring the samples (3 mL) with 200 mg of tetradecanoate-coated MNPs for 20 min, 40
isolating the sorbent with a Nd-Fe-B magnet and eluting BPA with methanol. The extraction 41
efficiency was not influenced by salt concentrations up to 1 M and pH values over the range 4-9. 42
No cleanup of the extracts was needed, and the method proved matrix-independent. The extracts 43
were analyzed by liquid chromatography, electrospray ionization tandem mass spectrometry. 44
Quantitation was performed by internal standard calibration using BPA-13C12. The limit of 45
quantitation obtained for the method, 0.03 ng mL-1, was below the usual range of concentrations 46
reported for BPA in soft drinks (0.1-3.4 ng mL-1). The proposed method was successfully 47
applied to the determination of BPA in different samples acquired from various supermarkets in 48
southern Spain; the concentrations found ranged from 0.066 to 1.08 ng mL-1. Recoveries from 49
samples spiked with 0.33 ng mL-1 of BPA ranged from 91 to 105% with relative standard 50
deviations from 3 to 8%. 51
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Keywords: bisphenol A, soft drinks, magnetic SPE, chemisorbed hemimicelles, liquid 56
chromatography, tandem mass spectrometry57
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1. Introduction63
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Bisphenol A (BPA) is a high production volume chemical [1] widely used in the manufacture of 65
polycarbonate polymers and epoxy resins [2]. The food industry uses the former for food 66
packaging and plastic bottles, and the latter as internal protective lining for food and beverage 67
cans, coating on metal lids for glass jars and bottles and surface-coating on drinking water 68
storage tanks and wine vats [3]. Migration of BPA from plastics to food is mainly due to the 69
presence of non-polymerized residues or the hydrolysis of ester bonds, which is accelerated by 70
heat and contact with either acid or basic contents in cans [4]. 71
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Intake of BPA-contaminated foods constitutes the primary route of human exposure to this 73
chemical [5]. Concentrations reported for BPA range in the interval 0.1-3.4 ng mL-1 and 0.3-458 74
ng g-1 for drink and food, respectively [6]. Estimated intakes of BPA for adults, infants and 75
children are all well below the Tolerable Daily Intake (TDI) of 0.05 mg/kg body weight/day set 76
by the European Food Safety Authority (EFSA) for this substance in 2006. However, new 77
findings from ongoing studies on low dose effects observed in rodents [7-10] have urged EFSA 78
to launch a full re-evaluation on BPA, focusing on human exposure, how and how much is 79
absorbed by the human body and possible low dose effects [11]. Reassessment of human 80
exposure to BPA makes it necessary to take into account all the possible dietary sources and 81
consequently, to analyze a vast array of products and brands. In this context, it is recognized the 82
need for development of simple, high-throughput analytical methods for the determination of 83
BPA in high consumption, low BPA-content food such as drinks. 84
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Only a few methods sensitive and selective enough to give accurate data of BPA levels in soft 86
drinks and mineral water have been reported [reviewed in 6]. Sample preparation still constitutes 87
the key-step for the determination of BPA in drinks and it is the origin of the main drawbacks in 88
the available methodologies. Solvent extraction and solid phase extraction (SPE) are by far the 89
most used extraction techniques for both isolation of BPA and clean-up of matrix components. 90
Ethyl acetate [12], chloroform [13] and dichloromethane [14] have been used as solvents, the 91
overall consumption ranging from 60 mL [14] to 300 mL [12]. Oasis HLB has been proposed as 92
a sorbent for the SPE of BPA using sample sizes between 50 mL and 2 L [15]. In both cases, 93
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evaporation of the solvent for further treatment or BPA concentration is necessary, that rendering 94
the respective sample treatments laborious and time-consuming. On-line SPE [16,17] and a 95
number of microextraction techniques have been proposed as good alternatives for beverage96
analysis, namely, stir bar sorptive extraction (SBSE) [18], supramolecular solvent 97
microextraction [6], solid-phase microextraction (SPME) [19-21] and ultrasound-assisted 98
emulsification-microextraction (USAEME) [22]. The need for matrix matched calibration 99
[16,17] and long extraction times (e.g. 3 h for SBSE[18], 40 min for SPME [21]) are some 100
disadvantages of these methodologies.101
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Magnetic nanoparticles have attracted increasing attention in SPE owing to their unique 103
properties, namely high surface area, small diffusion resistance, easiness of surface modification 104
and easy and fast separation from sample solution by applying an external magnetic field. 105
Surface modification is essential to avoid nanoparticle aggregation and alteration of their 106
magnetic properties, as well as to improve sorbent capacity and selectivity for target analytes. 107
Reported coatings for MNPs include a variety of materials such as carbon, carbon nanotubes, 108
polymers, surfactants, biological active compounds, ionic liquids [23-32], etc. In this context, 109
molecularly imprinted polymer (MIP) coated-MNPs have been proposed for the selective 110
extraction of BPA from packed food [33] and different types of water [34]. 111
112
Among MNPs coatings, surfactant physisorption results in the formation of different surfactant 113
concentration-dependent types of aggregates (e.g. admicelles, hemimicelles and their mixtures) 114
that offer a variety of mechanisms for interaction with solutes. Although outstanding applications 115
have been reported using surfactant-coated MNPs [25,26,30,32], the easy disruption of the 116
physisorbed surfactant during analyte elution produces surfactant-rich extracts. This surfactant 117
can co-elute with the target compounds in LC, that causing interferences in UV, fluorescent and 118
MS detection or incompatibility with the analysis of the sample by gas chromatography or 119
capillary electrophoresis. These shortcomings have been recently overcome by coating MNPs 120
with chemisorbed surfactants [35,36].121
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In the present study, alkyl carboxylates chemisorbed onto MNPs [35] are proved to serve as a 123
simple-handling, efficient and low time-consuming method for extraction and cleanup of BPA. 124
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This sample treatment, combined with LC separation and electrospray ionization tandem mass 125
spectrometric detection, provides a sensitive and reliable method for the determination of BPA in 126
drinks. 127
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2. Experimental129
2.1. Chemical and apparatus130
All chemicals were of analytical reagent-grade and were used as supplied. Bisphenol A and iron 131
(II, III) oxide nanopowder with mean diameter of 20-30 nm were purchased from Aldrich (St. 132
Louis, MO, USA). Sodium n-tetradecanoate and n-octadecanoate were obtained from Sigma (St. 133
Louis, MO, USA). Sodium chloride, and LC grade methanol and acetonitrile were supplied by 134
Sigma-Aldrich (France), while sodium hydroxide was purchased from Merck (Darmstadt, 135
Germany). Bisphenol A (ring-13C12), used as internal standard (IS) was supplied by IS 136
Cambridge Isotope Laboratories (Andover, USA) as a solution of 100 mg L-1 in acetonitrile. BPA 137
and BPA-13C12 standard stock solutions (100 ng mL-1) were prepared in methanol and stored at 4 138
°C. Ultrahigh-quality water was obtained from a Milli-Q water purification system (Millipore, 139
Madrid, Spain).140
A PrecisTerm water bath from P Selecta (Barcelona, Spain) was used for synthesizing magnetic 141
nanoparticles. Glass vials (i.d. 25 mm) with metal caps were employed for extraction of samples 142
that were stirred in a multi-position vortex VorTemp 1550 from Labnet International (Edison, 143
NJ, USA). An Nd-Fe-B magnet (viz. a disk 2 cm in diameter and 1 cm thick from Farplas, S.L., 144
Barcelona, Spain) was used for isolation of MNPs after extraction. A high speed brushless 145
centrifuge MPW-350 R from MPW Med-Instruments (Warschow, Poland) was used for 146
separation of fruit pulps in samples containing lemon or orange extract. Some precautionary 147
measures were established to prevent BPA background contamination coming LC equipment 148
polymers, solvents or labware. Milli-Q water was filtered through styrene DVB (SDB-XC) disks 149
of 47 mm from Empore (3M, St Paul, Minnesota, USA) and glassware and eppendorf microtubes 150
were rinsed with methanol several times before their use. Contamination blanks were routinely 151
run with each batch of samples and were always below the quantification limit.152
153
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2.2. Synthesis of tetradecanoate-coated magnetic nanoparticles154
The tetradecanoate-coated MNPs (C14-MNPs) were synthesized according to our previous report 155
[35]. Briefly, 200 mg of MNPs were mixed with 50 mg of tetradecanoic acid sodium salt in 25 156
mL deionized Millipore water. The mixture was manually homogenized and placed in a water 157
bath at 85 ºC for 30 min. Following chemisorption, C14-MNPs were separated from the 158
equilibrium solution using a Nd-Fe-B magnet and washed three times with 4 mL of methanol to 159
remove physisorbed surfactant. The SPE material thus obtained was stored in a glass container at 160
4ºC until use. For synthesizing more amount of adsorbent, the reagents ratio can be increased at 161
will. The synthesis of octadecanoate-coated MNPs, also tested as a sorbent, was performed 162
similarly, but an amount of 62 mg of octadecanoic acid sodium salt was used instead.163
2.3. Determination of bisphenol A in soft drinks and drinking water164
2.3.1. Sample collection and preparation165
Nine beverages including different types of canned soft drinks were purchased from several166
supermarkets in Cordoba (Spain). They were stored unopened at room temperature until analysis. 167
Carbonated samples were degassed by sonication for 30 min. Samples containing orange or 168
lemon, were centrifuged for 15min at 15000 rpm to separate the fruit pulps. The pH of samples 169
ranged in the interval 2.5-3.5 and it was adjusted in the interval 4-9 with some drops of sodium 170
hydroxide (50%, w/v). 171
2.3.2. Magnetic solid phase extraction of BPA172
A volume of sample of 3 mL, at pH in the interval 4-9 and containing 1 ng of BPA-13C12 (10 µL 173
of the 100 ng mL-1 stock solution), and 200 mg of C14-MNPs were mixed in a glass vial and 174
vortex stirred for 20 min at 800 rpm. Then, the C14-MNPs were separated from the sample 175
solution by placing an Nd-Fe-B magnet in the bottom of the vial and pouring the solution away. 176
Next, the MNPs were washed with about 1 ml deionized water and the solution discarded. A177
mild nitrogen stream (~1bar for 2 min) was used for complete removal of the washing solution178
remaining on the MNPs. Finally, the analyte was eluted by vortex stirring (800 rpm) the dry179
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MNPs with 2 mL of methanol for 10 min. The magnet was again attached to the vial and a 180
desired portion of supernatant was transferred to LC vials for further analysis.181
2.3.3. Quantification of BPA by LC(ESI-) QQQ-MS2182
The separation and quantitation of BPA was accomplished by using a hybrid triple 183
quadrupole/linear ion trap (Applied Biosystems MSD Sciex 4000QTRAP, Foster City, CA, 184
USA) coupled to a liquid chromatograph (Agilent HP 1200 series, Palo Alto, CA, USA) with a 185
TurboIonSpray (TIS) interface. All data were acquired and processed using the Analyst 1.5.1 186
Software. A Symmetry Shield RP18 column (50 mm×2.1 mm ID, 3.5 µm, Waters, Ireland) was 187
used for LC separation. It was preceded by a C18 Guard Cartridge (Ascentis C18 Supelguard, 20 188
mm × 4 mm ID, 3 μm; Sigma-Aldrich). A Symmetry C18 Column (75 mm × 4.6 mm ID, 3.5 189
µm, Waters) was placed in the line of the mobile phase before the injection valve for retention of 190
the potential BPA leached from the plastic components of the LC system, so that it eluted later in 191
the chromatogram. The retention time for BPA from plastic components and the sample were 192
15.7 min and 12.6 min, respectively. The column oven was set at 40 ◦C, the flow rate was 400 193
µLmin−1, and the injection volume was 15 µL. The mobile phase consisted of methanol and 194
water. The gradient elution program used was 30% methanol during the first 2 min, ramp from 195
30% to 88.5% methanol over the next 13 min and then 100% methanol for 5 min. 196
Reconditioning the column took about 5 min. The eluates from the analytical column were 197
diverted to waste using the switching valve in the intervals 0-9 min and 14.50-25 min in order to 198
avoid the entrance of matrix components in the mass spectrometer. The mass spectrometer was 199
operated in ESI negative polarity and multiple-reaction monitoring (MRM) mode. Identification 200
and quantitation of BPA were performed by recording the transitions (m/z) 227→212 (quantifier 201
ion) and 227→133 (qualifier ion). BPA-13C12 used as an internal standard was monitored at (m/z) 202
239→224 and 239→139 transitions. The dwell time was set up at 150 ms. The TIS source values 203
were adjusted as follows: probe vertical y-axis position, 2 mm; probe horizontal y-axis position, 204
6 mm; curtain gas (N2), 50 psig; ion source gas 1 (nebulizer gas), 50 psig; ion source gas 2 (turbo 205
gas), 30 psig; temperature of the turbo gas, 650ºC; ion spray voltage: -4500 V; entrance 206
potential, -10 V; and declustering potential, -100 and -90 V for BPA and BPA-13C12, 207
respectively. Parameter values for the analyzer were as follows: 1.0 unit resolution for the first 208
and third quadrupoles; collision gas, 3.0x10-5 Torr; collision energy, -30, -36, -26 and -38 V; and 209
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collision cell exit potential, -15, -7, -11 and -15 V for the transitions 227→212, 227→133, 210
239→224 and 239→139, respectively. 211
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3. Results and discussion213
3.1. Optimization of the extraction of BPA with alkylcarboxylate-coated MNPs214
Hemimicellar magnetic SPE was selected as a convenient sorbent and format to efficiently 215
extract BPA and speed up sample treatment, respectively. Coating of MNPs with alkyl 216
carboxylates allowed the formation of stable hemimicellar aggregates, via the formation of 217
bidentate mononuclear complexes between carboxylate groups and iron atoms [37], that avoiding 218
their disruption during BPA elution and permitting the obtainment of surfactant free extracts. 219
Optimization of the magnetic SPE was accomplished by conducting triplicate tests that involved 220
extracting 2 mL of BPA (10 ng mL-1) aqueous standard solutions with coated MNPs under a 221
variety of experimental conditions. Because MS afforded instrumental quantitation limits low 222
enough to determine BPA in soft drinks without the need for preconcentration, the aim was to 223
develop an extraction/cleanup method efficient, simple and rapid, able to deal with a high 224
number of samples. Adsorption was investigated by measuring the remaining concentration of 225
BPA under equilibrium conditions. 226
Two alkyl carboxylates, namely tetradecanoate and octadecanoate, were assessed as coatings of 227
MNPs. After sorbent synthesis, magnetite was coated with both chemisorbed (~75%) and 228
physisorbed (~25%) surfactant. Removal of the latter was carried out by washing with methanol. 229
The maximum coverage of chemisorbed surfactant on MNPs was previously found to be ~0.35 230
mmol g-1, irrespective of the chain length of the surfactant [35]. It was calculated from the value 231
of the surface area of the magnetite (~60 m2 g−1) and the maximum amount of chemisorbed 232
surfactant obtained from the chemisorption isotherm. The chemisorbed surfactant was calculated 233
by measuring the remaining amount of surfactant in the equilibrium solution, after synthesis and 234
the subsequent washing steps, by LC-UV and subtracting it from the total amount of surfactant 235
used for synthesis. Maximal coverage required the use of at least 1 mmol of surfactant per gram 236
of magnetite in the synthetic procedure.237
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238
The coating of magnetite with single layers of alkyl carboxylates occurs via the formation of 239
bidentate mononuclear complexes between carboxylate groups and iron atoms. So dispersion 240
interactions between the aromatic rings of BPA and the alkyl chain of the surfactant were 241
expected to be the main forces driving extraction. Adsorption of BPA on both tetradecanoate-242
and octadecanoate-coated MNPs was similar at the different amounts of sorbents assayed. The 243
former was selected on the basis of its higher solubility in methanol which made easier the 244
removal of the physisorbed surfactant fraction. Figure 1A shows the dependence of the 245
percentage of adsorption of BPA on tetradecanoate- and octadecanoate-coated MNPs as a 246
function of the amount of sorbent. Percentages of adsorption above 90% with relative standard 247
deviations below 3% (n=3) were obtained from 200 mg of sorbent, this being the amount 248
recommended for further studies. 249
Adsorption of BPA exhibited no change with the concentration of NaCl in the range investigated 250
(0-1M), that making the method robust against changes in the ionic strength of the samples. The 251
pH, examined over the range 4-9, had no influence on the adsorption of BPA. More acid or 252
alkaline pHs were avoided to prevent MNPs from oxidation and BPA from ionization, 253
respectively. Regarding the extraction time, the extraction efficiency increased rapidly from 5 to 254
15 min (Figure 1B) and then reached a plateau. The precision raised as the extraction time did 255
(e.g. from RSD = 7.4% at 5 min to 0.09% at 60 min). Percentages of BPA adsorption above 90% 256
and RSDs below 3% were obtained at extraction times of 20 min and this value was selected as 257
optimal.258
Desorption of BPA from MNPs was investigated with MeOH and ACN using various elution 259
programs that involved solvent volumes from 1 to 3 mL, desorption times from 5 to 30 min and 260
1-3 elution steps. Complete removal of the water adsorbed onto the MNPs was required to avoid 261
a decrease in solvent desorption efficiency and changes in the final volume. Water was displaced 262
from MNPs by passing a nitrogen stream at ~1 bar for ~2 min while they were retained on the 263
magnet. 264
Extraction efficiencies for BPA were 81±4% and 74 ± 6.6% using 2 mL of MeOH and ACN, 265
respectively. The former was selected for further experiments, because of its slightly higher 266
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desorption ability and precision and the better chromatographic peak shape obtained. Extraction 267
efficiencies decreased by decreasing the volume of MeOH (e.g. 46.4±4.3% for 1 mL of solvent) 268
and they kept constant for higher volumes (e.g. 82.4 ±4.3% for 3mL of MeOH), so 2 ml were 269
selected as optimal. 270
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The number of steps used in the elution (e.g. 1x2 mL; 2x1mL; 3x0.7 mL) did not affect BPA 272
extraction efficiency but the precision decreased as the number of steps increased (e.g. 273
81.3±3.8%, 80.7±5.5% and 84.2±7.0% for 1, 2 and 3 steps, respectively). BPA desorption 274
reached equilibrium after vortex mixing the MNPs at 800 rpm for 10 min and that was the 275
selected elution time. 276
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Under the chosen experimental conditions (see section 2.3.2), extraction efficiencies kept 278
constant in the whole range of BPA amount tested (2.5-50 ng mL-1). Because of the low 279
concentration of BPA in drinks (0.1-3.4 ng mL-1) and its relatively high solubility in water (89 280
μg mL-1), the volume of sample was expected to greatly influence extraction efficiency. Figure 281
1C shows the results obtained as the volume of sample increased from 2 to 10 mL; extraction 282
efficiency progressively decreased from 3 mL of sample and it was about 56% at the maximal 283
sample volume tested. A volume of 3 mL was chosen as optimal for extraction and cleanup of 284
BPA. 285
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We assessed the possibility to concentrate the 2 mL of MeOH to 200 μL under evaporation under 287
a gentle stream of nitrogen. No losses were found to result from this drying operation and this 288
allowed the sensitivity to be increased 10-fold. However, the instrumental quantitation limit 289
afforded by MS (0.04 ng mL-1) is low enough to determine BPA in drinks without prior 290
preconcentration, so we propose dispensing with the evaporation step in order to make the 291
procedure simpler and faster for routine analysis. 292
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No leaching of tetradecanoate from the MNPs was observed under the recommended extraction 294
conditions, as checked by chromatographic analysis of the extracts. 295
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3.2. Analytical performance297
Internal standard calibration (n=16) was employed for quantification (BPA concentrations 298
calculated from the calibration curve obtained by plotting the ratio of analyte peak area to IS 299
peak area against the analyte concentration). The calibration equation was y=1.17x+0.0487 with 300
correlation coefficient (r) of 0.9993. Calibration standard solutions were performed in methanol 301
in the range 0.04-30 ng mL-1 of BPA, each solution containing 0.5 ng mL-1 of BPA-13C12. Linear 302
regression with a weighing 1/x was selected for quantification. The instrumental limits of 303
detection (LOD) and quantification (LOQ), calculated from blank determinations by using a 304
signal-to-noise ratio of 3 and 10 were 0.01 and 0.04 ng mL-1, respectively, for 15 µL injection 305
volumes. The method LOQ (estimated from the actual method concentration factor) was 0.03 ng 306
mL-1. Consequently, the proposed method affords the quantification of BPA at concentrations 307
below the usual range found for BPA in soft drinks (0.1-3.4 ng mL-1). Figure 2 shows the 308
chromatograms obtained, under optimal magnetic SPE conditions, for 3 mL of aqueous standard 309
solutions containing (A) 0.67 ng mL-1 of BPA and (B) 0.33 ng mL- 1 of BPA-13C12. Under these 310
conditions (section 2.3.2), extraction efficiencies for BPA and BPA-13C12 were similar and kept 311
constant at 81 ± 3 %.312
Because the instrumental sensitivity was high enough to quantify BPA in soft drinks without 313
preconcentration, the need for sample clean-up was investigated. For this purpose, the slope of 314
the calibration curve (n=10) obtained from fortified aqueous standard solutions was compared 315
with those obtained from fortified soft drinks. Concentrations of BPA were in the range 0.04-30 316
ng mL-1. The concentration of BPA-13C12 in all the solutions was 0.5 ng mL-1. Removal of 317
carbonic acid and/or separation of fruit pulps (section 2.3.1) were the only treatment applied to 318
the samples. The difference between the slopes was found to be statistically significant by 319
applying an appropriate Student´s test [38] for the three randomly selected soft drinks. The 320
calculated t-values for samples of lemon tea (4.90), orange carbonated drink (2.84) and energy 321
drink (2.18) were above the critical t-value (2.14) being significance established at the 0.05 level. 322
So, clean-up of samples will be necessary to get accurate results. Using clean-up with 323
hemimicellar MNPs, the difference between the slopes of calibration curves obtained from 324
fortified blank samples and the solvent were not significantly different. 325
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326
3.3. Analysis of soft drinks327
The suitability of the proposed method for use with real-world samples was established by 328
applying it to the determination of BPA in a variety of soft drinks belonging to different 329
trademarks. Table 1 shows the concentrations found as well as the recoveries obtained after 330
spiking the samples with 0.33 ng mL-1 of BPA. Both the concentration of analyte and recoveries 331
were expressed as the mean value of three independent determinations, besides their 332
corresponding standard deviations. Both blank and BPA-spiked samples were fortified with 0.33 333
ng mL-1 of BPA-13C12 before extraction. As can be seen, relative recoveries changed from 91 to 334
105% with relative standard deviations from 3 to 8%. BPA was present at quantifiable levels in 335
all the analyzed samples, the concentrations ranging from 0.066 to 1.08 ng mL-1, which is in 336
accordance with the values previously reported in the literature [6]. Figure 3 shows the 337
chromatograms obtained from a sport drink (A,B) and a lemon tea (C,D) before (A,C) and after 338
spiking with BPA at 0.33 ng mL- 1 of concentration level (B,D) and applying the proposed 339
hemimicellar magnetic SPE method. As can be seen, no interference from matrix components 340
was detected in the samples. 341
342
4. Conclusion343
A simple, rapid and inexpensive dispersive magnetic SPE has been developed for the extraction 344
and cleanup of BPA in soft drinks. Hemimicelles of tetradecanoate chemisorbed onto MNPs, 345
provide surfactant- and matrix components-free extracts for LC-MS BPA analysis. The 346
extraction procedure is independent of the pH and ionic strength in a wide range, as well as 347
matrix-independent, that making it robust. 348
349
Compared to sample treatments based on liquid-liquid extraction [12, 14, 41,42], the present 350
method is faster and much less solvent consumer (see Table 2). On the other hand, the use of 351
dispersive magnetic SPE simplifies the general procedure of conventional SPE, and as it is 352
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applied to BPA, it also prevents the contamination arising from the SPE plastic cartridges353
[15,16,39,45-48]. 354
355
The detection system used is essential to get detection limits low enough to quantify the usual 356
low BPA concentrations found in beverages (viz 0.1-3.4 ng mL-1, [6]). Thus, ultraviolet [45,47],357
fluorescence [46] or electrochemical [12] detection are not sensitive enough to cover the whole 358
range of BPA concentrations present in these matrices and the use of MS is mandatory for this 359
purpose (Table 2). Both LC/MS and GC/MS meet the requirements of sensitivity to quantify 360
BPA in beverages, the latter with the disadvantage of requiring derivatization. These techniques 361
feature similar LODs, and solvent evaporation [14] or a high sample size [15] will be always 362
required to achieve LODs below 1 ng L-1. 363
364
365
Acknowledgments366
The authors gratefully acknowledge financial support from Spanish MICINN (Project CTQ2011-367
23849) and from the Andalusian Government (Junta de Andalucía, Spain, Project P09-FQM-368
5151). FEDER also provided additional funding. S. Raouf Yazdinezhad thanks the Ministry of 369
Science, Research and Technology of the Islamic republic of Iran for its financial support for her 370
stay in the University of Córdoba. 371
References372
373
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[2] O.C. Dermer, in: J.J. McKelta, G.E.Weismantel (Eds.), Encyclopedia of Chemical Processing 375
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441
442
443
444
445
446
447
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Figure Captions448
449
Figure 1. (A,B) Dependence of the adsorption of BPA onto (1) tetradecanoate- and (2) 450
octadecanoate-coated MNPs on (A) the amount of sorbent and (B) the extraction time. (C) 451
Dependence of the extraction efficiency on the volume of sample. Error bars mean the standard 452
deviation of triplicate measurements.453
454
Figure 2. Chromatograms obtained from the analysis of 3 mL of deionized water spiked with 455
(A) 0.67 ng mL-1 of BPA and (B) 0.33 ng mL- 1 of BPA-13C12 after applying the proposed 456
hemimicellar magnetic SPE method457
458
Figure 3. Chromatograms obtained from the analysis of 3 mL of a sport drink (A,B) and a lemon 459
tea (C,D) before (A,C) and after spiking with 0.33 ng mL- 1 of BPA (B,D) and applying the 460
proposed hemimicellar magnetic SPE method.461
462
463
464
465
466
467
468
469
470
471
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A
0
20
40
60
80
100
0 20 40 60 80
BPA
ads
orpt
ion
(%)
Extraction time (min)
B
2030405060708090
0 5 10 15
BPA
reco
very
(%)
Sample volume (mL)
C
•
0
2040
60
80100
120
0 100 200 300 400
BPA
ads
orpt
ion
(%)
Alkyl carboxylic - coated MNPS (mg)
1
2
Figure 1472
473
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%
100
11.5 12.5 13.5 14.5
BPA
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
2.00e3
BPA-13C12
2.00e3A B
%
100
11.5 12.5 13.5 14.5
BPA
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
2.00e3
BPA-13C12
2.00e3A B
%
100
11.5 12.5 13.5 14.5
BPA
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
2.00e3
BPA-13C12
2.00e3A B
%
100
11.5 12.5 13.5 14.5
BPA
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
2.00e3
BPA-13C12
2.00e3A B
Figure 2473
474
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20
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
100
11.5 12.5 13.5 14.50
%
100
11.5 12.5 13.5 14.50
BPA1.05e3
BPA
1.05e3
A B
C
%
100
11.5 12.5 13.5 14.50
%
100
11.5 12.5 13.5 14.50
BPA1.05e3
BPA
1.05e3
D
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
100
11.5 12.5 13.5 14.50
%
100
11.5 12.5 13.5 14.50
BPA1.05e3
BPA
1.05e3
A B
C
%
100
11.5 12.5 13.5 14.50
%
100
11.5 12.5 13.5 14.50
BPA1.05e3
BPA
1.05e3
D
%
11.5 12.5 13.5 14.5
Time (min)
0
%
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
11.5 12.5 13.5 14.5
Time (min)
0
%
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.05e3
BPA
1.05e3
A B
C
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.05e3
BPA
1.05e3
D
%
11.5 12.5 13.5 14.5
Time (min)
0
%
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
11.5 12.5 13.5 14.5
Time (min)
0
%
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.49e3
BPA
1.49e3
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.05e3
BPA
1.05e3
A B
C
%
100
11.5 12.5 13.5 14.5
Time (min)
0
%
100
11.5 12.5 13.5 14.5
Time (min)
0
BPA1.05e3
BPA
1.05e3
D
474
Figure 3475
476
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476477
Table 1. Mean concentrations and recoveries, along with their respective standard deviations (SD), found 478for BPA in the analysis of soft drinks 479
480Canned soft drink Mean concentration±SDa
(ng mL-1)
Mean recoveryb±SDa
(%)
Cola drink 0.16 ± 0.02 98 ± 8Light Cola drink 0.066 ± 0.005 98 ± 5Sports drink, brand 1 0.36 ± 0.02 102 ± 5Sports drink, brand 2 1.08 ± 0.04 96 ± 8Lemon (6%) carbonated drink 0.09 ± 0.01 99 ± 3Orange (8%) carbonated drink 0.09 ± 0.01 91 ± 4Energy drink 0.16 ± 0.01 105 ± 3Non-alcoholic bitter drink 0.091 ± 0.003 96 ± 5Lemon tea 0.44 ± 0.02 105 ±6an=3, b Fortification level: 0.33 ng mL-1481
482
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Table 2. Comparison of the analytical features of current methodologies for the determination of BPA in beverages483
aMethod detection limit; bOverall solvent consumption per sample during the sample preparation steps484
485
Sample size(mL)
Sample treatment aMLD/ (ngL-1)
bOverall solvent consumption(mL)
Solvent evaporation
Recovery (%) Separation/Detection technique
Reference
50 Solvent extraction (acetonitrile)Derivatization
-- 40 Yes 81-103 GC/MS 42
50 Solvent extraction (acetonitrile)Derivatization
-- 40 Yes 42-112 GC/MS 41
10 Solvent extraction(dichloromethane)Two times aqueous back-extraction for clean upDerivatization
0.17 60 Yes 99.5-105.7 GC/MS 14
500 Solvent extraction(ethylacetate)
5700 300 Yes 63 LC/ED 12
10 Dispersive liquid-liquidmicroextraction (tetrachloroethylene/acetonitrile) Derivatization
10 -- No 68-114 GC/MS 44
10 SPE (nylon6 nanofibers membrane) 150 1.15 Yes 95 LC/UV 45
10 SPE ( 45 -- -- 99.9-101 GC/MS 39
50 SPE (Oasis HLB) 0.6 13 Yes 82.1-96.5 LC/MS/MS 15
1 On-line SPE (C18) 15-25 -- No 85-100 LC/MS 16
- SPE (C18) 1200 21 95.8 LC/F 46
200 SPE (bamboo-charcoal) 170 10 No 90.7 LC/UV 47
3 Magnetic SPE 7 2 No 91-105 LC/MS/MS Present method
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FeO4
FeO4
FeO 4
FeO 4
FeO4FeO4
FeO4FeO4
FeO4
FeO4
FeO4
FeO4
FeO 4
FeO 4
FeO4FeO4
FeO4FeO4
FeO4
FeO4
HEMIMICELLAR MAGNETIC SPE OF BPA
BPA
LC-MS/MS QUANTITATION
*Graphical Abstract
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Analytica Chimica ActaHighlights
●A single-step extraction and cleanup process is proposed for bisphenol A in soft drinks
●Hemimicelles of tetradecanoate adsorbed onto magnetic nanoparticles are used as a sorbent
●Magnetic SPE/LC-MS/MS provides a reliable method for evaluation of human BPA intake from drinks