Ion-Selective Electrode for Anionic Surfactants Using Hexadecyl Trimethyl Ammonium Bromide-Sodium Dodecylsulfate as an Active Ionophore

Wang, Junwei; Du, Zhiping; Wang, Wanxu; Xue, Wei

doi:https://doi.org/10.4061/2011/958647

International Journal of Electrochemistry

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Volume 2011 | Article ID 958647 | https://doi.org/10.4061/2011/958647

Ion-Selective Electrode for Anionic Surfactants Using Hexadecyl Trimethyl Ammonium Bromide-Sodium Dodecylsulfate as an Active Ionophore

Junwei Wang,¹Zhiping Du,¹Wanxu Wang,¹and Wei Xue¹

Academic Editor: Hassan Ali Zamani

Received09 May 2011

Revised02 Sept 2011

Accepted05 Sept 2011

Published22 Nov 2011

Abstract

The construction and characteristic performance of PVC membrane electrode responsive to sodium dodecylsulfate (SDS) are described in this paper. The electrode is based on hexadecyl trimethyl ammonium bromide-Sodium dodecylsulfate (CTA⁺DS⁻) ion pair as ionophore in PVC membrane, which displays a Nernstian slope of −58 ± 0.9 mV/decade in a 5.0 × 10⁻⁶ to 2.5 × 10⁻³ mol L⁻¹ concentration range and a limit of detection of 2.9 × 10⁻⁶ mol L⁻¹. The electrode can be used for 3 months without showing significant changes in the value of slope or working range. Also the electrode has wide pH range of application and short response time. The electrode shows a selective response to SDS and a poor response to common inorganic anions. The selective sequence found was SDS > HCO₃ ⁻ > CH₃COO⁻ > Cl⁻ > I⁻ > NO₃ ⁻≈ Br⁻ > F⁻ > CO₃ ²⁻ > C₆H₅O₇ ³⁻ > C₂O₄ ²⁻ > SO₄ ²⁻ > C₄H₄O₆ ²⁻ > SO₃ ²⁻ > PO₄ ³⁻. The potentiometric selectivity coefficients determined are indicating that common anions would not interfere in the SDS determination. The electrode has been utilized as an end point indicator electrode for potentiometric titration involving hyamine as titrant.

1. Introduction

Anionic surfactants are widely used in the industrial and domestic field, for example, in washing agents, household detergents, and personal care products. Traditional analysis methods of anionic surfactant concentration require tedious procedures (such as liquid and gas chromatography), or the use of large amounts of undesired solvents (such as chloroform in the spectrophotometric “Methylene Blue” method) [1–4]. An alternative to these methods is the use of electrodes (such as ion-selective electrodes [5–10] or ion-selective field-effect transistors [11–15]). Potentiometric methods using ion-selective electrodes have found wide applications in diverse fields of analysis for being of low cost, sensitive, and applicable over a wide range of experimental conditions [16].

Surfactant titrations are based on so-called antagonist reaction, where an ionic surfactant reacts with an oppositely charged ion forming a water insoluble salt (ion pair) [17–20]; when the oppositely charged ion surfactants react with each other at equal mol, the potential of the electrode has greatly changed; then the end point can be detected by the electrode.

The use of surfactant selective electrodes for the potentiometric determination of anionic surfactants concentration has been described in several papers. The surfactant selective electrode based on single-walled carbon nanotubes constructed by Najafi et al. [21] was used to determine the concentration of CTA⁺ and DS⁻. Juan Soto and coworkers [1, 22] constructed an ion-selective electrode for anionic surfactants using a new aza-oxa-cycloalkane and cyclam derivative as active ionophore in PVC membrane.

The present work investigates the feasibility of the preparation of stable, long life, high selectivity, and fast response anionic surfactant ion-selective electrode. The PVC membrane electrode is based on hexadecyl trimethyl ammonium bromide-sodium dodecylsulfate (CTA⁺DS⁻) ion pair as ionophore and di-n-octyl-phthalate (DOP) as plasticizer. The sensitivity and stability offered by this electrode configuration are high enough to allow accurate determination of low levels of anionic surfactant by direct potentiometry and potentiometric titration.

2. Experimental

2.1. Reagents

Sodium dodecylsulfate (SDS), hexadecyl trimethyl ammonium bromide (CTAB), hyamine and poly (vinyl chloride) of high molecular weight were from Aldrich (analytical grade). Di-n-octyl-phthalate (DOP) and tetrahydrofuran (THF) are both from Tianjin kermel Chemical Reagent Company. All other reagents used for the preparation of electrode were of analytical grade. Distilled water was used for the preparation of the solutions and for the cleaning of all glassware and apparatus in the experiments.

2.2. Apparatus

The potentiometric measurements were performed with a pH^s 3C pH/mV meter and a saturated calomel electrode (SCE) was used as external reference electrode. pH^s 3C pH/mV meter and saturated calomel electrode were purchased from Shanghai Precision and Scientific Instrument Co., Ltd. The indicating electrode was self-made anionic surfactant selective electrode. Potentiometric titrations were conducted with the help of an automatic burette and a titroprocessor (Beijing Xianquweifeng Technology Development Company) using a 25.0 ± 0.1°C water-thermostated vessel and an automatic burette.

2.3. Preparation of Electrode

The surfactant ion-selective electrode was made according to the classical method described in the literature [23] and the preparation could be formulated as follows.

2.3.1. Preparation of the Ion Pair

The ion pair CTA⁺DS⁻ was prepared by pouring together equimolar amounts of sodium dodecyl sulfate (SDS) and hexadecyl trimethyl ammonium bromide (CTAB) in hot aqueous solution. The ion pair CTA⁺DS⁻ is formed as a white precipitate, which was filtered off, washed with distilled water, and recrystallized twice from hot acetone.

2.3.2. Preparation of the Membrane

The best membranes, obtained with PVC : DOP 2 : 3, contained 10⁻³mol CTA⁺DS⁻ ion pair per kilogram of PVC and DOP mixture. PVC, DOP, and CTA⁺DS⁻ ion pair were dissolved in tetrahydrofuran, poured on a flat-bottomed glass dish. Tetrahydrofuran evaporated from the solution at room temperature for 48 h, and then the requisite membrane was obtained.

2.3.3. Construction of the Electrode

A disk of 1.0 cm in diameter was cut from the obtained membrane and attached to the end of a PVC tube using the solution of PVC dissolved in tetrahydrofuran (THF) as adhesive. The Ag/AgCl electrode was used as inner reference electrode. 1.0 × 10⁻³mol L⁻¹ SDS and 1.0 × 10⁻³mol L⁻¹ KCl mixture solution was used as inner solution. Respectively, to fabricate an electrode, the electrode was preconditioned in 10⁻³mol L⁻¹ SDS solution for 24 h.

2.4. Theory

A rapid and reliable potentiometric analysis method with surfactant ion-selective electrode has been developed for the determination of surfactants; surfactant concentration and potential comply with Nernstian equation written as where stands for the equilibrium electrode potential, is the standard electrode formal potential, is the gas constant, is the temperature, is the transfer electron number of electrode reaction, is the Faradays constant, and is the activity of the SDS solution. Therefore, the surfactant concentration can be acquired from the potentiometry measured using surfactant ion-selective electrode.

2.5. Emf Measurements and Titration Procedure

The external reference electrode was a saturated calomel electrode and self-made electrode was used for all EMF measurements. Potentiometric measurements were carried out by using the following cell assembly: external reference electrode, Saturated KCl solution, sample solution, PVC membrane, inner solution, and Ag/AgCl. All potential measurements were carried out on a pH^s 3C pH/mV meter. Potentiometric selectivity coefficients were determined according to the fixed interference method using 2.5 × 10⁻²mol L⁻¹ solution of interfering ion. Calibration curves were constructed by plotting the potential, , versus the logarithm of the sodium dodecyl sulfate (SDS) concentration.

The electrode has been calibrated with standard solutions of SDS in the range of 1.0 × 10⁻⁷ to 5.0 × 10⁻²mol L⁻¹. The volume of tested solution used for titration was 25.0 mL. The titrant dosage rate was 0.1 mL s⁻¹. The concentration of titrant hyamine was 4.043 × 10⁻³mol L⁻¹. All the measurements and titration were performed at 25.0 ± 0.1°C.

3. Results and Discussion

3.1. Influence of Membrane Composition

The ion pair CTA⁺DS⁻ was synthesized and tested as ionophore in PVC membrane. As it has been reported, the response of ion-selective electrodes in terms of selectivity and sensitivity depends not only on the ionophore but also on the final composition of the membrane ingredients. Therefore, in a first step several compositions of the membrane ingredients ionophore, plasticizer, and PVC were tested. All the membranes prepared were studied against SDS. The three electrodes (1–3) prepared with different membrane compositions were shown in Table 1. The membrane of electrodes 1, 2, and 3 had a similar composition, and the only difference was the content of ion pair. A comparison of the response characteristics of electrodes 1–3 against SDS is shown in Figure 1 and Table 1. It can be found that Electrode 2 with the composition (wt%) of DOP (60%), PVC (33%), and ion pair (2%) showed a better performance than electrodes 1 and 3. On one hand it had the lowest detection limit and the best linear correlation coefficient, on the other hand the slope value is the nearest to theory value 59.2 mV/decade. So we chose the composition as the ingredients of electrode membrane for the following studies.

3.2. Response Behavior of the Electrode

Electromotive force of the membrane electrode 2 assembly dipped in the solution of anionic surfactant SDS investigated was given by Nernstian equation. The response characteristics of anion surfactant selective electrode in solutions of sodium dodecylsulfate (SDS) were shown in Figure 1 (curve 2). Statistical evaluation of the electrode characteristics was given in Table 1 (membrane 2). The slope value and correlation coefficients were calculated from the linear region of the calibration graph of the measurements using linear regression analysis.

Detection limit is defined as the concentration of SDS corresponding to the intersection of the extrapolated linear segments of the calibration graph [24] which was 2.9 × 10⁻⁶mol L⁻¹. The electrode investigated showed Nernstian response (−58.0 ± 0.9 mV/decade) between 5.0 × 10⁻⁶ and 2.5 × 10⁻³mol L⁻¹ for SDS. It can be seen that the electrode exhibits linear response for SDS.

3.3. Response Time

The static response time of the electrode was measured after successive immersion of the electrode in a series of SDS solutions, from 1.0 × 10⁻⁵ to 1.0 × 10⁻³mol L⁻¹. The response time of electrode was evaluated by measuring the time required to achieve a steady-state potential [25, 26]. As shown in Figure 2, a response time of 40 s was found as the time required for the electrode to reach a potential within ±1 mV of the final equilibrium. The standard deviation of the response time calculated from four measurements was ±5 s; the response time of the electrode was 40 ± 5 s.

3.4. Effect of pH

The influence of pH on the potential response of the electrode was studied at a fixed concentration of SDS of 1 × 10⁻⁴mol L⁻¹ and 1 × 10⁻³mol L⁻¹ over the pH range of 2–12. CTA⁺DS⁻ ion pair mainly response to DS⁻. DS⁻ can combine with H⁺ at low pH, and then DSH formed. At low pH [H⁺] > [DS⁻], the concentration of DS⁻ was decreased in the solution which is probably related to the increasing of DSH concentration. The pH values higher than 10 also affected the potential response of electrode. Potential increases most likely due to a membrane response to the OH⁻ anion, that is because in such medium OH⁻ ions compete with DS⁻ ions. So out of the pH range 4 and 10, the potential was not the same as in the pH range 4–10. As illustrated in Figure 3, potentials remained constant between pH 4–10, which was chosen as the pH range for the studies [1].

3.5. Life Time of the Electrode

The electrode characteristics obtained at various time intervals were illustrated in Table 2 and Figure 4. The electrode exhibited good reproducibility in slope, linear concentration range, and detection limit for 13 weeks, but slight drifts in its slope and detection limit were observed after 14 weeks. The life time of the electrode was more than 3 months [1].

3.6. Determination of Potentiometric Selectivity Coefficients

We carried several studies with the electrode in relation to its response in the presence of SDS. As can be seen in Figure 5, the electrode displayed a remarkable selective response to SDS and a very poor change of the potential in the presence of the anions F⁻, Cl⁻, Br⁻, I⁻, NO₃ ⁻, SO₄ ²⁻, PO₄ ³⁻, SO₃ ²⁻, CO₃ ²⁻, HCO₃ ⁻, CH₃COO⁻, C₂O₄ ²⁻, C₄H₄O₆ ²⁻, and C₆H₅O₇ ³⁻. As it can be seen that the electrode displays negligible response to these anions when compared with that found for SDS.

In order to quantify the selective behavior found for the electrode towards SDS, we have carried out studies to determine potentiometric selectivity coefficients. Selectivity is one of the most important characteristics of electrodes that gives an idea of the preference of the electrode for the primary ion with respect to potentially interfering species and display the ability to distinguish this ion from a complex mixture. The potentiometric selectivity coefficients () of the electrode were calculated by means of the fixed interference method considering SDS as the principal anion and using concentration of 2.5 × 10⁻²mol L⁻¹ for interfering anions. was calculated with the following equation [27] where is the activity of the primary ion of , is the activity of the corresponding interfering ion, and and are the corresponding charge of the primary ion and the interfering ion, respectively. The calculated potentiometric selectivity coefficients were listed in Table 3. The selectivity sequence for the electrode was SDS > HCO₃ ⁻ > CH₃COO⁻ > Cl⁻ > I⁻ > NO₃ ⁻≈ Br⁻ > F⁻ > CO₃ ²⁻ > C₆H₅O₇ ³⁻ > C₂O₄ ²⁻ > SO₄ ²⁻ > C₄H₄O₆ ²⁻ > SO₃ ²⁻ > PO₄ ³⁻. As can be seen in Table 3, the logarithm of the potentiometric selectivity coefficients determined for the electrode are generally lower than −3.0 indicating that most of the anions would not significantly disturb the determination of SDS in real samples.

3.7. Analytical Applications

Our investigations showed that the electrode can not only be used for direct determination of SDS, but also was found useful as a sensor in titration of SDS with precipitating reagent (hyamine). As an example, it was applied in the titration of an SDS solution with hyamine. The amount of SDS in solution can be accurately determined by the electrode. In order to determine the concentration of SDS in model solutions, the electrode has been used for the determination of SDS in water by potentiometric titration in conjunction with SCE (saturated calomel electrode) as reference electrode and the results have been compared with those obtained using the reference standard technique the two-phase titration [28]. A typical sigmoid shape titration curve obtained from the titration of SDS was shown in Figure 6. The titration volume was estimated at the inflection point of the titration curve. As shown in Table 4, the results recorded by potentiometric titration are in good accordance with those given by the two-phase titration. Relative standard deviation of potentiometric titration and two-phase titration method for triplicate measurements are less than 1.6%.

For the determination of SDS in commercial detergents, 15–30 mg sample was dissolved in 2 mL methanol and diluted to 100 mL with water and 20 mL portion applied to the determination of SDS in samples by the electrode. The results of the potentiometric titration using the electrode were compared with those obtained using the two-phase titration. As shown in Table 5, the results recorded by the potentiometric titration are in good accordance with those given by two-phase titration.

4. Conclusion

Comparison with previously similar reported works was shown in Table 6. It can be found that the response slope to SDS of those electrodes was similar. The membrane containing new cyclic aza-oxa-cycloalkane as ionophore had the widest linear range and the lowest detection limit. The membrane containing CTA⁺DS⁻ ion pair as ionophore had the widest pH usage range and also had the lowest detection limit. An anionic surfactant selective electrode based on CTA⁺DS⁻ ion pair as an active ionophore provided advantages of easy preparation, simplicity, fast, and clean method of analysis of anion surfactant. This electrode displayed a Nernstian slope of −58.0 ± 0.9 mV/decade over the 5.0 × 10⁻⁶ to 2.5 × 10⁻³mol L⁻¹ concentration range and shows a limit of detection of 2.9 × 10⁻⁶mol L⁻¹. The electrode can be applied in a pH range of 4–10. Response time is 40 ± 5 s in average and can be used more than 3 months without showing significant changes in the value of slope. The electrode showed a clear anionic response to SDS. The selective sequence found for the electrode was SDS > HCO₃ ⁻ > CH₃COO⁻ > Cl⁻ > I⁻ > NO₃ ⁻≈ Br⁻ > F⁻ > CO₃ ²⁻ > C₆H₅O₇ ³⁻ > C₂O₄ ²⁻ > SO₄ ²⁻ > C₄H₄O₆ ²⁻ > SO₃ ²⁻ > PO₄ ³⁻. Furthermore, the potentiometric selectivity coefficients determined were relatively low, indicating that common anions would not interfere in the SDS determination. Also it can be used for the determination of SDS in water samples by titration procedures.

Acknowledgments

This work was supported by Natural Fund of Shanxi Province (2010011017), Natural Science Fund of China (21073234, 21103228), and Shanxi Province Science Fund for Youths (2011021010-2).

References

J. L. Lizondo-Sabater, R. M. Máñez, F. Sancenón, M. J. Seguí, and J. Soto, “Ion-selective electrodes for anionic surfactants using a cyclam derivative as ionophore,” Talanta, vol. 75, no. 1, pp. 317–325, 2008.
View at: Publisher Site | Google Scholar
A. Shaheen, I. Kaur, and R. K. Mahajan, “Potentiometric studies of micellization behavior of cationic surfactants in the presence of glycol additives and triblock polymer (Pluronic F68), using surfactant-selective sensors based on neutral ion-pair complexes,” Industrial & Engineering Chemistry Research, vol. 46, no. 13, pp. 4706–4709, 2007.
View at: Publisher Site | Google Scholar
K. Vytras, J. Kalous, and J. Jezkova, “Automated potentiometry as an ecologic alternative to two-phase titrations of surfactants,” Egypt Journal of Analytical Chemistry, vol. 6, no. 1, pp. 107–123, 1997.
View at: Google Scholar
C. Vogt and K. Heinig, “Trace analysis of surfactants using chromatographic and electrophoretic techniques,” Fresenius' Journal of Analytical Chemistry, vol. 363, no. 7, pp. 612–618, 1999.
View at: Google Scholar
Q. He and H. Chen, “Flow injection spectrophotometric determination of anionic surfactants using methyl orange as chromogenic reagent,” Fresenius' Journal of Analytical Chemistry, vol. 367, no. 3, pp. 270–274, 2000.
View at: Google Scholar
T. Fujinaga, S. Okazaki, and H. Freiser, “Ion selective electrodes responsive to anionic detergents,” Analytical Chemistry, vol. 46, no. 12, pp. 1842–1844, 1974.
View at: Google Scholar
M. Gerlache, Z. Sentürk, J. C. Viré, and J. M. Kauffmann, “Potentiometric analysis of ionic surfactants by a new type of ion-selective electrode,” Analytica Chimica Acta, vol. 349, no. 1–3, pp. 59–65, 1997.
View at: Publisher Site | Google Scholar
B. Kovács, B. Csóka, G. Nagy, and A. Ivaska, “All-solid-state surfactant sensing electrode using conductive polymer as internal electric contact,” Analytica Chimica Acta, vol. 437, no. 1, pp. 67–76, 2001.
View at: Publisher Site | Google Scholar
N. Alizadeh and H. K. Tazekendi, “Linear alkylbenzenesulfonate (LAS) ion-selective electrode based on electrochemically prepared polypyrrole and PVC,” Sensors and Actuators B, vol. 75, no. 1-2, pp. 5–10, 2001.
View at: Publisher Site | Google Scholar
J. Sànchez and M. Del Valle, “A new potentiometric photocurable membrane selective to anionic surfactants,” Electroanalysis, vol. 13, no. 6, pp. 471–476, 2001.
View at: Publisher Site | Google Scholar
R. K. Mahajan and A. Shaheen, “Effect of various additives on the performance of a newly developed PVC based potentiometric sensor for anionic surfactants,” Journal of Colloid and Interface Science, vol. 326, no. 1, pp. 191–195, 2008.
View at: Publisher Site | Google Scholar
L. Campanella, M. Battilotti, A. Borraccino, C. Colapicchioni, M. Tomassetti, and G. Visco, “A new ISFET device repsonsive to anionic detergents,” Sensors and Actuators B, vol. 19, no. 1–3, pp. 321–328, 1994.
View at: Google Scholar
J. Sànchez, A. Beltran, J. Alonso, C. Jiménez, and M. D. Valle, “Development of a new ion-selective field-effect transistor sensor for anionic surfactants: application to potentiometric titrations,” Analytica Chimica Acta, vol. 382, no. 1-2, pp. 157–164, 1999.
View at: Publisher Site | Google Scholar
J. Sànchez and M. D. Valle, “Photocurable ISFET for anionic surfactants. Monitoring of photodegradation processes,” Talanta, vol. 54, no. 5, pp. 893–902, 2001.
View at: Publisher Site | Google Scholar
W. H. Chan, A. W. M. Lee, and J. Z. Lu, “Optode for the specific determination of anionic surfactants,” Analytica Chimica Acta, vol. 361, no. 1-2, pp. 55–61, 1998.
View at: Publisher Site | Google Scholar
J. Sánchez and M. del Valle, “Determination of anionic surfactants employing potentiometric sensors—a review,” Critical Reviews in Analytical Chemistry, vol. 35, no. 1, pp. 15–29, 2005.
View at: Publisher Site | Google Scholar
M. M. Hassanien, K. S. Abou-El-Sherbini, and G. A. E. Mostafa, “A novel tetrachlorothallate (III)-PVC membrane sensor for the potentiometric determination of thallium (III),” Talanta, vol. 59, no. 2, pp. 383–392, 2003.
View at: Publisher Site | Google Scholar
R. W. Cattrall and H. Freiser, “Coated wire ion selective electrodes,” Analytical Chemistry, vol. 43, no. 13, pp. 1905–1906, 1971.
View at: Google Scholar
H. James, G. Carmack, and H. Freiser, “Coated wire ion selective electrodes,” Analytical Chemistry, vol. 44, no. 4, pp. 856–857, 1972.
View at: Google Scholar
T. Fujinaga, S. Okazaki, and H. Freiser, “Ion selective electrodes responsive to anionic detergents,” Analytical Chemistry, vol. 46, no. 12, pp. 1842–1844, 1974.
View at: Google Scholar
M. Najafia, L. Maleki, and A. A. Rafati, “Novel surfactant selective electrochemical sensors based on single walled carbon nanotubes,” Journal of Molecular Liquids, vol. 159, pp. 226–229, 2011.
View at: Google Scholar
M. J. Seguí, J. L. Sabater, R. M. Máñez, T. Pardo, F. Sancenón, and J. Soto, “Ion-selective electrodes for anionic surfactants using a new aza-oxa-cycloalkane as active ionophore,” Analytica Chimica Acta, vol. 525, no. 1, pp. 83–90, 2004.
View at: Publisher Site | Google Scholar
D. O. Hummel, Handbook of Surfactant Analysis, Wiley, New York, NY, USA, 1999.
G. A. E. Mostafa, “s-Benzylthiuronium PVC matrix membrane sensor for potentiometric determination of cationic surfactants in some pharmaceutical formulation,” Journal of Pharmaceutical and Biomedical Analysis, vol. 41, no. 4, pp. 1110–1115, 2006.
View at: Publisher Site | Google Scholar
R. P. Buck and E. Lindner, “Recommendation for nomenclature of ion-selective electrodes,” Pure and Applied Chemistry, vol. 66, no. 12, pp. 2527–2536, 1994.
View at: Google Scholar
C. Maccà, “Response time of ion-selective electrodes: current usage versus IUPAC recommendations,” Analytica Chimica Acta, vol. 512, no. 2, pp. 183–190, 2004.
View at: Publisher Site | Google Scholar
IUPAC, “Recommendations for nomenclature of ion-selective electrodes,” Pure and Applied Chemistry, vol. 48, no. 1, pp. 127–132, 1976.
View at: Google Scholar
APHA-AWWA-SPCF, “Standard methods for examination of water and waste-water,” in Proceedings of the 16th American Public Health Association, p. 512A, Washington, DC, USA, 1985.
View at: Google Scholar

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Copyright © 2011 Junwei Wang et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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