Potentiometric Surfactant Sensor Based on 1,3-Dihexadecyl-1H-benzo[d]imidazol-3-ium for Anionic Surfactants in Detergents and Household Care Products

A 1,3-dihexadecyl-1H-benzo[d]imidazol-3-ium-tetraphenylborate (DHBI-TPB) ion-pair implemented in DHBI-TPB surfactant sensor was used for the potentiometric quantification of anionic surfactants in detergents and commercial household care products. The DHBI-TPB ion-pair was characterized by FTIR spectroscopy and computational analysis which revealed a crucial contribution of the C–H∙∙∙π contacts for the optimal complex formation. The DHBI-TPB sensor potentiometric response showed excellent analytical properties and Nernstian slope for SDS (60.1 mV/decade) with LOD 3.2 × 10−7 M; and DBS (58.4 mV/decade) with LOD 6.1 × 10−7 M was obtained. The sensor possesses exceptional resistance to different organic and inorganic interferences in broad pH (2–10) range. DMIC used as a titrant demonstrated superior analytical performances for potentiometric titrations of SDS, compared to other tested cationic surfactants (DMIC > CTAB > CPC > Hyamine 1622). The combination of DHBI-TPB sensor and DMIC was successfully employed to perform titrations of the highly soluble alkane sulfonate homologues. Nonionic surfactants (increased concentration and number of EO groups) had a negative impact on anionic surfactant titration curves and a signal change. The DHBI-TPB sensor was effectively employed for the determination of technical grade anionic surfactants presenting the recoveries from 99.5 to 101.3%. The sensor was applied on twelve powered samples as well as liquid-gel and handwashing home care detergents containing anionic surfactants. The obtained results showed good agreement compared to the outcomes measured by ISE surfactant sensor and a two-phase titration method. The developed DHBI-TPB surfactant sensor could be used for quality control in industry and has great potential in environmental monitoring.


Introduction
Tensides or surfactants are surface active agents. There are four main types of surfactants: anionic, cationic, nonionic and amphoteric. They are used for washing, cleaning and were also performed. Finally, newly developed DHBI-TPB electrode was employed for the quantification of anionic surfactants in detergents and household care products.

Computational Analysis
Computational analysis was performed to provide an insight into the dynamics and behavior of the DHBI + cation in the aqueous solution, and to identify intermolecular interactions responsible for its complex formation with TPB − , particularly focused on characterizing the DHBI-TPB complex through electronic, geometric and energetic features.
Despite having a rigid benzimidazole skeleton, DHBI + is a very flexible molecule, attributed to its two unconstrained lipophilic C-16 chains, whose flexibility over the anionic TPB − counterpart is clearly evident in the calculated RMSD display ( Figure S2). As the following discussion will show, it is precisely this feature of DHBI + that we identified as crucial for its efficient recognition of TPB − . DHBI-TPB complexation is a favorable event, yet the adduct formation and its dissociation into components exchange over the simulation time. As an illustration, the relevant B(TPB)···N(DHBI) distances stretch well beyond 40 Å, while assuming values below 7 Å in around 22% of the obtained structures ( Figure S3). Still, the MM-PBSA binding free energy between DHBI + and TPB − is exergonic at ∆G BIND = −5.0 kcal mol −1 , thus confirming the feasibility of the process. To put this number in a proper context and given the highly favorable analytical features of the DHBI-TPB sensor, the calculated value appears optimal as it needs to assure the stability of the ion-pair, but also the reversibility of the salt formation and the potential exchange with other anionic analytes for sensing purposes. The representative structure of the complex (Figure 1) reveals two types of favorable interactions, namely (i) the π-π stacking contacts between benzimidazole in DHBI + and one of the phenyl rings in TPB − , and (ii) a range of C-H···π interactions that both C-16 chains are forming with other phenyl rings in TPB − . Moreover, the corresponding B(TPB − )···N(DHBI + ) distances assume 4.8 and 5.1 Å, being in good agreement with the relevant overall RDF graph that predicts the largest number of these interactions occurring at 5.4 Å ( Figure S4), thus confirming the validity of the presented structure as representative.
mances were also performed. Finally, newly developed DHBI-TPB electrode w ployed for the quantification of anionic surfactants in detergents and househo products.

Computational Analysis
Computational analysis was performed to provide an insight into the dynam behavior of the DHBI + cation in the aqueous solution, and to identify intermolec teractions responsible for its complex formation with TPB -, particularly focused acterizing the DHBI-TPB complex through electronic, geometric and energetic fea Despite having a rigid benzimidazole skeleton, DHBI + is a very flexible m attributed to its two unconstrained lipophilic C-16 chains, whose flexibility over onic TPBcounterpart is clearly evident in the calculated RMSD display (Figure the following discussion will show, it is precisely this feature of DHBI + that we id as crucial for its efficient recognition of TPB -. DHBI-TPB complexation is a favorable event, yet the adduct formation and i ciation into components exchange over the simulation time. As an illustration, the B(TPB)•••N(DHBI) distances stretch well beyond 40 Å, while assuming values be in around 22% of the obtained structures ( Figure S3). Still, the MM-PBSA bind energy between DHBI + and TPBis exergonic at ΔGBIND = −5.0 kcal mol -1 , thus con the feasibility of the process. To put this number in a proper context and given th favorable analytical features of the DHBI-TPB sensor, the calculated value appea mal as it needs to assure the stability of the ion-pair, but also the reversibility of formation and the potential exchange with other anionic analytes for sensing pu The representative structure of the complex ( Figure 1) reveals two types of favor teractions, namely (i) the π-π stacking contacts between benzimidazole in DHBI + of the phenyl rings in TPB -, and (ii) a range of C-H•••π interactions that both C-1 are forming with other phenyl rings in TPB -. Moreover, the corresponding )•••N(DHBI + ) distances assume 4.8 and 5.1 Å, being in good agreement with the overall RDF graph that predicts the largest number of these interactions occurrin Å ( Figure S4), thus confirming the validity of the presented structure as represen  Given the opposing charges on both constituents, one could assume that electrostatic charge-charge attraction is governing the binding. Yet, this does not appear to be the case following from the atomic charge analysis ( Figure S5). It turns out that, prior to binding, the benzimidazole unit within DHBI + accumulates only a third of the excess positive charge (0.33 |e|), while the rest is deposited within the C-16 chains-a situation which is not changed even in the formed complex. In fact, upon the DHBI-TPB adduct formation, only 2% of the charge is transferred among components, as the total atomic charges on DHBI + and TPB − are +1.02 and −0.98 |e|, which clearly excludes electrostatic charge-charge attraction as predominant for the complex stability. Along these lines, by analyzing structures during simulations and extracting those where the centers of mass among benzimidazole in DHBI + and either of the phenyls in TPB − are found below 4 Å, it was revealed that only in 6.3% of structures did there occur notable π-π stacking contacts, which renders this type of interaction as moderately important as well.
In contrast, what appears to be crucial for the DHBI-TPB complex formation are C-H···π interactions between both C-16 chains in DHBI + and phenyls in TPB − (Figure 1). To confirm that, we have repeated MD simulations with two modified DHBI + systems, in which, firstly, one C-16 chain is replaced by the methyl group, and, secondly, both C-16 chains are substituted by methyls. In those cases, the matching binding free energy was reduced by 0.7 kcal mol −1 to ∆G BIND = −4.3 kcal mol −1 , for the system with one C-16 chain, and further, by as much as 3.3 kcal mol −1 down to ∆G BIND = −1.0 kcal mol −1 , for the system without C-16 chains. The latter strongly underlines the crucial importance of the lipophilic chains for the design of useful analytical devices through allowing the formation of efficient ion-pair sensors.

Sensor Response to Anionic Surfactants
A Nernst Equation (1) describes the sensor potential response (E) on anionic surfactants concentration (a A − ): where E= electromotive force of the system E o = constant potential term S= sensor slope a A − = anionic surfactant sensor activity Response characteristics of a DHBI-TPB surfactant sensor were observed against the SDS and DBS anionic surfactants in deionized water and 0.01 M Na 2 SO 4 solution. The Na 2 SO 4 solutions were used to observe the response in high ionic strength solution. Detailed data on the response characteristics and statistics are presented in Table 1. Notably, the high ionic strength did not lead to the strong effect on the surfactant sensor characteristics, as the slope values, in mV per decade of activity, are near-Nernstian for SDS (60.1 ± 0.5 and 59.7 ± 0.4 mV/decade) and DBS (58.4 ± 0.6 and 58.7 ± 0.5 mV/decade), both in water and Na 2 SO 4 solution. The correlation coefficients (R 2 ) were in the range from 0.9993 to 0.9995, meaning the signal was stable, with broad linear trend. Useful linear concentration range for SDS in water was 4.6 × 10 −7 to 5.1 × 10 −3 M (LOD 3.2 × 10 −7 M) and 6.8 × 10 −7 to 5.1 × 10 −3 (LOD 4.2 × 10 −7 M) in Na 2 SO 4 solution, respectively. Useful linear concentration ranges for DBS in water and Na 2 SO 4 were 8.9 × 10 −7 to 4.1 × 10 −3 M, with LOD 6.1 × 10 −7 M.

pH Influence and Interference Study
The pH influence on the response characteristics of the DHBI-TPB surfactant sensor was measured in a broad pH range from 2 to 12. The signal change was stable and was not affected by the pH change. Small changes in the signal were observed for pH 10 and higher. The latter observations indicate that the DHBI-TPB sensor could also be used in determination of anionic surfactants in commercial formulations.
Interference study was performed by incremental addition of SDS in 0.01 M interfering ion solution. A fixed interference method [17] to calculate the logarithm of the selectivity ) for all selected interfering anions commonly employed in the commercial products formulations was used ( Table 2). As presented, the concentration of SDS was in the range from 4 × 10 −6 to 4 × 10 −3 M. The DHBI-TPB surfactant sensor showed great selectivity for anionic surfactant SDS for all investigated inorganic and organic anions. In order to select the best performing titrant, four analytical grade cationic surfactants-Hyamine 1622, CPC, CTAB and DMIC (all 4 × 10 −3 M), were used for the titrations of SDS (4 × 10 −3 M). The titration curves and their first derivatives (∆E/∆V) are presented in Figure 2. First derivatives for all titration curves showed high potential change in equivalence point. Although DMIC had superior properties as the highest signal change (potential jump in equivalence point) and the highest first derivative signal change was observed, the titration curves for Hyamine 1622, CPC and CTAB showed useful analytical performances as well. In general, falling properties of cationic titrants were DMIC > CTAB > CPC > Hyamine 1622. Since DMIC was proven to be the superior titrant, not only for high anionic surfactant concentrations, but also for very low concentrations, the latter was used for further studies. The studied concentrations of anionic surfactants were in the range usually found in commercial product formulations. tential jump in equivalence point) and the highest first derivative signal change was observed, the titration curves for Hyamine 1622, CPC and CTAB showed useful analytical performances as well. In general, falling properties of cationic titrants were DMIC > CTAB > CPC > Hyamine 1622. Since DMIC was proven to be the superior titrant, not only for high anionic surfactant concentrations, but also for very low concentrations, the latter was used for further studies. The studied concentrations of anionic surfactants were in the range usually found in commercial product formulations.

Titrations of Alkane Sulfonate Homologues
Alkane sulfonate homologues with short chain-lengths are exceptionally soluble in water and therefore, are often difficult to analyze by potentiometric titrations as well as by two-phase titrations. DMIC (4 × 10 −4 M) showed excellent analytical properties ( Figure 2) and was tested as titrant in potentiometric titration of alkane sulfonate homologues with chain-lengths from 7 to 11 having concentration 4 × 10 −4 M. As shown in Figure 3, the titration curves had defined and sharp inflexion points with high potential signal change and well-defined first derivative signal change, except for the shortest chain heptanesulfonate. However, the titration curve for heptanesulfonate still possesses a visible inflexion point and useful potential signal change, with moderately defined first derivative

Titrations of Alkane Sulfonate Homologues
Alkane sulfonate homologues with short chain-lengths are exceptionally soluble in water and therefore, are often difficult to analyze by potentiometric titrations as well as by two-phase titrations. DMIC (4 × 10 −4 M) showed excellent analytical properties ( Figure 2) and was tested as titrant in potentiometric titration of alkane sulfonate homologues with chain-lengths from 7 to 11 having concentration 4 × 10 −4 M. As shown in Figure 3, the titration curves had defined and sharp inflexion points with high potential signal change and well-defined first derivative signal change, except for the shortest chain heptanesulfonate. However, the titration curve for heptanesulfonate still possesses a visible inflexion point and useful potential signal change, with moderately defined first derivative signal change.

The Influence of Nonionic Surfactant on Titrations
Commercial formulations often contain a mixture of anionic surfactants and nonionic surfactants, such as ethoxylated nonionic surfactants (EONSs). Nonionic surfactants are usually used to enhance washing properties of commercial products. Thus, we also examined the influence of EONSs on the potentiometric titrations of anionic surfactants. We considered the different molar ratio of SDS and EONS having 10 EO groups as well as S; the influence of the EONS' number of EO groups on the potentiometric titrations was studied.
Selected EONS having 10 EO groups employing cationic surfactant DMIC (4 × 10 −3 M) as a titrant and a DHBI-TPB surfactant sensor as an end-point indicator are presented in Figure 4. Potentiometric titration curves for titration of mixtures with different molar ratio of anionic surfactant SDS (4 × 10 −3 M) are presented in Figure 5. Selected SDS to EONS molar ratios were 1:0, 1:1, 1:2, 1:3 and 1:6. Increased molar ratio of EONS had a significant negative influence on the shape, inflexion and the size of potentiometric titration curves. With increased EONS molar ratio, the titration curve appeared more flattened. This might negatively influence the direct potentiometric determination of the anionic surfactants in the samples.  (7), nonansulfonate (9) and undecanesulfonate (11) with DMIC (4 × 10 −4 M).

The Influence of Nonionic Surfactant on Titrations
Commercial formulations often contain a mixture of anionic surfactants and nonionic surfactants, such as ethoxylated nonionic surfactants (EONSs). Nonionic surfactants are usually used to enhance washing properties of commercial products. Thus, we also examined the influence of EONSs on the potentiometric titrations of anionic surfactants. We considered the different molar ratio of SDS and EONS having 10 EO groups as well as S; the influence of the EONS' number of EO groups on the potentiometric titrations was studied.
Selected EONS having 10 EO groups employing cationic surfactant DMIC (4 × 10 −3 M) as a titrant and a DHBI-TPB surfactant sensor as an end-point indicator are presented in Figure 4. Potentiometric titration curves for titration of mixtures with different molar ratio of anionic surfactant SDS (4 × 10 −3 M) are presented in Figure 5. Selected SDS to EONS molar ratios were 1:0, 1:1, 1:2, 1:3 and 1:6. Increased molar ratio of EONS had a significant negative influence on the shape, inflexion and the size of potentiometric titration curves. With increased EONS molar ratio, the titration curve appeared more flattened. This might negatively influence the direct potentiometric determination of the anionic surfactants in the samples.  Increased number of EO groups had a significant negative influence on the shape, inflexion and the size of potentiometric titration curves. As presented, the growing number of EO groups induces a more flattened titration curve and for this reason it is harder to find the end-point and it is more difficult to quantify the anionic surfactants in commercial samples.  Potentiometric titration curves for titration of the mixtures of anionic SDS (4 × 10 −3 M) and nonionic surfactant EONS with different number of EO groups (0, 6, 10 and 20 EO) at fixed DS to EONS molar ratio (1:2), with cationic surfactant DMIC (4 × 10 −3 M) as a titrant and a DHBI-TPB surfactant sensor as an end-point indicator, are presented in Figure 5. Increased number of EO groups had a significant negative influence on the shape, inflexion and the size of potentiometric titration curves. As presented, the growing number of EO groups induces a more flattened titration curve and for this reason it is harder to find the end-point and it is more difficult to quantify the anionic surfactants in commercial samples.

Titration of Technical Grade Surfactants
Potentiometric titrations of four technical grade anionic surfactants (4 × 10 −3 M) with DMIC (4 × 10 −3 M) as a titrant and the DHBI-TPB surfactant sensor as an end-point indicator are shown in Figure 6. The titration curves exhibit sharp inflexion points and high signal change with high first derivative signal change. Based on the titrations, the falling properties of selected technical grade anionic surfactants could be described as DBS > SDS > LES > SAS. The accuracy of technical grade anionic surfactants determinations was estimated by the standard addition method, where an exact amount (30 µmol) of technical grade anionic surfactants was added to the sample titrated with DMIC (4 × 10 −3 M) as a titrant and with the DHBI-TPB surfactant sensor as an end-point indicator ( Table 3). As shown, experimentally found and added amounts for all four anionic surfactants, i.e., dodecyl sulfate, dodecyl benzenesulfonate, lauryl ether sulfate and secondary alkane sulfonate, were in good agreement and the recoveries varied from 99.5 to 101.3%. Proposed DHBI-TPB surfactant sensor was successfully employed for technical grade surfactant titrations. The accuracy of technical grade anionic surfactants determinations was estimated by the standard addition method, where an exact amount (30 µmol) of technical grade anionic surfactants was added to the sample titrated with DMIC (4 × 10 −3 M) as a titrant and with the DHBI-TPB surfactant sensor as an end-point indicator ( Table 3). As shown, experimentally found and added amounts for all four anionic surfactants, i.e., dodecyl sulfate, dodecyl benzenesulfonate, lauryl ether sulfate and secondary alkane sulfonate, were in good agreement and the recoveries varied from 99.5 to 101.3%. Proposed DHBI-TPB surfactant sensor was successfully employed for technical grade surfactant titrations.

Titrations of Commercial Samples
Twelve commercial samples of detergents for household care, containing anionic surfactants, were used to quantify anionic surfactant content by DHBI-TPB surfactant sensor (Table 4). The developed DHBI-TPB surfactant sensor method was compared to ISE surfactant sensor and with a two-phase titration method. Three groups of detergents were analyzed: powdered (four samples), liquid-gel (four samples) and handwashing detergents (four samples). The pH was adjusted to 3 to avoid the interfering effect of amphoteric surfactants sometimes present in the product formulations. The results for five independent repetitions were in good agreement and within expected errors for all the tested detergent formulations. Analyzed samples containing handwashing detergent formulations showed the highest anionic surfactant content from 13.98 to 15.89%, powdered detergent samples anionic surfactant content was from 5.75 to 6.88% and liquid gel detergents had 2.01 to 2.56% of anionic surfactants, respectively. Student's t-test (at 95% confidence level) was applied to compare the difference between the results of the two-phase titration or ISE surfactant sensor and those obtained with the DHBI-TPB surfactant sensor. No significant difference was found between data sets.
All salt solutions were prepared using analytical grade chemicals. Twelve commercial detergents for household care (powdered, liquid-gel and handwashing) were purchased from the local stores.

Ionophore Characterization by FTIR
The DHBI-TPB ion-pair presented in Figure 7 was prepared by the procedure described earlier [16]. ATR-FT-IR spectrometer Spectrum Two (Perkin Elmer, Waltham, MA, USA) was used to characterize the DHBI-TPB ion-pair and to compare it with pure DHBI and TPB ( Figure S1).

Ionophore Characterization by FTIR
The DHBI-TPB ion-pair presented in Figure 7 was prepared by the procedure described earlier [16]. ATR-FT-IR spectrometer Spectrum Two (Perkin Elmer, Waltham, MA, USA) was used to characterize the DHBI-TPB ion-pair and to compare it with pure DHBI and TPB ( Figure S1).

Computational Details of Ionophore Characterization
DHBI + cation was parameterized through RESP charges at the HF/6-31G(d) level to be consistent with the employed GAFF force field, while TPBanion was considered according to literature recommendations [18]. The aforementioned ions were solvated in a 15 Å rectangular box of water, which allowed for 7.528 solvent molecules, calculated to match experimental solvent densities, and submitted to the geometry optimization in the AMBER 16 program [19] by employing periodic boundary conditions in all directions. Optimized systems were gradually heated from 0 to 300 K and equilibrated during 30 ps using NVT conditions, followed by productive and unconstrained MD simulations of 300 ns, employing a time step of 2 fs at a constant pressure (1 atm) and temperature (300 K), the latter held constant using a Langevin thermostat with a collision frequency of 1 ps -1 . The nonbonded interactions were truncated at 11.0 Å. The binding free energies among components, ΔGBIND, were calculated using the established MM-PBSA protocol [19,20], all in line with our earlier reports on similar systems [21][22][23]. For that purpose, every second snapshot, 75.000 in total, collected from the entire MD trajectory, were utilized.

Preparation of Surfactant Sensor
The sensor membrane was prepared by the previously described procedure [16]. The high molecular weight PVC (33%) was mixed with a plasticizer (66%) and the DHBI-TPB ionophore (1%). After drying, the sensing membrane was inserted in the electrode body with 3 M NaCl inner electrolyte and used for further research.

Computational Details of Ionophore Characterization
DHBI + cation was parameterized through RESP charges at the HF/6-31G(d) level to be consistent with the employed GAFF force field, while TPB − anion was considered according to literature recommendations [18]. The aforementioned ions were solvated in a 15 Å rectangular box of water, which allowed for 7.528 solvent molecules, calculated to match experimental solvent densities, and submitted to the geometry optimization in the AMBER 16 program [19] by employing periodic boundary conditions in all directions. Optimized systems were gradually heated from 0 to 300 K and equilibrated during 30 ps using NVT conditions, followed by productive and unconstrained MD simulations of 300 ns, employing a time step of 2 fs at a constant pressure (1 atm) and temperature (300 K), the latter held constant using a Langevin thermostat with a collision frequency of 1 ps −1 . The nonbonded interactions were truncated at 11.0 Å. The binding free energies among components, ∆G BIND , were calculated using the established MM-PBSA protocol [19,20], all in line with our earlier reports on similar systems [21][22][23]. For that purpose, every second snapshot, 75.000 in total, collected from the entire MD trajectory, were utilized.

Preparation of Surfactant Sensor
The sensor membrane was prepared by the previously described procedure [16]. The high molecular weight PVC (33%) was mixed with a plasticizer (66%) and the DHBI-TPB ionophore (1%). After drying, the sensing membrane was inserted in the electrode body with 3 M NaCl inner electrolyte and used for further research.

Apparatus
Metrohm 794 Basic Titrino paired with Metrohm 781 pH/mV meter was used to measure response characteristics, pH influence and interferences. Metrohm 808 Titrando was employed for potentiometric titrations, nonionic surfactant influence study and real sample titrations. A Metrohm pH electrode was used to check the pH and a Metrohm silver/silver (I) chloride was used as a referent electrode for all investigations.
3.6. Procedure 3.6.1. Potentiometric Sensor Characterization To fully characterize the DHBI-TPB surfactant sensor on anionic surfactants, response measurements were performed. SDS and DBS anionic surfactants were incrementally added to deionized water and 0.01 M Na 2 SO 4 solution (for high ionic strength study). Anionic surfactant concentrations of 4 × 10 −3 M and 4 × 10 −4 M were used to reach the logarithmic activity range from approximately −2 to −8.
Interference study was performed by incremental addition of SDS in 0.01 M interfering ion solution. A fixed interference method [17] to calculate the selectivity coefficient for all selected interfering anions was employed.
The pH influence on DHBI-TPB surfactant sensor properties was observed in the pH range 2-12. Corresponding amounts of 0.5 M HCl and 0.5 M NaOH were added to reach certain pH values.
After each measurement, surfactant sensor was washed with deionized water.

Potentiometric Titrations
Potentiometric titrations were performed in dynamic equivalent point titration (DET) mode with signal drift 5 mV/min. Waiting time between increments was 15 to 30 s.
An aliquot of 5 mL anionic surfactant was added to 20 mL deionized water and used for titrations.
The influence of nonionic surfactants on titrations of SDS (4 × 10 −3 M) with DMIC (4 × 10 −3 M) was investigated by the addition of nonionic surfactants with 6 EO, 10 EO and 20 EO groups and by varying 10 EO group nonionic surfactants in different molar ratios with SDS.
After each measurement, surfactant sensor was washed with deionized water.

Conclusions
The 1,3-dihexadecyl-1H-benzo[d]imidazol-3-ium-tetraphenylborate (DHBI-TPB)-based surfactant sensor was successfully applied for the quantification of anionic surfactants in commercial household detergent products. The DHBI-TPB surfactant sensor showed excellent resistance to interferences produced by the different organic and inorganic anions usually used in product formulations. The developed device could also be used in the broad pH range from pH 2-10. The DHBI-TPB ionophore was successfully characterized by ATR FT-IR. Computational analysis confirmed the formation of the DHBI-TPB ionophore in the aqueous solution with optimal exergonicity to allow for the beneficial analytical responses. In addition, it underlined C-H···π interactions as crucial for the recognition of the components, surpassing electrostatic charge-charge attractions and π-π stacking interactions, both with moderate significance. DMIC was selected as the most reliable titrant for the use in potentiometric titrations with DHBI-TPB surfactant sensor as an end-point indicator. High solubility alkane sulfonate homologues with chain-lengths from 7 to 11 were successfully titrated with DMIC and DHBI-TPB surfactant sensor as an end-point indicator. Nonionic surfactants had a negative impact on titration curves, shape, inflexion and signal change of anionic surfactants when the EO concentration or the number of EO groups was increased. The titration curves appeared more flattened; in addition, the inflexion points were harder to detect from the first derivation curve. The DHBI-TPB sensor was successfully tested to measure technical grade anionic surfactants concentrations with recoveries from 99.5 to 101.3%. DHBI-TPB surfactant sensor was effectively employed for quantification of anionic surfactants in twelve samples of powered, liquid-gel and handwashing home care detergents. The results were compared with ISE surfactant sensor and a two-phase titration method and showed good agreement.
Thus, the DHBI-TPB surfactant sensor has advantages not only in terms of analytical properties, but also in terms of price, simplicity, speed and lack of need for the use of organic solvents or other additives, compared to the usually employed two-phase titration method. The DHBI-TPB surfactant sensor could be considered as a new and reliable analytical tool and has a promising perspective for its implementation in industry for quality control or in environmental monitoring.