1 Introduction

Water behaviour in different environments is an important factor in chemical systems. In biology water is found in cells where it hydrates membranes and large biomolecules. In geology interfacial water molecules can control ion adsorption and mineral dissolution. In chemistry water is an important polar solvent that is often in contact with various interfaces, for example, in ion-exchange resin systems (Fayer 2012).

Due to commonness of metals application and increasing aggressiveness of the natural environment as a result of water and air pollution a special attention should be paid to the phenomenon of corrosion. It is subject of intensive investigations by scientists searching better and better as well as more effective preventive methods. One of the ways of its reduction is the use of corrosion inhibitors (Obot et al. 2014; Deng et al. 2014; Solmaz 2014). Effective action of these substances depends largely on their adsorption properties as well as kind of metal and environment. Owing to their great effectiveness, simplicity of production and relatively low price, ionic and non-ionic surfactants are effective inhibitors of steel, copper, aluminium, and iron corrosion (Fuchs-Godec and Žerjav 2009; El-Tabei and Hegazy 2013). Application of surfactants and other organic substances mixtures can improve significantly effectiveness of corrosion prevention (Fuchs-Godec 2007).

The study of organic compounds adsorption at the electrode/solution interface allows to describe the structure of the electrical double layer, the kinetics of electron transfer and the effect of metal corrosion inhibitors (Munoz et al. 1992; Nieszporek et al. 2012; Nosal-Wiercińska 2012, 2014, 2013; Nosal-Wiercińska and Dalmata 2010).

A comprehensive analysis of the experimental data concerning adsorption of surface-active compounds on different solid metals seems to support the view that the mixed adsorption on the mercury surface should proceed analogously.

In the previous studies the competitive adsorption between the 6-mercaptopurine–Triton X-100 or mixed micelles were observed (Nosal-Wiercińska et al. 2018).

The influence of 6-mercaptopurine–Triton X-100 and water activity on the double layer parameters at the mercury/chlorates(VII) interface is examined in the present paper.

The choice of water as the medium which affects the parameters of the double layer at the mercury/chlorates(VII) interface (Nosal-Wiercińska et al. 2018) was motivated by its specific properties and the fact that most chemical processes takes place in the aqueous environment. The measurements conducted in the solutions of different water activity [2, 4 and 6 mol dm−3 chlorate(VII) corresponding with water activities: 0.927, 0.832 and 0.704, respectively (Komorsky-Lovrič et al. 1993)] would allow to describe better both 6-mercaptopurine–Triton X-100 adsorption and the influence of the degree of electrode surface hydration on the adsorption–desorption processes.

2 Experimental

2.1 Materials and methods

The experiments were performed using a three-electrode cell with a hanging controlled growth mercury drop electrode (CGMDE) (Entech, Cracow, Poland) as the working electrode (electrode area was 0.009487 cm2, drop time was 3 s), Ag/AgCl/saturated NaCl as the reference electrode and a platinum spiral as the counter electrode (Scheme 1).

Scheme 1
scheme 1

Three-electrode cell

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The measurements were made in thermostated cells at 298 K with the electrochemical analyzer µAutolab/GPES (Version 4.9) (Eco Chemie, Utrecht, the Netherlands) (Scheme 2).

Scheme 2
scheme 2

Electrochemical analyzer µAutolab

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The differential capacity of the double layer (Cd) at the mercury/ supporting electrolyte interface was measured by the impedance method. The reproducibility of the differential capacitance measurements was 5%. The potential of zero charge (Ez) was determined using a streaming electrode. For the whole polarisation range, the capacity dispersion was tested at different frequencies changing in the range 200–1000 Hz. The occurrence of frequency dispersion was found for all examined systems. As a result of the differential capacitance extrapolation to zero frequency, the differential capacity curves corresponding to the adsorption equilibrium were obtained.

The surface tension at the potential of zero charge (γz) was measured using the method of the highest pressure inside the mercury drop. Both Ez and γz were determined using a capillary electrometer (Scheme 3) (Nosal-Wiercińska 2012), with the accuracy respectively: ± 0.1 mV for Ez and ± 0.2 mNm−1 for γz.

Scheme 3
scheme 3

Capillary electrometer

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Analytical-grade reagents: 6-mercaptopurine (Fluka), NaClO4 (Fluka) and HClO4 (Fluka), Triton X-100 (Sigma-Aldrich) were used without further purification. The solutions were prepared using doubly-distilled water. Before the measurements the solutions were deaerated using high-purity nitrogen. Nitrogen was passed over the solution during the measurements.

2, 4 and 6 mol dm−3 chlorate(VII) solutions, mixed at proper ratios [x mol dm−3 NaClO4 + 1 mol dm−3 HClO4 (where 0 ≤ x ≤ 5)] were used as a basic electrolyte.

The solutions were prepared just before measurements. The concentrations of 6 MP were in the range of 0.5–50 × 10−3 mol dm−3 whereas those of Triton X-100 were in the range 1 × 10−6–1 × 10−3 mol dm−3.

3 Results and discussion

The changes of adsorption parameters as a function of the supporting electrolyte concentration point out to the competitive adsorption in 6-mercaptopurine–Triton X-100 system as well as the electrostatic interactions between the adsorbate and the water molecules.

Figures 1, 2 and 3 show the capacitance curves in 2, 4, 6 mol dm−3 chlorates(VII) in the presence of 6-mercaptopurine. In the region of the “hump” potentials, appearing in chlorate(VII) without the studied substances (≈ − 200 to − 800 mV) after the addition of 6-mercaptopurine, the height of the “hump” decreases. It should be pointed out that in the 4, 6 mol dm−3 chlorates(VII) this area of potentials is still broader being from − 100 to − 1000 mV. The increase in the concentration of the studied substances causes a further decrease in differential capacitance in the region of “hump” potentials. Such picture of capacity curves indicates strong adsorption properties of 6-mercaptopurine. In the region of higher potentials (≈ 200 mV) the adsorption peaks occur in the presence of 6-mercaptopurine (Figs. 1, 2, 3), however in the area of the most negative potentials (about-1000) mV the desorption peak appears. Both peaks increase with the increasing adsorbate concentration in the basic electrolyte solution.

Fig. 1
figure 1

Differential capacity–potential curves of double layer interface Hg/2 mol dm−3chlorate(VII) with various concentrations of 6-mercaptopurine: (closed circle) 0, 0,5 (cross), 1,0 (open diamond), 5,0 (open square) (in mol dm−3)

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Fig. 2
figure 2

Differential capacity–potential curves of double layer interface Hg/4 mol dm−3chlorate(VII) with various concentrations of 6-mercaptopurine: (closed circle) 0, 0,5 (cross), 1,0 (open diamond), 5,0 (open square)

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Fig. 3
figure 3

Differential capacity–potential curves of double layer interface Hg/6 mol dm−3chlorate(VII) with various concentrations of 6-mercaptopurine: (closed circle) 0, 0,5 (cross), 1,0 (open diamond), 5,0 (open square)

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However, it should be stressed that in the solutions of the basic electrolyte of the smallest water activity the desorption peak (especially for the high concentration of 6MP) is poorly defined. This indicates competitive electrostatic interactions between the 6MP molecules, \(ClO_{4}^{ - }\) ions and water dipoles. Undoubtedly, water molecules are the largest hindrance in the 6-mercaptopurine adsorption on the mercury surface. An increased concentration of chlorate(VII) ions characterized by great ability to destroy water structure seems to be very advantageous (Nosal-Wiercińska 2013).

The earlier studies showed the specific adsorption of 6-mercaptopurine on the mercury surface (Nosal-Wiercińska et al. 2018).

Figures 4, 5 and 6 present the capacitance curves in 2, 4, 6 mol dm−3 chlorates(VII) in the presence of 1·10−3 mol dm−3 6-mercaptopurine and the increasing Triton X-100 concentrations. The addition of the surfactant to the basic electrolyte solution containing mercaptopurine does not change the picture of capacity curves. This confirms distinct domination of 6MP in formation of adsorption equilibria of the mixed adsorption layers of 6MP-TritonX-100. It should be noticed that the increase in TritonX-100 concentration in the basic electrolyte results in the evident decrease of adsorption and desorption peaks. The desorption peaks even disappear which can be particularly observed in 6 mol dm−3 chlorates(VII). This should be also associated with the effect of Triton X-100 on the adsorption equilibria formation (Wiśniewska et al. 2012). However, one should not exclude mutual interactions of 6MP and the surfactant molecules leading to the formation of a much less compact structure of adsorption layers. One should also mention about reduction of hydration degree of electrode surface due the increasing concentration of the basic electrolyte. This affects reorientation of water molecules and changes the electrostatic interactions between the adsorbed molecules (Parsons and Reeves 1981).

Fig. 4
figure 4

Differential capacity–potential curves of double layer interface Hg/2 mol dm−3 chlorate(VII) with 1 × 10−3 mol dm−3 6-mercaptopurine and with various concentrations of TritonX-100: (closed circle) 0, 1,0 (+), 4,0 (open diamond), 6,0 (open circle), 20 (open square) (in mol dm−3)

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Fig. 5
figure 5

Differential capacity–potential curves of double layer interface Hg/4 mol dm−3 chlorate(VII) with 1 × 10−3 mol dm−3 6-mercaptopurine and with various concentrations of TritonX-100: (closed circle) 0, 1,0 (cross), 4,0 (open diamond), 6,0(open circle), 20 (open square) (in mol dm−3)

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Fig. 6
figure 6

Differential capacity–potential curves of double layer interface Hg/6 mol dm−3 chlorate(VII) with 1 × 10−3 mol dm−3 6-mercaptopurine and with various concentrations of TritonX-100: (closed circle) 0, 1,0 (cross), 4,0 (open diamond), 6,0(open circle), 20 (open square) (in mol dm−3)

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Tables 1 and 2 present the values of the potentials of zero charge and those of the surface tension γz at the zero charge potential for the studied systems. As follows from Table 1 the addition of 6-mercaptopurine to the 2, 4, 6 mol dm chlorates(VII) solution causes shift of Ez towards more negative potentials. This indicates that the adsorption of the 6-mercaptopurine dipoles proceeds via the sulfur atom oriented towards the mercury surface (Gugała-Fekner et al. 2009).

Table 1 Potential of zero-charge Ez versus Ag/AgCl electrode and surface tension γz for Ez of 2, 4 and 6 mol dm−3 chlorates(VII) solutions + different 6-mercaptopurine systems
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Table 2 Potential of zero-charge Ez versus Ag/AgCl electrode and surface tension γz for Ez of 2, 4, 6 mol dm−3 chlorates(VII) solutions + 3 × 10−5 mol dm−3 TritonX-100 + different 6-mercaptopurine concentration systems
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Moreover, with the increase in the 6-mercaptopurine concentration the Ez values shift significantly towards evidently more negative potential values. Such changes of Ez with the increasing concentration suggest change of 6MP molecules orientation on the mercury surface.

For the mixed adsorption layers of 6-mercaptopurine–Triton X-100 a similar behaviour is observed. However, the shifts of potentials are significantly smaller. This can be due to both 6MP and Triton X-100 molecules interactions leading to formation of a more or less compact structure of adsorption layers and the synergetic effect (Szymczyk and Jańczuk 2008).

The values of surface tension γz at the zero charge potential (Tables 1, 2) decrease for all studied systems, as proved by the adsorption phenomenon (Nosal-Wiercińska 2013). The adsorption properties of both studied systems grow with the reduction in water activity. It should be noted that the reduction is slightly larger for the mixed adsorption layer compared to the system containing only 6MP.

4 Conclusions

It was proved that both 6-mercaptopurine, mixed adsorption layer of 6-mercaptopurine–Triton X-100 and activity of water have a significant effect on the parameters of the double layer at the Hg/chlorates(VII) interface. The changes of adsorption parameters as a function of the supporting electrolyte concentration (with the water activity decrease: from 0.927, through 0.832 to 0.704) point at competitive adsorption of 6-mercaptopurine and \(ClO_{4}^{ - }\) ions as well as electrostatic interactions between the adsorbate and the water molecules. In the case of the mixed adsorption layer of 6-mercaptopurine–Triton X-100, the dominance of 6MP in adsorption equilibria formation as well as the competitive adsorption between the 6MP and TritonX-100 molecules occur. Moreover, the formation of chemimicelles in 2 mol dm−3 chlorates(VII) is also possible.