Stabilization of the (C2H5)4NHSO4 High-Temperature Phase in New Silica-Based Nanocomposite Systems

In this study, the electrotransport, thermal and structural properties of composite solid electrolytes based on (C2H5)4NHSO4 plastic phase and silica (1 − x)Et4NHSO4−xSiO2, where x = 0.3–0.9) were investigated for the first time. The composites were prepared by mechanical mixing of silica (300 m2/g, Rpore = 70Å) and salt with subsequent heating at temperatures near the Et4NHSO4 melting point. Heterogeneous doping is shown to change markedly the thermodynamic and structural parameters of the salt. It is important that, with an increase in the proportion of silica in the composites, the high-temperature disordered I41/acd phase is stabilized at room temperature, as this determines the properties of the system. Et4NHSO4 amorphization was also observed in the nanocomposites, with an increase in the matrix contents. The enthalpies of the endoeffects of salt melting and phase transitions (160 °C) changed more significantly than the Et4NHSO4 contents in the composites and completely disappeared at x = 0.9. The dependence of proton conductivity on the mole fraction reached a maximum at x = 0.8, which was three or four orders of magnitude higher than the value for pure Et4NHSO4, depending on the composition and the temperature. The maximum conductivity values were close to those for complete pore filling. The conductivity of the 0.2Et4NHSO4-0.8SiO2 composite reached 7 ∗ 10−3 S/cm at 220 °C and 10−4 S/cm at 110 °C.


Introduction
One of the new, significant and interesting ways of improving the conductivity of ionic salts is heterogeneous doping with highly dispersed inert materials, for example, metal oxides with a high specific surface area and a large pore size [1][2][3]. The conductivity of composite systems can increase by several orders of magnitude due to surface interactions between the components, which lead to the formation of high defect concentrations in the areas of interfacial contact in composites (the so-called space charge regions) [4]. In some cases, especially in nanocomposites, changes in the thermodynamic parameters of ionic salts are observed [5,6]. This has been observed in a number of nanocomposites based on silica, zirconium, titanium dioxides and acid salts of alkali metals, as well as lithium salts [7][8][9][10][11][12].
For a number of acid salts of alkali metals, as a rule, having superionic phases, the possibility of creating highly conductive proton composite electrolytes has been shown [13][14][15]. In [16,17], composites based on CsHSO 4 and highly dispersed silicon dioxide (1 − x)CsHSO 4− xSiO 2 with different specific surface areas and pore sizes were studied. It was shown that the conductivity of the low-temperature phase of CsHSO 4 in the composite increased by up to 2.5 orders of magnitude, depending on the composition and type of silicon dioxide, and passed through a maximum. At the same time, decreases in temperature and the enthalpies of phase transitions and melting were observed, which were associated with the dispersion and amorphization of the salt. The largest size effect was obtained for composites based on SiO 2 with a specific surface area of~300-500 m 2 /g, which had a uniformly porous structure and an average pore radius of 35-70 Å [16][17][18].
temperature and the enthalpies of phase transitions and melting were observed, which were associated with the dispersion and amorphization of the salt. The largest size effect was obtained for composites based on SiO2 with a specific surface area of ~300-500 m 2 /g, which had a uniformly porous structure and an average pore radius of 35-70 Å [16][17][18]. The introduction of a dispersed matrix resulted in an increase in the conductivity of the low-temperature phase of the salt and a decrease in the high-temperature region due to the effect of conductor-insulator percolation. Thus, the properties of the composites were significantly affected not only by the types of heterogeneous components and the chemical natures of the surfaces, but also by the features of the porous structures of the matrices, in particular, the sizes of grains and pores and the nature of the pore size distribution.
As for organic plastic crystals, which have attracted the interest of researchers in recent years [19,20], there are no data in the literature on composite systems based on them. The class of quaternary ammonium salts, which have the general formula R4N + X (R-alkyl, aryl group), consisting of both polar (N + ) and non-polar (R) groups, exhibit a variety of physicochemical properties. Some of the quaternary ammonium compounds have ferroelectric properties, many of them are ionic liquids and parts of them are constituted by organic plastic crystals [21][22][23]. Accordingly, they are distinguished by a wide range of applications, being used as reagents, surfactants, catalysts, ionic liquids and electrolytes. As for the subgroup of quaternary ammonium hydrogen sulfates, such as methyl-(Me),ethyl (Et), -propyl (Pr) and -butyl (Bu) ammonium, their structural, thermodynamic and electrotransport properties have not been studied enough. Recently, data have appeared on the structural properties and proton conductivities of Bu4NHSO4 [24,25] and Et4NHSO4 [26,27] compounds. As a rule, an increase in the length of the carbon chain of an alkyl group leads to a decrease in the melting temperature and a change in the symmetry of the unit cell from orthorhombic to monoclinic. The Et4NHSO4 compound is characterized by a rather high melting point due to the salts in this family of 245 °C [26]. At room temperature, Et4NHSO4 belongs to the monoclinic (P21/n) system with the unit cell parameters a = 9.7994 Å, b = 13.812 Å, c = 9.5968 Å and β = 89.368° [26]. In the crystal structure of the salt, layers of tetraethylammonium cations alternate with anionic hydrosulfate layers (Figure 1). Figure 1. Schematic presentation of Et4NHSO4 crystal structure according to [26].
Et4N + cations have the shape of a Nordic cross with S4 symmetry and are much larger than the anions. The symmetry of SO4 groups is close to tetrahedral, with small deviations in the O-S-O angle from 109.28° for an ideal tetrahedron. Two sulfate tetrahedra are linked  [26]. Et 4 N + cations have the shape of a Nordic cross with S 4 symmetry and are much larger than the anions. The symmetry of SO 4 groups is close to tetrahedral, with small deviations in the O-S-O angle from 109.28 • for an ideal tetrahedron. Two sulfate tetrahedra are linked into dimers by strong hydrogen bonds. The dimers are ordered into layers that are isolated from each other at a relatively large distance of 6.53 Å [26]. At T = 160 • C, the tetragonal phase I4 1 /acd is formed with the unit cell parameters a = 14.0430 Å and c = 25.686 Å and exists up to the melting point of Et 4 NHSO 4 [27].
The proton conductivity of Et 4 NHSO 4 is quite low and does not exceed 5·10 −6 S/cm at temperatures below 200 • C, which is due to the structural features of the compound and the presence of strong hydrogen bonds. The activation energy of conductivity varies non-linearly with temperature from 1.2 eV up to~140 • C to 0.58 eV in the 140-200 • C temperature range. Further, a sharp increase in conductivity can be observed due to the achievement of temperatures close to the compound's premelting temperature. The nature of the temperature dependence of the conductivity corresponds to the structural phase transitions of Et 4 NHSO 4 . A sequence of reversible phase transitions was established at 147 • C and 160 • C with enthalpies of −3.28 and −8.99 J/g, respectively [24,27]. Given the large size of Et 4 N + , the cationic subsystem constitutes the less mobile core of the crystal lattice. The most probable charge carriers are protons associated with SO 4 tetrahedra.
This study aimed to synthesize proton composite electrolytes of (1 − x)Et 4 NHSO 4− xSiO 2 (where x = the mole fraction of silica) with a wide range of compositions and investigate their electrotransport and structural properties. Silicon dioxide with a specific surface area of 300 m 2 /g, a pore size of 70 Å with a uniform pore size distribution and a pore volume of 0.9 cm 3 /g was used as a matrix, which, as was shown earlier, was characterized by the optimal morphology for the composites based on the acid salts of alkali metals [28].

Materials and Methods
Composite electrolytes of (1 − x)Et 4 NHSO 4− xSiO 2 , in which the molar fraction of SiO 2 , x, varied from 0 to 0.90, were prepared. Commercial reagent Et 4 NHSO 4 of analytical grade (Sigma-Aldrich) was used. Silicon dioxide samples with the trademark "KSKG" were preliminarily heated in air at 500 • C for 3 h. The porous structure of silica was analyzed using the nitrogen adsorption technique on a Quantochrome AutosorbiQ gas sorption analyzer at 77 K. Then, SiO 2 was carefully ground in an agate mortar with tetraethylammonium hydrogen sulfate, at a certain molar ratio. The molar fractions were selected following various degrees of pore filling, including the complete filling of SiO 2 pores with salt. The homogenized powder mixture was pressed at P = 500 MPa with the application of silver or platinum electrodes. The resulting tablets were heated in air for 20 min at a temperature (T) = 220-230 • C, close to the melting point of the salt. The electrical conductivity was measured with a two-electrode circuit and an alternating current using an IPU-1RLC-1/2008 impedance meter (frequency range: 0.1 Hz-3.3 MHz) in a temperature range of 25-250 • C by the complex impedance method. The measurements were carried out in the slow cooling mode at a rate of 0.5-1 deg/min in air, with a relative humidity of 15-20%.
The phase composition of the (1 − x)Et 4 NHSO 4− xSiO 2 electrolytes was analyzed by X-ray diffraction with a D8 Advance diffractometer (Cu-Kα radiation). Fourier transform infrared spectroscopy (FTIR) spectra in the attenuated total reflectance (ATR) mode were recorded on a Bruker Tensor 27 spectrometer. The morphology of the samples was investigated using a Hitachi S3400N scanning electron microscope. Differential scanning calorimetry (DSC) data were obtained with a DSC 500 differential calorimeter in heating mode in the temperature range of 25-260 • C with an argon flow at a rate of 10 • C/min.

Results and Discussion
The powder X-ray diffraction (PXRD) patterns of the synthesized (1 − x)Et 4 NHSO 4− xSiO 2 composites at room temperature are presented in Figure 2. The PXRD pattern of Et 4 NHSO 4 (P2 1 /n) at room temperature completely coincided with the results of [26]. The intensity of reflexes of the composites decreased significantly, and the peaks broadened with the composition x = 0.5. It was clear that at x = 0.5 all reflections corresponded to the Et 4 NHSO 4 (P2 1 /n) crystal structure ( Figure 2a). Therefore, chemical interaction between the salt and the dispersed SiO 2 matrix in the composite could be excluded. The intensity of reflexes decreased more significantly than the mass fraction of Et 4 NHSO 4 in the composite compounds. A more detailed view of the main intense reflections is shown in Figure 2b. For example, the intensity of some of the peaks in the monoclinic phase (011, 110, 020) decreased more than 10 times for the x = 0.5 composition, while the salt content in the composite was 79 w%; at x = 0.7, the intensity decreased up to 35 times when the salt content in the composite was equal to 62 w% (Figure 2b). With a further increase in the heterogeneous matrix content up to x = 0.7, the reflections of the high-temperature I4 1 /acd phase appeared; they are indicated by asterisks in Figure 2a. In a number of intermediate compositions, the existence of two phases of Et 4 NHSO 4 , both low-temperature (P2 1 /n) and high-temperature (I4 1 /acd), was observed.
broadened with the composition x = 0.5. It was clear that at x = 0.5 all reflections corre-sponded to the Et4NHSO4 (P21/n) crystal structure ( Figure 2a). Therefore, chemical interaction between the salt and the dispersed SiO2 matrix in the composite could be excluded. The intensity of reflexes decreased more significantly than the mass fraction of Et4NHSO4 in the composite compounds. A more detailed view of the main intense reflections is shown in Figure 2b. For example, the intensity of some of the peaks in the monoclinic phase (011, 110, 020) decreased more than 10 times for the x = 0.5 composition, while the salt content in the composite was 79 w%; at x = 0.7, the intensity decreased up to 35 times when the salt content in the composite was equal to 62 w% (Figure 2b). With a further increase in the heterogeneous matrix content up to x = 0.7, the reflections of the high-temperature I41/acd phase appeared; they are indicated by asterisks in Figure 2a. In a number of intermediate compositions, the existence of two phases of Et4NHSO4, both low-temperature (P21/n) and high-temperature (I41/acd), was observed. At x > 0.8, the PXRD patterns showed that the salt in the composite was mainly in the high-temperature I41/acd phase with a significantly reduced intensity of reflections and their conspicuous broadening. This was due to the formation of Et4NHSO4 in the amorphous state on the highly dispersed SiO2 surface and pores. At x > 0.85, the reflexes almost disappeared. In addition, the reflexes of Et4NHSO4 in the composites moved towards larger angles due to a slight decrease in the Et4NHSO4 unit cell parameters on the surface At x > 0.8, the PXRD patterns showed that the salt in the composite was mainly in the high-temperature I4 1 /acd phase with a significantly reduced intensity of reflections and their conspicuous broadening. This was due to the formation of Et 4 NHSO 4 in the amorphous state on the highly dispersed SiO 2 surface and pores. At x > 0.85, the reflexes almost disappeared. In addition, the reflexes of Et 4 NHSO 4 in the composites moved towards larger angles due to a slight decrease in the Et 4 NHSO 4 unit cell parameters on the surface of the silica (Figure 2b). Thus, the PXRD patterns showed that the salt was retained in the composites with the crystal structure of Et 4 NHSO 4 (P2 1 /n) at lower silica additive levels (up to x = 0.5). With further increase in x, two disordered Et 4 NHSO 4 phases with decreased unit cell parameters existed in the composites, and then, with an increase in x, at x ≥ 0.8 the high-temperature phase (I4 1 /acd) stabilized and existed in the composites at a low temperature. It is remarkable that almost the same changes were observed in the FTIR spectrum for CsHSO 4 [15], indicating that in the composite with highly dispersed silicon dioxide (Ssp~300 m 2 /g) CsHSO 4 was stabilized in the more disordered phase II (P2 1 /c) with weaker hydrogen bonds, or, depending on the composition, there was a mixture of phases III (P2 1 /m) and II, with phase II being the most prevalent.
For a more detailed investigation of the change in structural, thermodynamic and electrotransport properties, we chose the compositions corresponding to various degrees of pore filling, including an excess or deficiency of salt relative to the available pore volume. The dependences of the volume of Et 4 NHSO 4 (V salt ) and the total pore volume of silica (V pore ) per 1 g of composite as a function of the mole fraction, x, are shown in Figure 3. As discussed below, the salt content exceeded the pore volume in the composites up to x = 0.8. The complete filling of the pores could be observed at x = 0.8 in the case of an ideal distribution of components. At x > 0.8, the volume of the matrix pores exceeded markedly the volume of the salt, which can lead to incomplete pore filling and a significant decrease in conductivity, due to disruption of the formed conduction channels. Therefore, the compositions close to the complete filling of pores were studied in more detail.
dioxide (Ssp ~300 m 2 /g) CsHSO4 was stabilized in the more disordered phase II (P21/c) with weaker hydrogen bonds, or, depending on the composition, there was a mixture of phases III (P21/m) and II, with phase II being the most prevalent.
For a more detailed investigation of the change in structural, thermodynamic and electrotransport properties, we chose the compositions corresponding to various degrees of pore filling, including an excess or deficiency of salt relative to the available pore volume. The dependences of the volume of Et4NHSO4 (Vsalt) and the total pore volume of silica (Vpore) per 1 g of composite as a function of the mole fraction, x, are shown in Figure  3. As discussed below, the salt content exceeded the pore volume in the composites up to x = 0.8. The complete filling of the pores could be observed at x = 0.8 in the case of an ideal distribution of components. At x > 0.8, the volume of the matrix pores exceeded markedly the volume of the salt, which can lead to incomplete pore filling and a significant decrease in conductivity, due to disruption of the formed conduction channels. Therefore, the compositions close to the complete filling of pores were studied in more detail. The pore-filling effect was supported by the results of the scanning electron microscopy studies presented in Figure 4. As can be seen from the figure, the initial Et 4 NHSO 4 powder consisted of coarse crystalline particles 100-300 µm in size (Figure 4a).  Pure silica powder is characterized by a wide particle size distribution, with the particle size ranging from 5 to 100 μm (Figure 4b). The morphology of the 0.2Et4NHSO4-0.8SiO2 composite (Figure 4c) is similar to that for pure silica. The disappearance of large crystallites of Et4NHSO4 may be explained by the imparting of the salt into the pores of the silica, the morphology of the silica particles being unaffected.
DSC data for Et4NHSO4 and the (1 − x)Et4NHSO4−xSiO2 composites are presented in Figure 5. It can be seen that the enthalpies of the endoeffects of the melting and phase transitions changed more significantly than the salt content in the composites and completely disappeared with an increase in x to 0.9. The temperature and enthalpy of melting for the composite when x = 0.5 were closer to the original salt (244.8 °C and -71.97 J/g, Pure silica powder is characterized by a wide particle size distribution, with the particle size ranging from 5 to 100 µm (Figure 4b). The morphology of the 0.2Et 4 NHSO 4 -0.8SiO 2 composite (Figure 4c) is similar to that for pure silica. The disappearance of large crystallites of Et 4 NHSO 4 may be explained by the imparting of the salt into the pores of the silica, the morphology of the silica particles being unaffected.
DSC data for Et 4 NHSO 4 and the (1 − x)Et 4 NHSO 4− xSiO 2 composites are presented in Figure 5. It can be seen that the enthalpies of the endoeffects of the melting and phase transitions changed more significantly than the salt content in the composites and completely disappeared with an increase in x to 0.9. The temperature and enthalpy of melting for the composite when x = 0.5 were closer to the original salt (244.8 • C and -71.97 J/g, accordingly) and the enthalpy for x = 0.75 decreased markedly and was equal to -14.8 J/g. The temperature of melting shifted to 239 • C. The temperature of the phase transition also decreased to 158.7 • C. With the further increase in x to x = 0.9, the endoeffects due to the melting and phase transitions disappeared. Pure silica powder is characterized by a wide particle size distribution, with the particle size ranging from 5 to 100 μm (Figure 4b). The morphology of the 0.2Et4NHSO4-0.8SiO2 composite (Figure 4c) is similar to that for pure silica. The disappearance of large crystallites of Et4NHSO4 may be explained by the imparting of the salt into the pores of the silica, the morphology of the silica particles being unaffected.
DSC data for Et4NHSO4 and the (1 − x)Et4NHSO4−xSiO2 composites are presented in Figure 5. It can be seen that the enthalpies of the endoeffects of the melting and phase transitions changed more significantly than the salt content in the composites and completely disappeared with an increase in x to 0.9. The temperature and enthalpy of melting for the composite when x = 0.5 were closer to the original salt (244.8 °C and -71.97 J/g, accordingly) and the enthalpy for x = 0.75 decreased markedly and was equal to -14.8 J/g. The temperature of melting shifted to 239 °C. The temperature of the phase transition also decreased to 158.7 °C. With the further increase in x to x = 0.9, the endoeffects due to the melting and phase transitions disappeared. FTIR spectra for Et4NHSO4 are shown in Figure 6 for hydrogen bond networks (a) and SO4 tetrahedra and Et4N + (b). The wavenumbers of the stretching and bending vibrations of the SO4 tetrahedra in Et4NHSO4 correspond to inorganic hydrogen sulfate data [29,30] and other salts with organic cations [31][32][33]. There were intense absorption bands FTIR spectra for Et 4 NHSO 4 are shown in Figure 6 for hydrogen bond networks (a) and SO 4 tetrahedra and Et 4 N + (b). The wavenumbers of the stretching and bending vibrations of the SO 4 tetrahedra in Et 4 NHSO 4 correspond to inorganic hydrogen sulfate data [29,30] and other salts with organic cations [31][32][33]. There were intense absorption bands at 3500-1500 cm −1 , corresponding to the strong hydrogen bond network, and~1243 cm −1 , characteristic of acid sulfates. The decreased symmetry of the T d for SO 4 2 -containing compounds to C 3v symmetry for HSO 4 − resulted in the splitting of the characteristic tetrahedral bands. Since the symmetrical stretching vibrations of Et 4 N + extended into the area of absorption bands of the sulfate ion, the spectrum was less easily interpreted. The characteristic ABC structure, observed for strong hydrogen bonds of Et 4 NHSO 4 , should be explained based on Fermi resonance between the OH stretching, the overtone of the out-of-plane bending vibrations 2γ(OH) and the combination of the in-plane bending δ(OH) mode and the out-of-plane bending vibrations γ(OH), which give rise to the characteristic doublet with maxima at ca. 2941 cm −1 (A), 2607-2534 cm −1 (B) and the broad, weakly expressed band at ca 1630 cm −1 (C). The in-plane bending mode (δ OH ) of the hydrogen bond gave a strong band at 1236 cm −1 . A more detailed correlation of absorption bands for an organic cation is presented in [27,34,35].
The FTIR spectrum of the Et 4 NHSO 4 -SiO 2 composite can be interpreted as the sum of the spectra for SiO 2 and Et 4 NHSO 4 . In the Et 4 NHSO 4 -SiO 2 composites, the intensity of the absorption bands in the region of hydrogen bonds decreased significantly and the centers of gravity of the corresponding absorption bands slightly shifted to the higher frequencies. The a.b in the range of 2564 cm −1 shifted to 2573 cm −1 at x = 0.5 and to 2583 cm −1 at x = 0.8, while the center of gravity of the silica absorption bands of 3442 cm −1 shifted to 3353 cm −1 at x = 0.9 due to the formation of weak hydrogen bonds between the salt and the matrix. The changes were also observed in the spectral range of the sulfate group: the absorption bands decreased markedly in intensity for x > 0.75 and the a.b. in the range of 1148 cm −1 shifted to 1158 cm −1 , while the a.b of 802 cm −1 shifted to 790 cm −1 for x > 0.75. The changes were associated with a slight strengthening of the S-O bonds and a weakening of the hydrogen bond network of the salt upon binding to the silica matrix. The differences between the FTIR spectrum of the composite at x = 0.8 and the spectrum of Et 4 NHSO 4 were more pronounced. There was a shift-a significant decrease in the intensity of the absorption bands-corresponding to the stretching and bending vibrations of SO 4 and their relative broadening, which corresponded to an increase in the symmetry of SO 4 tetrahedra and an increase in the orientational disorder of HSO 4 -ions.The impedance plots of the composites (x = 0.8) at different temperatures are presented in Figure 7. The Nyquist plot (showing the dependence of imaginary and real parts of resistivity) consists of an arc representing the electrode processes (in the region of lower frequencies) and parts of semicircles due to electrolyte transfer in the higher frequency region. The proton conductivity was calculated from the resistance values with the minimum of capacitive components. With increasing temperature, the radii of the semicircles decreased markedly, so the proton conductivity increased due to an increase in the number of current carriers and their mobility. The FTIR spectrum of the Et4NHSO4-SiO2 composite can be interpreted as the sum of the spectra for SiO2 and Et4NHSO4. In the Et4NHSO4-SiO2 composites, the intensity of the absorption bands in the region of hydrogen bonds decreased significantly and the centers of gravity of the corresponding absorption bands slightly shifted to the higher frequencies. The temperature dependencies of the conductivity for (1 -x)Et 4 NHSO 4 -xSiO 2 in comparison with the original salt are presented in Figure 8. The low-temperature conductivity of Et 4 NHSO 4 obeys the Arrhenius law, with an activation energy of~1.2 eV. The conductivity of the Et 4 NHSO 4 was rather low and did not exceed 5·10 −6 S/cm at temperatures below 210 • C, which corresponded to the structural data and the strong hydrogen bond network of the compound. The activation energy of conductivity varied with the temperature from 1.2 eV up to~140 • C and then showed a linear region at 140-200 • C with the activation energy of 0.58 eV.
plot (showing the dependence of imaginary and real parts of resistivity) consists of an arc representing the electrode processes (in the region of lower frequencies) and parts of semicircles due to electrolyte transfer in the higher frequency region. The proton conductivity was calculated from the resistance values with the minimum of capacitive components. With increasing temperature, the radii of the semicircles decreased markedly, so the proton conductivity increased due to an increase in the number of current carriers and their mobility. The temperature dependencies of the conductivity for (1 -x)Et4NHSO4-xSiO2 in comparison with the original salt are presented in Figure 8. The low-temperature conductivity of Et4NHSO4 obeys the Arrhenius law, with an activation energy of ~1.2 eV. The conductivity of the Et4NHSO4 was rather low and did not exceed 5ꞏ10 −6 S/cm at temperatures below 210 °C, which corresponded to the structural data and the strong hydrogen bond network of the compound. The activation energy of conductivity varied with the temperature from 1.2 eV up to ~140 °C and then showed a linear region at 140-200 °C with the activation energy of 0.58 eV.  A significant increase in conductivity by three orders of magnitude for Et4NHSO4 was observed at temperatures above 210 °C, close to the melting point, where the conductivity reached ~8ꞏ10 −3 S/cm, characteristic of the melts. Heterogeneous doping of Et4NHSO4 resulted in a significant increase in the conductivity by three or four orders of magnitude, depending on the composition and temperature. The conductivity increased by up to one order of magnitude in the investigated composites (with small x values up to x = 0.5), which may be connected to the dispersion of salt and the formation of space charge regions at the interphase with the amorphous state of Et4NHSO4 on the highly dispersed SiO2 surface (x > 0.5) and in pore spaces. Two regions of temperature dependence of the conductivity could also be distinguished for the composite Et4NHSO4-SiO2 systems with a change in the activation energy. At temperatures lower than 170 °C, the activation energy was equal to 1.1 eV for x = 0.5, decreased to 1.0 eV for x = 0.75 and was equal to 0.76 eV for x = 0.8. A decrease in the activation energy with an increase in the inert highly dispersed additive is typical for composite solid electrolytes and is described by partial could also be distinguished for the composite Et 4 NHSO 4 -SiO 2 systems with a change in the activation energy. At temperatures lower than 170 • C, the activation energy was equal to 1.1 eV for x = 0.5, decreased to 1.0 eV for x = 0.75 and was equal to 0.76 eV for x = 0.8. A decrease in the activation energy with an increase in the inert highly dispersed additive is typical for composite solid electrolytes and is described by partial salt amorphization and the contribution of the interfaces to the overall conductivity, the number of which increases with x [17,36]. At higher temperatures, >170 • C, close to the phase transition to I4 1 /acd phase, the activation energy changed to 0.45 eV for x = 0.75-0.9. The maximum conductivity reached high values of~7·10 −2 S/cm at 220 • C for x = 0.8. This composition corresponded to the complete filling of pores ( Figure 3) and was characterized by high conductivity values in low and high temperature ranges. This indicated high values of salt adhesion and meant that the selected highly dispersed silica matrix with the pore radius of 70 Å and uniform pore size distribution was optimal for the Et 4 NHSO 4 . In this case, not only did salt dispersion, disordering and amorphization occur; the high-temperature I4 1 /acd phase was also stabilized at low temperatures. The conductivity values for the studied systems are some of the highest among acid hydrogen sulfate composites [16]. Such size effects have been observed for a number of compounds. Phenomena of size effect, in which the dispersion of salts in the fine pores of an inert component (r pore < 100 Å) leads to qualitative changes in their bulk structure, including the appearance of hightemperature modifications, partial or complete amorphization and change in the number of thermodynamic characteristics, such as the enthalpies of the melting and phase transitions, and temperature, have been shown in previous studies [16][17][18][37][38][39][40][41]. For example, in the case of the SiO 2 matrix with a small pore radius (40 Å), only the high-temperature modification of KNO 3 and the amorphous CsCl phase were detected, which, according to the authors, were stable at room temperature for a long time. Figure 9 shows isotherms of conductivity as a function of the mole fraction of silica for different temperatures. high-temperature modifications, partial or complete amorphization and change in the number of thermodynamic characteristics, such as the enthalpies of the melting and phase transitions, and temperature, have been shown in previous studies [16][17][18][37][38][39][40][41]. For example, in the case of the SiO2 matrix with a small pore radius (40 Å), only the high-temperature modification of KNO3 and the amorphous CsCl phase were detected, which, according to the authors, were stable at room temperature for a long time. Figure 9 shows isotherms of conductivity as a function of the mole fraction of silica for different temperatures. The dependence of conductivity on the mole fraction reached a maximum, with a value up to three to four orders of magnitude higher than that of the pure Et4NHSO4, depending on composition and temperature. The conductivity reached a maximum at x = 0.8 at lower and higher temperatures, which was close to that for the filling of pores. At higher silica contents (x > 0.8), the pore volume exceeded markedly the total volume oc-  The dependence of conductivity on the mole fraction reached a maximum, with a value up to three to four orders of magnitude higher than that of the pure Et 4 NHSO 4 , depending on composition and temperature. The conductivity reached a maximum at x = 0.8 at lower and higher temperatures, which was close to that for the filling of pores. At higher silica contents (x > 0.8), the pore volume exceeded markedly the total volume occupied by the salt, and the conductivity decreased due to the conductor-insulator percolation effect. A significant size effect for the heterogeneous matrix influence on the electrotransport, structural and thermodynamic properties for plastic tetraalkyl ammonium hydrosulfate crystals was obtained for the first time. The effect was associated with the optimal morphology of silica with a pore size of 70 Å and a high energy of adhesion. Further research is important for more detailed elucidation of the mechanism of the formation of nanocomposites and their conductivity.

Conclusions
Composite solid electrolytes based on plastic tetraalkyl ammonium crystals and silica (1 − x)Et 4 NHSO 4− xSiO2 (x = 0.3-0.9) in a wide range of compositions were synthesized and investigated for the first time. The heterogeneous doping with silica changed markedly the thermodynamic, structural and electrotransport parameters of the salt. The morphology, pore size and surface nature of the silica were optimal for the introduction of Et 4 NHSO 4 , which determined the properties of the salt in the nanocomposites. Compositions close to the complete filling of pores were studied in more detail. Significant structural changes in the phase composition of Et 4 NHSO 4 in the composites were found, depending on the silica mole fraction and the degree of filling of the pore space of the matrix. The existence of two disordered phases, the original low-temperature (P2 1 /n) and high-temperature (I4 1 /acd) phases of Et 4 NHSO 4 , was observed under normal conditions in the nanocomposites. With increase in the silica mole fraction, the content of the high-temperature phase increased. At x = 0.8, which corresponds to the complete filling of the pores, the Et 4 NHSO 4 salt in the composites was mainly in the disordered high-temperature I4 1 /acd phase. A slight decrease in the Et 4 NHSO 4 unit cell parameters in the silica pores was observed. The thermodynamic, structural and electrotransport properties were in full agreement. The enthalpies of endoeffects of salt melting and phase transitions (160 • C) changed more significantly than the salt content of Et 4 NHSO 4 in the composites and completely disappeared with x = 0.9 due to salt amorphization. The intensity of absorption bands corresponding to P-O and hydrogen bond networks decreased significantly with x content, and the a.b. slightly shifted to higher frequencies as a result of the formation of weak hydrogen bonds between the salt and the matrix. The dependence of proton conductivity on mole fraction reached a maximum at x = 0.8, with the value up to three or four orders of magnitude higher than that of pure Et 4 NHSO 4 , depending on the composition and the temperature, which was close to that for complete pore filling. The conductivity of the 0.2Et 4 NHSO 4 -0.8SiO2 composite reached 7 * 10 −3 S/cm at 220 • C. A significant size effect of the influence of the heterogeneous matrix on the electrotransport, structural and thermodynamic properties of plastic tetraalkyl ammonium crystals was obtained for the first time and was due to the optimal morphology of silica with a pore size of 70Å and the energy of adhesion.

Conflicts of Interest:
The authors declare no conflict of interest.