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Proceeding Paper

Solvatochromic Behavior of Polarity Indicators in PILs and Their Mixtures with Molecular Solvents: Autoprotolysis and Its Relation to Acidity †

by
Claudia Guadalupe Adam
,
Lucía Gamba
and
Maria Virginia Bravo
*
Laboratory of Organic Physicochemistry, Institute of Applied Chemistry of the Littoral (IQAL) (UNL-CONICET), Faculty of Chemical Engineering, University National of Litoral, Santa Fe CP3000, Argentina
*
Author to whom correspondence should be addressed.
†
Presented at the 25th International Electronic Conference on Synthetic Organic Chemistry, 15–30 November 2021; Available online: https://ecsoc-25.sciforum.net/.
Chem. Proc. 2022, 8(1), 92; https://doi.org/10.3390/ecsoc-25-11746
Published: 14 November 2021
(This article belongs to the Proceedings of The 25th International Electronic Conference on Synthetic Organic Chemistry)
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Versions Notes

Abstract

:
It is interesting to know the behavior of Protic Ionic Liquids (PILs) within the binary mixture of molecular solvents, since it is usual to carry out processes such as organic and inorganic synthesis, or liquid–liquid extractions in the presence of another solvent. Moreover, on certain occasions, the absence of water is strictly required. In this sense, it is important to note that the addition of small amounts of IL to the molecular solvent allows a fine adjustment in its microscopic properties, obtaining “new solvent systems” with particular properties. The solvatochromic dyes are traditionally used as microscopic descriptors to determine the molecular microscopic properties of solvents, so we aim to re-evaluate the behavior of these probes and reconsider the validity of traditional polarity scales such as ET(30) in alkylammonium-based PILs, as well as in their mixtures with molecular solvents, knowing that the real composition of these PILs depends on the equilibrium of autoprotolysis. The characterization of systems was completed in terms of a change in the ∆pKa of the precursor species of a PIL. A thermal analysis was also employed to determine the acid strength’s role in an ion’s complete formation in pure PILs.

1. Introduction

Ionic liquids (ILs) have a great advantage over other types of solvents because of the wide versatility that they present with different applications (especially for electrochemical applications), due to their physicochemical properties, such as high ionic conductivity [1,2,3,4,5,6,7,8,9,10,11,12]. For this reason, they are called the ‘new materials’. In general, ILs can be classified into Protic ILs (PILs) and Aprotic ILs (AILs). PILs are a kind of IL, formed by the proton transfer from a Brønsted acid (AH) to a Brønsted base (B) [13,14]. One of the structural features of PILs is the formation of strong H bonds between cations and anions that define their unique physicochemical properties [15,16,17]. We have determined by cyclic voltammetry that neutral acidic and basic precursor species can coexist in PILs because of the equilibrium of autoprotolysis [18], which can affect its properties, such as viscosity, density, and conductivity.
Additionally, it is interesting to know the behavior of PILs within the binary mixture of molecular solvents, since it is usual to carry out certain processes such as organic and inorganic synthesis or liquid–liquid extractions in the presence of a second solvent. Moreover, on certain occasions the absence of water is strictly required. In this sense, it is important to mention that the addition of small amounts of IL to molecular solvent allows the optimization of its microscopic properties, obtaining “new solvent systems” [19,20]. Taking into account that solvatochromic indicators are traditionally used as microscopic descriptors to determine the molecular microscopic properties of solvents, [21] we aim to re-evaluate the behavior of solvatochromic probes and reconsider the validity of traditional polarity scales such as ET(30) [22,23] in alkylammonium-based PILs and in their mixtures with molecular solvents, knowing that the real composition of these PILs depends on the equilibrium of autoprotolysis.
We have detected certain challenges in the last years when working with IL, such as the effects of different acid-base equilibria between the free precursor species of the PILs and these indicators. Thus, the parameters that are obtained by these scales would be contaminated and would not represent reliable results within the normalized values that constitute the scales. This is also a problem, since the solvents that are used to construct these scales are molecular and do not involve ionic species. Complementing this, some authors [24] establish that it is possible to discuss the physicochemical properties in terms of a change in the ∆pKa of the precursor species of a PIL, in order to analyze the degree of proton transfer and thermal stability as a function of the change in the ∆pKa. In addition, thermal analyses are employed to relate the degree of the acidity in an ion’s complete formation in pure PILs.

2. Materials and Methods

For the analysis, we have selected Reichard’s dye (I) (Scheme 1) and the PILs: ethylammonium nitrate (NEA); diethylammonium nitrate (NDEA); and tributylammonium nitrate (NTBA), and the chemical precursors of the PILs are: ethylamine, diethylamine, tributylamine, and nitric acid.
The molecular solvents are methanol (MeOH) with hydrogen bond donor (HBD) and hydrogen bond acceptor (HBA) properties, and dimethylsulfoxide (DMSO) with HBA properties.
The response of the indicators was analyzed for different ranges of concentrations of the PILs in the binary mixtures (molar concentrations (C(M)) and molar fractions (x)), in order to evaluate the solvation effect of molecular solvents.

2.1. Synthesis of Ionic Liquids

The investigated PILs were synthesized, as detailed in the literature [8].

2.2. Microsensors and Spectroscopic Behavior—UV-Vis Spectroscopy

General Procedure: The spectroscopic data were obtained with a SHIMADZU UV-1800 spectrophotometer, equipped with a thermostatic cell holder. The pure solvents were mixed in appropriate proportions by weight to give binary solvent mixtures at different compositions. The temperature was maintained at 25 ± 0.1 °C. The concentrations of the indicators solutions were: 0.1 and 0.25 mM for the Reichardt’s dye (I).
The parameter ET(30) was determined from the wavelength corresponding to the maximum of the UV-Vis absorption band of betaine (I) and calculated by Equation (1):
E T ( 30 ) [ kcal · mol − 1 ] = hc ν ˜ N = 2.859 × 10 − 3 ν ˜ ( cm − 1 )
where h is Planck’s constant, c is the speed of light, N is Avogadro’s number, and n is the wave number in cm−1. This equation relates the electronic transition in the probe to the corresponding intramolecular charge transfer energy in kcal/mol.

2.3. Thermogravimetric Analysis (TGA)

The decomposition temperatures (Td) of the PILs were determined by using a thermogravimetric analyzer (TGA) in the thermal stability analysis [25,26,27,28,29]. An approximate 10 mg of sample was weighted in a crucible pan and the analysis was performed in the temperature range of 30–650 °C under 20 mL/min of nitrogen flow with a heating rate of 10 °C/min.

3. Results and Discussion

3.1. Solvatochromic Behavior of the Reichardt´s Dye (I)

3.1.1. Range of Mole Fractions (x)

Figure 1 shows that there are no significant changes in the spectrum from xPIL ~0.2 to 1 for dye I, which is sensitive to polarity and acidity. This possibly indicates that the ionic lattice is organized, and as a consequence, the solvation effect of the molecular solvent is negligible.
Taking as a reference the observed behavior of NTBA by cyclic voltammetry, [8] where NO free molecular species were detected for this PIL in its pure state, we can associate the behavior of the probe with molar fractions that are close to 1 (xPIL~1) as an indicator of a microenvironment ionic polar.
Clearly, from xPIL ~0.2 to 1, the interaction with dye I is governed by the ion pair of the PILs, independently of the molecular solvent, as shown in Figure 2 for NEA and NTBA. This would also indicate that the effect of ionic species on the probe prevails and not the mixed solvent (SM) or the PIL-SM intersolvent complex. This comparison could not be made for NDEA due to its limited solubility in the molecular solvents that were compared.
On the other hand, we observe a shift to lower values of λ as the PIL concentration increases for lower molar fractions of the PIL in the range 0 < x < 0.3. This could indicate that initially there are higher concentrations of free molecular species in the equilibrium of autoprotolysis due to a greater solvation effect by the molecular solvents that are found in a higher proportion.

3.1.2. Solvatochromic Behavior of Dye I in the Range of Mole Fractions

Figure 3 shows the response patterns of the factor ET(30) as a function of the xLI for all the solvent systems under study. The analysis was developed according to the deviation from the ideality of the curves “property vs. solvent composition”.
Generally, in this study, the same response pattern could be observed for the ET(30) parameter (Figure 3). This observation could be related to the possibility of forming PIL–SM complexes. This possibility produces ionic species with different degrees of association in respect to the Pure PIL. The highest percentage of change in the properties was observed up to a value of xPIs~0.2.
It could also be noted that certain solvent systems showed synergism on the parameter and other mixtures showed positive deviation with respect to the ideal behavior. This property depends on the cation; for example, for NTBA, synergism was observed with the solvents MeOH and DMSO. In this case, we can associate the lowest polarity values ET(30) corresponding to a microenvironment with high ionic character when xNTBA ~1.
From the analysis of the solvatochromic scales, we deem that it would not be appropriate to analyze the values of a normalized ET(30) parameter (ETN), since ionic organic compounds are not involved in the normalization calculation. If it has a series of ET(30) values for several LIs, a new scale could be proposed.

3.1.3. Range of Molar Concentration (C) vs. x

In this study, the same behavior was observed in both solvents. We observed the protonation of the indicator by the acidic species precursor of the PILs in each solvent system for the C (M) range. However, surprisingly, we have detected that the indicator´s band returns as a shoulder in all binary solvent mixtures of type [PILs + Molecular Solvent] here studied, when the I microsensor concentration is about 0.4 mM and the PILs concentration in the binary mixture is the order molar fraction. Figure 4 shows the behavior of Reichardt’s dye (I) for the ([NDEA] + MeOH/DMSO) system binary for both ranges of working concentrations. This system was taken as a model, but similar behaviors were observed for all the binary systems here studied.
The behavior of the probe in the presence of PILs in the range of molar concentrations is manifested as an indicator signal that turns off. This is clearly due to the presence of free acid in the medium and the consequent protonation of the indicator that absorbs at lower wavelengths.
When the [PILs] is in molar fraction, the dye signal returns to ‘switching-on’. At first, this unexpected behavior could, in principle, be explicated through the equilibrium of autoprotolysis at different amounts of PILs.

3.2. ∆pKa

Some authors have analyzed the physicochemical properties in terms of a change in the ∆pKa of its precursor species ( Δ pKa solvent = pKa AmH + / B − pKa HA / A ) [14]. They have also analyzed the applicability of the relationships between different parameters with the ∆pKa of the PILs to establish a generalized concept, in order to understand the physicochemical properties. In this analysis, special emphasis is given to the degree of proton transfer and thermal stability depending on the change in the ∆pKa. Based on the above, we may find some relationship in molecular solvents between the parameters that are determined in our work and the ∆pKa of the PIls that are analyzed here. Consequently, we could be able to analyze the degree of ion pair formation that these PILs present in MeOH and DMSO, in order to apply them to non-aqueous systems. This is important because most of the reported data were obtained in aqueous systems.
In addition, Angell et al. specifically demonstrated that an ∆pKa of >10 is required to ensure sufficient proton transfer to produce highly ionized PILs [30]. So, if the PILs have a high ∆pKa, then their ionic behavior will be high as well. This may indicate complete proton transfer and weaker interactions between the cation and the anion. However, MacFarlane et al. proposed that ∆pKa = 4 is sufficient for the completion of proton transfer [31]. ILs with lower ∆pKa values indicate incomplete proton transfer and the formation of ion-pairs or ion-aggregates between the protonated cation and the anion, similar to AILs [32]. These PILs with a low ∆pKa exhibit poor ionic behavior, indicating the hydrogen bonding interaction between the cation and the anion through the N–H bond as a result of an incomplete proton transfer [24].
Knowing the above, we can compare the ∆pKa of the PILs in MeOH and DMSO (Table 1).
We obtained an ∆pKa > 10 for the PILs in water and DMSO, which indicates a sufficient proton transfer to produce a PIL with a high ionic character, while in MeOH, the character of the IL as an ionic pair is evidently lower. This is consistent with the highest ET(30) values that are obtained for the MeOH solvent in the range of xPILs between 0 and 0.2, corresponding to a poor ionic character. The above also agrees with the lower value of pKa that is determined by the indicator method (Table 2) in MeOH in respect to DMSO, due to the greater dissociation of the PILs in MeOH generating free HNO3. We could corroborate the high degree of ionization that is observed in DMSO by comparing the pKa values of HNO3 (Table 1), being more acidic in DMSO. However, these PILs with high pKa values showed low amounts of free acid in this solvent.
The previously published pKa values show that in DBH solvents, such as MeOH, there is a shift from the equilibrium of autoprotolysis towards molecular species, while DBH solvents such as DMSO cause the opposite effect, favoring the existence of PILs mainly as ionic pairs.
Some authors propose that PILs with weaker bases are poor ionic liquids [38,39,40,41]. If we compare the different cations EA, DEA, and TBA for the same acid, we corroborate that for the strongest amine with TBA as a base, the PILs with the highest ionic character are obtained in the pure state. However, the presence of molecular solvents modifies this fact due to the solvation effect, with NTBAs being the most acidic PILs in both solvents.

3.3. TGA

Some authors have established that strong hydrogen bonds between the cation and anion are present in PILs through N–H bonds, in addition to inter-ionic interactions such as Coulombic interactions and van der Waals forces, which are seen in aprotic ionic liquids (AILs) [42,43,44]. Furthermore, they have demonstrated that the bond strength may vary by changing the structure and strength of the constituent acids and bases of the PILs. The successive breaking of hydrogen bonds with temperature explains the characteristic properties of PILs, such as a relatively low ionic character and its decrease with temperature [45]. In this sense, the study of the thermal analysis of a substance is crucial, as it provides information on the behavior of a compound with the variation of the temperature.
The thermal stability of the PIL was examined by a thermogravimetric analysis (TGA), and the TGA profiles are graphically presented in Figure 5. The TGA was performed at scanning rate of 10 °C/min. In the TGA study, the main factor of thermal stability depends on the strength of the heteroatom–carbon and heteroatom–hydrogen bond [46].
The Td (decomposition temperature) was determined as the initial temperature at which weight loss began in the TGA analysis, also called the initial decomposition. All the data were fitted using the the Boltzmann equation. Figure 5 shows the results that were obtained in TGA for PILs.
In general, the studied PILs showed thermal stabilities in the range of approximately 25 to 90 °C. For the analyses of the PILs, it was observed that the Td increased as the substitution of the cation increased in the N, which corresponded to a greater thermal stability for the NTBA. Greater thermal stability means that there is a lower amount of free precursor species of PILs in the autoprotolysis equilibrium.
The TGA profiles of the studied PILs indicate a one-step decomposition temperature for all ammonium-based PILs, except for NEA. In this case, it is a two-stage decomposition. In the first stage, about 10% decomposed at 93.94 °C and the other 90% disappeared at 300 °C in the second stage.

3.4. Correlations

Td vs. ∆pKa and pKa

We can analyze the physicochemical properties in terms of changes in the ∆pKa of PILs. The PILs with a low ∆pKa indicate that free acids and bases are present in the system. In this sense, to understand the physicochemical properties and the behavior of these PILs, we could analyze the relationship between the experimental weight loss that indicates their thermal stability and the changes in ∆pKa for the MeOH and DMSO solvents. Special emphasis was given to the degree of proton transfer and thermal stability depending on the change in the ∆pKa. Additionally, we were able to compare the previous parameters with the pKa data that were previously determined with the indicator method.
It is interesting to observe the relationship between the different parameters that are obtained, in order to compare the information that they provide on the state of the PILs that are studied in the molecular solvents MeOH and DMSO. For this, these parameters are plotted and shown in Figure 6.
Figure 6 shows the NTBA with a higher Td, indicating greater thermal stability; therefore, in the pure state, they would present negligible amounts of free precursor species corresponding to a high ionic character. However, when PILs are found in molar concentrations in molecular solvents, their autoprotolysis equilibrium is affected by the nature of the molecular solvent and its acid-base properties by free precursor species, resulting in more basic or more acidic global systems. This can be seen in their pKa values, which are lower in MeOH in relation to DMSO. For this reason, we observed a marked solvent effect on the ionization of PILs, where the highest values of ∆pKa or higher ionic character were conditioned with high values of pKa (∆pKaDMSO > ∆pKaMeOH y pKaDMSO > pKaMeOH)).

4. Conclusions

For the range of molar fractions from xPIL ~0.2 to 1, no considerable changes are observed in the spectrum of sensor I. This may indicate that the ionic lattice is organized, and as a consequence, the effect of the molecular solvent and therefore its solvation effect is negligible. For the range of molar concentration, we observed the protonation of indicator I by the acidic species that were the precursor of the PILs in each solvent. On the other hand, an increment in the capacity of the molecular solvent HBD resulted in an increment in the acidity of the PILs, while showing a weak cation–anion interaction, and the proton being more available for solvation.
High ∆pKa values ensure a PIL with a high ion pair character in DMSO, while the opposite is observed in MeOH. This agrees with the reported values of pKaPILs that are determined by the indicator method [21], where an increment in the H-bonding capacity of the molecular solvent results in a decrease in these values. For the pure PILs, it was observed that Td increased as the substitution in the N of the cation increased, which corresponded to a greater thermal stability for NTBA, being mainly found as an ionic pair. This was consistent with what was determined by cyclic voltammetry, where no neutral free species were detected for this PIL. However, in diluted solutions, the effect of molecular solvents in the solvation process for NTBA is evidenced, presenting the highest acidity values.

Author Contributions

C.G.A. is the director of the research project that funds this work. She is the researcher responsible and actually she works in the design of the synthesis of ionic liquids for its use in different applications. She has also carried out different investigations in the study of solvent and solvatochromic proves. M.V.B. has researched the design and synthesis of ionic liquids, as well as solvent studies and solvatochromic indicators. Currently she is working on modified β-cyclodextrins with ionic liquids. L.G. is working with a scientific initiation scholarship in our group. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by Research and Development Project: “New ionic materials on the structural basis of ionic liquids. Synthesis and characterization. Application to various physicochemical processes”. CAI+D. PIC-UNL. From 02-2021 to 02-2023. Project No 50620190100106LI. Amount $180,000 Director: Dr. Claudia G. Adam. Co-Director: Dr. Graciela Fortunato.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

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Chemproc 08 00092 sch001 550
Scheme 1. Structure of the Reichardt’s dye (I): betaine 2,6-diphenyl-4-(2,4,6-triphenyl-1-pyridinium)-1-phenolate.
Scheme 1. Structure of the Reichardt’s dye (I): betaine 2,6-diphenyl-4-(2,4,6-triphenyl-1-pyridinium)-1-phenolate.
Chemproc 08 00092 sch001
Chemproc 08 00092 g001 550
Figure 1. Variation of λ (nm) of I vs. the xPIL in the mixtures: (a) (MeOH + PIL) y (b) (DMSO + PIL). ( Chemproc 08 00092 i001 NEA, Chemproc 08 00092 i003 NDEA, Chemproc 08 00092 i002 NTBA).
Figure 1. Variation of λ (nm) of I vs. the xPIL in the mixtures: (a) (MeOH + PIL) y (b) (DMSO + PIL). ( Chemproc 08 00092 i001 NEA, Chemproc 08 00092 i003 NDEA, Chemproc 08 00092 i002 NTBA).
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Figure 2. Variation of the λ (nm) of the indicator I vs. the xLI for NEA and NTBA in: (a) Chemproc 08 00092 i003 MeOH y (b) Chemproc 08 00092 i002 DMSO.
Figure 2. Variation of the λ (nm) of the indicator I vs. the xLI for NEA and NTBA in: (a) Chemproc 08 00092 i003 MeOH y (b) Chemproc 08 00092 i002 DMSO.
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Chemproc 08 00092 g003 550
Figure 3. Variation of parameter ET(30) vs. xPIL in mixtures: (a) (MeOH + PIL) y (b) (DMSO + PIL). ( Chemproc 08 00092 i001 NEA, Chemproc 08 00092 i003 NDEA, Chemproc 08 00092 i002 NTBA).
Figure 3. Variation of parameter ET(30) vs. xPIL in mixtures: (a) (MeOH + PIL) y (b) (DMSO + PIL). ( Chemproc 08 00092 i001 NEA, Chemproc 08 00092 i003 NDEA, Chemproc 08 00092 i002 NTBA).
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Figure 4. The UV/Vis absorption spectra of Reichardt’s dye dissolved for (a) [I] = 4 × 10−4 M in MeOH, after addition of increasing amounts of [NDEA] in concentration (mol L−1) (—) and mole fraction (- - - ). (b) [I] = 2.5 × 10−4 M in DMSO, after addition of increasing amounts of [NDEA] in concentration (mol L−1) and mole fraction.
Figure 4. The UV/Vis absorption spectra of Reichardt’s dye dissolved for (a) [I] = 4 × 10−4 M in MeOH, after addition of increasing amounts of [NDEA] in concentration (mol L−1) (—) and mole fraction (- - - ). (b) [I] = 2.5 × 10−4 M in DMSO, after addition of increasing amounts of [NDEA] in concentration (mol L−1) and mole fraction.
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Figure 5. TG curves of PILs recorded at 10 °C/min for NEA, NDEA, and NTBA.
Figure 5. TG curves of PILs recorded at 10 °C/min for NEA, NDEA, and NTBA.
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Figure 6. Variation of pKa, ∆pKa and Td values for the PILs analyzed.
Figure 6. Variation of pKa, ∆pKa and Td values for the PILs analyzed.
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Table
Table 1. Calculated ∆pKa values for PILs in MeOH and DMSO. pka values of amines and HNO3 in MeOH, DMSO and water were taken from reference [33,34,35,36,37].
Table 1. Calculated ∆pKa values for PILs in MeOH and DMSO. pka values of amines and HNO3 in MeOH, DMSO and water were taken from reference [33,34,35,36,37].
SpeciespKawpKaMeOHpKaDMSOΔpKaWΔpKaMeOHΔpKaDMSO
HNO3−1.33.18−1.72Am/HNO3
EA10.6311.0010.9011.937.8212.62
DEA10.9811.0010.5012.287.8212.22
TBA10.8910.788.412.197.6010.12
Table
Table 2. Acidity constants for selected PILs in MeOH and DMSO [21].
Table 2. Acidity constants for selected PILs in MeOH and DMSO [21].
PILspKaPIL
MeOHDMSO
NEA5.388.67
NDEA5.217.87
NTBA4.346.33
pKadye5.108.90
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Adam, C.G.; Gamba, L.; Bravo, M.V. Solvatochromic Behavior of Polarity Indicators in PILs and Their Mixtures with Molecular Solvents: Autoprotolysis and Its Relation to Acidity. Chem. Proc. 2022, 8, 92. https://doi.org/10.3390/ecsoc-25-11746

AMA Style

Adam CG, Gamba L, Bravo MV. Solvatochromic Behavior of Polarity Indicators in PILs and Their Mixtures with Molecular Solvents: Autoprotolysis and Its Relation to Acidity. Chemistry Proceedings. 2022; 8(1):92. https://doi.org/10.3390/ecsoc-25-11746

Chicago/Turabian Style

Adam, Claudia Guadalupe, Lucía Gamba, and Maria Virginia Bravo. 2022. "Solvatochromic Behavior of Polarity Indicators in PILs and Their Mixtures with Molecular Solvents: Autoprotolysis and Its Relation to Acidity" Chemistry Proceedings 8, no. 1: 92. https://doi.org/10.3390/ecsoc-25-11746

APA Style

Adam, C. G., Gamba, L., & Bravo, M. V. (2022). Solvatochromic Behavior of Polarity Indicators in PILs and Their Mixtures with Molecular Solvents: Autoprotolysis and Its Relation to Acidity. Chemistry Proceedings, 8(1), 92. https://doi.org/10.3390/ecsoc-25-11746

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