Solvatochromism in Solvent Mixtures: A Practical Solution for a Complex Problem

: Many reactions are carried out in solvent mixtures, mainly because of practical reasons. For example, E2 eliminations are favored over S N 2 substitutions in aqueous organic solvents because the bases are desolvated. This example raises the question: how do we chose binary solvents to favor reaction outcomes? This important question is deceptively simple because it requires that we understand the details of all interactions within the system. Solvatochromism (solvent-dependent color change of a substance) has contributed a great deal to answer this difficult question, because it gives information on the interactions between solvents, solute-solvent, and presumably transition state-solvent. This wealth of information is achieved by simple spectroscopic measurements of selected (solvatochromic) substances, or probes . An important outcome of solvatochromism is that the probe solvation layer composition is almost always different from that of bulk mixed solvent. In principle, this difference can be exploited to “tune” the composition of solvent mixture to favor the reaction outcome. This minireview addresses the use of solvatochromic probes to quantify solute-solvent interactions, leading to a better understanding of the complex effects of solvent mixtures on chemical phenomena. Because of their extensive use in chemistry, we focus on binary mixtures containing protic-, and protic-dipolar aprotic solvents.


Reasons for Using Mixed Solvents in Chemistry
Solvent mixtures are extensively employed in chemistry for practical reasons.For example, the solubilities of inorganic bases, such as KOH, and other electrolytes in alcohols are enhanced in presence of water [1,2].Cellulose that is insoluble in water is, however, readily soluble in some aqueous electrolyte solutions [3], water-DMSO mixtures [4], and mixtures of ionic liquids-molecular solvents (ILs-MSs) [5][6][7][8]].In the latter example, cellulose dissolution is attributed to the disruption of the strong hydrogen-bonding (H-bonding) between the hydroxyl groups of the anhydroglucose units, as well as to the hydrophobic interactions between cellulose chains, as shown in Figure 1a (IL-DMSO).Consequently, addition of protic non-solvents to solutions of cellulose in IL-MS causes biopolymer precipitation because the non-solvent efficiently solvates the ions of the IL (Figure 1b).
In addition to enhanced biopolymer solubility, the use of mixed solvents also causes noticeable changes in the physicochemical properties, such as a reduction in viscosity, leading to better heat and mass transfer, as shown by Figure 2a,c.(a) A simplified scheme for cellulose dissolution in ionic liquid-DMSO.The dissolution is attributed to interactions of its hydroxyl groups with the ions of the ionic the dipole of DMSO.Reproduced with permission from [9].(b) Effects of the addition non-solvent (such as water or ethanol) on the dissolution of cellulose IL-dipolar solven of the non-solvent leads to cellulose precipitation.Reprinted with permission from [7].
In addition to enhanced biopolymer solubility, the use of mixed solvents a noticeable changes in the physicochemical properties, such as a reduction in leading to better heat and mass transfer, as shown by Figure 2a,c.(a) A simplified scheme for cellulose dissolution in ionic liquid-DMSO.The biopolymer dissolution is attributed to interactions of its hydroxyl groups with the ions of the ionic liquid and the dipole of DMSO.Reproduced with permission from [9].(b) Effects of the addition of a protic non-solvent (such as water or ethanol) on the dissolution of cellulose IL-dipolar solvent.Addition of the non-solvent leads to cellulose precipitation.Reprinted with permission from [7].Reprinted with permission from [11].(c) Effects of increasing the mole fraction of DMSO (χS) on the viscosity of cotton cellulose in binary mixtures of DMSO with the ILs AlMeImCl (1-allyl-3-methylimidazolium chloride) and BuMeImCl.The insert is the logarithm-linear plot of the reduced viscosity ratio versus DMSO mole fraction at 25 °C Reprinted with permission from [12].

A Rationale for Effects of Mixed Solvents on Chemical Phenomena
How do we explain these interesting and very useful effects of binary solvent mixtures on diverse chemical phenomena?While deceptively simple, this question cannot be answered in a straightforward manner.Consider, for example, the fact that most physicochemical properties of binary mixtures are not ideal.That is, the property of the binary mixture does not vary in a simple way as a function of binary solvent composition, as shown in Figure 3a-c.Reprinted with permission from [11].(c) Effects of increasing the mole fraction of DMSO (χS) on the viscosity of cotton cellulose in binary mixtures of DMSO with the ILs AlMeImCl (1-allyl-3methylimidazolium chloride) and BuMeImCl.The insert is the logarithm-linear plot of the reduced viscosity ratio versus DMSO mole fraction at 25 °C Reprinted with permission from [12].

A Rationale for Effects of Mixed Solvents on Chemical Phenomena
How do we explain these interesting and very useful effects of binary solvent mixtures on diverse chemical phenomena?While deceptively simple, this question cannot be answered in a straightforward manner.Consider, for example, the fact that most physicochemical properties of binary mixtures are not ideal.That is, the property of the binary mixture does not vary in a simple way as a function of binary solvent composition, as shown in Figure 3a-c.

A Rationale for Effects of Mixed Solvents on Chemical Phenomena
How do we explain these interesting and very useful effects of binary solvent mixtures on diverse chemical phenomena?While deceptively simple, this question cannot be answered in a straightforward manner.Consider, for example, the fact that most physicochemical properties of binary mixtures are not ideal.That is, the property of the binary mixture does not vary in a simple way as a function of binary solvent composition, as shown in Figure 3a-c.
The reason behind this non-ideality is clearly the interactions between components of the binary solvent mixture.To a first approximation, one expects that the composition of the solvation layer of a dissolved substance (which we will refer to as "probe") should be the same as that of bulk binary mixture.Consequently, the same explanations given for bulk binary mixtures should apply to the solvation layers of the dissolved probes.This simple view, however, does not hold in most cases because probe-solvent nonspecific and specific interactions were not taken into consideration.These interactions change the composition of the solvation layers relative to bulk solvent mixtures, as shown below.The reason behind this non-ideality is clearly the interactions between components of the binary solvent mixture.To a first approximation, one expects that the composition of the solvation layer of a dissolved substance (which we will refer to as "probe") should be the same as that of bulk binary mixture.Consequently, the same explanations given for bulk binary mixtures should apply to the solvation layers of the dissolved probes.This simple view, however, does not hold in most cases because probe-solvent nonspecific and specific interactions were not taken into consideration.These interactions change the composition of the solvation layers relative to bulk solvent mixtures, as shown below.
The composition of the solvation layer of a probe may deviate from that of an (already non-ideal) bulk solvent mixture due to the so-called "preferential solvation" of the probe by one component of the mixture (Figure 4).In principle, this phenomenon includes contributions from probe-independent "dielectric enrichment", and probe-solvent interactions.

A Rationale for Effects of Mixed Solvents on Chemical Phenomena
How do we explain these interesting and very useful effects of binary solvent mixtures on diverse chemical phenomena?While deceptively simple, this question cannot be answered in a straightforward manner.Consider, for example, the fact that most physicochemical properties of binary mixtures are not ideal.That is, the property of the binary mixture does not vary in a simple way as a function of binary solvent composition, as shown in Figure 3a-c.The composition of the solvation layer of a probe may deviate from that of an (already non-ideal) bulk solvent mixture due to the so-called "preferential solvation" of the probe by one component of the mixture (Figure 4).In principle, this phenomenon includes contributions from probe-independent "dielectric enrichment", and probe-solvent interactions.The first mechanism is operative in mixtures of nonpolar/low polar solvents, such as cyclohexane-THF (Tetrahydrofuran).It denotes enrichment of the probe solvation layer (relative to that of bulk solvent mixture) by the component of larger dielectric constant (or relative permittivity), due to non-specific probe dipole-solvent dipole interactions [14][15][16].
solvents, HOH…O(H)R and HOH…O(H)=S(CH3)2 [17]; this turns analysis of the solvation data more complex.In summary, most significant consequence of preferential solvation is that compositions of the solvation layers of most probes are different from those of the corresponding bulk solvent mixtures; these composition differences are probe-, and temperature-dependent [18,19].How do we calculate the "effective" (or local) composition of the solvation layer of a probe?Several techniques were employed to solve this problem, including FTIR [20], resonance Raman spectroscopy [21], and X-ray diffraction (for solvated crystals) [22].It is our view that the most useful approach is to use solvatochromic indicators as models for the compounds of interest, e.g., reactants.Solvatochromic probes are substances whose absorption or emission spectra are sensitively dependent on the solvent or the composition of solvent mixtures (Figure 5).The reason for solvatochromism is that the energy difference between the probe s ground and excited states is sensitively affected by probe-solvent interactions, leading to medium-dependent values of λmax, and hence a change in solution color.For most probes, the solvatochomism is negative, meaning there is a hypsochromic shift of the longest wavelength absorption band with increasing medium polarity.The reason is that solvents stabilize the zwitterionic ground state much more than the diradical excited state (see Figure 6 for light-induced transition of the probe t-Bu5RB).The second solvation mechanism is dominant in protic solvents (such as aqueous alcohols) and their mixtures with strongly dipolar solvents (water-DMSO, alcohol-DMF, etc.).It is essentially due to solute-solvent H-bonding and hydrophobic interactions.One additional complication is that solvent-solvent H-bonding generates an additional or "mixed" solvent species that should be considered.For example, in mixtures of water (W) and alcohol (ROH), and W-DMSO, we have in solution both the parent and the mixed solvents, HOH. ..O(H)R and HOH. ..O(H)=S(CH 3 ) 2 [17]; this turns analysis of the solvation data more complex.In summary, most significant consequence of preferential solvation is that compositions of the solvation layers of most probes are different from those of the corresponding bulk solvent mixtures; these composition differences are probe-, and temperature-dependent [18,19].
How do we calculate the "effective" (or local) composition of the solvation layer of a probe?Several techniques were employed to solve this problem, including FTIR [20], resonance Raman spectroscopy [21], and X-ray diffraction (for solvated crystals) [22].It is our view that the most useful approach is to use solvatochromic indicators as models for the compounds of interest, e.g., reactants.Solvatochromic probes are substances whose absorption or emission spectra are sensitively dependent on the solvent or the composition of solvent mixtures (Figure 5).The reason for solvatochromism is that the energy difference between the probe's ground and excited states is sensitively affected by probe-solvent interactions, leading to medium-dependent values of λ max , and hence a change in solution color.For most probes, the solvatochomism is negative, meaning there is a hypsochromic shift of the longest wavelength absorption band with increasing medium polarity.The reason is that solvents stabilize the zwitterionic ground state much more than the diradical excited state (see Figure 6 for light-induced transition of the probe t-Bu 5 RB).The latter corresponds to a so-called FranckCondon excited state, because the time scale of the electronic excitation (ca. 10 −15 s) is much shorter than that required for the solvent molecule to reorient in order to stabilize the probe's excited state.The energy of this transition furnishes the solvatochromic property of interest, vide infra.
Liquids 2024, 4, FOR PEER REVIEW 6 The latter corresponds to a so-called FranckCondon excited state, because the time scale of the electronic excitation (ca. 10 −15 s) is much shorter than that required for the solvent molecule to reorient in order to stabilize the probe s excited state.The energy of this transition furnishes the solvatochromic property of interest, vide infra.and dichloromethane [23].Part (b) is that for the empirical polarity probe t-Bu5RB, Figure 6), in (mineral) diesel oil and its mixtures with 25, 50, 75% bioethanol, and in pure bioethanol, respectively.Reprinted with permission from [24].Part (c) shows the dependence of solution color on the structure of the solvatochromic probe.Reprinted with permission from [25].The structures and names of these probes are shown in Figure 7. Reprinted with permission from [24].Part (c) shows the dependence of solution color on the structure of the solvatochromic probe.Reprinted with permission from [25].The structures and names of these probes are shown in Figure 7.
This approach was advanced thanks to the work of professor C. Reichardt, initially under the supervision of professor K. Dimroth at Marburg university [26,27].The experimental part is relatively simple: register the UV-Vis spectrum of a solvatochromic probe → calculate the value of λ max of a specific peak (the longest wavelength, due to intermolecular charge-transfer within the probe) → use the value of λ max to calculate the desired property, or descriptor, of the solvent or solvent mixture.The power of solvatochromism is that it can be employed to calculate the overall (or empirical) solvent polarity scale, E T (in kcal/mol), as well as the individual solvent descriptors that contribute to E T , namely solvent Lewis acidity (SA), solvent Lewis basicity (SB), solvent dipolarity (SD), and solvent polarizability (SP), where S refers to solvent.Other abbreviations that were employed for designating these descriptors include SdP and SP for solvent dipolarity and polarizability, respectively.For consistency, however, we use two letters to designate each solvent descriptor.
Equation (1) shows the relationship of these solvent descriptors: where E T (probe) 0 corresponds to gas phase, the descriptors (SA, SB, SD, SP) are those defined above, and (a, b, d, and p) are the corresponding regression coefficients.Figure 7 shows some solvatochromic probes used to calculate the descriptors of Equation ( 1).In the Taft-Kamlet-Abboud approach, similar solvatochromic parameters and different symbols were employed to describe probe-solvent interactions, α, β, and π* for solvent Lewis acidity, Lewis basicity, and (combined) dipolarity/polarizability [28].The signs of the coefficients in Equation ( 1) indicate whether the property of the solvent considered increases (positive sign) or decreases (negative sign) the empirical solvent polarity [29].This approach was advanced thanks to the work of professor C. Reichardt, under the supervision of professor K. Dimroth at Marburg university [26,27].Th mental part is relatively simple: register the UV-Vis spectrum of a solvatochrom → calculate the value of λmax of a specific peak (the longest wavelength, due to int ular charge-transfer within the probe) → use the value of λmax to calculate the property, or descriptor, of the solvent or solvent mixture.The power of solvatoch is that it can be employed to calculate the overall (or empirical) solvent polarity (in kcal/mol), as well as the individual solvent descriptors that contribute to ET solvent Lewis acidity (SA), solvent Lewis basicity (SB), solvent dipolarity (SD), and polarizability (SP), where S refers to solvent.Other abbreviations that were empl designating these descriptors include SdP and SP for solvent dipolarity and polar

A Model for the Solvation of Probes
A solvation model is required to calculate the local concentration of the species in the solvating layer of the probe.For simplicity, we consider a W-ROH mixture, containing a certain water mole fraction, χ W .We address the question of preferential solvation by using a series of exchange equilibria between the solvent species in the bulk binary mixture and those in the probe solvation layer.Any realistic model should consider, therefore, the exchange of the three solvents (W, ROH, and W-ROH) between the bulk solvent and the probe solvation layer, where the equilibria involving the mixed solvent are given by Equations ( 2)-( 4 Note that (m) is not the solvation number of the probe; it represents the number of solvent molecules whose exchange in the probe solvation layer affects its solvatochromism; usually, the value of (m) is close to unity.For example, for the solvation of WB in mixtures of water with 4 alcohols (methanol, 1-propanol, 2-propanol, and 2-methylethanol), the calculated values of (m) range from 1.06 to 1.70 [30].With this proviso (meaning of (m)), addressing the important point of probe-dependent volume of the solvation layer is not required for the analysis shown below.Additionally, using this model, one should be able to calculate the probe-induced preferential solvation, as expressed by the fractionation factor (φ) ,which represents the equilibrium constant for solvent exchange between the bulk binary mixture and the probe solvation layer.This model has been elaborated; Equations ( 5)-( 7) are for W-ROH, where (Bk) refers to bulk solvent:  (7) In Equation ( 5), φ W/ROH describes the preference of (W) for the probe solvation layer relative to bulk solvent mixture.Values of φ W/ROH > 1 indicate that the probe solvation layer is richer in (W) than the bulk solvent; the inverse is true for φ W/ROH < 1.In absence of preferential solvation, φ W/ROH is unity, indicating that solvent composition in the probe solvation layer is the same as that of the bulk solvent.The same line of reasoning applies to φ ROH-W/ROH (mixed solvent displaces ROH) and φ ROH-W/W (mixed solvent displaces W), as depicted in Equations ( 6) and (7).
The use of 1:1 stoichiometry for ROH-W is an assumption that has been employed elsewhere [31][32][33][34][35][36][37].Mixed solvents with a stoichiometry other than 1:1 can be regarded, to a good approximation, as mixtures of the 1:1 structure plus excess of a pure solvent.We stress that taking into account the presence of mixed solvents is more than a practical and convenient assumption; the presence of such species has been successfully employed in fitting results of spectroscopic techniques that are particularly suitable to determine the stoichiometry and association constant of solvents, e.g., NMR [38][39][40] and FTIR [41][42][43].The observed solvatochromic property, such as the E T Obs (probe), can be then calculated by iteration from Equations ( 8) and ( 9): refer to the number of molecules in the probe solvation layer that affects its solvatochromic response, and effective mole fractions of the appropriate species in bulk mixed solvent, respectively.Note that these effective mole fractions differ from the analytical or starting mole fractions due to the formation of the mixed solvent, e. are calculated from the dependence of a physical property (e.g., density on solution composition) by using the association model discussed by Katz et al. [44][45][46]; a list of the association constants of W-ROH has been published [47].
Figures 8 and 9 show the dependence of the effective concentrations of solvent species on the analytical mole fractions of the two solvents.
By using data such as those shown in Figure 8, and Equations ( 8) and ( 9), one can calculate the dependence of a solvatochromic property (e.g., solvent polarity or E T (probe)) as a function of binary solvent composition at a fixed temperature, or at a series of temperatures (referred to as thermo-solvatochromism), as shown in Figure 9.
The preceding discussion shows that it is relatively simple to calculate medium descriptors (e.g., SA and SB) for pure and mixed solvents; the use of the appropriate solvation model permits calculation of the composition of the solvation layers of the solvatochromic probes dissolved therein.Although there are a large number of solvatochromic probes that are employed to calculate the solvent descriptors, the results are consistent when different probes were employed.This is demonstrated by application of Equation ( 1) to a series of ILs, where the calculated empirical solvent polarities using the RB (Reichardt betaine-2,6diphenyl-4-(2,4,6-triphenylpyridinium-1-yl) phenolate) probe correlate linearly with the calculated values, based on the 4 descriptors (SA, SB, SD, SP), which were calculated using different solvatochromic probes (Figure 10).Values of φ were also calculated at different temperatures, showing the effect of temperature on the composition of the probe solvation layer (thermo-solvatochromism).
where (m),   ; ,   ; , and    ; refer to the number of molecules in the probe solvation layer that affects its solvatochromic response, and effective mole fractions of the appropriate species in bulk mixed solvent, respectively.Note that these effective mole fractions differ from the analytical or starting mole fractions due to the formation of the mixed solvent, e.g., ROH-W.The input data to solve these equations include    ,    ,    , and    , along with initial estimates of (m),     and the appropriate solvent fractionation factors.The values of   ; ,   ; , and    ; are calculated from the dependence of a physical property (e.g., density on solution composition) by using the association model discussed by Katz et al. [44][45][46]; a list of the association constants of W-ROH has been published [47].Figures 8 and 9 show the dependence of the effective concentrations of solvent species on the analytical mole fractions of the two solvents.The symbols employed are , ■, ▲ for IL, W, and the IL-W 1:1 complex, respectively.Reprinted with permission from [49].
Liquids 2024, 4, FOR PEER REVIEW 11 By using data such as those shown in Figure 8, and Equations ( 8) and ( 9), one can calculate the dependence of a solvatochromic property (e.g., solvent polarity or ET(probe)) as a function of binary solvent composition at a fixed temperature, or at a series of temperatures (referred to as thermo-solvatochromism), as shown in Figure 9.The preceding discussion shows that it is relatively simple to calculate medium descriptors (e.g., SA and SB) for pure and mixed solvents; the use of the appropriate solvation model permits calculation of the composition of the solvation layers of the solvatochromic probes dissolved therein.Although there are a large number of solvatochromic probes that are employed to calculate the solvent descriptors, the results are consistent when different probes were employed.This is demonstrated by application of Equation ( 1) to a series of ILs, where the calculated empirical solvent polarities using the RB (Reich-

Selected Examples of the Application of Solvatochromism to Understand Medium Effects on Chemical Phenomena
One of the most important applications is that the probes employed, when properly selected, can be used as models.Because most of these probes are dipolar or zwitterionic, and have varying hydrophilic/hydrophobic character, it should not be difficult to select the probes that are expected to match the reaction of interest.For a comprehensive list of solvatochromic probes, see references 19, 25, and 27.Consequently, the information obtained from the solvatochromic probe can be employed to understand the effects of medium composition on diverse chemical phenomena and processes.
Selected examples show the importance of the last phrase.Consider the following question: What is the medium effect on a chemical phenomenon of increasing probe hydrophobicity in a solvent mixture?An example is shown for the solvation in DMSO-W and 1-PrOH-W of 4 probes (Figure 11).Two of these are hydrophilic, 4-(pyridinium-1yl)phenolate and 2-(pyridinium-1-yl)phenolate (p-CB and o-CB, respectively)); the other two (RB and o-RB, 2,4-dimethyl-6-(2,4,6-triphenylpyridinium-1-yl)phenolate) have more elaborate, hydrophobic structures (Figure 7); the corresponding values of φ are shown in Table 1 [25].The straight lines in Figure 11 represent the case where there is no probeinduced preferential solvation, i.e., the composition of the probe solvation layer is equal to that of bulk solvent mixture.It is clear that this is not case; the deviation increases as a function of increasing probe hydrophobicity (RB is practically insoluble in water).Usually, more hydrophobic probes show more deviation from linearity [18].

Selected Examples of the Application of Solvatochromism to Understand Medium Effects on Chemical Phenomena
One of the most important applications is that the probes employed, when properly selected, can be used as models.Because most of these probes are dipolar or zwitterionic, and have varying hydrophilic/hydrophobic character, it should not be difficult to select the probes that are expected to match the reaction of interest.For a comprehensive list of solvatochromic probes, see references [19,25,27].Consequently, the information obtained from the solvatochromic probe can be employed to understand the effects of medium composition on diverse chemical phenomena and processes.
Selected examples show the importance of the last phrase.Consider the following question: What is the medium effect on a chemical phenomenon of increasing probe hydrophobicity in a solvent mixture?An example is shown for the solvation in DMSO-W and 1-PrOH-W of 4 probes (Figure 11).Two of these are hydrophilic, 4-(pyridinium-1yl)phenolate and 2-(pyridinium-1-yl)phenolate (p-CB and o-CB, respectively)); the other two (RB and o-RB, 2,4-dimethyl-6-(2,4,6-triphenylpyridinium-1-yl)phenolate) have more elaborate, hydrophobic structures (Figure 7); the corresponding values of φ are shown in Table 1 [25].The straight lines in Figure 11 represent the case where there is no probeinduced preferential solvation, i.e., the composition of the probe solvation layer is equal to that of bulk solvent mixture.It is clear that this is not case; the deviation increases as a function of increasing probe hydrophobicity (RB is practically insoluble in water).Usually, more hydrophobic probes show more deviation from linearity [18].
With one exception (o-CB in DMSO-W), all values for φ W/S are <1, showing that the organic solvents displace water from the probe solvation layer.All values of φ Mixed solvent/solvent (mixed solvents displacing pure solvents) are > 1, i.e., the complex solvents are more efficient than the parent ones.As expected, the calculated empirical polarity of the mixed solvent is greater than that of pure DMSO or 1-PrOH, because the mixed solvent contains (more polar) water molecules.The reason for the efficiency of the mixed solvent is that probe−solvent interactions include H-bonding to the probe phenolate oxygen, as well as hydrophobic interactions.Thus, 1-PrOH/W has more sites for hydrogen-bond donation/acceptance than water or 1-PrOH, while it is also capable of solvating the probe by the hydrophobic effect due to the organic "end" of the solvent.A similar reasoning can be advanced for the efficiency of DMSO/W relative to W and DMSO.All φ Solvent-W are larger for 1-PrOH/W than DMSO/W, and for p-RB than p-CB or o-CB.The first result underlines the importance of H-bonding to solvation, whereas the second one is in agreement with the dependence of preferential solvation (hence, the values of φ) on the hydrophobicity of the probe [51].With one exception (o-CB in DMSO-W), all values for φW/S are <1, showing that the organic solvents displace water from the probe solvation layer.All values of φMixed solvent/sol- vent (mixed solvents displacing pure solvents) are > 1, i.e., the complex solvents are more efficient than the parent ones.As expected, the calculated empirical polarity of the mixed solvent is greater than that of pure DMSO or 1-PrOH, because the mixed solvent contains (more polar) water molecules.The reason for the efficiency of the mixed solvent is that probe−solvent interactions include H-bonding to the probe phenolate oxygen, as well as hydrophobic interactions.Thus, 1-PrOH/W has more sites for hydrogen-bond donation/acceptance than water or 1-PrOH, while it is also capable of solvating the probe by the hydrophobic effect due to the organic "end" of the solvent.A similar reasoning can be    Likewise, for the solvation of the same probe in a series of structurally related solvents (e.g., alcohols) the fractionation factors, hence the compositions of the probe solvation layer are sensitively dependent on the hydrophobicity of ROH, as shown in Table 2, for the solvation of a hydrophobic-(WB; 2,6-dichloro-4-(2,4,6-triphenylpyridinium-1-yl)-phenolate; pKa = 4.78) and a hydrophilic probe (QB; 1-methylquinolinium-8-olate; pKa = 6.80), at 25 • C [23,52].
Table 2 shows that values of φ are probe-dependent, being larger for WB than for QB in any W-ROH mixture.Additionally, the values φ ROH-W/ROH and φ ROH-W/W increase on going from MeOH to 1-PrOH.If H-bonding to the phenolate oxygen of WB was the dominant probe-solvent interaction, then the expected order of φ ROH-W/ROH and φ ROH-W/W should have been QB (stronger base) > WB (weaker base); this is not the case.We conclude that solute-solvent hydrophobic interactions dominate the solvation of these probes.This also agrees with the dependence of φ on the hydrophobicity (or log P) of the alcohol (MeOH to 1-PrOH).Similar results were observed for the solvation of a series of merocyanine probes (see Figure 7), in binary mixture of W-ROH (MeOH, 1-PrOH) and W-MS (MeCN and DMSO) where the values of φ increase on going from MePMBr 2 (less hydrophobic probe) to OcPMBr 2 (2,6-dibromo-4-[(E)-2-(1-octylpyridinium-4-yl)ethenyl]; more hydrophobic probe) in every binary mixture, and from methanol to 1-PrOH for the same probe [23].This type of information cannot be easily obtained by other approaches and is important, e.g., for choosing the appropriate solvent mixture for a certain application.
As in the experimental determination of the activation energy of reactions, solvation was studied as a function of temperature.An example for the dependence of E T (probe) on T is shown in Figure 12, for the solvation of QB and MePMBr 2 in alkoxy-alcohols [53]. in mixtures of water and 9 alcohols and alkoxy-alcohols were calculated, which range between 2.1 and 3.7 kcal mol −1 .This is a sizeable energy, relative to the activation energies of many reactions (ca.10-12 kcal/mol).This underlines the importance of studying thermosolvatochromism to quantify the contribution of temperature-induced changes in solvation to the energetics of reactions in solution, a quantity that cannot be calculated, e.g., from rate data.
An example that shows the usefulness of solvatochromic probes as models for chemical reactions is the pH-independent hydrolysis of esters, including the hydrophobic 2,4dinitrophenyl carbonate [54], the relatively hydrophilic 4-nitrophenyl chloroformate (calculated log P = 1.66), and the very hydrophobic ester 4-nitrophenyl heptafluorobutyrate (calculated log P = 4.02) [55]; all reactions were studied in W-MeCN mixtures (see Scheme 1).These reactions show a complex dependence of reaction rate constants on water concentration, as shown in the left-hand parts of Figures 13 and 14.
Liquids 2024, 4, FOR PEER REVIEW 16 2.1 and 3.7 kcal mol −1 .This is a sizeable energy, relative to the activation energies of many reactions (ca.10-12 kcal/mol).This underlines the importance of studying thermo-solvatochromism to quantify the contribution of temperature-induced changes in solvation to the energetics of reactions in solution, a quantity that cannot be calculated, e.g., from rate data.
An example that shows the usefulness of solvatochromic probes as models for chemical reactions is the pH-independent hydrolysis of esters, including the hydrophobic 2,4dinitrophenyl carbonate [54], the relatively hydrophilic 4-nitrophenyl chloroformate (calculated log P = 1.66), and the very hydrophobic ester 4-nitrophenyl heptafluorobutyrate (calculated log P = 4.02) [55]; all reactions were studied in W-MeCN mixtures (see Scheme 1).These reactions show a complex dependence of reaction rate constants on water concentration, as shown in the left-hand parts of Figures 13 and 14.
Because addition of MeCN to water induces a series of structural changes in the medium that depends on binary solvent composition [56][57][58], we carried out a "protoninventory" study to probe the structures of the corresponding transition states [59].Our results showed that the complex dependence of reaction rate constants and activation parameters on [H 2 O] is not due to changes in the number of water molecules in the transition states.It reflects, however, the effects of acetonitrile-water interactions on solvation of reactants and transition states.We therefore expected that the dependence of kinetic data on [W] should be similar to that of model solvatochromic probes, as clearly illustrated by Figures 13 and 14.Note that these hydrolysis reactions are particularly suitable to test the potential of using solvatochromic probes as models for chemical phenomena, because complicating acid or base catalysis play no role.Another example of the application of solvatochromic probes to elucidate chemical reactions is retro-DielsAlder reaction (RDA) of anthracene-9,10-dione in aqueous solutions (Scheme 2).The RDA reaction proceeds exceptionally fast in water compared to organic solvents (Figure 15a) because this solvent greatly accelerates pericyclic reactions through H-bonding, which stabilizes the activated complex.[60].Figure 15b shows that this reaction has the Gibbs energy of activation clearly governed by the polarity of the solvent.Because addition of MeCN to water induces a series of structural changes in the medium that depends on binary solvent composition [56][57][58], we carried out a "proton-inventory" study to probe the structures of the corresponding transition states [59].Our results showed that the complex dependence of reaction rate constants and activation parameters on [H2O] is not due to changes in the number of water molecules in the transition states.It reflects, however, the effects of acetonitrile-water interactions on solvation of reactants and transition states.We therefore expected that the dependence of kinetic data on [W] should be similar to that of model solvatochromic probes, as clearly illustrated by Figures 13 and 14.Note that these hydrolysis reactions are particularly suitable to test the potential of using solvatochromic probes as models for chemical phenomena, because complicating acid or base catalysis play no role.
Another example of the application of solvatochromic probes to elucidate chemical reactions is retro-DielsAlder reaction (RDA) of anthracene-9,10-dione in aqueous solutions (Scheme 2).The RDA reaction proceeds exceptionally fast in water compared to organic solvents (Figure 15a) because this solvent greatly accelerates pericyclic reactions through H-bonding, which stabilizes the activated complex.[60].Figure 15b shows that this reaction has the Gibbs energy of activation clearly governed by the polarity of the solvent.We end this discussion by showing how the results of solvatochromism can be employed to determine the relative importance of solvent descriptors to cellulose dissolution.First, solvatochromism of WB was studied in several IL-DMSO mixtures, at χ DMSO = 0.6 and 40 • C [61].This study generated an equation showing the dependence of E T (WB) on solvent descriptors SA, SB, SD and SP.In a later study, microcrystalline cellulose (MCC) was dissolved in these binary mixtures and the mass of dissolved MCC (expressed as %m) was correlated with the same solvent descriptors, calculated from the solvatochromic study [5], see Equations ( 10) and ( 11): E T (WB) = 54.61+ 2.77 SA + 0.61 SB − 1.06 V M + 0.41 ƒ(n) → Based on solvatochromism in 13 IL-DMSO mixtures; R 2 = 0.939 (10) MCC-m% = 9.49 + 3.01 SA + 6.88 SB − 2.99 V M + 2.427 ƒ(n) → Based on MCC dissolution in 11 IL-DMSO mixtures; R 2 = 0.902 (11) where SA and SB are those defined above, V M and ƒ(n) are the molar volume of the neat IL, and the LorentzLorenz refractive index function; these were employed instead of SD and SP, as explained elsewhere [61].The signs of the regression coefficients in both equations are the same.That is, solvatochromism and MCC dissolution are enhanced by solvent Lewis acidity, Lewis basicity and polarizability; the inverse is true for the molar volume of the IL.The different relative importance of SA/SB in both cases can be explained because MCC is a H-bond acceptor and donor, whereas the probes are only H-bond acceptors.The relevant point, however, is that two very different chemical process can be similarly correlated with the same set of solvent descriptors.This agreement can be fruitfully employed, e.g., for screening possible candidates as solvents for cellulose and other biopolymers.

Conclusions
Solvent mixtures are extensively employed in chemistry for practical reasons.Their use leads to enhanced solubilities, increased rate constants, etc.These beneficial effects call for a clear understanding of solvent effects on chemical phenomena.This understanding is, however, hindered by two complications: (i) The dependencies of the physicochemical properties of the binary mixtures on its composition are usually not ideal, and (ii) The compositions of the solvation layers of the solutes are almost always different from those of the bulk solvents.The reasons for the latter differences are combinations of dielectric enrichment and, more importantly, H-bonding and solute-solvent hydrophobic interactions.This intricate situation has been greatly simplified by using solvatochromic probes as models for the reaction or process under consideration.By applying appropriate solvation models, the study of these probes furnishes a set of solvent-exchange equilibrium constants (φ) that permits calculation of the effective (or local) composition of the solvatochromic probe.If the latter is a good model for the reaction or process under consideration, one can access information (about the composition of the solvation layer) that is inaccessible by other techniques.To our view, this represents a practical solution for a complex problem.Theoretical calculations will certainly enhance our understanding of solvation, because they permit, inter alia, calculation of the UV-Vis spectra of probes in mixed solvents [62], and prediction of solvatochromism [63].
A list of all abbreviations employed is given below.The structures of the solvatochromic probes discussed are shown in Figure 7.

Figure 1 .
Figure 1.(a)A simplified scheme for cellulose dissolution in ionic liquid-DMSO.The dissolution is attributed to interactions of its hydroxyl groups with the ions of the ionic the dipole of DMSO.Reproduced with permission from[9].(b) Effects of the addition non-solvent (such as water or ethanol) on the dissolution of cellulose IL-dipolar solven of the non-solvent leads to cellulose precipitation.Reprinted with permission from[7].

Figure 1 .
Figure 1.(a)A simplified scheme for cellulose dissolution in ionic liquid-DMSO.The biopolymer dissolution is attributed to interactions of its hydroxyl groups with the ions of the ionic liquid and the dipole of DMSO.Reproduced with permission from[9].(b) Effects of the addition of a protic non-solvent (such as water or ethanol) on the dissolution of cellulose IL-dipolar solvent.Addition of the non-solvent leads to cellulose precipitation.Reprinted with permission from[7].

Figure 4 .
Figure 4. Schematic representation of the solvation of a solute in a binary solvent mixture composed of two solvents (A, B), and the "mixed" solvent A-B, whose formation is discussed below.The parts of the lower line represent from the left: ideal solvation, i.e. the composition of the probe solvation layer is the same as that of bulk solvent mixture; preferential solvation by the solvents (A, A-B); preferential solvation by the solvents (B, A-B).

Figure 4 .
Figure 4. Schematic representation of the solvation of a solute in a binary solvent mixture composed of two solvents (A, B), and the "mixed" solvent A-B, whose formation is discussed below.The parts of the lower line represent from the left: ideal solvation, i.e., the composition of the probe solvation layer is the same as that of bulk solvent mixture; preferential solvation by the solvents (A, A-B); preferential solvation by the solvents (B, A-B).

Figure 7 .
Figure 7. Structures and acronyms of some solvatochromic probes, employed to calculate the solvent descriptors shown in Equation (1).

Figure 7 .
Figure 7. Structures and acronyms of some solvatochromic probes, employed to calculate the solvent descriptors shown in Equation (1).
g., ROH-W.The input data to solve these equations include E obs T ,

Figure 9 .
Figure 9. (a) Dependence of solvent polarity scale, ET(probe), on analytical, χW Analytical (open symbols), and "effective", χW Effective (solid symbols) χW for MeOH-W mixtures at 25 °C.Reprinted with permission from [48].(b) Dependence of the empirical solvent polarity parameter ET(MePMBr2) on the mole fraction of water, χW, at 25 °C, for mixtures of water with ILs.The straight lines connecting the polarities of the pure solvents are theoretical, plotted merely to depict the ideal solvation of the probe by the binary mixtures.Reprinted from [49].

Figure 9 .
Figure 9. (a) Dependence of solvent polarity scale, E T (probe), on analytical, χ W Analytical (open symbols), and "effective", χ W Effective (solid symbols) χ W for MeOH-W mixtures at 25 • C. Reprinted with permission from [48].(b) Dependence of the empirical solvent polarity parameter E T (MePMBr 2 ) on the mole fraction of water, χ W , at 25 • C, for mixtures of water with ILs.The straight lines connecting the polarities of the pure solvents are theoretical, plotted merely to depict the ideal solvation of the probe by the binary mixtures.Reprinted from [49].

Figure 10 .
Figure 10.Correlation between experimentally determined ET(RB) and those calculated by Equation (1a) for ionic liquids.Reprinted with permission from [50].

Figure 10 .
Figure 10.Correlation between experimentally determined E T (RB) and those calculated by Equation (1a) for ionic liquids.Reprinted with permission from [50].

Figure 11 .
Figure 11.Dependence of ET N (probe) on the χW for W-DMSO (left) and W-1-PrOH (right) mixtures.The black and green squares are for (hydrophilic) p-CB, and o-CB, respectively.The red spheres are for (hydrophobic) p-RB (or RB).The curves clearly show that the deviation form ideality increases as a function of increasing probe hydrophobicity.Reprinted with permission from [25].

Table 1 .
Solvatochromism of p-RB, p-CB, and o-CB in binary mixtures of W-DMSO and W-1-PrOH at 25 °C.Reprinted with permission from [25].

Figure 11 .
Figure 11.Dependence of E T N (probe) on the χ W for W-DMSO (left) and W-1-PrOH (right) mixtures.The black and green squares are for (hydrophilic) p-CB, and o-CB, respectively.The red spheres are for (hydrophobic) p-RB (or RB).The curves clearly show that the deviation form ideality increases as a function of increasing probe hydrophobicity.Reprinted with permission from [25].

Table 1 .
Solvatochromism of p-RB, p-CB, and o-CB in binary mixtures of W-DMSO and W-1-PrOH at 25 • C. Reprinted with permission from [25].

Figure 12 .Figure 12 .
Figure 12.Dependence of the empirical solvent polarity on temperature, for the solvation of WB (a), QB (b), and MePMBr2 (c) in aqueous alcohols.Reprinted with permission from [53].Plots (not shown) of ET(probe)Solvent versus T gave excellent straight lines, the negative slopes of which are given by ΔET(probe)Solvent/ΔT (in kcal mol −1 K −1 ).These were calculated for pure solvents; the order is |ΔET(probe)ROH| > |ΔET(probe)W|, reflecting the greater effect of temperature on the structure of ROH.Consequently, H-bonding of water with the probe ground state is less susceptible to temperature increases than ROH.Values of ΔET(probe)Solvent for 50 °C intervals (ΔET(10 °C)-(ΔET(60 °C) for WB and MePMBr2 in mixtures of water and 9 alcohols and alkoxy-alcohols were calculated, which range between Figure 12.Dependence of the empirical solvent polarity on temperature, for the solvation of WB (a), QB (b), and MePMBr2 (c) in aqueous alcohols.Reprinted with permission from [53].Plots (not shown) of E T (probe) Solvent versus T gave excellent straight lines, the negative slopes of which are given by ∆E T (probe) Solvent /∆T (in kcal mol −1 K −1 ).These were

Figure 13 .
Figure 13.(A) Dependence of log (kobs), the observed rate constant on χw, the mole fraction of water in aqueous acetonitrile, at different temperatures.The points are experimental, and the solid sigmoidal lines were calculated by a fourth power polynomial dependence of log (kobs) o χw.(B) Dependence of the empirical solvent polarity ET(RB) on χw.The solid curve was calculated from a fifth power polynomial dependence of ET(RB) on χw.Reprinted with permission from [54].

Figure 13 .
Figure 13.(A) Dependence of log (k obs ), the observed rate constant on χ w , the mole fraction of water in aqueous acetonitrile, at different temperatures.The points are experimental, and the solid sigmoidal lines were calculated by a fourth power polynomial dependence of log (k obs ) o χ w .(B) Dependence of the empirical solvent polarity E T (RB) on χ w .The solid curve was calculated from a fifth power polynomial dependence of E T (RB) on χ w .Reprinted with permission from [54].

Figure 13 .
Figure 13.(A) Dependence of log (kobs), the observed rate constant on χw, the mole fraction of water in aqueous acetonitrile, at different temperatures.The points are experimental, and the solid sigmoidal lines were calculated by a fourth power polynomial dependence of log (kobs) o χw.(B) Dependence of the empirical solvent polarity ET(RB) on χw.The solid curve was calculated from a fifth power polynomial dependence of ET(RB) on χw.Reprinted with permission from [54].

Figure 14 .
Figure 14.Plots of the dependence of log (kobs) and of ET(probe) on log [W], at 25 °C.Reduced log (kobs) and reduced ET(probe) are employed, so that the results of different species (esters, probes) may be directly compared.Values of ET(probe) of pure water and pure MeCN are, respectively, 64.62 and 52.97 kcal mol −1 (QB) and 70.24 and 54.72 kcal mol −1 (WB).Reprinted with permission from [51].

Figure 14 .
Figure 14.Plots of the dependence of log (k obs ) and of E T (probe) on log [W], at 25 • C. Reduced log (k obs ) and reduced E T (probe) are employed, so that the results of different species (esters, probes) may be directly compared.Values of E T (probe) of pure water and pure MeCN are, respectively, 64.62 and 52.97 kcal mol −1 (QB) and 70.24 and 54.72 kcal mol −1 (WB).Reprinted with permission from [51].

Table 2 .
[30]lts for the solvation of WB and QB in water-alcohol mixtures at 25 • C[30].