Heats of Solution of Liquid Solutes in Various Solvents

e values of the heats of solution (2131 solutions) of different liquid solutes in organic and inorganic solvents were obtained from the literature data on the heat of mixing (ΔmixHH) in the wide range of concentrations. e limit values of the heat of solution of a solute (ii) in a solvent (jj) (ΔsolnHHiiijj) were calculated from the limit data of the dependence ΔmixHH/xxii versus xxii at xxii → 0 and the values of that of a solute (jj) in a solvent (ii) (ΔsolnHHjjiii) from the limit data of the dependence ΔmixHH/xxjj versus xxjj at xxjj → 0, respectively.


Introduction
At the present, there are a lot of data on the heats of mixing of binary liquid systems [1][2][3][4][5] and considerably less data on the heats of solution from direct calorimetric measurements [6][7][8][9][10][11].In two handbooks [1,2] about 2500 tables of data on the heats of mixing (Δ mix ) of the different liquid solutes in organic and inorganic solvents have been collected, whence the values of the enthalpies of solution were calculated.
It is generally known that the enthalpy of solution is the enthalpy change associated with the dissolution of a substance in a solvent at constant temperature and pressure, resulting in in�nite dilution.is process can mentally be separated on three steps: Here, Δ evap  A is the energy of breaking of all the solute-solute interactions in molecular liquid (A), equal to the enthalpy of evaporation (invariably endothermic process), Δ hole  S is the enthalpy of optimal destruction and rearrangement of the solvent-solvent part of interactions (invariably endothermic process), and Δ int  A−S is the enthalpy of interaction of the isolated molecule of solute (A) placed in the prepared hole of the solvent (S) (invariably exothermic process).e value of the overall enthalpy change is the sum of the individual enthalpy changes of each of these steps and can be positive (endothermic process) or negative (exothermic process).In the case of ideal solution, there is a complete compensation of breaking and forming energy in (1) with zero value of Δ soln  AS .In overwhelming majority of measurements, the values of the heat of solution differ from zero and supply with the additional information for analysis of the nature of these steps [10,11].Enthalpy transfer from the gas phase to solution is the enthalpy of solvation (Δ solv  AS ) and can be calculated as follows: (2) From (2) follows that the relative change of the enthalpy of solvation (Δ solv  AS ) of compound (A) in the series of solvents is equal to the difference in the enthalpy of solution ( soln Δ AS ).
For all enthalpy cyclic processes, there is the possibility to calculate the unknown values of the enthalpy transfer on the base of relative changes of the enthalpy of solution.
As an example, the relative changes of the enthalpy of T 1: Heat of the mixing (Δ mix /J mol −1 solution) of methyl alcohol and dimethyl sulfoxide at the mole fraction of dimethyl sulfoxide, 25 ∘ C ( solvation of a transition state (Δ solv  TS ) can be calculated corresponding to the following: Here, Δ soln  (1,2),(S  ) −Δ soln  (1,2),(So) is the enthalpy transfer of reagents 1 and 2 from the reference solvent (S 0 ) to other one (S  ), and Δ ≠ (S  ) and  ≠ (So) are the enthalpies of activation of reaction in these solvents [12,13].
From comparison of the independent values of Δ solv  TS for the direct and back reactions, a good correlation was observed in line with the common nature of activated complex for the reversible reactions [13].

Methodology
e heats of mixing [1,2], Δ mix  = Q mix /( 1 +  2 ), are in J mol −1 of solution ( 1 +  2 = 1), and concentrations were presented in the mole fractions.e limit value of the heat of solution of solute (1) in the solvent (2) can be calculated from the curvature of Δ mix  versus  1 in the range of  1 from nearzero to ∼(0.3-0.5).e value of derivative Δ mix / 1 of the best-�tted function at  1 → 0 is equal to the heat of solution of the compound (1) in the solvent (2).Similar calculations were performed for the heat of solution of compound (2) in the solvent (1) at  1 → 1. e same results were obtained from the limit data of the dependence Δ mix / 1 versus  1 at  1 → 0 or from the limit data of the dependence Δ mix / 2 versus  2 at  2 → 0, respectively.As an example, let us consider here the values of the heats of mixing of methyl alcohol and dimethyl sulfoxide at 25 ∘ C (Table 1).
From the data of the �rst and third columns, the dependence Δ mix / DMSO versus  DMSO can be easy calculated, and the value of Δ soln  of DMSO in methyl alcohol follows as −0.90 ± 0.05 kJ mol −1 .Using similar calculation from the data in the fourth and sixth columns, the value of Δ soln  of methyl alcohol in DMSO follows as −1.30 ± 0.05 kJ mol −1 .From these results, everyone can conclude that the hydrogen bond methanol-DMSO is stronger than that in methanolmethanol in agreement with experimental data [14].In these calculations, the more impotent data of Δ mix  are at the values of   → 0 and   → 1.But as a rule, the lowered heat of mixing is accompanied by the larger error.erefore, the curvature of the dependence Δ mix /  versus   gives oen more correct data than that of single value of Δ mix /  at the small concentration of   .
Very sharp curvature of the dependence Δ mix /  versus   is usually observed at  1 → 0 for solution of H-bonded solutes, as alcohols, in inert solvents (alkanes, cycloalkanes, and carbon tetrachloride).For such solutions, the experimental data on the heat of mixing with relatively high concentration of solutes were excluded from consideration.Usually the errors of the heats of solution of alcohols in alkanes were up to ±(1-2) kJ mol −1 and for other solutions up to ±(0.1-0.3)kJ mol −1 .is range of errors of calculated heats of solution is in agreement with the precise data of direct calorimetric measurements [6][7][8][9][10][11].Some conclusions can be made from the consideration of the obtained data on Δ soln  (Dataset Item 1 (Table )).
From the analysis of the wide experimental data of the heats of solution and solvation of different solutes in the medium of cycloalkanes, very interesting and useful relation was observed [10].e value of enthalpy of solvation (Δ solv  A/-hexane /kJ mol −1 ) can be predicted from the highreliable (4) [10]: Here, MR A is the molecular refraction (cm 3 mol −1 ) of solute.It means that enthalpy of destruction of the solvent-solvent interactions (Δ hole  S ) and the enthalpy of interaction of the isolated molecule of solute (A) with cyclohexane (Δ inter  A−S ) are determined only by the ability of -hexane--hexane interactions and by the value of MR A of solute.In other words, the relative enthalpy of interaction of -hexane with different types of solutes will be the same as in -hexane with -hexane.With the known experimental data of enthalpy of solution in -hexane (Δ soln  A/-hexane ) and calculated value of Δ solv  A/-hexane (see ( 4)), everyone can calculate (see (5)) the important parameter, the unknown value of the enthalpy of evaporation of A: e possibility of chloroform (entries 484-538) and pentachloroethane (entries 1611-1615) to generate the H-bonds with the -donor solvents, even with alcohols, follows from the exothermic values of the heat of solution.Very strong interactions of the liquid Lewis acids with the -donor solvents with formation of  -complexes can be concluded from observed data (entries 1858-1881).Additional conclusions can be done by the reader.

Dataset Description
e dataset associated with this Dataset Paper consists of one item which is described as follows.
Dataset Item 1 (Table ).Enthalpies of solution (Δ soln , kJ mol −1 ) of solutes in various solvents (alphabetic order).e calculated limit values of the enthalpies of 2131 solutions were collected.In the �rst column are indicated the entries� numbers of solutions (Number).In the second column are shown the names of solutes followed by their values of the enthalpies of evaporation in parenthesis from [15].In the third column, the solvents appeared in an alphabetical order.
In the fourth column are collected the calculated values of enthalpies of solution (Δ soln , kJ mol −1 ), aer slash is given the temperature, ∘ C, and in parenthesis is the number of tabulated data of the heat of mixing (Δ mix ) from textbook [1] or [2].As an example, the data of solution of dimethyl sulfoxide in methanol (entry 946 in the table), −0.9/25 (319-1), means that −0.9 is the enthalpy of solution in kJ mol −1 , 25 is the temperature of the measurements, ∘ C, and (319-1) is the number (319) of the table of the heat of mixing in the textbook [1].

Concluding Remarks
Analysis of an experimental data on the enthalpy of solution, collected in Dataset Item 1 (Table ), helps to estimate the total energy of solute-solvent interactions.ese data can be useful for the selection of appropriate solvents for the practical goals in the synthesis and puri�cation and for the theoretical consideration of the constituents of the solution and solvation processes.

Dataset Availability
e dataset associated with this Dataset Paper is dedicated to the public domain using the CC0 waiver and is available at http://dx.doi.org/10.7167/2013/823638/dataset.