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In the present work a thermochemistry of solution and solvation of mono- and di-substituted chloro- and nitrobenzenes in binary mixtures was studied. The infinite dilution solution enthalpies of 1,2-dichlorobenzene,1,4-dichlorobenzene, 1,2- dinitrobenzene, 1,4-dinitrobenzene, 1-chloro-2-nitrobenzene and 1-chloro-4-nitrobenzene in binary mixtures of benzene-cyclohexane, benzene-acetonitrile, carbon tetrachloride-acetonitrile at different molar ratios (0, 0.25, 0.50, 0.75, 1.00) solvents were measured at 298.15 K. Based on experimental data the solvation enthalpies in binary mixture were calculated. It was shown that the solvation enthalpies slightly depend on neither the location of chloro- and nitro - substituents in aromatic ring nor a composition of binary mixture.

The thermochemical study of hydrogen bonding of water with different proton acceptor ionic liquids was carried out. Along with the available experimental data, the solution enthalpies of water in [BMIM][TfO], [BMIM][BF4] and [BMIM][PF6] were measured. The hydrogen bonding enthalpies of water with various ionic liquids were determined by using previously developed method of solvation enthalpy separation into the nonspecific solvation enthalpy and the specific solute-solvent interaction enthalpy (hydrogen bonding). The findings indicate the formation of a complex, where one molecule of water is bound to two molecules of ionic liquids. Similarly, hydrogen bonding enthalpies of methanol with the same proton acceptor ionic liquids were determined.

In present work a thermochemistry of hydrogen bond formation of proton acceptors (B) in the medium of linear (N-methylformamide (NMF)) and cyclic (2-pyrrolidone (Py)) amides was studied. The infinite dilution solution enthalpies of nitriles, ketones, esters, ethers and amines in amides were measured at 298.15 K. Enthalpies of hydrogen bonding of proton acceptors in solution linear and cyclic amides were calculated and compared with previously determined the enthalpies of hydrogen bonding of amides in proton acceptor media. The cooperative effects of hydrogen bonding in multi-particle complexes of amides with proton acceptors were evaluated. It was shown that cooperativity coefficients were decreased with increasing the basicity of proton acceptors.

In work a thermochemistry of solution, solvation and hydrogen bond formation of linear (diethyl ether and diglyme) and cyclic ethers (1,4-dioxane, 12-crown-4, 15-crown-5 and 18-crown-6) in proton acceptor and proton donor solvents were studied. The infinite dilution solution enthalpies of ethers in cyclohexane, carbon tetrachloride, benzene, ethyl acetate, N,N-dimethylformamide, dimethylsulfoxide, acetone, pyridine, chloroform and methanol were measured at 298.15 K. The solvation and hydrogen bonding enthalpies of ethers in the solvent are calculated. The influence of number of active centers in ethers on thermochemical parameters is shown. It was found that the formation of hydrogen bonds for linear and cyclic ethers with proton donors are different.

In this work thermochemistry of solution and solvation of mono- and di-substituted chloro- and nitro-benzenes in 1-butyl-3-methylimidazolium tetrafluoroborate ([BMIM][BF4]), 1-butyl-3-methylimidazolium trifluoromethanesulfonate ([BMIM][TfO]) and 1-butyl-3-methylimidazolium bis(trifluoromethylsulfonyl)imide ([BMIM][NTf2]) ionic liquids was studied. Enthalpies of solution at infinite dilution of benzene, chlorobenzene, nitrobenzene, 1,2-, 1,3-, 1,4-dichlorobenzenes, 1,2-, 1,3-, 1,4-dinitrobenzenes, 1-chloro-2-nitrobenzene, 1-chloro-3-nitrobenzene, and 1-chloro-4-nitrobenzene in three ionic liquids were measured at 298.15 K. On the basis of experimental data enthalpies of solvation of substituted benzenes in ionic solvents were calculated. Values of Cl and NO2 group contributions to the enthalpies of solvation were derived and compared with molecular solvents. Enthalpies of solvation of each series of dichlorobenzenes, chloronitrobenzenes and dinitrobenzenes in studied ionic liquids are equal and do not depend on the mutual position of substituents. This fact shows that dipole moment does not affect the enthalpy of solvation of organic solutes in ionic liquids. Enthalpies of solvation of disubstituted benzenes in ionic liquids calculated through group contribution approach were in good agreement with experimental data.

In this work the thermodynamics of intermolecular interactions for imidazolium based ionic liquids in solutions of proton donor solvent chloroform and proton acceptor solvent tetrahydrofuran was studied using solution calorimetry technique. Enthalpies of solution of 1-ethyl- and 1-butyl-3-methylimidazolium based ionic liquids with tetrafluoroborate, methylsulfate, ethylsulfate, butylsulfate, dicyanoamide, trifluoromethanesulfonate, thiocyanate anions were measured in two solvents over concentration range 0.18-3.60 mmol kg−1 at 298.15 K. Enthalpies of transfer from tetrahydrofuran to chloroform derived from experimental data were exothermic for all studied ionic liquids. Proton acceptor scale of ionic liquids as solutes was proposed on the basis of thermochemical data. Enthalpy of hydrogen bonding of ionic liquids with proton donor solvent chloroform increases in the range of anions [BF4]−

The present work focuses on hydrogen bonding of linear and cyclic amides (formamide, N-methylformamide, acetamide, N-methylacetamide, N,N-dimethylacetamide, 2-pyrrolidone) in several ionic liquid (1-butyl-3-methylimidazolium bis(trifluoromethanesulfonyl)imide [BMIM][NTf2], 1-butyl-3-methylimidazolium tetrafluoroborate [BMIM][BF4], 1-butyl-3-methylimidazolium trifluoromethanesulfonate [BMIM][TfO], 1-butyl-3-methylimidazolium hexafluorophosphate [BMIM][PF6], triethylsulfonium bis(trifluoromethylsulfonyl)imide [Et3S][NTf2], Trimethylpropylammonium bis(trifluoromethylsulfonyl)imide [TMPAm][NTf2]). The solution enthalpies of amides in ionic liquids were measured by solution calorimetry at infinite dilution. The hydrogen bond enthalpies were calculated based on solution enthalpies of amides in ionic liquids. The hydrogen bond enthalpies of linear and cyclic amides in ionic liquids and organic proton acceptors were compared. The influence of active proton donor center on the formation of hydrogen bond complexes between amides and ionic liquids was analyzed.

In the present work thermochemistry of intermolecular interactions of organic compounds in solutions of imidazolium based ionic liquids (ILs) has been studied using solution calorimetry method. Enthalpies of solution at infinite dilution of non-polar (alkanes, aromatic hydrocarbons) and polar (alcohols, amides, and etc.) organic solutes in two ionic liquids 1-butyl-3-methylimidazolium tetrafluoroborate and 1-butyl-3-methylimidazolium trifluoromethanesulfonate were measured at 298.15 K. The scale of van der Waals interactions of imidazolium based ILs has been proposed on the basis of solution enthalpies of n-alkanes in their media. The effect of the cation and anion structure of ILs on the enthalpies of solvation was analyzed. Enthalpies of hydrogen bonding of organic solutes with imidazolium based ILs were determined. It has been shown that these values are close to zero for proton acceptor solutes. At the same time, enthalpies of hydrogen bonding of proton donor solutes with ionic liquids are increased depending the anion: tetrafluoroborate ≈ bis(trifluoromethylsulfonyl)imide

Article on the effect of halogen substitution on the enthalpies of solvation and hydrogen bonding of organic solutes in chlorobenzene and 1,2-dichlorobenzene derived using multi-parameter correlations.

The work focuses on a thermochemical study of solvation of organic non-electrolytes in various binary mixed solvents. The enthalpies of solution of pyrrole, methanol and chloroform in carbon tetrachloride – pyridine binary mixture were measured at 298.15 K. Data on solution enthalpies of solute – binary solvent for more than 350 systems has been collected. The specific and non-specific terms to the enthalpies of solvation of proton donors have been evaluated for the first time for the mixed solvent using the model previously adapted for individual solvents.