The investigation on p-nitrophenylacetonitrile solubility in ethanol, methanol, isopropanol, n-propanol, acetonitrile, acetone, ethyl acetate, toluene, n-butanol, cyclohexane, 2-butanone, isobutanol, acetic acid, 1,4-dioxane, water, and ethylbenzene was performed via the shake-flask technique covering the temperature range from 278.15 to 333.15 K at local atmospheric pressure. The mole fraction solubility of p-nitrophenylacetonitrile increased with an increase of the studied temperature and followed a sequence in the 16 solvents with the exception of 1,4-dioxane: ethyl acetate > acetone > (acetonitrile, 2-butanone) > toluene > acetic acid > ethylbenzene > methanol > ethanol > n-propanol > n-butanol > isopropanol > isobutanol > cyclohexane > water. There was no solvation or polymorphic transformation during the experiment process. Correlation was made for the obtained p-nitrophenylacetonitrile solubility in the 16 solvents using the λh, Apelblat, Wilson, and NRTL models. The obtained maximum relative average deviation was 2.67%, and root-mean-square deviation, 2.57 × 10–3. The solute–solvent and solvent–solvent interactions were studied based on the linear solvation energy relationship approach. Furthermore, the thermodynamic dissolution properties, reduced excess enthalpy, and activity coefficient under infinitesimal condition were also computed.

The present work mainly reports the terephthalaldehydic acid solubility in aqueous solutions of methanol, ethanol, isopropanol, and NMP, which was achieved through a steady-state method covering a temperature range from 283.15 to 323.15 K under 101.1 kPa. The terephthalaldehydic acid solubility increased positively as the mass fraction of methanol (ethanol, isopropanol, and NMP) increased for the investigated mixtures of methanol (ethanol, isopropanol, and NMP) and water. At the same temperature and mass fraction of methanol (ethanol, isopropanol, and NMP), the mole fraction solubility of terephthalaldehydic acid was higher in the NMP and water mixture than in the other three mixtures. The solid equilibrating with saturated liquor was indentified through X-ray power diffraction, which showed no crystal transition, polymorphic transformation, or solvate formation. Three models, the Van’t Hoff–Jouyban–Acree, Jouyban–Acree, and Apelblat–Jouyban–Acree, were used here to correlate the obtained solubility data. The back-calculated values were in good agreement with the determined ones. The values of RAD and RMSD were, respectively, no greater than 3.63% and 6.66 × 10–4. Preferential solvation of terephthalaldehydic acid in the four mixtures was analyzed by employing the method of inverse Kirkwood–Buff integrals. The preferential solvation parameter δx 1,3 by NMP (methanol, ethanol, or isopropanol; 1) is positive within the composition range of 0.16 < x 1 < 1 for NMP, 0.32 < x 1 < 1 for methanol, and 0.25 < x 1 < 1 for ethanol and isopropanol. As it can be speculated that in the regions where terephthalaldehydic acid is preferentially solvated by NMP (methanol, ethanol, or isopropanol), terephthalaldehydic acid acts as a Lewis acid with NMP (methanol, ethanol, or isopropanol) molecules.

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The method of shake-flask was used in studying the solubility of flubendazole in water, n-propanol, ethanol, isopropyl alcohol, methanol, isobutyl alcohol, n-butanol, N,N-dimethylformamide, 1,4-dioxane, 2-butanone, dimethyl sulfoxide (DMSO), and N-methyl-2-pyrrolidone. The determination was made over the temperatures from 283.15 K to 333.15 K under ambient pressure p = 101.2 kPa. The values of flubendazole solubility in mole fraction in these solvents increased with rising temperature. They were highest in DMSO and lowest in water. The gained solubility was mathematically described through the Apelblat equation. The maximum average relative deviation and root-mean-square deviation were 2.69% and 3.60 × 10–5, respectively. In addition, using the relationship analysis of linear solvation energy of solvent effect, the degree and type of solvent–solvent and solute–solvent interactions were identified.