The solubility of 2,3,4,5-tetrabromothiophene in (ethanol + tetrahydrofuran) binary solvent mixtures was measured within the temperature range from (278.15 to 322.15) K. The solubility increases with the rise of temperature, while it decreases with increasing ethanol content at constant temperature. The experimental data were fitted using the two variants of the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K) equation and the Jouyban–Acree equation, respectively. All the three equations were proven to give good representations of the experimental values. Computational results showed that the variant two of CNIBS/R–K equation was superior to the other two equations. The thermodynamic properties of the solution process, including the Gibbs free energy, enthalpy, and entropy, were calculated by the van’t Hoff analysis. The values of both the enthalpy change and the standard molar Gibbs free energy change of solution were positive, which indicated that the process was endothermic.
Yumei Kai,Yonghong Hu,Zheng Cao,Xiang Liu,Yan Liu,Wenge Yang
The solubilities of l -malic acid in pure and mixture organic solvents were measured from 278.15 to 323.15 K using the laser monitoring observation system. The modified Apelblat equation, the semi-empirical Buchowski–Ksiazczak λh equation and the Combined Nearly Ideal Binary Solvent/Redlich (CNIBS/R-K) equation were proposed to correlate the experimental data. In pure and mixed solvents, the 100RD (relative deviation) <3.61 and 7.58, respectively, the 10 4 RMSD (root-mean-square deviations) <3.07 and 2.28, respectively, so the equations selected in this work fit the data very well. Van’t Hoff equation was used to predict the dissolution enthalpy and entropy of l -malic acid in the corresponding solvents.
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