Experimental study on binary (solid + liquid) equilibrium and solubility analysis of N-fluorobenzenesulfonimide in 16 organic solvents at temperatures ranging from 273.35 to 322.85 K under 101.3 kPa

The solubility of N-fluorobenzenesulfonimide in sixteen pure organic solvents, including methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, n-pentanol, isopentanol, ethyl acetate, 2-butanone, 2-pentanone, acetone, toluene, acetonitrile, ethyl formate, and methyl acetate, was measured using the gravimetric method in the temperature range of 273.35 K to 322.85 K under 101.3 kPa. Five thermodynamic models, namely the modified Apelblat equation, the λh equation, the Non Random Two Liquid (NRTL) equation, the Wilson equation and the Yaws model, were applied to correlate the measured solubility data. The correlation results were evaluated using relative mean deviation (RAD) and root mean square deviation (RMSD). The results indicate that the molar solubility increases with increasing temperature in all sixteen solvents, and all five relevant models can provide satisfactory results. A preliminary evaluation of the potential for chemical bond formation between solute and solvent was conducted by examining the electrostatic potential energy surface of the solute. Density functional theory (DFT) was utilized to calculate the interaction between solute and solvents during the dissolution process. The KAT-LSER model was introduced to analyze solvent effects, and the results showed that hydrogen bond acidity is not conducive to dissolution, while hydrogen bond alkalinity, dipole interaction, and the ability of electron polarization to stabilize charges are conducive to dissolution. The thermodynamic properties of the mixture, such as enthalpy, entropy, and Gibbs free energy, were calculated, and the results showed that the dissolution process of N-fluorobenzenesulfonimide is spontaneous and favorable.