Solid-liquid phase equilibrium and thermodynamic properties analysis of 2,4,5-trimethoxybenzaldehyde in mono-solvents

Abstract

Solid-liquid equilibrium solubility of 2,4,5-trimethoxybenzaldehyde (ANH) in nineteen kinds of mono-solvents (i.e., methanol, ethanol, n-propanol, i-propanol, n-butanol, i-butanol, s-butanol, n-pentanol, i-pentanol, acetone, 2-butanone, cyclohexanone, acetonitrile, N, N-dimethylformamide, tetrahydrofuran, ethyl formate, methyl acetate, ethyl acetate, and toluene) was determined by a gravimetric method over a temperature ranging from 278.15 K to 323.15 K under approximately 0.1 MPa. The solubility was positively correlated with temperature in all the selected solvents. The maximum solubility value occurred in DMF (x1 = 0.1923 mol·mol−1, T = 323.15 K) and the minimum solubility value occurred in i-propanol (x1 = 0.001971 mol·mol−1, T = 278.15 K). The modified Apelblat model, Yaws model, NRTL model and Wilson model were used to correlate the experimental data. The NRTL model fits best among all the models with RAD no larger than 0.0047 (ethanol) and a RMSD value less than 0.000236 (DMF). Dissolution properties of ANH, including dissolution enthalpy ΔdisH, dissolution entropy ΔdisS and dissolution Gibbs energy ΔdisG, were calculated according to the Wilson model. The dissolution process of ANH is demonstrated to be endothermic, spontaneous, and entropy-driven in the chosen mono-solvents. The solubility data, thermodynamic parameters and dissolution properties are of guiding significance to the further investigation of ANH.