Solubility Behavior and Data Correlation of Sulfinpyrazone in Thirteen Pure Solvents from 283.15 to 323.15 K

Abstract

This present work is the investigation of the solubility for sulfinpyrazone in 13 monosolvents, water, methanol, ethanol, n-propanol, isopropanol, n-butanol, sec-butanol, acetone, acetonitrile, 2-butanone, methyl acetate, ethyl acetate, and npentanol, via a static gravimetric method at temperatures ranging from 283.15 to 323.15 K under atmospheric pressure. The solubility magnitudes are in positive correlation with the absolute temperature in each solvent. Within the experimental temperature range, the solubility is the highest in acetonitrile (103.286 × 10 −3 at 323.15 K) and lowest in water (0.03597 × 10 −3 at 283.15 K). The rough sequences of solubility values in different solvents are methanol > n-pentanol > n-propanol > n-butanol > sec-butanol > ethanol > isopropanol and acetonitrile > acetone > 2-butanone > methyl acetate > ethyl acetate > water in alcohols and nonalcohol solvents, respectively. The results demonstrate that the solubility behaviors of sulfinpyrazone are affected by the combined effects of several factors involving solvent polarity, solvent−solvent intermolecular interactions (quantitatively characterized by cohesive energy density), and molecular structures (molecular sizes and properties of functional groups) of solvents and solutes. Additionally, the Apelblat equation and Yaws equation were employed to correlate the experimental solubility data of sulfinpyrazone in each investigated solvent. The results of average relative deviations and root-mean-square deviations as well as the values of Akaike Information Criterion and Akaike weights reveal that the calculated solubility values by the Apelblat equation are more consistent with the experimental data compared to those by the Yaws equation.

Solid-Liquid Equilibrium Behavior and Data Correlation of Furosemide in 12 Pure Solvents from 283.15 to 323.15 K

“…The level of difficulty for the formation of hydrogen bonds between solvent and solute molecules can be quantitatively characterized by the summation of hydrogen bond donor/acceptor propensities . The formation of a solvent–solute intermolecular hydrogen bond may generally enhance the solubility and different abilities of hydrogen bonding could result in various dissolving capabilities. , In contrast to solvent–solute intermolecular interactions, the solvent–solvent intermolecular interactions which can be quantitatively represented by the cohesive energy density of solvent could lead to the decrease of the solubility for a solute in solid–liquid equilibrium systems . Generally, a higher value of cohesive energy density means stronger solvent–solvent intermolecular interactions. ,− …”