Solubility Measurement and Data Correlation of 5,5-Dimethylhydantoin in 12 Pure Solvents at Temperatures from 283.15 to 323.15 K

Abstract

The solubility of 5,5-dimethylhydantoin (DMH) in 12 pure solvents including water, methanol, ethanol, 1-propanol, isopropyl alcohol, 1-butanol, isobutyl alcohol, 2-butanol, 1-pentanol, ethyl acetate, propyl acetate, and acetonitrile was measured at temperatures from 283.15 to 323.15 K under atmospheric pressure by a gravimetric method. The values of the mole fraction solubility of DMH in these solvents increase with increasing temperature and present the following order at a fixed temperature: methanol > ethanol > 2-butanol > isopropyl alcohol > 1-propanol > isobutyl alcohol (1-butanol) > 1-pentanol > water > acetonitrile > ethyl acetate > propyl acetate. They were mathematically correlated by the modified Apelblat equation, van’t Hoff equation, λh equation, and the Wilson model. The results showed a satisfactory correlation for each model.

Solubility Behavior and Polymorphism of N-Acetyl-dl-methionine in 16 Individual Solvents from 283.15 to 323.15 K

“…As an important physicochemical scalar, the cohesive energy density can reflect the strength of the solvent–solvent interaction in the solubility behavior. Generally, the higher cohesive energy density means the stronger solvent–solvent intermolecular interaction, which results in lower solubility. ,, Among the selected solvents, water has the largest cohesive energy density value, showing a remarkably high order of magnitude, which leads to the low solubility of NAM in water.…”

“…Generally, the higher cohesive energy density means the stronger solvent−solvent intermolecular interaction, which results in lower solubility. 39,42,43 Among the selected solvents, water has the largest cohesive energy density value, showing a remarkably high order of magnitude, which leads to the low solubility of NAM in water.…”

Solid–Liquid Equilibrium of l-Thioproline in Nine Neat Solvents and Water + Acetonitrile Binary Solvent System from 283.15 to 323.15 K: Solubility Determination and Data Modeling

“…It is well known that polarity is commonly used to characterize the strength of the intermolecular van der Waals force between the solvent and solute. 38 Except polarity, solvent−solvent interactions (reflected by cohesive energy density) may also affect the solubility of a solute. In general, the higher the cohesive energy density, the stronger intermolecular interaction of solvent−solvent is, which may lead to a lower solubility.…”

“…As a result, solvent polarity seems to be of great significance for influencing the solubility behavior of l -thioproline in the studied solvent systems, but it is not the sole factor. It is well known that polarity is commonly used to characterize the strength of the intermolecular van der Waals force between the solvent and solute . Except polarity, solvent–solvent interactions (reflected by cohesive energy density) may also affect the solubility of a solute.…”

“…Except polarity, solvent–solvent interactions (reflected by cohesive energy density) may also affect the solubility of a solute. In general, the higher the cohesive energy density, the stronger intermolecular interaction of solvent–solvent is, which may lead to a lower solubility. − It can be seen from Table that methanol has the highest cohesive energy among the three alcoholic solvents. On the other hand, the solubility behavior could also be affected by the molecular structure of a solute and a solvent.…”