Solubilities of Diethyl Phthalate, Dicyclopentadiene, and Styrene in Ionic Liquid 1-Ethyl-3-methylimidazolium Acetate

Abstract

Solubilities of diethyl phthalate (DEP), dicyclopentadiene (DCPD), and styrene in ionic liquid 1-ethyl-3-methylimidazolium acetate ([Emim][OAc]) were measured in the temperature range T = (283.15− 353.15) K and at atmospheric pressure (101.3 kPa) the corresponding temperature−composition phase diagrams were obtained. Solubilities of DEP and DCPD in [Emim][OAc] increase with temperature but the solubility of styrene in [Emim][OAc] decreases with temperature. The ternary liquid−liquid equilibrium data for the system of styrene + glycerol + [Emim][OAc] were also determined at temperatures of 298.15, 308.15, 318.15, and 328.15 K, and the results indicate that the addition of glycerol can significantly reduce the solubility of styrene in [Emim][OAc]. For the ternary system, when the amount of glycerol is enough, the solubility of styrene in [Emim][OAc] increases with temperature. The experimental data were correlated by the nonrandom two-liquid activity coefficient model and the binary interaction parameters were obtained.

The role of hydrogen‐bond in solubilizing drugs by ionic liquids: A molecular dynamics and density functional theory study

“…23 Currently, several effective based-model approaches, such as nonrandom two-liquid (NRTL) model, universal quasi-chemical correlation activity coefficient (UNIQUAC) model, and universal quasichemical functional-group activity coefficient (UNIFAC) model, have been successfully used to explore the solvation behavior of IL-containing systems for developing better ILs. [24][25][26][27][28] For instance, Bogel-Łukasik et al applied NRTL and UNIQUAC models to predict drug solubility in different ILs. 25,26 Although these classical models play an important role in the design of subsequent pharmaceutical processes, the interaction mechanism between drugs and ILs during the solvation process at the molecular level has not been deeply expounded.…”

“…Consequently, a promising alternative is to use a reliable computational tool to gain a general relation between the solvation mechanism and ILs structure, which is of great value for both reducing experimental attempts and quickly determining promising candidate solvents 23 . Currently, several effective based‐model approaches, such as nonrandom two‐liquid (NRTL) model, universal quasi‐chemical correlation activity coefficient (UNIQUAC) model, and universal quasi‐chemical functional‐group activity coefficient (UNIFAC) model, have been successfully used to explore the solvation behavior of IL‐containing systems for developing better ILs 24–28 . For instance, Bogel‐Łukasik et al applied NRTL and UNIQUAC models to predict drug solubility in different ILs 25,26 .…”

Alkyl Vinyl Imidazolium Ionic Liquids as Fuel Binders for Photo-curable Energetic Propellants

“…Since good mechanical properties are essential for final propellant compositions, the possibility of tuning the mechanical properties of the fuel-binder polymer through variation of the monomer structure, for example, by increasing the degrees of freedom of the substituents for plasticization, was explored. The use of classical plasticizers, such as phthalates, was deemed unsuitable due to their low solubility in ionic liquids. − Furthermore, their tendency to phase-separate from the polymer matrix and migrate to interfaces negatively affects the desired mechanical properties and limits the shelf-life of the finished product. − Yet another reason for avoiding classical plasticizers stems from our effort to optimize the redox properties of the composition to maximize the polymer to oxidizer ratio. Most classical plasticizers are effective fuels, having a highly negative OB, for example, bis­(2-ethylhexyl) phthalate, OB = −258%, Δ H f ° = −268.2 kcal mol –1 .…”

Solubility Measurement and Correlation of Fosfomycin Sodium in Six Organic Solvents and Different Binary Solvents at Temperatures between 283.15 and 323.15 K

“…The results suggest that the solubility of FOM-Na decreases with increasing temperature in selected solvents, indicating that the dissolving processes of FOM-Na are exothermic within the experimental temperature range, which is observed during the experiments. It may be attributed to functional groups existing in FOM-Na and the solvent, such as hydrogen bond between the solvent and the solution, some of the clathrates may be destroyed at a high temperature, thus, the solubility decreases with the increasing of the temperature. − …”