Measurement and Modeling of Solubility of para-tert-Butylbenzoic Acid in Pure and Mixed Organic Solvents at Different Temperatures

Abstract

The solid−liquid phase equilibrium of para-tertbutylbenzoic acid in methanol, ethanol acetic acid, propan-2-ol, hexane, toluene, 1-octanol, para-tert-butyltoluene, methyl 4-tert-butylbenzoate, and binary (methanol + methyl 4-tertbutylbenzoate) mixed solvent have been determined experimentally within the temperature range of 293.15−333.15 K at atmospheric pressure using a static equilibrium method. The solubility of para-tert-butylbenzoic acid increased with the increase in temperature for the pure solvents, while in the case of methanol + methyl 4-tert-butylbenzoate a maximum solubility effect is achieved at 0.6115 solute-free mole fraction of methanol. The experimental solubility data in pure and binary solvent system were correlated by the modified Apelbat equation, the λh (Buchowski) equation, and the NRTL model, among which the modified Apelbat equation provided better agreement than those with the other models. Furthermore, to understand the nature of interactions involved in a solute−solvent system, the dissolution thermodynamic properties, including enthalpy, entropy, and Gibbs free energy, were determined. This experimental data will be an aid for the design and optimization of the separation and purification processes involving para-tert-butylbenzoic acid.

Measurement and Correlation of Solubility of Two Isomers of Cyanopyridine in Eight Pure Solvents from 268.15 K to 318.15 K

“…The solubility of 3- and 4-CNP was determined using the gravimetric method. − Excessive amounts of 3- and 4-CNP were added into various organic solvents in sealed glass jacketed cells (50 mL) with magnetic stirrer. The temperature from 268.15 K to 318.15 K was controlled by a Julabo FP51 thermostatic bath (±0.01 K).…”

Solubility Modeling and Mixing Thermodynamics of Thiamphenicol in Water and Twelve Neat Organic Solvents from T = (278.15 to 318.15) K

“…The evaluation of thermodynamic functions of mixtures is essential for modeling liquid–solid equilibrium investigations. The mixing enthalpy (Δ mix H °) varies on the basis of the interactions of solvent–solvent, solvent–solute, and solute–solute, whereas the entropy change (Δ mix S °) is a function of the disorder degree or randomness of a mixture . Thus, so as to understand the solubility behavior of thiamphenicol in the selected neat solvents, the thermodynamic properties of mixtures are evaluated.…”

“…Thus, so as to understand the solubility behavior of thiamphenicol in the selected neat solvents, the thermodynamic properties of mixtures are evaluated. Since all the mixtures under consideration are nonideal, the mixing enthalpy (Δ mix H ), mixing entropy (Δ mix S ), and the Gibbs energy change of mixing (Δ mix G ) may be evaluated as the following equation. , where M E refers to the excess property in actual mixtures. Δ mix H , Δ mix S , and Δ mix G represent the mixing enthalpy, mixing entropy, and change of mixing Gibbs energy, respectively.…”

“…The mixing enthalpy (Δ mix H°) varies on the basis of the interactions of solvent−solvent, solvent−solute, and solute−solute, whereas the entropy change (Δ mix S°) is a function of the disorder degree or randomness of a mixture. 39 Thus, so as to understand the solubility behavior of thiamphenicol in the selected neat solvents, the thermodynamic properties of mixtures are evaluated. Since all the mixtures under consideration are nonideal, the mixing enthalpy (Δ mix H), mixing entropy (Δ mix S), and the Gibbs energy change of mixing (Δ mix G) may be evaluated as the following equation.…”

“…Since all the mixtures under consideration are nonideal, the mixing enthalpy (Δ mix H), mixing entropy (Δ mix S), and the Gibbs energy change of mixing (Δ mix G) may be evaluated as the following equation. 39,40…”