The solubility of florfenicol form A in eight pure organic solvents (propionic acid, ethanol, 1-propanol, 1-butanol, 2-propanol, 2-methyl-1-propanol, 3-methyl-1-butanol, and 2-ethyl-1-hexanol) and three binary solvents (dimethyl sulfoxide + ethanol, dimethyl sulfoxide + 1-propanol, and dimethyl sulfoxide + 1-butanol) was measured by a laser dynamic method at temperature from 283.15 to 323.15 K. The experimental results show that the mole fraction solubility of florfenicol in the pure solvents decreased according to the following order: ethanolThe experimental results show that the mole fraction solubility of florfenicol form A in the binary solvents increased with the increase of temperature and dimethyl sulfoxide mass fraction. The experimental solubility data were well correlated with the four thermodynamic models: modified Apelblat equation, λh equation, NRTL model equation, and Wilson model equation. The modified Apelblat model equation was regarded as the best one to fit the experimental values in the pure solvents.

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Solubility of phenylphosphonic acid (PPOA) in 15 solvents (methanol, ethanol, n-propanol, isopropyl alcohol, 1-butanol, 1-pentanol, 1-hexanol, 1-heptanol, 1-octanol, 2-methoxyethanol, 2-ethoxyethanol, 2-propoxyethanol, 2-butoxyethanol, acetone, and 1,4-dioxane) was measured by the isothermal saturation method under 0.1 MPa. Solubility of PPOA increased with increasing temperature. The interaction energies between PPOA and selected solvents were calculated by molecular simulation to explain the solubility order. Experimental solubility was correlated by five thermodynamic models including the modified Apelblat equation, uniquac, the nonrandom two-liquid (NRTL)-segment activity coefficient (SAC), NRTL, and the Wilson model. The modified Apelblat equation, NRTL, and NRTL-SAC were more applicable for fitting of solubility data of PPOA. Thermodynamic properties of the mixing process including the mixing Gibbs energy (Δmix G), mixing enthalpy (Δmix H), and mixing entropy (Δmix S) were investigated by the Wilson equation. The mixing process was spontaneous, exothermic, and entropy-driven.

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