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Isobaric vapor−liquid equilibrium data at 101.325 kPa have been determined for the binary systems 3-methyl-1-butanol 3-methyl-1-butyl ethanoate and 1-pentanol pentyl ethanoate. The data were obtained using a vapor recirculating-type equilibrium still. Vapor pressures of 3-methyl-1-butanol and 3-methyl-1-butyl ethanoate were measured in a Swiestoslawski apparatus. Calculations of the nonideality of the vapor phase were made with the second virial coefficients evaluated from the Hayden−O’Connell method. The activity coefficients and boiling points of the solutions were well-correlated with the mole fraction using the Wilson, nonrandom two-liquid (NRTL), and universal quasichemical activity coefficient (UNIQUAC) equations. The mixtures do not present an azeotrope. [ABSTRACT FROM AUTHOR]

The solubilities of lauric acid in n-hexane, acetone, 2-propanol, propanol, 1-bromopropane, and trichloroethylene have been measured using a dynamic equilibrium method from (279.0 to 315.3) K. All systems present positive deviations of the ideal behavior. The solvent that presented the lowest average deviation, concerning the ideality of the system, was trichloroethylene, and the highest value of deviation was found in acetone. The experimental solubility data were correlated with the NRTL, Wilson, and UNIQUAC models. In the n-hexane case, the correction for the existence of dimers was applied. The best results were obtained using UNIQUAC with 0.26 K average root-mean-square deviation of temperature. The solubility in pure solvents decreased in the order: trichloroethylene > 1-bromopropane > 2-propanol > propanol > acetone > n-hexane. [ABSTRACT FROM AUTHOR]

The solubility of stearic acid was measured in ethanol, 2-propanol, heptane, hexane, acetone, and trichloroethylene and in the azeotropic mixtures of the solvents (ethanol−heptane; hexane−ethanol; ethanol−trichloroethylene; acetone−heptane; heptane−2-propanol; acetone−hexane; hexane−2-propanol; 2-propanol−trichloroethylene), by the phase disappearance method, from (290 to 325) K. The stearic acid−pure solvent experimental data were correlated with the Van Laar, Wilson, NRTL, and UNIQUAC equations and the solubility of stearic acid in azeotropic mixtures with the NIBS/Redlich−Kister equation. The UNIFAC solubility prediction improved when the correction for the existence of stearic acid dimers was applied except for systems with trichloroethylene and 2-propanol. The solubility of stearic acid increased in azeotropic mixtures regarding pure solvents except for the heptane−acetone and hexane−acetone mixtures. [ABSTRACT FROM AUTHOR]

The solubility of palmitic acid has been measured in ethanol, 2-propanol, acetone, heptane, hexane, and trichloroethylene and in the azeotropic mixtures of the solvents (ethanol−heptane; hexane−ethanol; ethanol−trichloroethylene; acetone−heptane; heptane−2-propanol; acetone−hexane; hexane−2-propanol; 2-propanol−trichloroethylene), by a dynamic method, from (290 to 325) K. Solubility data in pure solvents were fitted by the Wilson, NRTL, and UNIQUAC equations and the solubility of palmitic acid in azeotropic mixtures with the NIBS/Redlich−Kister equation. For all calculated results, the root-mean-square deviations of solubility temperatures vary from (0.2 to 0.82) K, depending on the equation used. The solubility in pure solvents decreased in the order: trichloroethylene > 2-propanol > hexane > heptane > acetone > ethanol. The solubility of the palmitic acid increased in azeotropic mixtures compared to the pure solvents, except for the ethanol−trichloroethylene mixture where the solubility was similar to the one in pure trichloroethylene. [ABSTRACT FROM AUTHOR]