Thermodynamics Research Center / ThermoML | Journal of Chemical Thermodynamics

ABSTRACT

The solubility of 5-nitro-8-hydroxyquinoline in ten organic solvents including methanol, ethanol, acetone, acetonitrile, acetic acid, n-propanol, toluene, isopropanol, ethyl acetate and 1-butanol was determined experimentally by using the isothermal saturation method over a temperature range from (278.15 to 313.15) K under 101.3 kPa. For the temperature range studied, the solubility of 5-nitro-8- hydroxyquinoline in the solvents increased with a rise of temperature. In general, they obeyed the following order from high to low in different solvents: acetone greater than ethyl acetate greater than toluene greater than acetic acid greater than acetonitrile greater than 1-butanol greater than (n-propanol, ethanol) greater than isopropanol greater than methanol. The acquired solubility data of 5-nitro-8-hydroxyquinoline in the solvents studied were correlated by using the modified Apelblat equation, kh equation, Wilson model and NRTL model. The maximum values of root-mean-square deviation (RMSD) and relative average deviation (RAD) were 1.10 10 4 and 1.39%, respectively. Generally, the RAD values acquired with the modified Apelblat equation were smaller than those with the other three models for a certain solvent. Generally, the four thermodynamic models were all acceptable for the systems of 5-nitro-8-hydroxyquinoline in these solvents. Furthermore, the mixing Gibbs energy, mixing enthalpy, mixing entropy, activity coefficient at infinitesimal concentration (c1 1 ) and reduced excess enthalpy (HE;1 1 ) were obtained. The solution process of 5-nitro-8-hydroxyquinoline was spontaneous and endothermic in the studied solvents. The obtained solubility and thermodynamic studies would be very helpful for optimizing the purification process of 5-nitro-8-hydroxyquinoline.