The solubility of cefradine form I in five pure solvents from (283.15 to 308.15) K was experimentally determined by using an equilibrium method. It was found that the solubility of cefradine form I in all tested solvents increased with the increase of temperature. Four thermodynamic models were used to correlate the experimental, solubility data. The infinite-dilution activity coefficient and mixing properties including the mixing free Gibbs energy, enthalpy, and entropy of cefradine form I solution were also calculated by using the nonrandom two-liquid (NRTL) model. It was found that the correlated results by the van't Hoff equation, the modified Apelblat equation, and the NRTL model agreed well with the experimental data.