The solubility of a solid in a given solvent is decided jointly by its thermodynamic stability and the solute-solvent intermolecular forces. The melting point and enthalpy of melting of 1,9‑Nonanedioic acid as well as its heat capacities at solid and melt state were determined by DSC. The solubilities of 1,9‑Nonanedioic acid in ethanol, acetone, acetic acid and ethylene glycol were measured at temperatures from 276 to 337 K. The solubilities in the four solvents at constant temperature are in the order of ethanol > acetic acid > acetone > ethylene glycol while the temperature dependence is in the opposite order. The experimental solubility data were correlated with the van't Hoff, Wilson and the λh equations with the measured melting properties. The three models with optimized parameters are all able to reproduce the experimental data well, among which the λh equations has lowest average standard deviation and seems to be more consistent with the experimental data. Thermodynamic analysis of the obtained model parameters shows that the dissolution of 1,9‑Nonanedioic acid in the four solvents are all endothermic and mainly driven by the enthalpy change of the solution. The positive excess enthalpy of mixing the 1,9‑Nonanedioic acid melt and the solvent indicates the solute-solvent intermolecular interactions are dominated by repulsive forces.