The solubility of 2-methylnaphthalene in different organic solvents was experimentally studied by the equilibrium method at temperatures from (278.15 to 303.15) K under atmospheric pressure. The solubility of 2-methylnaphthalene in all solvents increased with the increasing temperature. The solubility data were correlated with four thermodynamic models including the vant Hoff equation, modified Apelblat equation, lambda h equation, and Wilson model. It was found that the calculated solubility with modified Apelblat equation provided a good agreement with the experimental values for the solubility behavior of 2-methylnaphthalene. The thermodynamic properties of the standard dissolution enthalpy, standard entropy, and the standard mole Gibbs free energy were evaluated based on the vant Hoff analysis. The values of enthalpy of dissolution are positive, which indicate that the dissolution process of 2-methylnaphthalene in different organic solvents is endothermic.