A review of existing experimental phase equilibrium data for systems of near- and/or supercritical fluids (SCF) and ionic liquids (IL) shows that usually the SCF solubility increases with increasing pressure and decreasing temperature. Additionally, polar SCF are better soluble in IL than nonpolar SCF. The experimental data could be correlated by means of the Peng-Robinson equation of state as well as the Van der Waals mixing rules. As a result, the experimental solubility can be calculated reasonably well using two binary interaction parameters.