The solubilities of carbon dioxide and nitrous oxide in three liquid solvents were measured under static phase equilibrium conditions at temperatures of 290.8, 300.9, and 310.1 K and pressures up to 12.34 MPa. The solubility data were determined from the liquid phase density obtained from an Anton-Paar densitometer, and the level of liquid phase expanded by supercritical and subcritical gases. The solubility of N2O in each solvent increased with pressure, but decreased with temperature, and in each case, was greater than that of CO2. Both CO2 and N2O showed the highest solubility in cyclohexanone and the least solubility in N,N-dimethylformamide.