By the analytical gravimetric technique, the equilibrium saturated solubilities of L-serine and L-isoleucine in aqueous solutions of sodium nitrate (NaNO3) and potassium nitrate (KNO3) were measured at six different temperatures in the range of 288.15 to 313.15 K. The theoretical studies on the standard transfer Gibbs free energies were performed with the help of experimental solubility data. The molar volume, transfer enthalpy of cavity, transfer Gibbs free energy, and dipole-dipole interactions were also measured to explore complete thermodynamical aspects of these molecules in aqueous electrolytes. In addition, the solute-solute, solute-solvent, and solvent-solvent interactions in terms of transfer Gibbs energies due to chemical interactions and transfer entropy for the present amino acids (AA'S) were calculated by deducting the cavity interaction and dipole-dipole interaction from the total transfer Gibbs free energy (Delta G(t)(0) (i)) and transfer entropies (T Delta S-t(0) (i)). Finally, the stability owing to the chemical nature of the amino acids in aqueous electrolytic solutions is explained by introducing the abovementioned thermodynamical parameters.