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In this tutorial, we revisit solution chemistry, focusing on the dissolution and dissociation of ionic solids in aqueous solutions. We connect this with thermodynamics, highlighting the distinction between spontaneous and nonspontaneous processes. Specifically, we analyze the free energy of dissolution. For sodium chloride to dissolve, individual ions must become solvated, meaning they separate from the ionic lattice and are surrounded by water molecules. This results in ion-dipole interactions, where sodium ions interact with the negative end of water's dipole, and chloride ions interact with the positive end. These interactions facilitate the dissolution process.