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We have previously discussed solution chemistry and the process of ionic solids dissolving in water. We also covered thermodynamics, specifically the distinction between spontaneous and nonspontaneous processes. Now, we will explore the concept of free energy in relation to dissolution. For sodium chloride to dissolve in water, the individual sodium and chloride ions must dissociate from their lattice and become solvated, meaning they are surrounded by water molecules. The positively charged sodium ions interact with the negative end of water's dipole, while the negatively charged chloride ions interact with the positive end. This interaction is key to the dissolution process.
