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Weve already discussed solution chemistry at great length, so we understand the process by which an ionic solid can dissolve and dissociate in aqueous solution. We have also discussed the basics regarding thermodynamics and spontaneity, so we understand the difference between a spontaneous and nonspontaneous process. Lets now combine these two concepts to examine the free energy of dissolution. As we recall, in order for something like sodium chloride to dissolve in water, the individual ions must become solvated. That is to say, the ions must separate from one another, leaving the lattice, and become surrounded by water molecules so as to generate ion-dipole interactions. The positively charged sodium ions will interact with the negative end of the net dipole on a number of water molecules, and the negatively charged chloride ions will interact with the positive end of the net dipole on a number of water molecules. This is what prompts dissolution, becau
