1. Acid-Base Equilibria a Summary “C” indicates the analytical concentration. For example, C A would be the molarity of an acid solution assuming no dissociation. C B and C S would be the same for a base and a salt.

2. Acid-Base Equilibria a Summary So we might express an acid equilibrium equation as: K A = [H + ][A - ] / [HA] = X 2 /( C A -X) ~ X 2 / C A or (base): K B = X 2 / C B or (acid buffer) K A = X*C S / C A

3. Acid-Base Equilibria a Summary Solutions of Salts: SBSA: pH = 7 SBWA:pH > 7 WBSA:pH < 7 WBWA: pH depends on the K B of the base and the K A of the acid

4. Acid-Base Equilibria a Summary For SBWA salts, it is possible to show: K A *K B = K W where “K B ” is the equilibrium constant for the WA anion. For WBSA salts the same equations holds, but “K A ” is the equilibrium constant for the WB cation.