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### 11 Cards in this Set

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 acid produces H+ base produces OH- Bronsted-Lowry Acid and Base Acid = donates protons Base = accepts protons Lewis Acid and Base acid = electron-pair acceptor base = electron-pair donor pH ph = -log[H+] = log(1/[H+]) pOH pOH = -log[OH-] = log(1/[OH-]) Water Dissociation Constant (Kw) Kw = [H+][OH-] = 10^(-14) gives pH + pOH = 14 Percent Ionization PI = (ionized acid concentration at equilibrium) / (initial concentration of acid) x 100% Acid Dissociation Constant (Ka) Ka = [H3O+][A-] / [HA] Base Dissociation Constant (Kb) Kb = [B+][OH-] / [BOH] Henderson-Hasselbalch Equation pH = pKa + log([conjugate base] / [weak acid]) pOH = pKb + log([conjugate acid] / [weak base])