Acid-Base Equilibria (Chemistry)

Recall cards on aqueous acid-base equilibria: the Bronsted-Lowry model (proton donors and acceptors, conjugate acid-base pairs, amphiprotic species, and the autoionization of water with its ion-product constant Kw); the pH and pOH scales (their definitions, the 25 C relation pH + pOH = 14, and acidic, neutral, and basic ranges); relative acid and base strengths (strong versus weak, Ka and Kb, percent ionization, the Ka x Kb = Kw relation for a conjugate pair, the leveling effect, and molecular-structure trends in binary and oxyacids); salt hydrolysis and the acidity of hydrated metal ions; polyprotic acids and their successive ionization constants; buffers (composition, action, capacity, and the Henderson-Hasselbalch equation); and acid-base titrations (titration curves, equivalence and end points, and indicator choice).