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11 Cards in this Set

  • Front
  • Back
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])