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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])