REACTIONS OF
ACIDS AND BASES
I. Acid with Water
  Acid donates proton (H+) to water.
  Remaining anion = conjugate base
  HF(aq) + H2O(l)  H3O+(aq) + F–(aq)
Acid
Conjugate base
  Conjugate bases of strong acids are neutral.
  HI(aq) + H2O(l)  H3O+(aq) + I–(aq)
Neutral
II. Strong Base with Water
  Base releases hydroxide ions (OH–).
  Remaining cation = conjugate acid
  Neutral for strong bases.
  NaOH(aq) + H2O(l)  Na+(aq) + OH–(aq) + H2O(l)
Base
Conjugate acid
III. Weak Base with Water
  Base accepts proton from water; OH– left over
  Conjugate acid is acidic (can donate protons).
  CH3NH2(aq) + H2O(l)  CH3NH3+(aq) + OH–(aq)
Base
Conjugate acid
  For amines (CHx-NHy) extra H adds to N, not C.
IV. Neutralization
  Acid + Base  Water + Salt
  HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq)
Salt
  Double displacement
  Weak Bases…
  HF(aq) + NH3(aq)  NH4F(aq)
IV. Neutralization
  Diprotic acid (2 H’s)
  1) H2SO4(aq) + KOH(aq)  H2O(l) + K+(aq) +
HSO4–(aq) (strong)
  2) HSO4–(aq) + KOH(aq)  H2O + K+(aq) +
SO42–(aq) (weak)