quiz 5 (5/10)

• Bronsted-Lowry: Acids are proton donors and bases are proton acceptors

  lewis definition: acids are electron acceptors (empty orbital) and bases are electron donors (lone pair)
• strong acids (H+)

  • fully dissociate
  • HCL HBr HI HNO3 H2SO4 HClO3 HClO4

  stong bases (OH-)

  • fully dissociate
  • LiOH NaOH KOH RbOH Sr(OH)2 Ba(OH)2
• weak acids (HA / BH)

  • do not fully dissociate
  • "-ic acid" at end of name
  • "ammonium" / + on N
  • COOH
  • CH_ groups = not acidic
  • ex: CH3CH2NH3+ / CH3COOH / tartaric acid / malonic acid

  weak bases (A- / B)

  • do not fully dissociate
  • "-ate" in name
  • "amine" / neutral N
  • COO- group
  • ex: (CH3)2NH / triethylamine / CH3CHCHCOO- / acetate
• amphiprotic: has both acidic proton and can act as a base

  • water / HSO4- / HCO3-
• spectator ions: do not affect pH

  • all ions from strong acids or strong bases
• polyprotic acids: acids that can donate more than one proton

  • ex: H2SO4- but not NH3
• order of identifying letters form strongest to weakest pH:

  1. H+ (1)
  2. BH+/HA (4)
  3. H2O (7)
  4. A-/B (9)
  5. OH- (14)