quiz 7 (5/5)

• 5 neutralization equations:

  1. strong acid + strong base [H+ + OH- <-> H2O]
  2. strong acid + neutral weak base [H+ + B <-> BH+ (+H2O)]
  3. strong acid + basic salt [H+ + A- <-> HA (+H2O)]
  4. strong base + neutral weak acid [OH- + HA <-> A- (+H2O)]
  5. strong base + acidic salt [OH- + HB+ <-> B (+H2O)]
• identifying buffers after neutralization

  • look for weak substance + their conjugates
  • ex: HCOOH (A-) + NaHCOOH (HA)
  • ex: NH4 (B) + NH4ClO4 (BH+)

  post neutralization:

  • both compounds must be present
  • strong < weak = buffer will form
  • 1:2 ratio (less of conjugate)
• steps for buffer neutralization calculation:

  1. remove spectators
  2. identify strong
  3. identify buffer
  4. create RICE table of rxn
  5. find moles + find LR
  6. buffer calculation
  7. convert to pH/pOH
• titration:

  strong v strong:

  1. remove spectators
  2. H+/OH- M --> mol
  3. find LR with RICE table
  4. convert remaining mol --> M (with new vol)
  5. convert to pH/pOH

  weak v strong:

  1. remove spectators
  2. convert M to mol
  3. LR with RICE table
  4. determine if in buffer region
  5. if buffer --> Ka(Ca/Cb) / Ka(Cb/Ca)
  6. if not buffer --> solve for [H+]=Ca/[OH-]=Cb
  7. convert to pH/pOH

  weak v strong equivalence point:

  use weak acid calculation --> [X] = (KxCx)^1/2