acid bases chem

  1. SA WB salt
    • soln will be acidic
    • weak base results in a stronger conjugate acid so that ion will make soln more acidic
  2. SB WA
    • soln will be basic
    • WA will give a stronger base that'll make soln more basic
  3. WA WB
    state of soln depends on Ka and Kb, whichever is larger
  4. SB SA
    • neutral pH
    • both ions in the salt will be non reactive cus they're both from strong species
  5. relationships
    • Kw=KaKb=1x10^-14
    • pH+pOH=14
    • pH=-log[H]
    • [H]=10^-pH
    • pKa= -logKa
    • pKa + pKb=pKw=14
  6. pKa and Ka relationships
    • the larger the Ka, the smaller the pKa
    • the larger the Ka, the stronger the acid
    • the smaller the pKa, the stronger the acid
  7. acid-base tit.
    • if both strong, equiv point at neutral
    • WA SB, equiv point pH basic
    • Wb SA, equiv point pH acidic
  8. half-equiv point
    • the point where [HA]=[A-]
    • as the base is being added, the acid is dissociating and creating a buffer as the [A-] goes up
  9. equivalence point
    the point where all moles of HA are neutralized/used
  10. buffer
    • resists extreme changes to pH by alternating btwn its acid and conjugate form
    • ideal buffers have equal concentrations and so pH=pKa
  11. henderson-hechlbach
    pH=pKa + log[A-]/[HA]
Card Set
acid bases chem
chem mcat