Acid/Base Equilibria

Subdecks (1)

Cards (110)

  • Bronsted-Lowry Acid

    Proton donor (H+)
  • Bronsted-Lowry Base

    Proton acceptor
  • Lewis Acid
    Electron pair Acceptor
  • Lewis Base
    Electron pair donor
  • Buffer
    An aqueous solution that resist changes in pH when added to an acid or base
  • Buffers
    • Weak acid with conjugate base
    • Weak base with conjugate acid
  • Phosphate buffer
    Commonly used buffer
  • Ka
    Acid ionization constant/ acid dissociation constant
  • Weak acid equilibrium
    • HF (hydrofluoric acid): Ka= 3.5 x 10^-4
    • CH3COOH (acetic acid): Ka= 1.8 x 10^-5
    • CH3OH (methanol): Ka= 2.9 x 10^-16
  • Weak base equilibrium
    • NH3 (Ammonia): Kb= 1.8 x 10^-5
    • C6H5NH2 (Aniline): Kb= 4.3 x 10^-10
  • Ka x Kb
    Always equal Kw
  • Stronger/higher Kb

    The weaker Kb
  • pKa + pKb
    = 14
  • Neutral salt solution
    Neither the cation or anion will react in water or solution
  • Neutral salt solutions
    • Ba(NO3)2
    • NaCl
  • Basic salt solution
    The cation does not react in water, but the anion does
  • Basic salt solutions
    • Ba(CH3COO)2
    • NaClO
  • Acidic salt solution
    The cation will react with water but the anion will not react with water
  • Acidic salt solutions
    • NH4NO3
    • AlCl3
  • Acidic, Neutral, or Basic salt solution
    The cation and anion both interact with water
  • Acidic, Neutral, or Basic salt solution
    • (NH4)2CO3
  • Increasing the concentration of one of the products

    Shifts the equilibrium to the left
  • the larger the Ka value= the stronger the acid
  • the smaller the Ka value= the weaker the acid
  • the larger the Kb value= the stronger the base
  • the smaller the Kb value= the weaker the base