Ka

• HA (aq) ⇌ H+(aq) + A-(aq)

  Ka = [H+] [A-] / [HA]

  When the equation is equimolar you can assume that Ka = [H+]^2 / [HA]
• The larger the value of Ka, the stronger the acid

  • Ka < 1 , then the acid is weak
  • Ka > 1, the the acid is strong
• pKa = -log(Ka)

  • The lower the pKa, the larger the value of Ka, the stronger the acid
• Concentration of HA at the start of a reaction is equal to the conc of HA at equilibrium