12.2 - Acids, Bases & Proton Transfer

• Bronsted-Lowry acid

  proton donor
• oxoanion

  H3O+

  formed when H+ dissolves in water
• stron acids

  dissociate almost completely in water
• weak acids

  dissociate in water to an extent
• monoprotic/monobasic acids

  acids that donate one proton per molecule

  one mole of acid neutralises one mole of OH-
• examples of monoprotic acids

  HCl

  HNO3

  CH3COOH
• diprotic/dibasic acid

  acids that donate 2 protons per molecule

  1 mole of acid neutralises 2 moles of OH-
• examples of diprotic acids

  H2SO4

  HOOC-COOH (ethanedioc acid)
• triprotic/tribasic acids

  acids that donate 3 protons per molecule

  one mole of acid neutralises three moles of OH-
• example of triprotic acid

  H3PO4
• Bronsted-Lowry bases

  proton acceptors

  have a lone pair of electrons which can form a dative covalent bond with a proton
• example of Bronsted-Lowry bases

  oxide ion

  OH-

  NH3

  amines

  carbonate ions

  hydrogencarbonate ions
• strong bases

  dissociate almost completely in water
• weak bases

  slightly patronate in water
• conjugate pairs

  species linked by the transfer of a proton

  always on opposite sides of the reaction equation
• conjugate base

  species that gained a proton
• conjugate acid

  species that lost a proton