Write ionic equations to represent the dissociation of acids and bases in water, conjugate acid/base pairs in solution and amphiprotic nature of some salts

Acid/Base Reactions > Using Brønsted–Lowry Theory >

Dissociation of different acids/bases and their conjugate acid/base pair in solution:

  • Conjugate acid/base pair 1: H2SO4 (acid) / SO42- (conjugate base)
  • Conjugate acid/base pair 2: H2O (base) / H3O+ (conjugate acid)
  • Conjugate acid/base pair 1: HCl (acid) / Cl– (conjugate base)
  • Conjugate acid/base pair 2: H2O (base) / H3O+ (conjugate acid)
  • Conjugate acid/base pair 1: CH3COOH (acid) / CH3COO─ (conjugate base)
  • Conjugate acid/base pair 2: H2O (base) / H3O+ (conjugate acid)
  • Conjugate acid/base pair 1: NH3 (base) / NH4+ (conjugate acid)
  • Conjugate acid/base pair 2: H2O (acid) / OH– (conjugate base)
  • Notice that in case of dissociation of weak bases in water, water behaves like a base whereas in case of acidic dissociations, water showed acidic properties. Such nature of chemical entities to alter their behaviour based on the type of reactants present is known as amphiprotic nature.
  • Conjugate acid/base pair 1: HPO42- (base) / H2PO4─ (conjugate acid)
  • Conjugate acid/base pair 2: H2O (acid) / OH─ (conjugate base)