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Ampholyte (amphiprotic) substance Simplified Revision Notes

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Ampholyte (amphiprotic) substance

1. Definition of an Ampholyte

An ampholyte is a substance that can act as both an acid and a base, depending on its reaction partner.

Key Properties:

  • Acts as a base when reacting with an acid.
  • Acts as an acid when reacting with a base.
infoNote

2. Examples of Ampholytes

a) Water (H2O)(H₂O) as an Ampholyte

  • Water as an Acid:
  • H2O+NH3→OH−+NH4+H₂O + NH₃ → OH⁻ + NH₄⁺
  • H2O(acid)→OH−H₂O (acid) → OH⁻ (conjugate base)
  • NH3(base)→NH4+NH₃ (base) → NH₄⁺ (conjugate acid)
  • Water as a Base:
  • HCl+H2O→H3O++Cl−HCl + H₂O → H₃O⁺ + Cl⁻
  • H2O(base)→H3O+H₂O (base) → H₃O⁺ (conjugate acid)
  • HCl(acid)→Cl−HCl (acid) → Cl⁻ (conjugate base)

b) Hydrogen Sulphate Ion (HSO4−)(HSO₄⁻) as an Ampholyte

  • As an Acid:
  • HSO4−+H2O→SO42−+H3O+HSO₄⁻ + H₂O → SO₄²⁻ + H₃O⁺
  • HSO4−(acid)→SO42−HSO₄⁻ (acid) → SO₄²⁻ (conjugate base)
  • H2O(base)→H3O+H₂O (base) → H₃O⁺ (conjugate acid)
  • As a Base:
  • HSO4−+H3O+→H2SO4+H2OHSO₄⁻ + H₃O⁺ → H₂SO₄ + H₂O
  • HSO4−(base)→H2SO4HSO₄⁻ (base) → H₂SO₄ (conjugate acid)
  • H3O+(acid)→H2OH₃O⁺ (acid) → H₂O (conjugate base)

3. Identifying Ampholytes in Acid-Base Reactions

  • A substance is amphiprotic if it can both donate and accept a proton (H+)(H⁺).
  • Common examples include: H2O,HSO4−,HCO3−H₂O, HSO₄⁻, HCO₃⁻.

Exam Tip:

  • If a substance can lose H+H⁺ (act as an acid) and gain H+H⁺ $(act as a base), it is an ampholyte.

4. Summary Table

AmpholyteActs as AcidActs as Base
H2OH₂OH2O→OH−+H+H₂O → OH⁻ + H⁺H2O+H+→H3O+H₂O + H⁺ → H₃O⁺
HSO4−HSO₄⁻HSO4−→SO42−+H+HSO₄⁻ → SO₄²⁻ + H⁺HSO4−+H+→H2SO4HSO₄⁻ + H⁺ → H₂SO₄
HCO3−HCO₃⁻HCO3−→CO32−+H+HCO₃⁻ → CO₃²⁻ + H⁺HCO3−+H+→H2CO3HCO₃⁻ + H⁺ → H₂CO₃
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