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Introduction to Solubility Equilibria

Solubility equilibrium occurs when a solid solute dissolves in a solvent until the rate of dissolution equals the rate of precipitation, resulting in a dynamic equilibrium between dissolved ions and undissolved solid.

Key Concepts​

  • Represented as: AB(s) ⇌ A⁺(aq) + B⁻(aq)
  • Solubility Product (K_sp): Quantifies the equilibrium concentrations of ions
    • K_sp = [A⁺][B⁻]
  • Common-Ion Effect: Presence of a common ion reduces solubility
  • Temperature and pH can affect solubility

Example​

For AgCl(s) ⇌ Ag⁺(aq) + Cl⁻(aq):

  • K_sp = [Ag⁺][Cl⁻]
  • Adding NaCl increases [Cl⁻] → shifts equilibrium left → less AgCl dissolves

Importance​

  • Predicts solubility of salts in different solutions
  • Essential for precipitation reactions
  • Used in analytical chemistry and separation techniques

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