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Acid-Base Reactions and Buffers

Acid-base reactions involve the transfer of protons (H⁺), while buffers help resist changes in pH.

Key Concepts​

Acid-Base Reactions​

  • Arrhenius definition: Acid → produces H⁺, Base → produces OH⁻
  • Brønsted-Lowry definition: Acid → proton donor, Base → proton acceptor
  • Neutralization reactions: Acid + Base → Salt + Water

Buffers​

  • Buffer solution: Mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid
  • Function: Resists changes in pH when small amounts of acid or base are added
  • Henderson-Hasselbalch Equation:
    • pH = pKa + log([A⁻]/[HA])

Example​

  • Acetic acid (CH₃COOH) + Sodium acetate (CH₃COONa)
    • Addition of H⁺ → reacts with CH₃COO⁻ → minimal pH change
    • Addition of OH⁻ → reacts with CH₃COOH → minimal pH change

Importance​

  • Crucial for biological systems (blood pH regulation)
  • Used in industrial chemical processes
  • Fundamental for titration and analytical chemistry

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