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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