Ionic Equilibria
Maharashtra Board · Class 12 · Chemistry
Quick revision notes for Ionic Equilibria — Maharashtra Board Class 12 Chemistry. Key concepts, formulas, and definitions for last-minute revision.
Key Topics to Revise
Types of Electrolytes and Degree of Dissociation
- Strong electrolytes: Complete ionization (HCl, NaOH, salts)
- Weak electrolytes: Partial ionization with equilibrium establishment
- Degree of dissociation (α) = moles dissociated / total moles
Theories of Acids and Bases
- Arrhenius Theory: Acids produce H⁺, bases produce OH⁻ in water
- Brønsted-Lowry Theory: Acids are proton donors, bases are proton acceptors
- Lewis Theory: Acids accept electron pairs, bases donate electron pairs
Ostwald's Dilution Law and Dissociation Constants
- Applies to weak electrolytes in equilibrium state
- Degree of dissociation increases with dilution
- Ka and Kb are equilibrium constants for weak acids and bases
Autoionization of Water and pH Scale
- Pure water undergoes self-ionization: 2H₂O ⇌ H₃O⁺ + OH⁻
- Ionic product of water: Kw = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25°C
- pH = -log₁₀[H⁺], pOH = -log₁₀[OH⁻]
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