Ionic Equilibria — Chapter Summary
Maharashtra Board · Class 12 · Chemistry
Summary of Ionic Equilibria for Maharashtra Board Class 12 Chemistry. Key concepts: Strong electrolytes (HCl, Arrhenius and For weak acids.
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Overview
Ionic equilibria deals with the equilibrium between ions and unionized molecules in aqueous solutions. This chapter applies the principles of chemical equilibrium to understand the behavior of acids, bases, and salts in water. It covers fundamental concepts like pH, buffer solutions, hydrolysis, and
Key Concepts
Strong electrolytes (HCl
Strong electrolytes (HCl, NaOH, salts) ionize completely in water, while weak electrolytes (CH₃COOH, NH₄OH) ionize partially. Degree of dissociation (
Arrhenius
Arrhenius: Acids produce H⁺, bases produce OH⁻ in water. Bronsted-Lowry: Acids donate protons, bases accept protons (conjugate acid-base pairs). Lewis
For weak acids
For weak acids: Ka = α²c/(1-α), and for very weak acids Ka = α²c, so α = √(Ka/c). This shows that degree of dissociation increases with dilution. Simi
Water undergoes self
Water undergoes self-ionization: 2H₂O ⇌ H₃O⁺ + OH⁻. Ionic product Kw = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 298K. pH = -log[H⁺], pOH = -log[OH⁻], pH + pOH = 1
Salts of strong acid + strong
Salts of strong acid + strong base: No hydrolysis (neutral). Strong acid + weak base: Cation hydrolysis (acidic). Weak acid + strong base: Anion hydro
Learning Objectives
- Understand the concept of ionic equilibrium and classify electrolytes as strong or weak
- Learn different theories of acids and bases (Arrhenius, Bronsted-Lowry, Lewis)
- Calculate degree of dissociation and apply Ostwald's dilution law
- Understand autoionization of water and the pH scale
- Analyze salt hydrolysis and predict the nature of salt solutions
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Sources & Official References
Content is aligned to the official syllabus. Refer to the board website for the latest curriculum.
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