Ionic equilibrium Free Pdf notes|Chemistry|

Comprehensive Topic Outline

I. Core Concepts 

1. Electrolytes vs. Non-electrolytes 

    - Strong vs. weak electrolytes (e.g., HCl vs. CH₃COOH)   

    - Dynamic ionic equilibrium in weak electrolytes   

2. Degree of Ionization (α)  

    - Factors affecting α: concentration, dilution, temperature   

3. Ostwald’s Dilution Law

    - Derivation, limitations (only for weak electrolytes)   

II. Acid-Base Theories

1. Arrhenius Concept  

    - Limitations (e.g., fails for CO₂, NH₃)   

2. Brønsted-Lowry Theory 

    - Conjugate pairs (e.g., HCl/Cl⁻, H₃O⁺/H₂O)   

3. Lewis Theory

    - Electron-pair acceptors/donors (e.g., BF₃ as acid)   

III. Key Calculations 

1. pH & pOH

    - Ionic product of water (K_w = 10⁻¹⁴ at 25°C), pH = -log[H⁺]   

2. Salt Hydrolysis  

    - Acidic/basic/neutral salts (e.g., NH₄Cl → acidic, Na₂CO₃ → basic)   

3. Solubility Product (K_sp)

    - K_sp for salt types (AB → S², AB₂ → 4S³)   

    - Precipitation rules: Ionic product vs. K_sp   

IV. Exam-Critical Applications  

1. Common Ion Effect  

    - Suppression of ionization (e.g., CH₃COOH + CH₃COONa)   

    - Role in qualitative analysis (Group II sulfide precipitation)   

2. Buffers & Equilibrium Shifts

    - Le Chatelier’s principle: Concentration/temperature/pressure effects   

V. NEET/JEE Focus  

1. High-Yield Topics

    - pH calculations, hydrolysis predictions, K_sp problems   

2. Mnemonics & Mind Maps

    - Acid strength comparison: HI > HCl > CH₃COOH   

3. Exam Tips

    - Avoiding mistakes: Misapplying dilution law to strong electrolytes   

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