Ionic Equilibrium — Chapter Summary
Tamil Nadu Board · Class 12 · Chemistry
Summary of Ionic Equilibrium for Tamil Nadu Board Class 12 Chemistry. Part of the Tamil Nadu Board Class 12 Chemistry syllabus.
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Overview
Ionic Equilibrium deals with the behavior of acids, bases, and salts in aqueous solutions. This chapter extends the principles of chemical equilibrium to understand how ions behave in water and how their concentrations affect solution properties. From the carbonic acid-bicarbonate buffer system in o
Key Concepts
According to Svante Arrhenius
According to Svante Arrhenius, an acid is a substance that dissociates in water to produce H⁺ ions (or H₃O⁺), while a base produces OH⁻ ions. Examples
A more general definition where
A more general definition where an acid is a proton (H⁺) donor and a base is a proton acceptor. Example: HCl + H₂O ⇌ H₃O⁺ + Cl⁻. This theory explains
An acid accepts an electron pair
An acid accepts an electron pair (Lewis acid) while a base donates an electron pair (Lewis base). Examples: BF₃ + NH₃ → F₃B←NH₃. Lewis acids include e
Pure water undergoes auto
Pure water undergoes auto-ionization: H₂O + H₂O ⇌ H₃O⁺ + OH⁻. The ionic product of water (Kw) = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ at 25°C. In pure water, [H₃O
pH =
pH = -log[H₃O⁺] and pOH = -log[OH⁻]. At 25°C, pH + pOH = 14 (or pKw). pH values: <7 acidic, =7 neutral, >7 basic. For example, 0.001 M HCl has pH = 3
Learning Objectives
- Classify substances into acids and bases using Arrhenius, Lowry-Bronsted, and Lewis concepts
- Define the pH scale and establish the relationship between pH and pOH
- Describe water ionization equilibrium and calculate ion concentrations
- Apply Ostwald's dilution law to determine dissociation constants of weak electrolytes
- Recognize and explain the common ion effect and its applications
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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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