ACID–BASE TITRATION & BUFFERS
COMPLETE STUDY NOTES
Designed for senior high school / first-year college chemistry students.
Includes theory, formulas, worked examples, and exam tips.
1. Acids, Bases, and pH (Quick Review)
Acids and bases are substances that affect the concentration of hydrogen ions (H ⁺) in
solution.
Arrhenius Definition:
• Acid: Produces H⁺ ions in water (e.g., HCl → H⁺ + Cl⁻)
• Base: Produces OH⁻ ions in water (e.g., NaOH → Na⁺ + OH⁻)
Brønsted–Lowry Definition:
• Acid: Proton (H⁺) donor
• Base: Proton (H⁺) acceptor
pH Scale
The pH scale measures the acidity or basicity of a solution.
Formulas:
pH = −log[H⁺]
pOH = −log[OH⁻]
pH + pOH = 14 (at 25°C)
Key Points:
• pH < 7 → acidic
• pH = 7 → neutral
• pH > 7 → basic
Strong vs Weak Acids and Bases
Strong acids/bases completely ionize in water.
Examples:
• Strong acids: HCl, HNO₃, H₂SO₄
• Strong bases: NaOH, KOH
Weak acids/bases partially ionize.
Examples:
COMPLETE STUDY NOTES
Designed for senior high school / first-year college chemistry students.
Includes theory, formulas, worked examples, and exam tips.
1. Acids, Bases, and pH (Quick Review)
Acids and bases are substances that affect the concentration of hydrogen ions (H ⁺) in
solution.
Arrhenius Definition:
• Acid: Produces H⁺ ions in water (e.g., HCl → H⁺ + Cl⁻)
• Base: Produces OH⁻ ions in water (e.g., NaOH → Na⁺ + OH⁻)
Brønsted–Lowry Definition:
• Acid: Proton (H⁺) donor
• Base: Proton (H⁺) acceptor
pH Scale
The pH scale measures the acidity or basicity of a solution.
Formulas:
pH = −log[H⁺]
pOH = −log[OH⁻]
pH + pOH = 14 (at 25°C)
Key Points:
• pH < 7 → acidic
• pH = 7 → neutral
• pH > 7 → basic
Strong vs Weak Acids and Bases
Strong acids/bases completely ionize in water.
Examples:
• Strong acids: HCl, HNO₃, H₂SO₄
• Strong bases: NaOH, KOH
Weak acids/bases partially ionize.
Examples:
