Chapter 2: Acids, Bases, and Salts

 

Chapter 2: Acids, Bases, and Salts ATOM BOMB 

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Chapter 2: Acids, Bases, and Salts

Acids

• Definition: Substances that release hydrogen ions (H⁺) when dissolved in water.

• Properties: Sour taste, turn blue litmus red, conduct electricity, react with metals to release hydrogen.

• Examples: Hydrochloric acid (HCl), Sulfuric acid (H₂SO₄), Nitric acid (HNO₃).

Bases

• Definition: Substances that release hydroxide ions (OH⁻) in water.

• Properties: Bitter taste, slippery feel, turn red litmus blue, neutralize acids to form salt and water.

• Examples: Sodium hydroxide (NaOH), Potassium hydroxide (KOH).

Salts

• Definition: A product of the reaction between an acid and a base.

• Formation:

HCl+NaOH→NaCl+H2OHCl+NaOH→NaCl+H2O (Sodium chloride is formed).

Types of Salts:

1. Normal Salts: Completely neutralized acids (e.g., NaCl).

2. Acidic Salts: Formed by partial neutralization (e.g., NaHSO₄).

3. Basic Salts: Formed by partial neutralization of a base (e.g., Fe(OH)₂SO₄).

pH Scale

• Measures the acidity or basicity of a solution (scale 0 to 14).

  • pH = 7: Neutral (pure water).

  • pH < 7: Acidic (e.g., lemon juice, vinegar).

  • pH > 7: Basic (e.g., soap solution, NaOH).

Neutralization

• The reaction between an acid and a base to form salt and water.

• Example: HCl+NaOH→NaCl+H2OHCl+NaOH→NaCl+H2O

• Chapter 3: Metals and Non-Metals