Focuses on different ways to express the concentration of solutions, including molarity, molality, and mole fraction with practical calculations.
Moles of C₆H₁₂O₆ = 18/180 = 0.1 mol; moles of H₂O = 4 mol. Total moles = 4.1. Mole fraction = 0.1/4.1 ≈ 0.0244.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of NaCl = 0.1 mol. Moles of H₂O = 5 mol. Total moles = 5.1; mole fraction = 0.1/5.1 ≈ 0.0196.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of CH₃OH = 0.5 mol; moles of H₂O = 2 mol. Total moles = 2.5. Mole fraction = 0.5/2.5 = 0.2.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of H₂O = 0.5 mol; moles of C₂H₅OH = 0.5 mol. Total moles = 1. Mole fraction = 0.5.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of C₂H₅OH = 23/46 = 0.5 mol; moles of H₂O = 1 mol. Total moles = 1.5. Mole fraction = 0.5/1.5 ≈ 0.333.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
M₁V₁ = M₂V₂. 0.1 × 100 = M₂ × (100 + 200). M₂ = (0.1 × 100)/300 ≈ 0.0333 M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
10 ppm = 10 g SO₂ in 10⁶ g solution. Volume = 1000 L. Moles = 10/64 ≈ 0.15625 mol; molarity = 0.15625/1000 ≈ 1.5625 × 10⁻⁴ M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of H₂O = 2 mol; moles of C₂H₅OH = 1 mol. Total moles = 3. Mole fraction = 2/3 ≈ 0.667.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
25 ppm = 25 g NaNO₃ in 10⁶ g solution. Volume = 1000 L. Moles = 25/85 ≈ 0.2941 mol; molarity = 0.2941/1000 ≈ 2.941 × 10⁻⁴ M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
20 ppm = 20 g MgCl₂ in 10⁶ g water. Moles = 20/95 ≈ 0.2105 mol. Mass of solvent = 1000 kg. Molality = 0.2105/1000 ≈ 2.105 × 10⁻⁴ m.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles = 0.4 × 0.5 = 0.2 mol; mass of KNO₃ = 0.2 × 101 = 20.2 g. Mass of solution = 500 × 1.01 = 505 g. Mass % = (20.2/505) × 100 ≈ 4%.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
10 ppm = 10 g K₂SO₄ in 10⁶ g water. Moles = 10/174 ≈ 0.0575 mol. Mass of solvent = 1000 kg. Molality = 0.0575/1000 ≈ 5.75 × 10⁻⁵ m.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
