7 public questions tagged with this topic.
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
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
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
30 ppm = 30 g Na₂SO₄ in 10⁶ g solution. Volume = 10⁶/1 = 10⁶ mL = 1000 L. Moles = 30/142 ≈ 0.2113 mol; molarity = 0.2113/1000 ≈ 2.113 × 10⁻⁴ M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
15 ppm = 15 g CaCl₂ in 10⁶ g water. Moles = 15 / 111 ≈ 0.1351 mol. Mass of solvent = 10⁶ g = 1000 kg. Molality = 0.1351 / 1000 ≈ 1.351 × 10⁻⁴ m.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
5 ppm = 5 g NaCl in 10⁶ g water. Moles = 5 / 58.5 ≈ 0.0855 mol. Mass of solvent = 10⁶ g = 1000 kg. Molality = 0.0855 / 1000 ≈ 8.55 × 10⁻⁵ m.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
