#solution density

Solubility - of Solids and Gases in Liquids Henry's Law

A 0.4 M solution of KNO₃ (molar mass = 101 g/mol) has a density of 1.1 g/mL. What is the mass percentage of KNO₃ in 250

Moles = 0.4 × 0.25 = 0.1 mol . Mass of KNO₃ = 0.1 × 101 = 10.1 g . Total mass = 250 × 1.1 = 275 g . Mass % = (10.1/275) × 100 ≈ 3.673% .

Ref: NCERT Class 12 Chemistry > Chapter 1: Solutions > Topic: Solubility - of Solids and Gases in Liquids Henry's Law

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Colligative Properties - Depression of Freezing Point

A solution is prepared by dissolving 18 g of a solute in water to make 500 mL of solution with a density of 1.2 g/mL. If

Total mass = 500 × 1.2 = 600 g . Mass of water = 600 - 18 = 582 g = 0.582 kg . Molality = (moles/0.582) = 0.2 . Moles = 0.2 × 0.582 = 0.1164 . Molar mass = (18/0.1164) ≈ 154.64 g/mol .

Ref: NCERT Class 12 Chemistry > Chapter 1: Solutions > Topic: Colligative Properties - Depression of Freezing Point

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Stoichiometry and Stoichiometric Calculations and Limiting Reagent

A solution of HNO₃ has a molarity of 1.5 M and a density of 1.05 g/mL. What is its molality? (Molar mass: HNO₃ = 63 g/mo

Mass of 1 L solution = 1000 × 1.05 = 1050 g. Mass of HNO₃ = 1.5 × 63 = 94.5 g. Mass of water = 955.5 g = 0.9555 kg. Molality = 1.5 / 0.9555 ≈ 1.57 m.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent

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Reactions in Solutions and Mass Percentage and Numericals

A solution of H₂SO₄ has a molarity of 0.5 M and a density of 1.03 g/mL. What is its molality? (Molar mass: H₂SO₄ = 98 g/

Mass of 1 L solution = 1000 × 1.03 = 1030 g. Mass of H₂SO₄ = 0.5 × 98 = 49 g. Mass of water = 981 g = 0.981 kg. Molality = 0.5 / 0.981 ≈ 0.51 m.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Reactions in Solutions and Mass Percentage and Numericals

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Laws of Chemical Combination - Conservation Mass Definite Multiple

A solution of KOH has a density of 1.1 g/mL and a molarity of 2 M. What is its molality? (Molar mass: KOH = 56 g/mol)

Mass of 1 L solution = 1000 × 1.1 = 1100 g. Mass of KOH = 2 × 56 = 112 g. Mass of water = 988 g = 0.988 kg. Molality = 2 / 0.988 ≈ 2.02 m.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Laws of Chemical Combination - Conservation Mass Definite Multiple

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Importance and Nature of Chemistry and Properties of Matter

A solution of HCl has a molarity of 2 M and a density of 1.06 g/mL. What is its molality? (Molar mass: HCl = 36.5 g/mol)

Mass of 1 L solution = 1000 × 1.06 = 1060 g. Mass of HCl = 2 × 36.5 = 73 g. Mass of water = 987 g = 0.987 kg. Molality = 2 / 0.987 ≈ 2.03 m.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Importance and Nature of Chemistry and Properties of Matter

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Concentration Terms - Molarity Molality and Mole Fraction

A 400 mL solution of HCl has a molarity of 0.25 M and a density of 1.01 g/mL. What is the mass percentage of HCl? (Molar

Moles = 0.25 × 0.4 = 0.1 mol; mass of HCl = 0.1 × 36.5 = 3.65 g. Mass of solution = 400 × 1.01 = 404 g. Mass % = (3.65/404) × 100 ≈ 0.904%.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction

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Concentration Terms - Molarity Molality and Mole Fraction

A 500 mL solution of H₂SO₄ has a molarity of 0.2 M and density 1.02 g/mL. What is the mass percentage of H₂SO₄? (Molar m

Moles = 0.2 × 0.5 = 0.1 mol; mass of H₂SO₄ = 0.1 × 98 = 9.8 g. Mass of solution = 500 × 1.02 = 510 g. Mass % = (9.8/510) × 100 ≈ 1.92%.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction

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