7 public questions tagged with this topic.
Mass % = (Mass of solute/Total mass) × 100 . For 40%: 40 = (50/50 + w) × 100 . 0.4 (50 + w) = 50 , 50 + w = 125 , w = 75 g .
Ref: NCERT Class 12 Chemistry > Chapter 1: Solutions > Topic: Solubility - of Solids and Gases in Liquids Henry's Law
Molarity = (Moles of solute/Volume in liters) . Moles = Molarity × Volume = 0.2 mol/L × 0.5 L = 0.1 mol .
Ref: NCERT Class 12 Chemistry > Chapter 1: Solutions > Topic: Solubility - of Solids and Gases in Liquids Henry's Law
Moles of glucose = (12/180) ≈ 0.0667 mol . Molality = (0.0667/0.6) ≈ 0.111 mol/kg . Δ Tb = 0.52 × 0.111 ≈ 0.0577 K .
Ref: NCERT Class 12 Chemistry > Chapter 1: Solutions > Topic: Colligative Properties - Relative Lowering and Elevation of Boiling Point
Total mass = 5.6 + 44.4 = 50 g. Mass % = (5.6/50) × 100 = 11.2%.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent
Moles of ethanol = 2.3/46 = 0.05 mol; moles of methanol = 4.8/32 = 0.15 mol. Total moles = 0.05 + 0.15 = 0.2 mol. Molarity = 0.2/0.25 = 0.8 M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of NaCl = 11.7/58.5 = 0.2 mol. Volume = 300 mL = 0.3 L. Molarity = 0.2/0.3 ≈ 0.667 M.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
Moles of CH₃OH = 8/32 = 0.25 mol; moles of H₂O = 54/18 = 3 mol. Total moles = 0.25 + 3 = 3.25. Mole fraction = 0.25/3.25 ≈ 0.0769.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Concentration Terms - Molarity Molality and Mole Fraction
