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Class 12 · Chemistry
→If the K_b value of the wrong solvent is used while calculating molar mass from boiling-point elevation, what will happen?
Class 12 · Chemistry
→If the mass of a non-dissociating solute remains the same but the mass of the solvent is doubled, what happens to the freezing-point depression?
Class 12 · Chemistry
→Why can an error occur in molar mass determination if the solution is too concentrated?
Class 12 · Chemistry
→If the osmotic pressure of a 0.1 M solution is to be found at 300 K and the solute is non-dissociating, which formula is simplest?
Class 12 · Chemistry
→A solution contains 2 g of solute in 500 mL of solution. If the molar mass is 100 g mol⁻¹, what is the molar concentration?
Class 12 · Chemistry
→If a solute associates to form dimers, why does the molar mass obtained from colligative properties generally increase?
Class 12 · Chemistry
→If the van’t Hoff factor is 2 and the normal molar mass is 100 g mol⁻¹, what is the observed molar mass?
Class 12 · Chemistry
→In the freezing-point depression method, what problem occurs if the total mass of the solution is mistakenly used as the mass of the solvent?
Class 12 · Chemistry
→For a non-dissociating solute, Kb = 0.52 K kg mol⁻¹ and the molality is 0.5 mol kg⁻¹. What is the elevation in boiling point?
Class 12 · Chemistry
→If 1 g of solute is dissolved in 200 g of solvent and its molar mass is 50 g mol⁻¹, what is the molality of the solution?
Class 12 · Chemistry
→In the osmotic-pressure method, 0.01 mol of a non-electrolyte solute is present in 1 L of solution. At 300 K, if R = 0.082 L atm K⁻¹ mol⁻¹, what is the osmotic pressure?
Class 12 · Chemistry
→Which of the following colligative properties can be used to determine the molar mass of a solute?
Class 12 · Chemistry
→While determining molar mass from lowering of vapour pressure, the mole fraction of the solute is related to which quantity?
Class 12 · Chemistry
→The depression in freezing point of a solution is 0.186 K. If K_f = 1.86 K kg mol⁻¹ and the molality of the solution is 0.1 mol kg⁻¹, what is the van’t Hoff factor?
Class 12 · Chemistry
→If an electrolyte gives an observed molar mass lower than its normal molar mass during molar-mass determination, what is the reason?
Class 12 · Chemistry
→In the boiling-point elevation method, 2 g of a non-electrolyte solute is dissolved in 100 g of solvent. If K_b = 0.5 K kg mol⁻¹ and the elevation in boiling point, ΔT_b, is 0.25 K, what is the molar mass of the solute?
Class 12 · Chemistry
→If the observed molar mass is greater than the normal molar mass, what is the simplest possible reason?
Class 12 · Chemistry
→If the normal molar mass is 120 g mol⁻¹ and the observed molar mass is 60 g mol⁻¹, what is the van’t Hoff factor?
Class 12 · Chemistry
→Which method is safest for determining the molar mass of large biomolecules because it does not require a large temperature change?
Class 12 · Chemistry
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