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Freezing Point Depression

Class 12 Chemistry के इस tag से जुड़े questions। हर question के साथ chapter, topic, level और difficulty दी गई है।

ChemistryIf the freezing point of a solution is 272.44 K and that of the pure solvent is 273.00 K, what is ΔT_f?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Easy ChemistryIf a 0.2 m nonelectrolyte solution has Kf = 1.86 K kg mol⁻¹, what is the depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 18Easy ChemistryIn the freezing-point-depression method, if the solute mass is doubled while the solvent mass remains constant, what happens to ΔT_f for a nonelectrolyte?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Easy ChemistryWhen 4.5 g of a nonelectrolyte is dissolved in 250 g of water, the freezing-point depression is 0.372 K. If Kf = 1.86 K kg mol⁻¹, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 3 g of a nonelectrolyte is dissolved in 500 g of water, ΔTf = 0.186 K. If Kf = 1.86 K kg mol⁻¹, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 1.5 g of a nonelectrolyte is dissolved in 100 g of water, the depression in freezing point is 0.279 K. If Kf = 1.86 K kg mol⁻¹, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryThe molar mass obtained from freezing-point depression is lower than expected. If the solute is an electrolyte, which reason is suitable?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 17Medium ChemistryWhat common principle is used in molar mass determination by both boiling-point elevation and freezing-point depression?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryIn the freezing-point-depression method, \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), \(\Delta T_f=0.93\,\mathrm{K}\), and the solute is non-dissociating. What is the molality?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Easy ChemistryIf a 0.2 mol kg⁻¹ non-dissociating solution has K_f = 1.86 K kg mol⁻¹, what is the freezing-point depression?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 17Easy ChemistryIf 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 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryIn 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 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryThe 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 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Easy ChemistryIn the freezing-point depression method, 1.0 g of solute is dissolved in 100 g of solvent. If Kf = 2.0 K kg mol⁻¹ and ΔTf = 0.20 K, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryWhen 1 g of a non-dissociated solute is dissolved in 100 g of water, the freezing-point depression is 0.093 K. If Kf = 1.86 K kg mol⁻¹, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhich sequence is most appropriate for determining molar mass from depression in freezing point?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryThe true molar mass of a substance is 60 g mol^-1, but the freezing-point method gives an observed molar mass of 30 g mol^-1. What is the value of the van't Hoff factor i?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 16Medium ChemistryIf 0.5 g of a solute dissolved in 50 g of water produces ΔT_f = 0.186 K, what is its molar mass when K_f = 1.86 K kg mol⁻¹?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 3 g of a non-dissociated solute is dissolved in 200 g of water, ΔT_f = 0.279 K. If K_f = 1.86 K kg mol⁻¹, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhich property forms the basis for determining the molar mass of a solute using a colligative property such as freezing-point depression?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium