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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।

ChemistryA non-volatile solute lowers the freezing point of a pure solvent. What is the microscopic reason?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium ChemistryIf a 0.2 m urea solution has a freezing-point depression x, what will be the approximate freezing-point depression of an ideal 0.2 m calcium chloride solution?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium ChemistryIf glucose, sodium chloride, and aluminium chloride are dissolved in three solutions of equal molality, what is the correct order of freezing-point depression under ideal conditions?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium ChemistryA 0.2 m solution has a freezing-point depression of 0.186 K. If Kf = 1.86 K kg mol⁻¹, what is the van’t Hoff factor and what does it indicate?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryA 0.1 m solution has a freezing-point depression of 0.279 K. If Kf = 1.86 K kg mol−1, what is the van’t Hoff factor i?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryIf the molality of a solution is 0.25 m, K_f = 1.86 K kg mol⁻¹, and the van’t Hoff factor is i = 2, what is the magnitude of the depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryA 0.4 m non-dissociated solution has a freezing-point depression of 0.744 K. What will be the freezing-point depression of a 0.2 m CaCl₂ solution in the same solvent if CaCl₂ dissociates completely?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Hard ChemistryDue to the salts dissolved in seawater, which statement is correct compared with pure water?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Easy ChemistryAssuming complete dissociation, which of the following aqueous solutions of equal molality will show the greatest depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryAmong aqueous solutions of equal molality, assuming complete dissociation, which solution will show the greatest depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryIn a solution, the observed depression in freezing point is 40% of the expected value for a non-dissociated solute. What is the most appropriate conclusion about the solute?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Hard ChemistryAmong aqueous solutions of equal molality, assuming complete dissociation, which will show the greatest depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryWhich solution will have the lowest freezing point at equal molality, if all solutes behave ideally and are either completely dissociated or non-dissociated?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Hard ChemistryWhen 2 g of a non-dissociated solute is dissolved in 250 g of water, the depression in freezing point is 0.186 K. If K_f = 1.86 K kg mol⁻¹, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 13Medium ChemistryAssuming complete dissociation, which solute will produce the greatest depression in freezing point in aqueous solutions of equal molality?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryFor a 0.1 m non-dissociated solution, the expected freezing-point depression is 0.186 K. The observed freezing-point depression is 0.279 K. What is the van’t Hoff factor i for the solute?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 13Medium ChemistryWhy is the freezing point of a solution lower than that of the pure solvent?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium ChemistryDissolving 4 g of a non-dissociated solute in 200 g of water produces a freezing-point depression of 0.465 K. If Kf = 1.86 K kg mol−1, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 14Hard ChemistryIf the freezing point of a solution is 1.86 K lower than that of the pure solvent and Kf = 1.86 K kg mol−1, what is the molality of the non-dissociated solute?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium ChemistryFor a 0.05 m AlCl₃ solution with complete dissociation, how will its freezing-point depression compare with that of a non-dissociated 0.05 m solution?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium