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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।

ChemistryWhich constant is used in the method of freezing-point depression?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16EasyChemistryIn molar mass determination using freezing-point depression, in which unit must the mass of the solvent be expressed?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16EasyChemistryWhich pair will produce nearly the same depression in freezing point at the same molality if both salts are completely dissociated?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistryFor a solution, i = 2.5 and molality is 0.2 m. If Kf = 1.86 K kg mol⁻¹, what is ΔTf?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistryA solution contains 5 g of solute in 100 g of solvent. If the same amount of solute is dissolved in 200 g of solvent, what happens to the depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistrySolutions A and B contain the same amount of solute. Solution A contains 500 g of solvent, whereas solution B contains 1000 g of solvent. Which solution has the greater depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistryIf the freezing point of a solution is 271.9 K and that of the pure solvent is 273.0 K, what is the depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15EasyChemistryWhich solution will have the lowest freezing point if all have molality 0.1 m and dissociation is complete?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16MediumChemistryA solution has a freezing-point depression of 0.372 K. In the same solvent and at the same molality, if the solute completely forms dimers, what will be the new freezing-point depression?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16MediumChemistryA solution contains 18 g of glucose in 1 kg of water. The molar mass of glucose is 180 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹. What is the depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16MediumChemistryIf a solvent has a higher Kf, which conclusion is correct for the same molality of a non-volatile solute?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15EasyChemistryTwo equimolal solutions are given. The first contains completely dissociated BaCl₂ and the second contains glucose. What is the ratio of their freezing-point depressions?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistryUnder which condition will a CaCl2 solution show a greater depression in freezing point than an equimolal NaCl solution?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15MediumChemistryIn a solution, solute particles normally remain completely unassociated. If half of the solute particles form dimers, how will the observed depression in freezing point compare with the ideal value at the same molality?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15HardChemistryA student calculates the molar mass from the depression in freezing point by treating calcium chloride as non-dissociating. What is the main error compared with ideal dissociation?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15HardChemistryWhich of the following properties ideally depends only on the number of solute particles present in a solution and not on their chemical nature?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryA solution has a freezing-point depression, ΔT_f = 0.372 K. If the cryoscopic constant is K_f = 1.86 K kg mol⁻¹ and the molality is m = 0.100 mol kg⁻¹, what is the van’t Hoff factor (i)?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14MediumChemistryA solution has i = 2.5 and molality 0.2 m. If Kf = 1.86 K kg mol⁻¹, what is ΔTf?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14MediumChemistryA 0.1 m solution shows a depression in freezing point lower than the expected value for a non-dissociated solute. What is the most suitable conclusion?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14HardChemistryFor the same solvent at the same temperature, which observation confirms that depression in freezing point is a colligative property?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14Medium