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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 of the following properties depends only on the number of solute particles present in a solution and not on their nature?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 15EasyChemistryA solution has ΔTf = 1.86 K, Kf = 1.86 K kg mol⁻¹, and molality m = 0.5 mol kg⁻¹. What is the van’t Hoff factor i?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14MediumChemistryWhich concentration unit is used directly in calculating freezing-point depression and boiling-point elevation?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryWhy does association of a solute decrease the observed depression in freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14MediumChemistryThe freezing point of a pure solvent is 273 K, while the freezing point of its solution is 271.5 K. What is the depression in the freezing point?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryIf a solute has i = 2, how will ΔT_f = iK_fm compare with the non-dissociated case?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryWhy is the freezing point of a solution lower than that of pure water?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryFor a solution, ΔTf = 3.72 K and Kf = 1.86 K kg mol⁻¹. What is the molality of the non-dissociating solute?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14EasyChemistryBetween equal molal solutions of NaCl and glucose, which will have greater freezing point depression if NaCl is assumed to dissociate completely?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 14MediumChemistryIf a solution has a much lower freezing point than the pure solvent, which conclusion may be correct?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 10MediumChemistryIf \(K_f = 1.86\) and \(\Delta T_f = 0.93\), what is the molality?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 10EasyChemistryA solution has freezing point \(-0.6^{\circ}C\) and pure solvent has freezing point \(0^{\circ}C\). What is \(\Delta T_f\)?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 9EasyChemistryIf molality is 0.4 and Kf = 2.0, what is ΔTf?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 9EasyChemistryIf ΔTf is observed greater than expected, which possibility is more suitable?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 11MediumChemistryWhich solution will have the greatest freezing point depression at the same molality?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 10EasyChemistryIf \(i = 3\), \(K_f = 1.8\) and \(m = 0.5\), what is \(\Delta T_f\)?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 10EasyChemistryIf the freezing point of pure water is \(0^{\circ}C\) and \(\Delta T_f = 1.5^{\circ}C\), what is the freezing point of the solution?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 8EasyChemistryIf \(K_f = 1.86\) and \(m = 0.25\), what is the value of \(\Delta T_f\)?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 9EasyChemistryIf K_f = 1.86 and molality is 0.5, what is ΔT_f?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 8EasyChemistryMelting of ice by adding salt is explained by which effect?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 6Easy