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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 solution contains 4.0 g of solute in 250 g of solvent. If Kf = 2.0 K kg mol⁻¹ and the freezing-point depression is 0.4 K, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 1.6 g of a substance is dissolved in 200 g of water, the freezing-point depression is 0.744 K. If the normal molar mass is 80 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹, what is the van’t Hoff factor i?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryA solution contains 1.0 g solute in 100 g water. If Kf = 1.86 K kg mol⁻¹, the depression in freezing point is 0.093 K, and the normal molar mass is 100 g mol⁻¹, what is the van’t Hoff factor?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 18Hard ChemistryWhen 1.5 g of a non-electrolyte substance is dissolved in 250 g of a solvent, the depression in freezing point is 0.1116 K. If the cryoscopic constant of the solvent is 1.86 K kg mol⁻¹, what is the molar mass of the substance?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 0.8 g of a substance is dissolved in 200 g of water, the depression in freezing point is 0.186 K. If the actual molar mass is 40 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹, what is the behaviour of the solute?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryWhen 1.0 g of a nonelectrolyte is dissolved in 50 g camphor, the freezing-point depression is 8 K. If K_f = 40 K kg mol⁻¹ for camphor, what is the molar mass of the substance?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryFor a solution, the observed freezing-point depression is 0.558 K. For the same amount assuming normal behaviour, the expected depression is 0.372 K. What is the van’t Hoff factor?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Medium ChemistryA 1.0 g sample of an AB-type salt dissolved in 100 g water gives ΔT_f = 0.372 K. If K_f = 1.86 K kg mol⁻¹ and the normal molar mass is 100 g mol⁻¹, what is the degree of dissociation?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryA 0.5 g solute dissolved in 100 g water gives ΔT_f = 0.093 K. If K_f = 1.86 K kg mol⁻¹ and the solute undergoes 50% dimer association, what is its normal molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryWhen 1.8 g of a nonelectrolyte is dissolved in 150 g of solvent, the depression in freezing point is 0.372 K. For the solvent, Kf = 1.86 K kg mol−1. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryFor the same solute, 1.0 g dissolved in 100 g of solvent gives ΔTf = 0.186 K. If 2.0 g of the same solute is dissolved in 250 g of the same solvent, what will be the new value of ΔTf?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Medium ChemistryWhen 4.0 g of a substance is dissolved in 200 g of water, ΔTf = 0.372 K. If its normal molar mass is 100 g mol−1 and Kf = 1.86 K kg mol−1, what is the van’t Hoff factor i in the solution?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Hard ChemistryWhen 1.2 g of a nonelectrolyte is dissolved in 100 g of solvent, the freezing point of the solution is 272.814 K. The freezing point of the pure solvent is 273.000 K and Kf = 1.86 K kg mol−1. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryWhen 2.4 g of a nonelectrolyte is dissolved in 300 g of water, the depression in freezing point is 0.1488 K. If Kf = 1.86 K kg mol⁻¹, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Hard ChemistryWhen \(10\,g\) of an unknown solute is dissolved in \(1\,kg\) of solvent, the freezing-point depression is \(\Delta T_f=0.093\,K\). If \(K_f=1.86\,K\,kg\,mol^{-1}\), what is the molar mass of the solute? Assume no association or dissociation.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf \(1.6\,g\) of solute dissolved in \(200\,g\) of water produces a freezing-point depression of \(\Delta T_f=0.372\,K\), and \(i=2\), what is the true molar mass? Take \(K_f=1.86\,K\,kg\,mol^{-1}\).Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryIf 1.86 g of a non-electrolyte solute dissolved in 100 g of water produces a depression in freezing point of 0.186 K, what is its molar mass? Take K_f = 1.86 K kg mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA non-dissociating solute weighing 4.8 g is dissolved in 300 g of water and produces a freezing-point depression of 0.372 K. What is the molar mass of the solute? Take Kf = 1.86 K kg mol−1.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen 2.0 g of a solute is dissolved in 250 g of water, the freezing-point depression is 0.372 K. If the solute has i = 2, what is its true molar mass? Take Kf for water as 1.86 K kg mol−1.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryThe molar mass of a solute determined by the freezing-point depression method is much lower than its true molar mass. Which reason is most probable?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 16Medium