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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।

ChemistryWhen 3 g of a solute is dissolved in 300 g of water, the depression in freezing point is 0.279 K. If the actual van’t Hoff factor is 1.5, what is the true molar mass? Take Kf for water as 1.86 K kg mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16HardChemistryWhen 4 g of a solute is dissolved in 500 g of water, the freezing-point depression is 0.186 K. If the solute is an AB-type solute that dissociates by 50%, what is its true molar mass? Take Kf for water as 1.86 K kg mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16HardChemistryWhen \(3.2\,\mathrm{g}\) of a solute is dissolved in \(400\,\mathrm{g}\) of water, the depression in freezing point is \(0.186\,\mathrm{K}\). Taking \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16MediumChemistryWhen \(2.4\,\mathrm{g}\) of a non-dissociating solute is dissolved in \(200\,\mathrm{g}\) of water, the freezing point decreases by \(0.372\,\mathrm{K}\). If \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16MediumChemistryWhen \(4.0\,\mathrm{g}\) of a solute is dissolved in \(400\,\mathrm{g}\) of solvent, \(\Delta T_f=0.50\,\mathrm{K}\). If \(K_f=5.0\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryIn a molar mass determination experiment, \(\Delta T_f\) is found to be greater than expected. If the solute is an electrolyte, what is the most suitable reason?Class 12Chapter 01: Solutions5: Colligative PropertiesLevel 17MediumChemistryA solution contains 1.8 g of solute dissolved in 90 g of solvent. If Kf = 1.5 K kg mol⁻¹ and ΔTf = 0.30 K, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryA solution has a freezing-point depression 1.5 times the expected value for a non-dissociated solute. If the solute dissociates into two ions, what is the degree of dissociation?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryEqual masses of two non-dissociating solutes are dissolved separately in equal masses of the same solvent. If both solutions show the same depression in freezing point (ΔTf), what can be concluded about their molar masses?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17HardChemistryIf 1.0 g of solute is present in 100 g of solvent, Kf = 1.86 K kg mol⁻¹, and the molar mass is 100 g mol⁻¹, what is the ideal ΔTf?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryA solution contains 2 g of solute in 200 g of solvent. If Kf = 4.0 K kg mol⁻¹ and ΔTf = 0.50 K, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryWhich property is required to determine the molar mass of a solute by the freezing-point-depression method?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17EasyChemistryWhen \(1.2\,\mathrm{g}\) of a substance is dissolved in \(60\,\mathrm{g}\) of solvent, \(\Delta T_f=0.40\,\mathrm{K}\). If \(K_f=2.0\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryIf the solvent mass in a freezing-point-depression experiment is incorrectly recorded as \(120\,\mathrm{g}\) instead of \(100\,\mathrm{g}\), while all other values are correct, how will the calculated molar mass compare with the actual value?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17HardChemistryWhen 5 g of an unknown solute is dissolved in 500 g of water, the freezing-point depression is 0.186 K. For water, K_f = 1.86 K kg mol⁻¹. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryWhile determining molar mass by the depression-in-freezing-point method, in which situation will the observed molar mass of a solute be greater than its actual molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18HardChemistryA substance has a normal molar mass of 120 g mol⁻¹, but freezing-point depression gives an observed molar mass of 60 g mol⁻¹. If it dissociates into two ions, what is the degree of dissociation?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18HardChemistryIn the freezing-point-depression method, 1.5 g of a solute is dissolved in 50 g of solvent. If K_f = 2.0 K kg mol^{-1} and ΔT_f = 0.60 K, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17MediumChemistryThe molar mass of a substance is determined using both freezing-point depression and boiling-point elevation. If the solvent is not the same in both methods, what should be kept in mind?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryFor a nonelectrolyte, K_f = 1.86 K kg mol⁻¹ and ΔT_f = 0.56 K. What is the approximate molality?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18Easy