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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 0.5 g of a solute is dissolved in 250 g of water, the freezing-point depression is 0.0186 K. If i = 1 and Kf for water is 1.86 K kg mol⁻¹, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 4.5 g of a solute is dissolved in 300 g of water, the depression in freezing point is 0.837 K. If i = 1.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryIf K_f = 1.86 K kg mol⁻¹, the solute mass is 4 g, the solvent mass is 200 g, the molar mass of the solute is 100 g mol⁻¹, and the van’t Hoff factor i = 1.5, what is the depression in freezing point, ΔT_f?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryWhen 1.5 g of a solute is dissolved in 100 g of water, the depression in freezing point is 0.186 K. If i = 0.75, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 3 g of a solute is dissolved in 250 g of water, the depression in freezing point is 0.465 K. If the van’t Hoff factor is 1.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 1.8 g of a solute is dissolved in 150 g of water, the depression in freezing point is 0.279 K. If i = 0.75, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 3.6 g of an AB solute is dissolved in 300 g of water, the depression in freezing point is 0.558 K. If the degree of dissociation is 25%, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryWhen 2.5 g of a solute is dissolved in 500 g of water, the depression in freezing point is 0.2325 K. If the van’t Hoff factor is 1.25, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryA student mistakenly uses 0.125 g instead of 125 g for the solvent mass in a freezing-point method. How will the calculated molar mass compare with the correct value?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryWhen 4.0 g of an AB₂-type solute is dissolved in 200 g of water, the freezing-point depression is 0.744 K. If dissociation is 50% and Kf = 1.86 K kg mol⁻¹, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 1.0 g solute is dissolved in 500 g water, the freezing-point depression is 0.0186 K. If i = 1, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen 3.0 g of a solute is dissolved in 200 g of water, the depression in freezing point is 0.558 K. If the van’t Hoff factor is 1.2, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryFor a non-dissociated solute, K_f = 1.86 K kg mol⁻¹, the solute mass is 2.5 g, the solvent mass is 250 g, and the molar mass is 100 g mol⁻¹. What is the depression in freezing point, ΔT_f?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Easy ChemistryWhen 2.0 g of a solute is dissolved in 100 g of water, the depression in freezing point is 0.186 K. If the van’t Hoff factor is 0.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryWhen 2.5 g of a solute is dissolved in 200 g of water, the depression in freezing point is 0.465 K. If the van’t Hoff factor is 1.25, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryWhen 0.9 g of a solute is dissolved in 100 g of water, the depression in freezing point is 0.279 K. If Kf = 1.86 K kg mol⁻¹ and the solute has i = 0.75 because of dimer formation, what is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryWhen 2.8 g of a solute is dissolved in 200 g of water, the depression in freezing point is 0.651 K. If the solute is AB-type and 50% dissociated, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryWhen 4 g of a solute is dissolved in 500 g of water, the depression in freezing point is 0.279 K. If the van’t Hoff factor is 1.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA student mistakenly takes 250 g solvent as 250 kg. In the freezing-point method, how will the calculated molar mass compare with the correct value?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen 3 g of an AB2-type solute is dissolved in 250 g water, ΔTf = 0.558 K. If dissociation is 50% and Kf = 1.86 K kg mol−1, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard