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Colligative Properties

Class 12 Chemistry के इस tag से जुड़े questions। हर question के साथ chapter, topic, level और difficulty दी गई है।

ChemistryWhen 2.0 g of a nonelectrolyte is dissolved in 100 g of solvent, the boiling point of the solution is 373.104 K. The boiling point of the pure solvent is 373.000 K and Kb = 0.52 K kg mol−1. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 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 ChemistryThe normal molar mass of a solute is 90 g mol⁻¹. If its observed molar mass obtained from a colligative-property measurement is 60 g mol⁻¹, what is the van’t Hoff factor?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 18Medium ChemistryA 3.6 g sample of a substance dissolved in 250 g of solvent produces a boiling-point elevation of 0.156 K. If Kb = 0.52 K kg mol⁻¹, what is the molar mass of the substance?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 ChemistryWhy is the osmotic-pressure method considered more reliable for determining the molar mass of large molecules?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium 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 ChemistryA \(250\,mL\) solution is prepared using \(2.5\,g\) of solute. At \(300\,K\), its osmotic pressure is \(\pi=1.23\,atm\). If \(i=2\), what is the true molar mass? Use \(R=0.082\,L\,atm\,K^{-1}\,mol^{-1}\).Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA solute has a van’t Hoff factor of \(i=0.75\) and an observed molar mass of \(160\,g\,mol^{-1}\). What is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf the elevation in boiling point is 0.312 K, K_b = 0.52 K kg mol⁻¹, the solvent mass is 100 g, and the solute mass is 3 g, what is the molar mass of the non-dissociated solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryFor a non-dissociated solute, K_f = 1.86 K kg mol⁻¹ and ΔT_f = 0.558 K. If 6 g of solute is dissolved in 250 g of solvent, what is its molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium 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 ChemistryWhen 2.7 g of a solute is dissolved in 150 g of solvent, the boiling-point elevation is 0.156 K. If Kb = 0.52 K kg mol−1 and the solute is non-electrolytic, what is its molar mass?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 ChemistryA 100 mL solution is prepared from 1.0 g of a solute. At 300 K, its osmotic pressure is 0.615 atm and i = 1.25. What is the true molar mass of the solute?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 ChemistryA student mistakenly uses 200 g of solvent as 200 kg while calculating molar mass from a colligative-property measurement. What will happen to the calculated molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium 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 16Hard