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

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 ChemistryA 300 mL solution is prepared using 1.8 g of solute. At 300 K, its osmotic pressure is 0.492 atm. If i = 1.2, what is the true molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard 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 ChemistryIf the true molar mass of a solute is 240 g mol⁻¹ and the colligative method gives an observed molar mass of 160 g mol⁻¹, what are i and the probable behaviour of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryWhen 2 g of a solute is dissolved in 0.4 kg of solvent, the effective molality is 0.10 m. If i = 0.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryIf a 0.3 m solution has i = 0.6, what molality would appear from a colligative property if the van’t Hoff factor correction were ignored?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryWhen 5 g of a solute is dissolved in 500 g of solvent, the elevation in boiling point is 0.078 K. If Kb = 0.52 K kg mol⁻¹ and i = 1.5, 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 ChemistryAn electrolyte of the type A₂B₃ has a van’t Hoff factor (i) of 3.4. On complete dissociation, one formula unit produces five particles. What is the degree of dissociation of the electrolyte?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium ChemistryA 500 mL solution is prepared using 2 g of solute. At 300 K, its osmotic pressure is 0.615 atm. If i = 1.25, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium 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 Chemistry3 g of a non-volatile solute is dissolved in 72 g of water. The relative lowering of vapour pressure is 0.04. What is the approximate molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryThe observed molar mass of an A₂B-type solute is 1/2.4 of its true molar mass. What is the degree of dissociation?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Hard ChemistryAn AB-type solute is 60% dissociated. If its observed molar mass is 75 g mol⁻¹, what is its true molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium ChemistryA substance forms trimers to the extent of 45%. If its true molar mass is 210 g mol⁻¹, what will be the approximate observed molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Hard ChemistryA substance undergoes 60% dimerization. If its observed molar mass is 200 g mol⁻¹, what is its true molar mass?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium ChemistryA solution has an actual molarity of 0.03 M and a van’t Hoff factor of 1.8. If the true molar mass of the solute is 180 g mol⁻¹, what observed molar mass would be obtained by a colligative-property method?Class 12Chapter 01: Solutions7: Abnormal Molecular MassLevel 17Medium ChemistryWhen 4.8 g of a solute is dissolved in 400 g of solvent, the elevation in boiling point is 0.156 K. If Kb = 0.52 K kg mol⁻¹ and i = 0.75, 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