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Molar Mass Determination

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

ChemistryA 0.04 m solution is formed by dissolving 2.0 g of a nonelectrolyte in 0.5 kg solvent. If 4.0 g of the same solute is dissolved in 0.25 kg of the same solvent, what will be the new molality?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryA 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 18MediumChemistryA 1.0 L solution is prepared by dissolving 2.2 g of a substance. Its osmotic pressure at 300 K is 0.451 atm. If R = 0.082 L atm K⁻¹ mol⁻¹, what is the approximate molar mass of the substance?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryIf 20% of a substance forms tetramers, what is the van’t Hoff factor?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18HardChemistryWhen 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 18HardChemistryA 0.05 mol kg⁻¹ solution is prepared by dissolving 3.0 g of a nonelectrolyte in 500 g of solvent. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryThe observed molar mass of a substance is 50 g mol⁻¹ and its van’t Hoff factor is 2.4. What is its normal molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryA solution contains 0.6 g of a solute in 0.2 L of solution. If its osmotic pressure at 300 K is 0.369 atm, what is the molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18HardChemistryIn a boiling-point elevation problem, w₂ = 2.0 g solute, w₁ = 400 g solvent, Kb = 0.52 K kg mol⁻¹, and ΔTb = 0.026 K. What is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18HardChemistryWhen 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 18MediumChemistryWhen 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 18MediumChemistryA polymer solution contains 0.2 g polymer in 200 mL solution. At 300 K, its osmotic pressure is 0.0205 atm. If R = 0.082 L atm K⁻¹ mol⁻¹, what is the molar mass of the polymer?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryA solution contains 1.5 g solute dissolved in 0.25 kg solvent. If its molality is 0.06 m, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryIn the vapour-pressure-lowering method, 1.8 g of a solute is dissolved in 9.0 g water. The relative lowering of vapour pressure is 0.10. If the molar mass of water is 18 g mol⁻¹, what is the approximate molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18MediumChemistryA 250 mL solution is prepared using 0.25 g of a polymer. Its osmotic pressure at 300 K is 0.041 atm. If R = 0.082 L atm K−1 mol−1, what is the molar mass of the polymer?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18HardChemistryA 2.5 g solute dissolved in 125 g of solvent produces a boiling-point elevation of 0.26 K. If Kb = 0.52 K kg mol−1, what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 18HardChemistryWhen 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 18HardChemistryFor 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 18MediumChemistryWhen 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 18HardChemistryWhen 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