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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।

ChemistryA 0.04 M solution has an osmotic pressure of 1.476 atm at 300 K. If the true molar mass is 150 g mol⁻¹, what will be the observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryAn AB₃-type solute is 40% dissociated. If its observed molar mass is 62.5 g mol⁻¹, what is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryA solute forms dimers. Its true molar mass is 120 g mol⁻¹ and its observed molar mass is 150 g mol⁻¹. What is the degree of association?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryThe true molar mass of MgCl₂ is 95 g mol⁻¹. If its observed molar mass from a colligative-property method is 47.5 g mol⁻¹, what is the degree of dissociation?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard ChemistryIn the vapour-pressure method, the mole fraction of a solute is 0.05. If 2.0 g of solute is dissolved in 18 g of water, what is the approximate molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryA 250 mL solution is prepared from 3.0 g of a solute. At 300 K, its osmotic pressure is 0.738 atm. If the solute has i = 0.75, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Hard 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 ChemistryWhich statement is most correct in molar-mass determination when a solute dissociates or associates?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 17Medium ChemistryA 1 L solution is prepared from 2.0 g of a solute. At 300 K, its osmotic pressure is 0.164 atm. If the solute forms dimers to the extent of 50%, 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 ChemistryIf a solute has i = 0.6 and a true molar mass of 90 g mol⁻¹, what will be the observed molar mass from a colligative method?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryAn AB solute has a van’t Hoff factor of 1.4 and an observed molar mass of 75 g mol⁻¹. What are its true molar mass and degree of dissociation, respectively?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf 0.2 g solute in 100 mL solution gives an osmotic pressure of 0.123 atm at 300 K and i = 1, what is the molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA 0.01 M solute has an osmotic pressure of 0.369 atm at 300 K. If R = 0.082 L atm mol⁻¹ K⁻¹, what are i and the likely behaviour of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA solute forms trimers to the extent of 25%. If its true molar mass is 150 g mol⁻¹, what will be the approximate observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryAn AB₂ solute has a true molar mass of 120 g mol⁻¹ and is 80% dissociated. What will be its observed molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA solute has van’t Hoff factor i = 2.4 and an observed molar mass of 50 g mol⁻¹. What is its true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen 5 g of a non-volatile solute is dissolved in 45 g water, the relative lowering of vapour pressure is 0.10. What is the approximate molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard 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_b = 0.52 K kg mol⁻¹, the solute mass is 1.2 g, the solvent mass is 100 g, and the molar mass is 60 g mol⁻¹. What is the elevation in boiling point, ΔT_b?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Easy