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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।

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 ChemistryAn unknown solute forms 750 mL of a 0.02 M solution and the solution contains 2.7 g of the solute. What is its molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf 250 mL of a 0.01 M solution contains 0.75 g of solute, what is the molar mass of the solute?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 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 ChemistryA 200 mL solution is prepared using 1.2 g of a solute. At 300 K, its osmotic pressure is 0.246 atm. If the solute forms dimers and its van’t Hoff factor is i = 0.5, what is the true molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryThe observed molar mass of an AB₂-type solute is half of its true molar mass. What is the degree of dissociation?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen 4 g of a solute is dissolved in 500 g of water, the freezing-point depression is 0.186 K. If the solute is an AB-type solute that dissociates by 50%, what is its true molar mass? Take Kf for water as 1.86 K kg mol⁻¹.Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Hard ChemistryA substance forms trimers. If its van’t Hoff factor is i = 0.6, what is the degree of association?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryThe true molar mass of CaCl₂ is 111 g mol⁻¹. If its observed molar mass is 55.5 g mol⁻¹, what is the degree of dissociation?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf the observed molar mass of an AB-type solute is 5/8 of its true molar mass, what is the degree of dissociation?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryIf the true molar mass of NaCl is 58.5 g mol⁻¹ and the colligative-property method gives an observed molar mass of 39 g mol⁻¹, what is the approximate van’t Hoff factor, i?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA \(1\,\mathrm{L}\) solution is prepared from \(6\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(1.23\,\mathrm{atm}\). The solute is non-dissociating. What is its molar mass?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen \(2\,\mathrm{g}\) of a non-dissociating solute is dissolved in \(100\,\mathrm{g}\) of solvent, the boiling-point elevation is \(0.208\,\mathrm{K}\). If \(K_b=0.52\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryWhen \(3.2\,\mathrm{g}\) of a solute is dissolved in \(400\,\mathrm{g}\) of water, the depression in freezing point is \(0.186\,\mathrm{K}\). Taking \(K_f=1.86\,\mathrm{K\,kg\,mol^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium ChemistryA solution of volume \(500\,\mathrm{mL}\) is prepared using \(1.5\,\mathrm{g}\) of solute. Its osmotic pressure at \(300\,\mathrm{K}\) is \(0.615\,\mathrm{atm}\). If \(R=0.082\,\mathrm{L\,atm\,mol^{-1}\,K^{-1}}\), what is the molar mass of the solute?Class 12Chapter 01: Solutions6: Molar Mass DeterminationLevel 16Medium