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Class 12 · Chemistry
→If a 0.2 m solution contains 0.04 mol of solute and the mass of the solute is 4.8 g, what is its molar mass?
Class 12 · Chemistry
→A 125 mL sample of a 0.04 M solution contains 0.9 g of solute. What is the molar mass of the solute?
Class 12 · Chemistry
→If 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 12 · Chemistry
→For 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 12 · Chemistry
→In a solution, the true molar mass of the solute is 100 g mol⁻¹, but the vapour-pressure method gives an observed molar mass of 50 g mol⁻¹. Which conclusion is correct?
Class 12 · Chemistry
→If 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 12 · Chemistry
→An 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 12 · Chemistry
→If 250 mL of a 0.01 M solution contains 0.75 g of solute, what is the molar mass of the solute?
Class 12 · Chemistry
→When 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 12 · Chemistry
→A 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 12 · Chemistry
→A 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 12 · Chemistry
→When 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 12 · Chemistry
→If the observed molar mass of a solute is 1.6 times its true molar mass, what is the van’t Hoff factor, i?
Class 12 · Chemistry
→If the observed molar mass of a solute is 0.8 times its true molar mass, what is the van’t Hoff factor, i?
Class 12 · Chemistry
→The molar mass obtained by the boiling-point elevation method is higher than the true molar mass. What is the most common reason?
Class 12 · Chemistry
→The 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 12 · Chemistry
→A 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 12 · Chemistry
→When 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 12 · Chemistry
→A 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 12 · Chemistry
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