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Class 12 · Chemistry
→When 2.0 g of a solute is dissolved in 100 g of water, the depression in freezing point is 0.186 K. If the van’t Hoff factor is 0.5, what is the true molar mass?
Class 12 · Chemistry
→The true molar mass of a solute is 150 g mol⁻¹, but its molar mass determined by a colligative-property method is 100 g mol⁻¹. What is the van’t Hoff factor, and what is the probable behaviour of the solute?
Class 12 · Chemistry
→When 1.5 g of a solute is dissolved in 0.3 kg of solvent, the observed (effective) molality is 0.05 mol kg⁻¹. If the solute has a van’t Hoff factor of 0.75, what is its true molar mass?
Class 12 · Chemistry
→If a solution has a true molality of 0.2 m and its van’t Hoff factor is 2, what molality would appear to be obtained from a colligative property if the i correction were ignored?
Class 12 · Chemistry
→When 3.6 g of a solute is dissolved in 400 g of solvent, the elevation in boiling point is 0.117 K. If Kb = 0.52 K kg mol⁻¹ and i = 1.5, what is the true molar mass?
Class 12 · Chemistry
→When 2.5 g of a solute is dissolved in 200 g of water, the depression in freezing point is 0.465 K. If the van’t Hoff factor is 1.25, what is the true molar mass?
Class 12 · Chemistry
→A solution contains 3.0 g of solute in 600 mL of solution. Its osmotic pressure at 300 K is 0.615 atm. If the van’t Hoff factor is i = 0.75, what is the true molar mass of the solute?
Class 12 · Chemistry
→If the true molar mass of a solute is 200 g mol⁻¹ and 20% dimerization occurs, what will be its approximate observed molar mass?
Class 12 · Chemistry
→A solute has an observed molar mass of 64 g mol⁻¹. If it is an AB₂-type electrolyte and is 25% dissociated, what is its true molar mass?
Class 12 · Chemistry
→In the vapour-pressure method, p⁰ = 100 mm Hg and p = 96 mm Hg. If 2 g of a non-volatile solute is dissolved in 36 g of water, what is the approximate molar mass of the solute?
Class 12 · Chemistry
→CaCl₂ is 75% dissociated in solution. If its observed molar mass is 44.4 g mol⁻¹, what is its true molar mass?
Class 12 · Chemistry
→An A₂B₃-type solute has a van’t Hoff factor i = 3. If complete dissociation produces five particles, what is the degree of dissociation?
Class 12 · Chemistry
→When 0.9 g of a solute is dissolved in 100 g of water, the depression in freezing point is 0.279 K. If Kf = 1.86 K kg mol⁻¹ and the solute has i = 0.75 because of dimer formation, what is its true molar mass?
Class 12 · Chemistry
→When 1.2 g of a solute is dissolved in 150 g of solvent, the elevation in boiling point is 0.104 K. If Kb = 0.52 K kg mol⁻¹ and the solute has a van’t Hoff factor i = 2, what is its true molar mass?
Class 12 · Chemistry
→If the observed molar mass of a solute is 1.25 times its true molar mass, what are the van’t Hoff factor (i) and the type of behaviour shown by the solute?
Class 12 · Chemistry
→If the observed molar mass of a solute is 0.625 times its true molar mass, what are the van’t Hoff factor (i) and the type of behaviour shown by the solute?
Class 12 · Chemistry
→A 250 mL solution is prepared from 3 g of solute. At 300 K, its osmotic pressure is 1.845 atm. If i = 1.5, what is the true molar mass?
Class 12 · Chemistry
→When 2.8 g of a solute is dissolved in 200 g of water, the depression in freezing point is 0.651 K. If the solute is AB-type and 50% dissociated, what is the true molar mass?
Class 12 · Chemistry
→When 2 g of a non-volatile solute is dissolved in 90 g of water, the relative lowering of vapour pressure is 0.02. What is the approximate molar mass of the solute?
Class 12 · Chemistry
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