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Class 12 · Chemistry · Medium
→A 0.05 M solution has the same osmotic pressure as a 0.10 M urea solution. At the same temperature, what is the van’t Hoff factor of that solute?
Class 12 · Chemistry · Easy
→If the relative lowering of vapour pressure of a solution is 0.02, what is the approximate mole fraction of the solute in a dilute solution?
Class 12 · Chemistry · Medium
→Two equimolal solutions are given. The first contains completely dissociated BaCl₂ and the second contains glucose. What is the ratio of their freezing-point depressions?
Class 12 · Chemistry · Medium
→If the elevation in boiling point of a solution is greater than the expected value, which reason is most suitable?
Class 12 · Chemistry · Easy
→Which colligative property is directly used to explain the bursting or shrinking of blood cells?
Class 12 · Chemistry · Medium
→At the same temperature, what is the ratio of the osmotic pressures of 0.1 M urea and 0.1 M completely dissociated K₂SO₄ solutions?
Class 12 · Chemistry · Hard
→A solution contains 0.2 mol of a non-volatile solute in 1 kg of water. If 50% of the solute molecules form dimers, what is the effective molality?
Class 12 · Chemistry · Medium
→Under which condition will a CaCl2 solution show a greater depression in freezing point than an equimolal NaCl solution?
Class 12 · Chemistry · Hard
→If the observed molar mass of a solute is greater than its normal molar mass, what is the most likely reason?
Class 12 · Chemistry · Hard
→Two solutions A and B have the same osmotic pressure at the same temperature. Solution A contains completely dissociated NaCl, while solution B contains a nonelectrolyte. In the same volume, which solution contains fewer actual moles of solute?
Class 12 · Chemistry · Medium
→The osmotic pressure of a polymer solution is very small. Which method is most suitable for determining its molar mass?
Class 12 · Chemistry · Medium
→Which colligative property is most suitable for determining the molar mass of high-molar-mass solutes such as proteins in dilute solutions?
Class 12 · Chemistry · Medium
→In an ideal solution, only the amount of solute is increased while the amount of solvent remains the same. Which statement is most correct?
Class 12 · Chemistry · Medium
→In which situation is the van’t Hoff factor of a solute expected to be less than 1?
Class 12 · Chemistry · Hard
→In a solution, solute particles normally remain completely unassociated. If half of the solute particles form dimers, how will the observed depression in freezing point compare with the ideal value at the same molality?
Class 12 · Chemistry · Hard
→A student calculates the molar mass from the depression in freezing point by treating calcium chloride as non-dissociating. What is the main error compared with ideal dissociation?
Class 12 · Chemistry · Hard
→A 0.1 M solute has a van’t Hoff factor i = 4. At the same temperature, how will its osmotic pressure compare with that of a 0.4 M non-dissociating solute?
Class 12 · Chemistry · Easy
→Which statement about the ebullioscopic constant \(K_b\) and cryoscopic constant \(K_f\) is correct?
Class 12 · Chemistry · Medium
→In which solution will the apparent molar mass determined from colligative properties be greater than the true molar mass because of association of solute particles?
Class 12 · Chemistry · Medium
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