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Class 12 · Chemistry
→In which situation will the observed molar mass of a solute be higher than its true molar mass?
Class 12 · Chemistry
→Among aqueous solutions of equal molality, assuming complete dissociation, which will show the greatest depression in freezing point?
Class 12 · Chemistry
→Which solute, when dissolved in benzene, generally has a van’t Hoff factor i less than 1?
Class 12 · Chemistry
→Which solution will have the lowest freezing point at equal molality, if all solutes behave ideally and are either completely dissociated or non-dissociated?
Class 12 · Chemistry
→A 0.2 mol kg⁻¹ aqueous Na₂SO₄ solution is 50% dissociated. What is its effective molality, expressed as the total concentration of solute particles?
Class 12 · Chemistry
→When 2 g of a non-dissociated solute is dissolved in 250 g of water, the depression in freezing point is 0.186 K. If K_f = 1.86 K kg mol⁻¹, what is the molar mass of the solute?
Class 12 · Chemistry
→If the vapour pressure of a pure solvent is 80 mmHg and that of the solution is 76 mmHg, what is the relative lowering of vapour pressure?
Class 12 · Chemistry
→A solution has a solute mole fraction of 0.08. Assuming that the solute is non-volatile, what is the relative lowering of vapour pressure?
Class 12 · Chemistry
→In which situation will the molar mass of a solute determined from a colligative property be less than its true molar mass?
Class 12 · Chemistry
→What molarity of a CaCl₂ solution will be isotonic with a 0.3 M glucose solution, if CaCl₂ is assumed to dissociate completely?
Class 12 · Chemistry
→Assuming complete dissociation, which solute will produce the greatest depression in freezing point in aqueous solutions of equal molality?
Class 12 · Chemistry
→In a solution of a non-volatile solute, which observation most clearly indicates association of solute molecules?
Class 12 · Chemistry
→Which colligative property is particularly suitable for determining the molar mass of a solute when the solution is very dilute?
Class 12 · Chemistry
→For a 0.1 m non-dissociated solution, the expected freezing-point depression is 0.186 K. The observed freezing-point depression is 0.279 K. What is the van’t Hoff factor i for the solute?
Class 12 · Chemistry
→In a solution of an unknown solute, the van’t Hoff factor (i) is found to be much greater than 1. What is the most suitable explanation?
Class 12 · Chemistry
→If the ebullioscopic constant K_b is larger, how will the elevation in boiling point behave for the same molality and the same van’t Hoff factor i?
Class 12 · Chemistry
→What happens to the vapour pressure of the solvent when the amount of a non-volatile solute in a solution is increased?
Class 12 · Chemistry
→A solution has van’t Hoff factor i = 2.2. If the boiling-point elevation calculated without dissociation is 0.05 K, what is the actual boiling-point elevation?
Class 12 · Chemistry
→A solution and a pure solvent are separated by a semipermeable membrane. During initial osmosis, toward which side will the solvent move?
Class 12 · Chemistry
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