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Class 12 · Chemistry
→If the soil solution outside a plant root becomes highly concentrated, what will happen to water absorption?
Class 12 · Chemistry
→If 0.1 M NaCl and 0.1 M glucose solutions are compared, what is the osmotic pressure of the NaCl solution, assuming complete dissociation?
Class 12 · Chemistry
→Why is the freezing point of a solution lower than that of the pure solvent?
Class 12 · Chemistry
→In which solution is the van’t Hoff factor likely to be less than 1 because of association of solute molecules?
Class 12 · Chemistry
→If the osmotic pressure of a solution is to be increased while the temperature remains constant, which change will most directly achieve this?
Class 12 · Chemistry
→In which situation will the observed molar mass of a solute be less than its true molar mass?
Class 12 · Chemistry
→What is the effective molar concentration of particles in a 0.1 M K₃PO₄ solution on complete dissociation?
Class 12 · Chemistry
→For a solution, ΔTb = 0.208 K, Kb = 0.52 K kg mol⁻¹, and i = 2. What is the molality of the solution?
Class 11 · Chemistry
→If CH₃COOH associates in benzene, what is the usual value of the van’t Hoff factor i?
Class 12 · Chemistry
→Dissolving 4 g of a non-dissociated solute in 200 g of water produces a freezing-point depression of 0.465 K. If Kf = 1.86 K kg mol−1, what is the molar mass of the solute?
Class 12 · Chemistry
→Which solution will have the highest osmotic pressure at the same temperature if all have a molarity of 0.05 M and dissociation is complete?
Class 12 · Chemistry
→When the molality of a solute is increased in a solution, with all other conditions unchanged, what happens to the elevation in boiling point?
Class 12 · Chemistry
→The osmotic pressure of a 0.1 M solution at 300 K is half of the expected value for a non-dissociated solute. What behaviour does this indicate?
Class 12 · Chemistry
→Which of the following statements about the osmotic pressure of a dilute solution is correct?
Class 12 · Chemistry
→If the freezing point of a solution is 1.86 K lower than that of the pure solvent and Kf = 1.86 K kg mol−1, what is the molality of the non-dissociated solute?
Class 12 · Chemistry
→If 0.5 mol of a solute is dissolved in 2 kg of solvent, what is the molality of the solution?
Class 12 · Chemistry
→Which pair will show the greatest difference in osmotic pressure at the same temperature and same molarity, assuming complete dissociation where applicable?
Class 12 · Chemistry
→For a 0.05 m AlCl₃ solution with complete dissociation, how will its freezing-point depression compare with that of a non-dissociated 0.05 m solution?
Class 12 · Chemistry
→A solution has a relative lowering of vapour pressure of 0.10. If it contains 0.90 mol of solvent, approximately how many moles of solute are present, assuming a very dilute solution?
Class 12 · Chemistry
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