The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution 0.01 M…
Solutions · Class 12 · JEE Main Previous Year Question
The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution 0.01 M in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in mol L⁻¹) in solution is
- a
- b
- c
- d✓
Strategy:\n> Relate the osmotic pressures () using the effective concentrations (). Assume complete dissociation to determine the van't Hoff factor ().\n\nStep 1: Determine effective concentration for } \ce{BaCl2} \text{\nFormula is , so ions ().\n\n\nStep 2: Determine effective concentration for XY\nWe are told .\n\n\nStep 3: Solve for } C_{XY} \text{\nFor a 1:1 electrolyte , .\n\n\n
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