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Vessel-1 contains w2 g of a non-volatile solute X dissolved in W1 g of water. Vessel-2 contains w2 g
of another non-volatile solute Y dissolved in W1 g of water. Both the vessels are at the same
temperature and pressure. The molar mass of X is 80% of that of Y. The van't Hoff factor for X is
1.2 times of that of Y for their respective concentrations. The elevation of boiling point for solution in Vessel-1 is % of the solution in Vessel-2.

50 mL of 0.2 molal urea solution (density = 1.012 g mL-1 at 300 K) is mixed with 250 mL of a solution
containing 0.06 g of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at 300 K is __
[Use : Molar mass of urea = 60 g mol-1; gas constant, R = 62 L Torr K-1 mol-1 ; Assume, △mixH = 0,
△mixV=0]

An aqueous solution is prepared by dissolving 0.1 mol of an ionic salt in 1.8 kg of water at 35 ℃. The salt remains 90% dissociated in the solution. The vapour pressure of the solution is 59.724 mm of Hg. Vapor pressure of water at 35 ℃ is 60.000 mm of Hg. The number of ions present per formula unit of the ionic salt is __

The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y x 10-2 C.
(Assume : Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.)
Use: Molal elevation constant (Ebullioscopic Constant), Kb = 0.5 K kg mol-1; Boiling point of pure water as 100℃.)
The value of x is __
The value of |y| is __

Liquids A and B form ideal solution for all compositions of A and B at 25°C. Two such solutions with
0.25 and 0.50 mole fractions of A have the total vapor pressures of 0.3 and 0.4 bar, respectively. What is the vapor pressure of pure liquid B in bar?

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JEE Advanced PYQ
Liquid Solution

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