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Osmotic Pressure and Osmotic Potential

Two liquids A...

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Two liquids A and B form an ideal solution, A 1: 1 mixture (by mole) boils at 80oC. At this temperature pure A has a vapour pressure of 560 mm Hg. The vapour pressure of pure B at this temperature will be: (a) 200 mm Hg (b) 760 mm Hg (c) 860 mm Hg (d) 960 mm Hg

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Q. Two liquids A and B from ideal solutions. At 300 K, the vapour pressure of solution containing 2 mole of A and 3 mole of B is 500 mm Hg. At the same temperature, if one more mole of B is added to this solution, the vapour pressure of the solution increses by 20 mm Hg. Determine the vapour pressure of A and B in their pure states (in mm Hg);

A

B

form ideal solutions. At

300 K

, the vapour pressure of solution containing

1

A

3

B

550 m m H g

. At the same temperature, if one more mole of

B

is added to this solution, the vapour pressure of the solution increases by

10 m m H g

. Determine the vapour pressure of

A

B

in the pure states (in

m m H g

80^{o}

C, the vapour pressure of pure liquid

A

250

H g

and that of pure liquid

B

1000

H g

. If a solution of

A

B

80^{o}

1

atm pressure, the amount of

A

in the mixture is?

1

= 760

Q. The vapour pressure of two pure liquids A and B forming an ideal solution are 400 mm Hg and 800 mm Hg respectively at temperature I. A liquid mixture containing 3:1 molar composition of A and B is present in a cylinder closed by a piston so that the pressure can be varied. The solution is slowly vaporised at temperature I by decreasing the applied pressure from a starting of 760 mm Hg. A pressure gauge (in mm Hg) is connected

80^{\circ} C

the vapour pressure of pure liquid A is 250 mm of Hg and that of pure liquid B is 1000 mm of Hg. If a solution of A and B boils at

80^{\circ} C

and 1 atm pressure, the amount of A in the mixture is (1 atm = 760 mm Hg)

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