JEE - Dilute Solution

Chemistry Level 2

The total vapour pressure of a 4 4 mole % solution of N H X 3 \ce{NH3} in water is 293 293 K is 50 50 torr, and the vapour pressure of pure water is 17 17 torr at this temperature.

Calculate the total vapour pressure (in torr) for a 5 5 mole % solution of N H X 3 . \ce{NH3}.

29.34 torr 47.40 torr 52.60 torr 58.25 torr

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1 solution

James Dohm
Jul 19, 2016

Assume an ideal solution and apply Raoult's Law. Let the vapor pressure of ammonia be x x . Then:

0.04 x + 0.96 ∗ 17 = 50 → x = 842 0.04x+0.96*17=50 \rightarrow x=842

0.05 ∗ 842 + 0.95 ∗ 17 = 58.25 0.05*842+0.95*17=58.25 torr

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