What is the solubility of a gas in water at $25^{\circ} C$ if the partial pressure is $0.346 \ bar$ (Henry's law constant is $0.159 \ mol \ dm^{-3} \ bar^{-1}$)?
- A$0.055 \ mol \ dm^{-3}$
- B$0.028 \ mol \ dm^{-3}$
- C$0.083 \ mol \ dm^{-3}$
- D$0.11 \ mol \ dm^{-3}$
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How many millimoles of nitrogen dissolve when nitrogen is passed in $1 \ L$ water at $293 \ K$ temperature? $[$ The value of $K_H$ is $7.648 \times 10^4 \ bar$ and partial pressure of $N_2$ gas is $0.987 \ bar.]$
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View SolutionWhich of the following statements is $NOT$ true about solubility?
As temperature increases,the value of $K_H$ increases,thus the value of solubility of a gaseous solute will $ . . . . . . $.
The relation between the solubility of a gas in a liquid at a constant temperature and external pressure is stated by which law?
Explain the solubility rule "like dissolves like" in terms of inter-molecular forces that exist in solutions.
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