Why is Henry's law generally applied to dilute solutions of gases in liquids?
ABecause at high gas concentration, ideal proportionality between pressure and mole fraction may fail
BBecause gases cannot dissolve at all beyond very low concentrations
CBecause the value of $K_H$ becomes zero in concentrated solutions
DBecause pressure has no effect on concentrated solutions
Answer & Solution
Correct answer: A. Because at high gas concentration, ideal proportionality between pressure and mole fraction may fail
Henry's law assumes a simple proportional relation between partial pressure and dissolved mole fraction. This approximation is most reliable for dilute solutions; at higher concentrations, deviations from ideal behavior may occur.
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