If, at 298 K water is the solvent, and Henry’s law constant for $C O_{2}$ is 1.67 kbar and the constant of argon is 40.3 kbar, which of the following statements is true?

Argon is more soluble than

C O_{2}

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Argon is less soluble than

C O_{2}

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Argon is insoluble in water

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Argon and

C O_{2}

are equally soluble

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Solution

The correct option is B Argon is less soluble than $C O_{2}$
Henry’s law is formulated as $P = K_{H} \times χ$ (mole fraction). From this, it is seen that as KH increases, mole fraction decreases in order to compensate the increase in partial pressure of the gas. Hence, higher the $K_{H}$ value lower is the solubility. Therefore, argon is less soluble in water than $C O_{2}$ at 298 K.

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