(A) : Solubility of inert gases in water increases down the group
(R) : Down the group dipole – induced dipole attractions become stronger

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(A) is true but (R) is false

Both (A) and (R) are correct and (R) is the correct explanation of (A)

Both (A) and (R) are false

Both (A) and (R) are correct but (R) is not the correct explanation of (A)

answer is A.

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Detailed Solution

The noble gases are not soluble in water.
The solubility in water increases as the size of noble gases increases.
Noble gas is soluble in water due to the dipole-induced dipole interaction.
As the size of noble gas increases, the gas can be easily polarized by water and distort the electrons.
Noble gases are the non-polar elements, so the only form of intermolecular force property that they have are london dispersion forces, the noble gases can dissolve in water, but in less amount, because some of the water molecules are be able to form dipole-induced dipole attractions with the noble gas atoms.
So, the Solubility of noble gases in the water is due to dipole-induced dipole interaction form.
As dipole-induced dipole interaction increases with the increase of molecular mass of noble gases, hence solubility of noble gases in water increases down the group.
So the solubility order is Xe > Kr > Ar > Na > He.

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