Question

Which is most soluble water at $ 293K $
A. Helium
B. Neon
C. Xenon
D. Krypton

Answer 1

Hint :The noble gases, also known as inert gases and aerogenes, are elements in the modern periodic table's group 18. This community includes the following elements: Helium is a gas that can be used to $ \left( {He} \right) $ , Argon $ \;(Ar) $ , Neon $ \left( {Ne} \right)\; $ Krypton is a fictional character from the Krypton $ \left( {Kr} \right) $ ,Xenon $ \left( {Xe} \right) $ and Radon $ \left( {Rn} \right). $

Complete Step By Step Answer:
From 298 to 561°K, the solubility of the noble gas $ Ar,{\text{ }}He,{\text{ }}Ne,{\text{ }}Kr,{\text{ }}and{\text{ }}Xe $ in pure water was measured. When combined with existing literature data, these data were extrapolated to the critical point of water, yielding a full set of Henry's law constants ranging from 274 to 647°K. There are also equations that describe the behaviour of the Henry's law constants over this temperature range.
Water does not dissolve noble gases. If the size of noble gases grows larger, so does their solubility in water. Because of the dipole-induced dipole interaction, noble gases are soluble in water. As the size of a noble gas grows larger, water can quickly polarise it, distorting the electrons.
Noble gas intermolecular interactions take the form of London dispersion forces, which are highly affected by the atom's polarizability, which increases as the atomic radius increases. This can be explained by the electrons being "less closely bound" to the nucleus as the atomic radius grows. As the atomic radius decreases in the group, so does the solubility.
In water, noble gases are just slightly soluble. As the size of noble gases grows larger, their solubility in water increases. Because of dipole mediated dipole interaction, noble gases are soluble in water (forces). As the size of a noble gas increases, water molecules can quickly polarise it, distorting the electron cloud. As a result, as the size of inert gases increases from $ \left( {He} \right) $ to $ \left( {Rn} \right). $ their solubility in water increases. Krypton is the most soluble in water among the noble gases at $ 293K $
As a result, option D is right.

Note :
Now a question may arise here that, Why isn't radon the simplest noble gas to dissolve? Since radon (and other heavy radioactive elements) are rare, they are often overlooked when discussing trends. While radon is the most soluble noble gas, its isotopes' half lives are on the order of hours or days, rendering it ineffective.