The boiling point of water in a 0.1 molal silver nitrate solution (solution $A$ ) is $x^{\circ} \mat

Question

The boiling point of water in a 0.1 molal silver nitrate solution (solution $A$ ) is $x^{\circ} \mathrm{C}$. To this solution $A$, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution $B$. The difference in the boiling points of water in the two solutions $A$ and $B$ is $y 	imes 10^{-2}{ }^{\circ} \mathrm{C}$.
(Assume: Densities of the solutions $A$ and $B$ are the same as that of water and the soluble salts dissociate completely.
Use: Molal elevation constant (Ebullioscopic Constant), $K_b=0.5 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$; Boiling point of pure water as $100^{\circ} \mathrm{C}$.)

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See detailed solution for explanation.