Question

The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is $x^{\circ }C.$ 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 $y\times {10}^{-2}$ ${}^{\circ }C$
(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), $K_b=0.5Kkgmo{l}^{-1};$
Boiling point of pure water as ${100}^{\circ }C$). The value of $x$ is

Answer 1

$0.1\text{molal}AgN{O}_3\left(aq\right)\text{solution}$
$AgN{O}_3\to A{g}^{+}\left(aq\right)+NO{{}_3}^{-}\left(aq\right)$
$i=2(\alpha =1,\text{given})$
$\Delta T_b=i\times k_b\times m$
$\Rightarrow \Delta T_b=2\times 0.5\times 0.1=0.1$
Let, the boiling point of solution $‘A^{\prime }$ is $x$
$\therefore 0.1{}^{\circ }C=x-100{}^{\circ }C$
$\Rightarrow x=100.1{}^{\circ }C$