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 ______${}^{\circ }C$.

Answer 1

Answer: 100.10

$0.1$ molal $AgN{O}_3$ (aq) solution
$AgN{O}_3⟶A{g}^{+}(aq)+N{O}_3{}^{-}(aq)$
$i=1+(2-1)\times 1=2(\alpha =1,$ given )
$\Delta T_b=i\times k_b\times m$
$\Delta T_b=2\times 0.5\times 0.1=0.1$
So, boiling point of solution ' $A$ ' is $=100.10^{\circ }C=x$