The boiling point of water in a $0.1$ molal silver nitrate solution (solution $\mathbf{A}$ ) is $\mathbf{x}^{\circ} \mathrm{C}$. To this solution $\mathbf{A}$, 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…

Question

The boiling point of water in a $0.1$ molal silver nitrate solution (solution $\mathbf{A}$ ) is $\mathbf{x}^{\circ} \mathrm{C}$. To this solution $\mathbf{A}$, 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 $\mathbf{A}$ and $\mathbf{B}$ is $\mathbf{y} \times 10^{-2}{ }^{\circ} \mathrm{C}$.
(Assume: Densities of the solutions $\mathbf{A}$ and $\mathbf{B}$ 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 $100^{\circ} \mathrm{C}$.)
The value of

x

is ___.

Aicharya · Accepted Answer

Given for solution A m = 0 . 1 i= 1 for AgNO 3 = 2 K b = 0 .5 &#160; Kg &#160; mol - 1 So &#916;T b = T b &#8722; T b &#8728; = 1 &#160; K b m T b &#8722; 100 &#8728; C = 2 &#215; 0 .5 &#215; 0 .1 T b = 100 &#8728; C + 0 .1 = 100 .1 &#8728; C

The boiling point of water in a $0.1$ molal silver nitrate solution (solution $\mathbf{A}$ ) is…

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