Comprehension

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), $K _{ b }=0.5 \,K \,kg\, mol ^{-1}$; Boiling point of pure water as $100^{\circ} C$)

Question: 1

The value of x is ______.

Updated On: May 22, 2024
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Correct Answer: 100.1

Solution and Explanation

Given molality of AgNO3 solution is 0.1 molal (solution-A)

ΔTb = ikb m

AgNO3 → Ag+ + NO3

van’t Hoff factor (i) for AgNO3 = 2

ΔTb = 2 × 0.5 × 0.1

(Ts – Tº) = 0.1

(Ts)A = 100.1ºC, so x = 100.1

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Question: 2

The value of \(|y|\) is ______.

Updated On: Mar 20, 2024
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Correct Answer: 2.5

Solution and Explanation

The value of \(|y|\) is 2.5.

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