SolutionHard
Question
The vapour pressure of a saturated solution of sparingly soluble salt (XCl3) was 17.20 mm Hg at 27°C. If the vapour pressure of pure water is 17.25 mm Hg at 27°C, then what is the solubility of the sparingly soluble salt XCl3 in mole per litre?
Options
A.4.04 × 10−2
B.8.08 × 10−2
C.2.02 × 10−2
D.4.04 × 10−3
Solution
$XCl_{3}(s) \rightleftharpoons \underset{S\text{ M}}{X^{3 +}} + \underset{3S\text{ M}}{3Cl^{-}}$
$\frac{P^{o} - P}{P} = \frac{n_{1}}{n_{2}} \Rightarrow \frac{17.25 - 17.20}{17.20} = \frac{4S}{1000/18} \Rightarrow S = 4.04 \times 10^{- 2}\text{ M}$
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