An amount of 0.01 mole of ${SO}_{2} {Cl}_{2}$ is hydrolysed completely in sufficient water (no gas is allowed to escape out) and the solution is diluted to 200ml. Which of the following statement(s) is/are correct? (Ag =108)

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The solution is 0.05 M in $H_{2} {SO}_{4}$ .

The solution is 0.1 M in HCl.

A volume of 20 ml of the solution exactly requires 20 ml of 0.2 M NaOH solution for complete neutralization.

When 100 ml of the solution is treated with excess of ${AgNO}_{3}$ solution, 1.435 g of AgCl will precipitate out

answer is A, B, C, D.

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Detailed Solution

$\underset{0.01 m o l e}{{SO}_{2} {Cl}_{2}} + 2 H_{2} O \to \underset{0.01 m o l e}{H_{2} {SO}_{4}} + \underset{0.02 m o l e}{2 HCl}$
A) $[H_{2} {SO}_{4}] = \frac{0.01}{200} \times 1000 = 0.05 M$
B) $[HCl] = \frac{0.02}{200} \times 1000 = 0.1 M$
C) $\frac{20 \times 0.05}{1000} \times 2 + \frac{20 \times 0.1}{1000} \times 1 = \frac{V \times 0.2}{1000} \times 1$
$\Rightarrow V_{NaOH} = 20 ml$
D) $\frac{100 \times 0.1}{1000} = \frac{w}{143.5} \Rightarrow W_{AgCl} = 1.435 g$