$\mathrm{SO}_{2} \mathrm{Cl}_{2}$ on reaction with excess of water results into acidic mixture
$$\mathrm{SO}_{2} \mathrm{Cl}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}+2 \mathrm{HCl}$$
16 moles of $\mathrm{NaOH}$ is required for the complete neutralisation of the resultant acidic mixture. The number of moles of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ used is :
Solution
$$\mathrm{SO}_{2} \mathrm{Cl}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}+2 \mathrm{HCl}$$
<br/><br/>
Moles of $\mathrm{NaOH}$ required for complete neutralization of resultant acidic mixture $=16$ moles
<br/><br/>
And 1 mole of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ produced 4 moles of $\mathrm{H}^{+}$.
<br/><br/>
$\therefore$ Moles of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ used will be $=\frac{16}{4}=4$ moles
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
This question is part of PrepWiser's free JEE Main question bank. 163 more solved questions on Some Basic Concepts of Chemistry are available — start with the harder ones if your accuracy is >70%.