Question

As per the following equation, 0.217 g of HgO (molecular mass = 217 g mol$^{-1}$) reacts with excess iodide. On titration of the resulting solution, how many mL of 0.01 M HCl is required to reach the equivalence point? \[ \text{HgO} + 4\text{I}^- + \text{H}_2\text{O} \rightarrow \text{HgI}_4^{2-} + 2\text{OH}^- \]

• A. 50 mL
• B. 200 mL
• C. 10 mL
• D. 5 mL

Hint:

Titration strategy: \begin{itemize} \item Calculate moles from stoichiometry \item Convert using $V = n/M$ \item Watch for effective OH$^-$ availability \end{itemize}

Answer 1

The Correct Option is C