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?

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

Hint:

Using a simple frame or just bolding for the box
Key Points:
Determine moles of reactant (HgO).
Use stoichiometry of the first reaction to find moles of product relevant to titration (OH$^-$).
Use stoichiometry of the titration reaction (acid-base neutralization, usually 1:1 for strong acid/strong base derived ions).
Calculate the required volume using Molarity = Moles / Volume.
Ensure units are consistent (e.g., moles, L, mL).