Search any question & find its solution
Question:
Answered & Verified by Expert
$\mathrm{MnO}_{4}{ }^{-}$oxidizes (i) oxalate ion in acidic medium at $333 \mathrm{~K}$ and and (ii) HCl. For balanced chemical equations, the ratios $\left[\mathrm{MnO}_{4}^{-}: \mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}\right]$ in (i) and $\left[\mathrm{MnO}_{4}^{-}: \mathrm{HCl}\right]$ in (ii), respectively, are-
Options:
Solution:
1393 Upvotes
Verified Answer
The correct answer is:
$2: 5$ and $1: 8$
$16 \mathrm{H}^{+}+2 \mathrm{MnO}_{4}^{-}+5 \mathrm{C}_{2} \mathrm{O}_{4}^{2-} \rightarrow 2 \mathrm{Mn}^{+2}+10 \mathrm{CO}_{2}+8 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{MnO}_{4}^{-}: \mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}=2: 5$
$2 \mathrm{KMnO}_{4}+16 \mathrm{HCl} \rightarrow 2 \mathrm{KCl}+2 \mathrm{MnCl}_{2}+5 \mathrm{Cl}_{2}+8 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{MnO}_{4}^{-}: \mathrm{HCl}=2: 16=1: 8$
$\mathrm{MnO}_{4}^{-}: \mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}=2: 5$
$2 \mathrm{KMnO}_{4}+16 \mathrm{HCl} \rightarrow 2 \mathrm{KCl}+2 \mathrm{MnCl}_{2}+5 \mathrm{Cl}_{2}+8 \mathrm{H}_{2} \mathrm{O}$
$\mathrm{MnO}_{4}^{-}: \mathrm{HCl}=2: 16=1: 8$
Looking for more such questions to practice?
Download the MARKS App - The ultimate prep app for IIT JEE & NEET with chapter-wise PYQs, revision notes, formula sheets, custom tests & much more.