To measure the quantity of \( \mathrm{MnCl}_{2} \) dissolved in an aqueous solution, it was comp...

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To measure the quantity of \( \mathrm{MnCl}_{2} \) dissolved in an aqueous solution, it was completely converted to \( \mathrm{KMnO}_{4} \) using the reaction, \( \mathrm{MnCl}_{2}+\mathrm{K}_{2} \mathrm{~S}_{2} \mathrm{O}_{8}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{KMnO}_{4}+\mathrm{H}_{2} \mathrm{SO}_{4}+ \) \( \mathrm{HCl} \) (equation not balanced). Few drops of concentrated \( \mathrm{HCl} \) were added to this solution and gently warmed. Further, - oxalic acid (225mg) was added in portions till the colour of the permanganate ion disappeard. The quantity of \( \mathrm{MnCl}_{2} \) (in \( \mathrm{mg} \) ) present in the initial solution is (Atomic weights in \( \mathrm{g} \mathrm{mol}^{-1} \mathrm{Mn}=55, \mathrm{Cl}=35.5 \) )
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