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Limiting Reagent or Reactant

To measure th...

Question

To measure the quantity of $M n C l_{2}$ dissolved in an aqueous solution, it was completely converted to $K M n O_{4}$ using the reaction, $M n C l_{2} + K_{2} S_{2} O_{8} + H_{2} O \to K M n O_{4} + H_{2} S O_{4} + H C l$ (equation not balanced).
Few drops of concentrated $H C l$ were added to this solution and gently warmed. Further, oxalic acid $(225 g)$ was added in portions till the colour of the permanganate ion disappeared. The quantity of $M n C l_{2}$ (in mg) present in the initial solution is:
(Atomic weights in $g m o l^{- 1} : M n = 55, C l = 35.5)$ .

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Solution

$M n C l_{2} a m o l + K_{2} S_{2} O_{8} + H_{2} O \to K M n O_{4} + H_{2} S O_{4} + H C l$
${C_{2} O_{4}}^{2 -} + {M n O_{4}}^{-} H^{+} - - \to C O_{2} + M n^{2 +}$
$m_{e q}$ of ${C_{2} O_{4}}^{2 -} = m_{e q}$ of ${M n O_{4}}^{-}$
$2 \times 225 / 90 = a \times 5$
$\Rightarrow a = 1$

$w = 1 \times [55 + 71]$
$= 126 m g$ .

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