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Stoichiometric Calculations

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 HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) 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 (Given atomic weights in $g m o l^{- 1}$ Mn=55,Cl=35.5)

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Solution

Number of meq of $M n C l_{2}$ = number of meq of $K M n O_{4}$ = number of meq of $H_{2} C_{2} O_{4}$
Number of meq of $H_{2} C_{2} O_{4}$ = $2 \times (\frac{225}{90}) = 5$
So number of meq of $M n C l_{2}$ =5
$\Rightarrow 5 \times (\frac{w}{126}) \times 10^{- 3} = 5$ (where w=mass of $M n C l_{2}$ present)
$w = 126 g$

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