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To measure the quantity of MnCl(2) diss...

To measure the quantity of `MnCl_(2)` dissolved in an aqueous solution, it was completely converted to `KMnO_(4)` using the reaction,
`MnCl_(2) + K_(2)S_(2)O_(8) + H_(2)O rarr KMnO_(4) + H_(2)SO_(4) + HCl`
(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 `MnCl_(2)` (in mg) present in the initial solution is _________. (Atomic weights in `gmol^(-1)` : Mn = 55, Cl = 35.5)

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To measure the quantity of MnCl_(2) dissolved in an queous solution, it was completely converted to KMnO_(4) using the reaction MnCl_(2)+K_(2)S_(2)O_(8)+H_(2)O to KMnO_(4)+K_(2)SO_(4)+HCl (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. Calculate the quantity of MnCl_(2) (in mg) presence in the initial solution. ( Atomic weights in g mol^(-1) : Mn=55,Cl=35.5)

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