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)

Answer

A, B

Explanation

`(126)underset("a mole")(MnCl_(2))+K_(2)S_(2)O_(8)+H_(2)Orarrunderset("a mole")(KMnO_(4))+H_(2)SO_(4)+HCl`
`C_(2)O_(4)^(-)+MnO_(4)^(-)overset(H^(+))rarrCO_(2)`
`m_(eq)" of "C_(2)O_(4)^(-)=m_(eq)" of "MnO_(4)^(-)`
`2xx0.225//90=axx5`
`a=1xx[55+71]`
`=126mg`