To measure the quantity of MnCl_(2) dissolved in an aqueous solution, it was completely converted to KMnO_(4) using the reaction.

To measure the quantity of MnCl_(2) dissolved in an aqueous solution,

1.	To measure the quantity of MnCl_(2) dissolved in an aqueous solution, it was completely converted to KMnO_(4) using the reaction.
Answer» Solution :The CHEMICAL equation involved in the conversion of `MnCl_(2) " to " KMnO_(4)` is : `MnCl_(2) +K_(2)S_(2)O_(8)+H_(2)O to KMnO_(4)+H_(2)SO_(4)+HCl` Balanced ionic equation will be : `2Mn^(2+)+5S_(2)O_(8)^(2-)+8H_(2)O to 2MnO_(4)^(2-) +10SO_(4)^(2-)+16H^(+)` Ionic equation involved in the oxidation of oxalic acid by `KMnO_(4)` in acid medium is : `2MnO_(4)^(-)+6H^(+)+5{:(COO^(-),),(\|,),(COO^(-),):}to2Mn^(2+)+8H_(2)O+10CO_(2)` Number of moles of `MnCl_(2)=("Number of moles of oxalic acid")/(2.5)` `=(0.225//90)/(2.5)=1xx10^(-3)` Mass of `MnCl_(2)=0.001xx126g` =0.126 g =126 mg