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)

Explanation

To calculate the quantity of `MnCl2` present in the initial solution, we will follow these steps:

### Step 1: Write the balanced chemical equations
We need to balance the reactions involved in the process. The two relevant reactions are:

1. The reaction of `MnCl2` with `K2S2O8`:
\[
2 \text{MnCl}_2 + 5 \text{K}_2\text{S}_2\text{O}_8 + 8 \text{H}_2\text{O} \rightarrow 2 \text{KMnO}_4 + 5 \text{K}_2\text{SO}_4 + 6 \text{HCl}
...