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 solve the problem of calculating the quantity of `MnCl2` present in the initial solution, we will follow these steps:

### Step 1: Write the balanced chemical equations
The first reaction involves the conversion of `MnCl2` to `KMnO4`:
\[ \text{MnCl}_2 + \text{K}_2\text{S}_2\text{O}_8 + \text{H}_2\text{O} \rightarrow \text{KMnO}_4 + \text{K}_2\text{SO}_4 + \text{HCl} \]

The second reaction is between `KMnO4` and `oxalic acid (C2H2O4)`:
\[ \text{KMnO}_4 + \text{C}_2\text{H}_2\text{O}_4 \rightarrow \text{Mn}^{2+} + \text{CO}_2 + \text{H}_2\text{O} \]
...