A mixture of `H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)` weighing `2.02 g` was dissolved in water and the solution made upto one litre. `10 mL` of this solution required `3.0 mL` of `0.1 N NaOH` solution for complete neutralization. In another experiment `10 mL` of same solution in hot dilute `H_(2)SO_(4)` medium required `4 mL` of `0.1N KMnO_(4)` for complete neutralization. Calculate the amount of `H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)` in mixture.

Explanation

To solve the problem, we need to determine the amounts of `H2C2O4` (oxalic acid) and `NaHC2O4` (sodium hydrogen oxalate) in a mixture weighing `2.02 g`. We will use the information from the neutralization reactions with `NaOH` and `KMnO4` to set up equations.

### Step 1: Define Variables
Let:
- \( A \) = mass of `H2C2O4` in grams
- \( B \) = mass of `NaHC2O4` in grams

From the problem, we know:
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