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 uptp 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) KMnO_(4)` for compltete 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 \( H_2C_2O_4 \) (oxalic acid) and \( NaHC_2O_4 \) (sodium hydrogen oxalate) in a mixture weighing 2.02 g. We will use the information provided about the neutralization reactions with NaOH and KMnO4 to set up equations and solve for the masses of the two components.

### Step-by-Step Solution:

1. **Define Variables:**
Let:
- \( A \) = mass of \( H_2C_2O_4 \) in grams
- \( B \) = mass of \( NaHC_2O_4 \) in grams
...