5.1 g sample of `H_2O_2` solution containg `x%H_2O_2` by weight requires x " mL of " `K_2Cr_2O_7` solution for complete oxidation under acidic condition. What is the molarity of `K_2Cr_2O_7` solution?

Explanation

To solve the problem, we need to find the molarity of the \( K_2Cr_2O_7 \) solution that reacts with a 5.1 g sample of \( H_2O_2 \) solution containing \( x\% \) \( H_2O_2 \) by weight. Here’s a step-by-step breakdown of the solution:

### Step 1: Calculate the weight of \( H_2O_2 \) in the solution
Given that the solution weighs 5.1 g and contains \( x\% \) \( H_2O_2 \):
\[ \text{Weight of } H_2O_2 = \frac{x}{100} \times 5.1 \text{ g} \]

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