Find the pH of resultant solution when 100 mL of 0.005 M `H_(2)SO_(4) " at " 25^(@)C` is diluted to 100 mL. What is the amount of NaOH required to be dissolved in 500 mL to exactly neutralise the above solution ?

Explanation

To solve the problem step by step, we will first find the pH of the resultant solution after dilution and then calculate the amount of NaOH required to neutralize it.

### Step 1: Calculate the moles of \( H_2SO_4 \)

Given:
- Volume of \( H_2SO_4 \) solution = 100 mL = 0.1 L
- Concentration of \( H_2SO_4 \) = 0.005 M

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