`10` ml of `H_(2)O_(2)` liberates `12.7 g` of iodine from an acidic `KI` solution. Calculate (a) normality, (b) molarity, (c) volume strength. (d) Strength and (c) percentage strength of `H_(2)O_(2)`.

Explanation

To solve the problem step by step, we will calculate the normality, molarity, volume strength, strength, and percentage strength of hydrogen peroxide (H₂O₂) based on the information given.

### Given:
- Volume of H₂O₂ = 10 mL
- Mass of iodine liberated = 12.7 g
- Molar mass of iodine (I₂) = 127 g/mol (for I, so for I₂ it is 254 g/mol)
- n-factor for H₂O₂ = 2 (since it acts as a reducing agent)
- n-factor for iodine (I₂) = 2 (since 2 moles of electrons are involved in the reduction of 2 moles of I⁻ to I₂)
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