50 mL of an aqueous solution of `H_(2)O_(2)` was treated with an excess of KI solution and dilute `H_(2)SO_(4)`. The liberated iodine required 20 mL 0.1 N `Na_(2)S_(2)O_(3)` solution for complete interaction. Calculate the concentration of `H_(2)O_(2)` in `g//L`.

Free iodine is titrated against standard reducing agent usually with sodium thiosulphate , i.e. K_(2)Cr_(2)O_(7) + 6Kl + 7H_(2)SO_(4) to Cr_(2)(SO_(4))_(3) + 4K_(2) SO_(4) + 7H_(2)O+l_(2) 2CuSO_(4) + 4Kl to Cu_(2)l_(2) + 2K_(2)SO_(4) + l_(2) l_(2) + Na_(2)S_(2)O_(3) to 2Nal + Na_(2)S_(4)O_(6) In iodometric titration, starch solution is used as an indicator. Starch solution gives blue or violet colour with free iodine .At the end point , blue or violet colour disappears when iodine is completely changed to iodide. 50 ml of an aqueous solution of H_(2)O_(2) was treated with excess of Kl in dil. H_(2)SO_(4) . The liberated iodine required 20 ml of 0.1 N Na_(2)S_(2)O_(3) for complete reaction. The concentration of H_(2)O_(2) is

When 100 mL of an aqueous of H_(2)O_(2) is titrated with an excess of KI solution in dilute H_(2)O_(2) , the liberated I_(2) required 50 mL of 0.1 M Na_(2) S_(2)O_(3) solution for complete reaction. Calculate the percentage strength and volume strength of H_(2)O_(2) solution.

When 100 " mL of " an aqueous solution of H_2O_2 is titrated with an excess of KI solution in dilute H_2SO_4 , the liberated I_2 required 50 " mL of " 0.1 M Na_2S_2O_3 solution for complete reaction. Calculate the percentage strength and volume strength of H_2O_2 solution.

When 25 " mL of " an aqueous solution of H_2O_2 is titrated with an excess of KI solution in dilute H_2SO_4 , the liberated I_2 required 20 " mL of " 0.3 N Na_2S_2O_3 solution for complete reaction.volume strength of H_2O_2 solution.