Hydrogen peroxide solution `(20 mL)` reacts quantitatively with a solution of `KMnO_(4) (20 mL)` acidified with dilute of `H_(2)SO_(4)`. The same volume of the `KMnO_(4)` solution is just decolourised by `10 mL` of `MnSO_(4)` in neutral medium simultaneously forming a dark brown precipitate of hydrated `MnO_2`. The brown precipitate is dissolved in `10 mL` of `0.2 M` sodium oxalate under boiling condition in the presence of dilute `H_(2)SO_(4)`. Write the balanced equations involved in the reactions and calculate the molarity of `H_(2)O_(2)`.

Hydrogen peroxide solution `(20 mL)` reacts quantitatively with a solu

1.	Hydrogen peroxide solution `(20 mL)` reacts quantitatively with a solution of `KMnO_(4) (20 mL)` acidified with dilute of `H_(2)SO_(4)`. The same volume of the `KMnO_(4)` solution is just decolourised by `10 mL` of `MnSO_(4)` in neutral medium simultaneously forming a dark brown precipitate of hydrated `MnO_2`. The brown precipitate is dissolved in `10 mL` of `0.2 M` sodium oxalate under boiling condition in the presence of dilute `H_(2)SO_(4)`. Write the balanced equations involved in the reactions and calculate the molarity of `H_(2)O_(2)`.
Answer» `2KMnO_(4)+3H_(2)SO_(4)+5H_(2)O_(2)toK_(2)SO_(4)+2MnSO_(4)+8H_(2)O` `2KMnO_(4)+3MnSO_(4)+2H_(2)Oto5MnO_(2)+2H_(2)SO_(4)+K_(2)SO_(4)` `MnO_(2)+Na_(2)C_(2)O_(4)+2H_(2)SO_(4)toMnSO_(4)+Na_(2)SO_(4)+2H_(2)O+2CO_(2)` millimoles of `Na_(2)C_(2)O_(4)=10xx0.2=2` `m" Eq of "Na_(2)C_(2)O_(4)=4` `m" Eq of "MnO_(2)=4` `m" Eq of "KKMnO_(4)=4` `m" Eq of "H_(2)O_(2)=4` millimoles of `H_(2)O_(2)=2` millimoles of `H_(2)O_(2)=` Molarity`xxV_(mL)` or `2=` molarity `xx20` or molarity `=0.1`

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The purity of `H_2O_2` in a given sample is `85%.` Calculate the weight of impure sample of `H_2O_2` which requires `10mL` of `M//5 KMnO_4` solution in a titration in acidic mediumA. 2 gB. 0.2 gC. 0.17 gD. 0.15 g
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`12. g` of an impure sample of arsenious oxide was dissolved in water containing `7.5 g` of sodium bicarbonate and the resulting solution was diluted to `250 mL`. `25 mL` of this solution was completely oxidised by `22.4 mL` of a solution of iodine. `25 mL` of this iodine solution reacted with same volume of a solution containing `24.8 g` of sodium thiosulphate `(Na_(2)S_(2)O_(3).5H_(2)O)` in one litre. Calculate teh percentage of arsenious oxide in the sample ( Atomic mass of `As=74`)
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