A `3.4g` sample of `H_(2)O_(2)` solution containing `x%H_(2)O` by mass requires `xmL` of a `KMnO_(4)` solution for complete oxidation under acidic conditions. The normality of `KMnO_(4)` solution is `:`

A sample of 28 mL of H_(2) O_(2) (aq) solution required 10 mL of 0.1 M KMnO_(4) (aq) solution for complete reaction in acidic medium. What is the volume strength of H_(2)O_(2) ? X

The pH of a solution of H_(2)SO_(4) is 1. Assuming complete ionisation, find the molarity of H_(2)SO_(4) solution :

Why is KMnO_4 solution used to clean surgical instruments in hospitals ?

How acidified KMnO_4 solution reacts with the following in acidic medium : H_2S .

Two litres of 0.5 M KMnO_4 solution have to be completely reduced in acidic medium. The number of Faradarys of electricity required will be

How acidified KMnO_4 solution reacts with the following in acidic medium : SO_2 .

1 mole of equimolar mixture of ferric oxalate and ferrous oxalate requires x mole of KMnO_4 in acidic medium for complete oxidation. x is :

A mixture of H_(2)SO_(4) and H_(2)C_(2)O_(4) (oxalic acid ) and some inert impurity weighing 3.185 g was dessolved in water and the solution made up to 1litre. 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another experiment 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO_(4) solution for complete reaction. The mass % of H_(2)SO_(4) in the mixture was:

32g of a sample of FeSO_(4) .7H_(2)O were dissolved in dilute sulphuric aid and water and its volue was made up to 1litre. 25mL of this solution required 20mL of 0.02 M KMnO_(4) solution for complete oxidation. Calculate the mass% of FeSO_(4) .7 H_(2)O in the sample.