## Question

### Solution

Correct option is

10.0

The balanced ionic equation for the reaction is

From the balanced equation, it is evident that

1 mole of KMnO4 ≡ 5 moles of FeSO

Applying molarity equation to the balanced redox equation,

Thus, the volume of M/8 KMnO4 solution required 10.0 mL.

#### SIMILAR QUESTIONS

Q1

To 1 mole of pyrophosphoric acid (H4P2O7) in aqueous solution 2 mole of NaOH are added. The salt formed is

Q2

What volume of 0.01 M K2Cr2O7 would be required to oxidize Fe (II) in 50ml of 0.03 M solution of ferrous ammonium sulphate in acidic medium?

Q3

100ml of 0.01 M KMnO4 oxidizes 10ml of H2O2 sample in acidic medium. The volume strength of H2O2 sample is

Q4

A sample of mixture of AO and A2O3 in 2 : 1 molar ratio takes 0.015 mole of K2Cr2O7 to oxidize the sample completely to from  in acidic solution. Millimoles of AO and A2O3 in the sample are respectively

Q5

0.01 mole of Fe3O4 is treated with excess of KI solution in presence of dilute H2SO4 whereby iron is reduced to Fe2+ along with liberation of iodine. What volume of 0.1 M Na2S2O3 will be needed to reduce the librated iodine?

Q6

In which of the following reaction, oxidation number of N remains unchanged?

Q7

KMnO4 acts as a strong oxidizing agent in acidic medium. The reaction that occurs is

What will be the effect on the electrode potential of a half-cell represented as  if the concentration of H+ ion is doubled in solution?

Q8

In which of the following oxidation state of phosphours is + 3?

Q9

Calculate the concentration of hypo (Na2S2O3.5H­2O) solution in g dm–3 if 10.0 of this solution decolourised 15 mL of M/40 iodine solution.

Q10

0.5 g of an impure sample of oxalate was dissolved in water and the solution made to 100 ml. On titration 10 ml of this solution required 15 ml of N/20 KMnO4 solution. Calculate the percentage of pure oxalate in the sample.