0.2 of sample H2O2 reduced 20 ml of 0.1 M KMnO4 solution in acidic medium. What is the percentage purity of H2O2?
No. of moles of KMnO4 present in 20 ml of 0.1 M KMnO4 solution
The balanced equation for the redox reaction is:
From the equation,
2 moles of KMnO4 ≡ 5 moles of H2O2
Mol. Wt. of H2O2 = 34
∴ Amount of H2O2 actually present = 34 × 5 × 10–3 = 0.17 g
In which of the following reaction, oxidation number of N remains unchanged?
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?
In which of the following oxidation state of phosphours is + 3?
Determine the volume of M/8 KmnO4 solution required to react completely with 25.0 cm3 of M/4 FeSO4 solution is acidic medium.
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.
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.
Predict whether zinc and silver react with 1 M sulphuric acid to give out hydrogen or not. Give that the standard potentials of zinc and silver are – 0.76 volt and +0.80 volt respectively.
Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal? Given that
or Is it possible to store copper soulphate solution in a nickel vessel?
16.6 g of pure potassium iodide was dissolved in water and the solution was made up to one litre. V cm3 of this solution was acidified with 20 cm3of 2 M HCl. The resulting solution required 10 cm3 of decinormal KIO3for complete oxidation of I– ions to ICl. Find out the value of V.
Both (aq) can be used to titrate Fe2+ (aq). If in a given titratoion, 24.50 cm3 of 0.1 M were used, then what volume of 0.1 M solution would have been used for the same titration?