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Hydrogen peroxide solution (20 ml) reacts quantitatively with a solution of KMnO4 (20 ml) acidified with dilute H2SO4. The same volume of the KMNO4 solution is just decolourised by 10 ml of MnSO4 in neutral medium simultaneously forming a dark brown precipitate is dissolved in 10 ,l of 0.2 M sodium oxalate under boiling condition in the presence of dilute H2SO4. Write the balanced equations involved in the reactions and calculate the molarity of H2O­2.

Amit Saxena , 11 Years ago
Grade upto college level
anser 1 Answers
Navjyot Kalra
Write the balanced chemical reaction for change and apply mole concept.
The given reaction are
MnO2 ↓ + Na2C2O2 + 2H2SO4
→ MnSO4 + CO2 + Na2SO4 + 2H2O
∴ Meq. Of MnO2 ≡ Meq of C2O4 = 10 * 0.2 * 2 = 4
∴ mM of MnO2 = 4/2 = 2 [Mn4+ + 2e → Mn2+ ∴ Valance factor of MnO2 = 2]
Now 2KMnO4 + 3MnSO4 + 2H2O
→ 5MnO2 ↓ + K2SO4 + 2H2O
Since eq. wt. of MnO2 is derived from KMnO4 and MnSO4 both, thus it is better to proceed by mole concept
mM of KMnO4 ≡ mM of MnI2 * (2/5) = 4/5
also 5H2O2 + 2KMnO4 + 3H2SO4
→ 2MnSO4 + K2SO4 + 8H2O + 5O2
∴ mM of H2O2 = mM of KMnO4 = mm OF KMnO4 * 5/2 = 4/5 * 5/2 = 2
∴ M_{H_{2}O^{_{2}}}* 20 = 2 or M_{H_{2}O^{_{2}}} = 0.1
2KMnO4 + 5H2O2 + 3h2SO4
→ K2SO4 + 2MnSO4 + 8H2O + 5O2
2KMnO4 +3KMnO4 + 2H2O
→ 5MnO2 + 2H2SO4 + K2SO4
MnO2 + Na2C­2O4 + 2H2SO­4
→ MnSO4 + 2CO2 + Na2SO4­ + 2H2O
Last Activity: 11 Years ago
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