Question

Using

0.200 ml H2O2

10 mL H2SO4 (aq) 1 M

Solution titrated with KMnO4(aq) 0.20M

In the reaction of the redox pairs MnO4- | Mn2+ and H2O2 | O2. Show reaction scheme and calculate the formal concentration c(H2O2)

Answer #1

When Solution acidified by H2SO4:

2MnO_{4}^{-} + 5H_{2}O_{2} +
6H^{+} --> 2Mn^{2+} + 5O_{2}(g) +
8H_{2}O(l)

2 KMnO_{4} + 5 H_{2}O_{2} + 3
H_{2}SO_{4} ====> K_{2}SO_{4} +
2 MnSO_{4} + 8 H_{2}O + 5 O_{2}

To calculate the concentration of H2O2 we need volume of KMnO4 .

7.9 ml of 0.2 M KMnO4 = 7.9 x 0.2 / 1000 = 0.00158 Moles

0.00158 Moles of KMnO4 that reactes with (0.00158 x 5/2) 0.00395 Moles of H2O2

0.00395 Moles of H2O2 = 0.00395 x 1000 / 0.2 = 1.975 M

1.975 M for 100% H2O2

Hence for 35% = 100 x 1.975 / 33 = 5.642 M

**Concentration of H2O2 for 35% solution = 5.642
M**

Using
0.200 ml H2O2
10 mL H2SO4 (aq) 1 M
Solution titrated with KMnO4(aq) 0.20M
In the reaction of the redox pairs MnO4- | Mn2+ and H2O2 | O2.
Show reaction scheme and calculate the formal concentration
c(H2O2)
35% h2o2 and density=1.126 g/ml

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