Redox Stoichiometry help?

Question

Hydrogen peroxide, H2O2, solution can be purchased in drug stores and used as an antiseptic. A sample of such a solution weighing 1.00 grams was acidified with sulfuric acid and titrated with .02000 M solution of KMnO4. The peroxide was oxidized to a gas. The titration required 17.60ml of KMnO4 solution. What is the mass percent of H2O2 in the original solution?

Roger the Mole · Answer

2 KMnO4 + 5 H2O2 + 3 H2SO4 → 8 H2O + 2 Mn{2+} + 5 O2 + 3 SO4{2-} + 2 K{+}

(0.01760 L) x (0.02000 mol/L KMnO4) x (5 mol H2O2 / 2 mol KMnO4) x (34.0147 g H2O2/mol) / (1.00 g) = 
0.02993 = 2.993% H2O2 by mass

Redox Stoichiometry help?

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