Problem: The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in 14.8 g of hair bleach was determined by titration with a standard potassium permanganate solution:2 MnO4 −(aq) + 5 H2O2(aq) + 6 H+(aq) ⟶ 5 O2(g) + 2 Mn2+(aq) + 8 H2O(l) How many moles of MnO4− were required for the titration if 43.2 mL of 0.105 M KMnO4 was needed to reach the end point?
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Problem Details
The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in 14.8 g of hair bleach was determined by titration with a standard potassium permanganate solution:
2 MnO4 −(aq) + 5 H2O2(aq) + 6 H+(aq) ⟶ 5 O2(g) + 2 Mn2+(aq) + 8 H2O(l)
How many moles of MnO4− were required for the titration if 43.2 mL of 0.105 M KMnO4 was needed to reach the end point?
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.