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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.
What textbook is this problem found in?
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.