How strong is your antiseptic? Hydrogen peroxide is a common drugstore chemical. As students look in the far reaches of their medicine cabinets at home, they are likely to find old bottles of hydrogen peroxide that have long since passed their prime. Since the amount of hydrogen peroxide in solution deteriorates over time, how can the real concentration be determined? Students analyze the percent hydrogen peroxide in a common “drugstore” solution using an oxidation–reduction titration with potassium permanganate. The stoichiometry of the balanced redox equation allows students to calculate the actual hydrogen peroxide concentration. A great experiment that ties together key concepts of oxidation–reduction and integrates prior knowledge of stoichiometry.
Includes all the necessary chemicals, along with reproducible student handouts, detailed background information, and complete Teacher Notes with sample data and answers to all questions.
Complete for 30 students working in pairs.
Additional ResourcesNo Additional Resources at the time.
Flinn Catalog/Reference Manual Page 474
You May Also Like
- Buret, Borosilicate Glass, withTeflon Stopcock, 50-mL
- Cylinder, Borosilicate Glass, 10 mL*
- The Hydrogen Peroxide Rainbow - Chemical Demonstration Kit
Redox and the Goddess of Beauty -
Chemical Demonstration Kit
- The Floating Tin Sponge - Chemical Demonstration Kit
- Iron Corrosion - Guided-Inquiry Kit
- The Silver Mirror Award - Chemical Demonstration Kit
- Single Replacement Reactions and Metal Activity - Student Laboratory Kit
- Oxidation-Reduction Basics - Student Laboratory Kit
- Oxidation and Reduction, Flinn ChemTopic Lab Book, Volume 16