Lab Session 22/01/13: Redox Reactions

Objective:  To calculate the amount of potassium permanganate we could dissolve in hydrogen oxide.

Materials we used for the experiment:
- Potassium permanganate (KMnO₄)    - Erlenmeyer flask
- Little cup                                            - Pipette
- Burette                                               - Hydrogen oxide
- Sulfuric acid 2M                                 - Stand
- Clamp                                                - Test tubes
- Test tube rack

Explanation

1) We first set up everything in place and then poured the Potassium permanganate in to the Burette until it was filled completely.

2) We then placed 4 mL of H₂O₂ in the Erlenmeyer flask along with 4 moles of Sulfuric acid and mixed it together.

3) We placed the Erlenmeyer flask underneath the Burette to start the titration.

4) We dissolved the Potassium permanganate until it came to a point that the substance in the Erlenmeyer flask started to change color. We came to a result that around 22 mL were dissolved therefore meaning that 28 mL were left in the Burette.

Results
- 50 mL of KMnO₄ in Burette
- 4 mL of H₂O₂ + 4M of HSO₄ in Erlenmeyer flask

50 mL of KMnO₄ – 22 mL = 28 mL of KMnO₄ left

Conclusion

We can conclude that the final result of the titration gives us a redox reaction. This means that one substance is reducing while the other is oxidizing. We stopped adding the Potassium permanganate once it started turning another color. We came up with a reddish brown color in the end.