Introduction
Redox titration is a method used to determine the concentration of an unknown solution by using a solution of known concentration. In this experiment, we will be using potassium permanganate as the oxidizing agent and an unknown solution as the reducing agent. The purpose of this lab report is to discuss the results obtained from the experiment.
Materials and Methods
The materials used in this experiment include a burette, a pipette, potassium permanganate solution, an unknown solution, and sulfuric acid. The unknown solution was placed in a flask and a few drops of sulfuric acid were added to it. The potassium permanganate solution was then added to the flask using a burette until a pink color was observed. The volume of the potassium permanganate solution added was recorded.
Results
The volume of the potassium permanganate solution added was 25 ml. The concentration of the potassium permanganate solution was 0.1 M. Therefore, the number of moles of potassium permanganate used was 0.0025 moles.
Discussion
The unknown solution was a reducing agent and reacted with the potassium permanganate solution. The reaction between the two solutions can be represented as follows: MnO4- + 5e- + 8H+ → Mn2+ + 4H2O The number of moles of the reducing agent can be calculated using the following equation: MnO4- × 5 × V = n × F Where V is the volume of the potassium permanganate solution added, n is the number of moles of the reducing agent, and F is the stoichiometric factor of the reducing agent.
Conclusion
In conclusion, the concentration of the unknown solution can be calculated using the number of moles of the reducing agent and the volume of the unknown solution used. This experiment demonstrates the use of redox titration in determining the concentration of an unknown solution. It is important to note that the accuracy of the results obtained depends on the accuracy of the equipment used and the technique employed during the experiment.