One of the possible systematic error that may occur in this experiment is that the hydrated (II) ammonium sulfate is contaminated as the iron (II) salt was left uncovered. The iron (II) salt was prepared by the lab assistant and the salt was left at the table uncovered for students to scoop the desired amount of salt they want. The iron (II) salt might be contaminated by dust particles and even saliva. This would cause the standard iron (II) solution to have less iron (II) salt in it and this means that less potassium permanganate solution is needed to titrate the iron (II) solution. This is a systematic error because the iron (II) solution used throughout the experiment. The only way to reduce the systematic error and improve the accuracy is to place the iron (II) salt in a sterile area and to make sure the lid of the iron (II) salt is closed. Another systematic error that may occur is that the burette, pipettes and measuring cylinder used in the experiment is wrongly calibrated by the manufacturer. This would result in more or less solution than the required amount of solution in the experiment. For example, 25.00mL of Iron (II) solution was retrieved using a pipette, and if the pipette was wrongly calibrated and …show more content…
In order for the reaction take place, the iron (II) solution is swirled so that the potassium permanganate added would be combined with the iron (II) solution. Some swirling rate might be faster and some slower. When the swirling rate is slower, some of the iron (II) solution would not be able to combine with the potassium permanganate solution. This random error would cause some results to be lower or higher than the actual. The only possible solution to improve the precision of the result is to use a magnetic stirrer to get a constant swirling