Measuring the mass of Iron in an iron sulphate tablet using REDOX titration
Aim
The aim of this experiment is to determine the mass of iron present in one iron sulphate tablet using REDOX titration under acidic conditions.
Safety
H2SO4: This is an irritant which may cause burns on skin and eyes; therefore care must be taken when handling this chemical. Protective gear (gloves, lab coat and safety goggles) must be worn at all times. If it comes in contact with skin or eyes, it should be washed immediately with water for at least 15 minutes and immediate medical procedures are necessary. (Fisher, n.d.)
KMnO4: This is harmful if swallowed or touches skin, therefore care must be taken while handling and protective gear must be worn at all …show more content…
Approximately 50 [cm3] of 1 [mol/dm3] sulphuric acid was added to the flask, and shaken well with the stopper. The name of the members and the date was written on the flask, and was left for a week for the iron sulphate tablets to fully dissolve in the acid.
After the tablets have fully dissolved, the whole solution was filtered using a filter paper and a funnel into a 100 [cm2] volumetric flask. The remaining residue in the filter paper was rinsed with a small amount of distilled water. Then, sulphuric acid was added to the 100 [cm2] mark on the volumetric flask. The solution was shaken well.
The burette was filled with 0.02 [mol/dm3] KMnO4 solution. Using a 25 [cm3] volumetric pipette, 25 [cm3] of the contents inside the 100 [cm3] volumetric flask was put into a 250 [cm3] conical flask. Then, KMnO4 solution was dropped from the burette into the 250 [cm3] conical flask, until the REDOX reaction ended. The ending point of the REDOX reaction was determined when the colour of the KMnO4 did no longer disappear in the acidic …show more content…
Although there were no anomalous results, there were room for error, especially the method taken to extract the Fe2+ from the tablets. During the filtration step, distilled water was used to rinse the residue of the tablets. This potentially causes two problems. Firstly, because water was used to rinse the residue, the concentration of the sulphuric acid decreases slightly. Secondly, as care was taken while rinsing the residue, only small amounts of water was used as to minimise the decrease in the concentration of the sulphuric acid. This means that there is a large possibility that the residue was not rinsed well, leaving some Fe2+ in the residue. This leads to a decrease in the amount of Fe2+ measured in this experiment, which also suggests why the result obtained is
Aim
The aim of this experiment is to determine the mass of iron present in one iron sulphate tablet using REDOX titration under acidic conditions.
Safety
H2SO4: This is an irritant which may cause burns on skin and eyes; therefore care must be taken when handling this chemical. Protective gear (gloves, lab coat and safety goggles) must be worn at all times. If it comes in contact with skin or eyes, it should be washed immediately with water for at least 15 minutes and immediate medical procedures are necessary. (Fisher, n.d.)
KMnO4: This is harmful if swallowed or touches skin, therefore care must be taken while handling and protective gear must be worn at all …show more content…
Approximately 50 [cm3] of 1 [mol/dm3] sulphuric acid was added to the flask, and shaken well with the stopper. The name of the members and the date was written on the flask, and was left for a week for the iron sulphate tablets to fully dissolve in the acid.
After the tablets have fully dissolved, the whole solution was filtered using a filter paper and a funnel into a 100 [cm2] volumetric flask. The remaining residue in the filter paper was rinsed with a small amount of distilled water. Then, sulphuric acid was added to the 100 [cm2] mark on the volumetric flask. The solution was shaken well.
The burette was filled with 0.02 [mol/dm3] KMnO4 solution. Using a 25 [cm3] volumetric pipette, 25 [cm3] of the contents inside the 100 [cm3] volumetric flask was put into a 250 [cm3] conical flask. Then, KMnO4 solution was dropped from the burette into the 250 [cm3] conical flask, until the REDOX reaction ended. The ending point of the REDOX reaction was determined when the colour of the KMnO4 did no longer disappear in the acidic …show more content…
Although there were no anomalous results, there were room for error, especially the method taken to extract the Fe2+ from the tablets. During the filtration step, distilled water was used to rinse the residue of the tablets. This potentially causes two problems. Firstly, because water was used to rinse the residue, the concentration of the sulphuric acid decreases slightly. Secondly, as care was taken while rinsing the residue, only small amounts of water was used as to minimise the decrease in the concentration of the sulphuric acid. This means that there is a large possibility that the residue was not rinsed well, leaving some Fe2+ in the residue. This leads to a decrease in the amount of Fe2+ measured in this experiment, which also suggests why the result obtained is