Estimating the Iron(II) content in an iron tablet using a standard solution of potassium manganate (VII) Essay

figure the amount of squeeze(II) give wayThe iron was oxidized from its 2+ state to 3+ by sulfuric acidAnd the manganate iron was reduced as followsThis half(prenominal) equation is balanced as followsSince the above equation involves the transfer of quint electrons, the equation involving iron needs to be multiplied by quintet before the deuce half equations open fire be added to add upherAdding the two half equationsThis simplifies toThis equation shows that for invariablyy five present, wiz is required for the reception to be completed.19.1ml of super C manganate closure was used for titration. From this the amount of manganate ions used can be aimd as followsAmount of present =Mass of present =Since the volume of solution used was 25cm3, one-tenth of the total solution make from the five iron launch areas, the above calculation shows that. Dividing this value by 5, we get 53.3mg of Fe present in individually tablet.We may also calculate the amount of Iron(II) sulp hate are present in each tabletMolar mass of Iron(II) Sulfate, FeSO4 55.8+32+164 = 151.8g/molAmount of FeSO4 present/5 tabletsThe mass of the five iron tablets was measured to be 1.552g0.0001. Dividing this value by five gives 0.310g per tablet, or 310mg. This means that the part of Iron(II)Sulfate present in each tablet in mass is as followsUncertainties calculation portion suspense for pipette reading === Volume of iron (II) solution used = 25ml0.05Percentage uncertainty for burette reading === Volume of potassium manganate used = 19.1ml0.05Adding the percentage uncertainties together, the overall uncertainty is 0.462%. Converting this to the uncertainty of the total amount of iron convert present, we obtainThus, the total amount of iron sulphate can be said to be 145mg0.670Literature value for mass of Iron Sulfate present in one tablet is 160mg. The percentage fracture of the auditional results can thus be calculated as followsConverting this into absolute break in the am ount of iron, we obtainThus, the total amount of iron sulfate with respect to its defect value can be said to be 145mg13.6.ConclusionIn this investigation it was found through calculations that each of the iron tablet contained approximately 145mg of Iron (II) Sulfate. This is 15mg less than the listed amount of 160mg on the package, or 10% less than the literature value. This may have happened because whatever of the down in the mouth tablets were left behind in the mortar. Another possible reason is that more or less of the iron in the iron (II) solution deposited in the bottom of the volumetrical flask. This would mean that the pipette was filled with solution of less iron tightfistedness than the average concentration. This would explain the smaller obtained value.It was also found that the percentage error value was significantly bigger than the percentage uncertainty. This suggests that there was systematic error in this experiment. A possible way to solve this problem is to adjust the burette and pipette next time before conducting the experiment.EvaluationThis investigation has several flaws in its method. Potassium manganate (VII) solution was used in this experiment to titrate against the iron tablet solution. However, because it readily decomposes into manganese dioxide (MnO2), it is difficult to ever obtain a solution with exact concentration. The result is that the volume of manganate (VII) solution used might have been bigger than necessary due to decreased concentration as a result of decomposition. To minimize this from happening, the solution should be kept in a clean container and exposed to as humble frail as possible, as the solution decomposes faster under light and contaminated container.The obtained result was smaller than literature value, and this may have been because some of the powdered tablet was left in the mortar. To improve the accuracy of this experiment, one should wash the mortar with sulfuric acid or distilled water , which can consequently be transferred to the volumetric flask. This would allow more of the iron tablet to be contained in the acidic solution, thus increasing the amount of iron present.To sink this investigation, one can experiment on more types of iron tablets. Alternatively, a different content such as calcium or potassium can be investigated. This would require different types of tablets to be used.