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

Calculating the amount of beseech(II) faceThe squeeze was oxidised from its 2+ state to 3+ by sulfuric acerbicAnd the manganate squeeze was reduced as followsThis half equation is balanced as followsSince the preceding(prenominal) equation involves the transfer of tailfin electrons, the equation involving iron needs to be multiplied by five before the two half equations feces be added togetherAdding the two half equationsThis simplifies toThis equation shows that for every five present, one is required for the reaction to be completed.19.1ml of potassium manganate source was utilize for titration. From this the amount of manganate ions used burn down be calculated as follows sum of present =Mass of present =Since the volume of final declaration used was 25cm3, one-tenth of the pith radical made from the five iron birth control pills, the above calculation shows that. Dividing this abide by by 5, we get 53.3mg of Fe present in apiece tablet.We may likewise calcu late the amount of Iron(II) Sulfate are present in each tabletMolar mass of Iron(II) Sulfate, FeSO4 55.8+32+164 = 151.8g/ groinAmount of FeSO4 present/5 tabletsThe mass of the five iron tablets was thrifty to be 1.552g0.0001. Dividing this value by five gives 0.310g per tablet, or 310mg. This means that the office of Iron(II)Sulfate present in each tablet in mass is as followsUncertainties calculationPercentage uncertainty for pipette reading ===> tawdriness of iron (II) termination 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 sum amount of iron sulfate present, we obtainThus, the total amount of iron sulfate can be said to be 145mg0.670Literature value for mass of Iron Sulfate present in one tablet is 160mg. The percentage error of the experimental results can thus be calculated as follo wsConverting this into absolute error in the amount of iron, we obtainThus, the total amount of iron sulfate with respect to its error value can be said to be 145mg13.6.ConclusionIn this investigation it was give through calculations that each of the iron tablet contained approximately 145mg of Iron (II) Sulfate. This is 15mg slight than the listed amount of 160mg on the package, or 10% less than the literature value. This may have happened because some of the crushed tablets were left behind in the mortar. other possible reason is that some of the iron in the iron (II) solution deposited in the bottom of the volumetric flask. This would mean that the pipette was filled with solution of less iron concentration than the average concentration. This would explain the smaller obtained value.It was also found that the percentage error value was significantly large than the percentage uncertainty. This suggests that there was systematic error in this experiment. A possible trend to solve this problem is to calibrate the burette and pipette next measure 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 quick decomposes into manganese dioxide (MnO2), it is difficult to ever obtain a solution with particular 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 disinfect container and exposed to as little light 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 wit h sulfuric acid or distilled water, which can then be transferred to the volumetric flask. This would allow to a greater extent of the iron tablet to be contained in the acidic solution, thus increase the amount of iron present.To extend this investigation, one can experiment on more types of iron tablets. Alternatively, a various content such as calcium or potassium can be investigated. This would require different types of tablets to be used.