A dietary iron supplement consist of tablets containing the metal in the form of ferrous ions (Fe2+). The metal content of these tablets can be determined by dissolving a weighed amount of tablet(s) in dilute sulphuric acid solution and titrating an aliquot of this solution with a standard potassium permanganate solution as follows: One of the tablets is finely ground and the resulting powder has a mass of 0.4500 g. Distilled water and some sulphuric acid is added until the sample is dissolved. This solution is transferred to a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0200 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns a bright pink due to the presence of excess permanganate ions. The average titration value is 6.23 mL of the KMnO4 solution. 2KMNO4+8H2SO4+10FeSO4= K2SO4 +2MnSO4 +8H20 +5Fe2(SO4)3 1.Determine the percentage of iron in the tablet. 2.Naturally occurring manganese consists of only the 55Mn isotope. Determine the moles of the manganese salt formed, and then calculate the total number of neutrons present in all the manganese ions in the final solution.
A dietary iron supplement consist of tablets containing the metal in the form of ferrous ions (Fe2+). The
metal content of these tablets can be determined by dissolving a weighed amount of tablet(s) in dilute
sulphuric acid solution and titrating an aliquot of this solution with a standard potassium permanganate
solution as follows:
One of the tablets is finely ground and the resulting powder has a mass of 0.4500 g.
Distilled water and some sulphuric acid is added until the sample is dissolved. This solution is
transferred to a 250.00 mL volumetric flask and made up to the mark.
A 25.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0200 M KMnO4
solution.
The endpoint of the titration is determined when the colourless solution in the conical flask turns a
bright pink due to the presence of excess permanganate ions.
The average titration value is 6.23 mL of the KMnO4 solution.
2KMNO4+8H2SO4+10FeSO4= K2SO4 +2MnSO4 +8H20 +5Fe2(SO4)3
1.Determine the percentage of iron in the tablet.
2.Naturally occurring manganese consists of only the 55Mn isotope. Determine the moles of the
manganese salt formed, and then calculate the total number of neutrons present in all the manganese
ions in the final solution.
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