Iron supplements contain soluble iron(II) salts to replenish them in the human b

Question

Iron supplements contain soluble iron(II) salts to replenish them in the human body in ease of deficiency. Iron is an essential mineral used in many functions, specifically in the transport of oxygen. Iron deficiency can occur through poor diet, or as a consequence of blood loss through menstruation or injury. There are two different ways the amount of iron(II) ion could be determined by titration. The iron tablet was placed in 250 mL beaker and dissolved and then that solution was placed in a burette. 25.00mL of a 0.0100 M solution was placed in an Erlenmeyer flask and titrated until the pink color disappeared. Finish the table below The reaction occurring is: MnO_4^- (aq) + 8H^+_(aq) + 3Fe^2+_(aq) rightarrow Mn^2+_(aq) + 4H_2 O_(l) + 5Fe^3+_(aq) Is iron being oxidized or reduced? Why? Using the average volume in the table, the molarity of the KMnO_4 and the above equation, calculate the mg of iron (II) ion that was in the tablet.

Explanation / Answer

Fe2+ is losing 1 electron to form Fe3+. Losing electrons is oxidation

Volume of Fe2+ = 27.9 mL

Volume of KMnO4 = 25 mL

Molarity of KMnO4 = 0.01M

Molarity of Fe2+ = 0.01*25/27.9 = 0.009M

amount of Fe2+ = 0.009 x 55.89 (iron atomic weight)

                         = 0.5 gr = 500mg

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