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 case 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) + 5Fe^2+ (aq) rightarrow Mn^2+(aq) + 4h_2O_(1) + 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

2) Volume used ---> 28.20 ml, 27.90 ml, 27.90 ml

3) It is a redox titration where oxidation of Iron occurs and manganese is reduced. Iron is oxidized because it loses electron which is known as oxidation.

4) average = 28 ml

question is not clear as it is given that you have taken 25 ml of KMnO4 but later more volume is used which is contradiction.

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