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Iron Iron Iton

In: English and Literature

Submitted By sjoiiiiiii
Words 1213
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Measurement of Fe2+ in Iron Pills
Redox Titration
Purpose:

You will prepare and standardize a potassium permanganate solution and use it to determine the amount of iron, specifically Fe2+, in iron pills.
Overview:
Titration is the volumetric measurement of a solution of known concentration when it reacts completely with a measured volume or mass of another substance. In the first part of this experiment, the potassium permanganate solution, the titrant, is standardized, by quantitatively reacting it with iron (II) ammonium sulfate hexahydrate, Fe(NH4)2(SO4)2•6H2O (abbreviated FAS). The second part of the lab uses the standardized potassium permanganate to determine the amount of the analyte, also iron (II), in iron supplement pills.

In this experiment, a purple-colored solution of potassium permanganate, KMnO4, with an approximate concentration of 0.02 M will be added to solutions containing Fe2+ ions. In redox titration the chemical reaction is an oxidation-reduction reaction with electrons transferred from one species to another. The total number of electrons lost in the oxidation half-reaction is equal to the total number of electrons gained in the reduction half-reaction. The permanganate ion, MnO4-, is a strong oxidizing agent which causes the Fe2+ to be oxidized to Fe3+ ions. The manganese gains five electrons and is reduced from a 7+ oxidation state in the permanganate ion to form colorless Mn2+ ions. The Fe2+ loses one electron as it is oxidized to Fe3+. The end point is indicated when the reaction is complete at the point when all of the Fe2+ ions in solution are oxidized and the colorless mixture retains the purple tint of unreacted permanganate. Note that the color may be somewhat orange in appearance, depending upon the concentration of the Fe3+(aq), which has an orange-yellow-green tint. A few drops of concentrated phosphoric acid,

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