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Unformatted text preview: EXPERIMENT 10: Determination of Iron by Reaction with Permanganate-A Redox Titration by Rodrigo Javier Andrew Klingsporn LAB PARTNER CHEM 212: General Chemistry II November 5, 2008 Laboratory Instructor: Dr. Chandana Meegoda Purpose To determine the percentage of iron in an unknown solid sample containing Iron(II) ammonium sulfate using a redox titration. Introduction Potassium permanganate, KMnO 4 , is often used as an oxidizing agent in redox titrations. MnO 4- ion is naturally purple in color and reacts in acid solution to yield Mn 2+ ion, which is colorless, by the following reaction: 8H + (aq) + MnO 4- (aq) + 5e Mn 2+ (aq) + 4H 2 O (l) Because of this, the end point of a titration using KMnO 4 can be taken as the lightest permanent shade of pink that appears. Using KMnO 4 , we can determine the percent of iron in an unknown sample of Iron(II) ammonium sulfate, Fe(NH 4 )(SO 4 ) 2 6H 2 O. The titration oxidizes Fe 2+ ion to Fe 3+ by permanganate ion and is carried out in acid solution so as to prevent early oxidation of Fe...
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