Notes - OXIDATION/REDUCTION TITRATION IRON IN TOTAL CEREAL...

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OXIDATION/REDUCTION TITRATION: IRON IN TOTAL CEREAL BRITTNEY BROWN, KENNESAW STATE UNIVERSITY, KENNESAW, GEORGIA. PARTNER: ERICA FRANCIS CHEM 2800L November 17, 2010
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Brown 11/3/2010 INTRODUCTION: The purpose of this experiment was to quantitatively determine the amount of iron in Total cereal. The experiment was broken down into several steps. First, the iron ore was decomposed and dissolved in HCl to form the complex of Fe(III). The dissolved sample then had to undergo a total reduction to the +2 state followed by an oxidative back to the +3 shown by Reaction (1): ++ + ++ + + 2Fe3 H3PO2 H2O 2Fe2 H3PO3 2H (1) The remaining hypophosphite was destroyed by boiling according to Reaction (2): + + + 3H3PO2 PH3 2H3PO3 2H (2) Pure iron filing was used as a primary standard to standardize the Ce(IV) oxidant. The molarity of Ce(IV) oxidant was then calculated using Equation (1): Measured mass Iron filings x Molecular weight Iron x Mole ÷ ( )= ( ) ratio Liters Ce IV Molarity Ce IV (1) A titration was performed with Ce(IV) on the iron extracted from the Total cereal given by Reaction (3): + + ( ) FeII CEIV FeIII Ce III (3) The mass of the iron in the cereal was calculated using Equation (2):
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This note was uploaded on 02/03/2011 for the course CHEM 2800 taught by Professor Staff during the Fall '08 term at Kennesaw.

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Notes - OXIDATION/REDUCTION TITRATION IRON IN TOTAL CEREAL...

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