Formal LAB - Abstract Experiment 5 Preparation of a Complex...

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Abstract: Experiment 5: “Preparation of a Complex Iron Salt” The equation: percent yield equals actual yield divided by theoretical yield times on hundred is used to determine the yield of the reaction K 3 Fe(C 2 O 4 ) 3 times 3H 2 O. Experiment 7: “Analysis of a Complex Iron Salt” The experiment calculated the titration of a complex iron salt. This experiment was used to determine the moles of C 2 O 4 per mole within the substance of K 3 Fe(C 2 O 4 ) 3 times 3H 2 O. Introduction: “Preparation of a complex Iron Salt”, experiment five was the first of two related experiments. In this part of the experiment, we took the necessary steps to synthesize the compound potassium ferric oxalate in order to prepare as great of a yield as possible of K 3 Fe (C 2 O 4 ) multiplied 3H 2 O using a specific calculation. After following the procedure given in our lab-manuals, a solid was produced and set aside for Experiment 7, which took place a few weeks later. In the experiment seven, “Analysis of a Complex Iron Salt”, the identity of the compound was confirmed through various methods including but not limited to, X-Ray diffraction, Nuclear Magnetic Resonance, Mass Spectrometry or Chemically. Our goal in Experiment 7, “Analysis of a Complex Iron Salt” was to synthesize the compound potassium ferric oxalate of potassium trisoxalatoferrate. The following stages of the use of titration were used: A) Standardization of a permanganate solution B) Analysis for oxalate in K 3 Fe(C 2 O 4 ) multiplied by 3H 2 0. After the calculation for the reaction of different elements was taken, the solid of the Iron Compound was titrated. After disposing of the Potassium Permanganate in the specific manner listed in
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This note was uploaded on 03/23/2009 for the course CHEM 2080-U taught by Professor Davidusher during the Spring '09 term at Cornell.

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Formal LAB - Abstract Experiment 5 Preparation of a Complex...

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