4A-C Report Paper Sample 02

4A-C Report Paper Sample 02 - Abstract Through...

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Abstract Through oxidation-reduction reaction between iron(II) ammonium sulfate reactant, hydrogen peroxide, and oxalic acid, an iron(III) oxalate coordination complex was synthesized and analyzed for its oxalate ligands and iron composition. In part A, a light green crystalline product was formed; 2.3997 grams of ferrous ammonium sulfate hexahydrate salt Fe(NH 4 ) 2 (SO 4 ) 2 ·6H 2 O was used to yield 2.1481 grams of the iron(III) oxalate complex. The product was then analyzed using oxidation-reduction titration and spectrophotometry in part B and C. Oxalate C 2 O 4 2- was found to have a weight percentage of 54.0 + 0.6% and 614 + 8 mmol per 100 grams of sample. The Fe 3+ ion was found to have a weight percentage of 12.0 + 1.2% and 214 + 22 mmol per 100 grams of sample. When comparing the millimoles of the oxalate to that of the Fe 3+ ion, the ratio was 3-to-1. Subsequently, the ratios of K + to Fe 3+ and H 2 O to Fe 3+ were both calculated to be 3-to-1 as well. The empirical formula of the iron(III) oxalate complex was thus determined to be K 3 [Fe(C 2 O 4 ) 3 ]·3H 2 O with a percent yield of 71.47%. 1. Introduction The purpose of the experiment is to synthesize an iron(III) oxalate coordination complex and to analyze its composition through titration and spectrophotometry so as to determine its empirical formula. In Part A of the lab, the iron(III) ion coordinates with the oxalate ion to form an iron(III) oxalate coordination complex. In Part B, the compound synthesized in Part A will be isolated and purified so it can undergo oxidation-reduction reaction through titration. Finally, in Part C, the Spectronic 20 was used to find the absorbance and concentration of diluted “Known” and “Unknown” solutions containing the synthesized compound. With the results collected from these three parts, the empirical formula of the iron(III) oxalate complex can be calculated. The iron(III) oxalate complex consists of a metal ion and one or more ligands. The metal ion in a coordination complex usually has a +2 or +3 charge in an aqueous solution. The metal ions are Lewis acids and tend to accept electrons. Ligands, on the other hand, are molecules or anions that can donate electron pairs to the metal ion, making them Lewis bases. The number of electron pairs transferred from the ligand to the metal is known as the metal’s coordination number. The electron pairs in a ligand are also known as coordination sites because it is where the ligand and the metal ion will coordinate. Ligands can be monodentate, bidentate, or multidentate, meaning that they can donate one, two, or multiple electron pairs respectively. In this lab, the oxalate ion has two coordination sites for the metal ion, making it bidentate. Therefore, it has a coordination number of 4. In part B of the lab, volumetric analysis is used to determine the weight percentage of the oxalate ligands in the complex K w [Fe x (C 2 O 4 ) y ]·zH 2 O. This part of the experiment involves oxidation-reduction titration where the solution changes color once stoichiometric endpoints of
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