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Iron Oxalate Lab

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Marina Horta Iron Oxalate Lab 10/22/09 Abstract; The purpose of this lab was to synthesize, isolate, and determine Fe content of a complex; and calculate the formula of the Potassium Oxalate Iron(III) Complex using chemical analyses. This lab used filtration, titration, acid base reactions, redox , synthesis, dilutions , beers law and red tide computer system to establish that the final formula for the complex was K3[Fe(C2O4)3] �2 H2O. Introduction; Part 1; The purpose of part 1 to synthesize, purify and, mass crystals of potassium oxalate ferrate (III) complex. Potassium oxalate ferrate (III) is a complex, an ion consisting of a ligand and a metal covalently bonded together. A ligand is an ion with the tendency to bond with metals because it typically donates electron pairs. This relationship between metals and ligands is only one of the key components for the synthesis of the crystals. For the precipitation of the complex ion alcohol was used to reduce solubility, Part: 2 Part two determines the percent oxalate in the complex produced in the previous lab. Using volumetric analysis a method (similar to gravimetric analyses) in which the volume of a known substance is used to quantitatively measure the volume of an unknown substance required to react with it, or standardization a process in which the value of a potential standard is fixed by a measurement made with respect to a standard whose value is known and can be used to determine the value of unknown. ...read more.


Hydrogen peroxide is an oxidizer and corrosive( lab one) Oxalic Acid and oxalate ions are toxic (lab one ) Ethanol is flammable (lab one) Permanganate solution is also poisonous and corrosive Take caution when handling hot glass wear (lab part two) Calculations; Table 1 Weight of Crystals (part 1) Initial trey 1.49 (g) Weight of crystal 1.3934 (g) Weight of both 2.88 (g) Table 2 Data (part 2) Data mass of 1 2 3 4 ii iron oxalate 1.4974 g 1.4994 g 1.4977 g 1.4994 g Crystals+ Trey 1.6286 g 1. 6175 g 1.6256 g 1.6247 g Mass of Crystal .1294 g .1181 g .1288 g .1253 g Titration ; (part 2) 1 2 3 4 Final 36.5ml 36.5ml 48.6 ml 48.4 ml Initial 6 ml 8.5ml 18 ml 18 ml Volume used 30.5ml 28 ml 30.6 ml 30.4 ml Moles Trial #1 (.01057 M)(.0305 ml) =.003224 m (5/2) = .0008059 Trial #2 (.01057M)(.028 ml) = .002959 m (5/2) =.0007398 Trail #3 (.01057M)(.0306 ml) = .0003234 m (5/2)=.0008085 Trail #4 (.01057 M)(.03 04 ml) = .0003213 m (5/2) = .00080325 Percent by Mass Oxalate Trial# 1 (.0008059 m)(87.99) =(.07091)(1/.1294)= 54% Trial #2 (.0007398m) (87.99) = (.06509)(1/.1181) = 55% Trail #3 (.0008085m)(87.99) = (.0711#)(1/.1288) = 55% Trial #4 (.00080325m )(87.99) = (.07067)(1/.1253) =56% Table 1: Standard Curve of Fe solution Dilution Conc[] Abs 0.1 0.00001209 0.054 0.2 0.00002418 0.116 0.3 0.00003627 0.214 0.7 0.00008463 0.645 [] std= 0.0001209 Table II [fe+2] for unknowns ...read more.


the Fe+, this error could be again because of the dilutions or it could be a result of misusing the red tide equipment however because time did not allow the negative values were kept and simply not included in the final calculations of the unknown. The actual percent iron calculated for this lab was 4.5% a value much too low to be correct or useful this lower percent Fe+ shows that the concentration of Fe+ was too low to begin or not enough of the solution was pipetted to the initial 100ml flask. The average of all the experiments 8.52 was also too low, in order to get a correct value using the empirical formula from the percent iron the percent had to be at least 11 % which shows a systematic error in the experiment. Using the empirical formula and the adjusted 11% iron the ratios of the iron and oxalate was calculated to be 3:1 instead of the original incorrect 4:1 ratio using the lower value for iron. The value for z was calculated within the reasonable 2 or 3 value, at 2.4. The final determination in the experiment was theoretical and percent yield from the moles of the third and grams of the second day. The theoretical yield was 1.848 grams while the results of the second day yielded only 1.3 resulting in a 69% yield overall. The final adjusted formula was finally determined to be K3[Fe(C2O4)3] �2 H2O. ...read more.

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