4A-C Report Paper Sample 01

4A-C Report Paper Sample 01 - 1 Synthesis and Analysis of...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Synthesis and Analysis of Iron (III) Oxalate Complex Abstract An iron (III) oxalate complex was synthesized and analyzed for its oxalate ligands and iron composition. The iron (III) oxalate complex was synthesized through the oxidation-reduction reaction between an iron(II) ammonium sulfate reactant, hydrogen peroxide, and oxalic acid. With the addition of ethanol, a crystalline product formed, which was then isolated and purified. _____ grams of ferrous ammonium sulfate hexahydrate (Fe(NH 4 ) 2 (SO 4 ) 2 · 6H 2 O) salt was used to yield ______ grams of neon-green crystals. The oxalate ligands in the iron (III) oxalate complex were then analyzed using oxidation-reduction titration and spectrophotometry. The oxalate (C 2 O 4 2- ) was found to have a weight percentage of __________% and ______ mmol per 100 grams of sample. The iron content was determined using spectrophotometry. The average amount of moles of Fe 3+ ion in a 100 gram sample was found to be ______ mmol with a weight percent of ______% . Comparing the millimoles of both ions, the ratio of oxalate to iron was found to be to 1 . The empirical formula of the iron (III) oxalate complex was found to be K 3 (Fe(C 2 O 4 ) 3 · 2H 2 O with a percent yield of _______%. 1. Introduction The purpose of this paper is to synthesize a complex of iron (III) oxalate and then analyze it by using titration and spectrophotometry in order to discover its empirical formula. An iron(III) ion will coordinate with the oxalate ion, forming an iron(III) oxalate coordination compound. After being isolated and purified, this coordination compound will then be analyzed through oxidation-reduction titration and spectrophotometry. With these results, the empirical formula of the iron (III) oxalate complex than then be calculated. The iron (III) oxalate complex is made up of two parts: a metal ion and one or more ligands. Usually the metal ion in a coordination complex has a +2 or +3 charge in an aqueous solution. This is because +2 and +3 charged metal ions are Lewis acids and therefore tend to accept electrons. Ligands are molecules or anions that can donate electron pairs to the metal ion, which then forms a bond between the ligand and the metal ion. The number of electron pairs transferred from the ligand to the metal is called the metal’s coordination number. The electron pairs in a ligand are also known as coordination sites, since this is where the ligand and the metal ion will coordinate. Ligands that are monodentate, bidentate, or multidentate will donate one, two, or multiple electron pairs respectively. In this case, the oxalate ion has two coordination sites for a metal ion, and is therefore bidentate, so it has a coordination number of 4 rather than 2. Volumetric analysis is used to determine the weight percentage of the oxalate
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 6

4A-C Report Paper Sample 01 - 1 Synthesis and Analysis of...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online