Chemical Property of FERRIC SODIUM OXALATE
Chemical Property:
- PSA：160.52000
- LogP:-7.03010
- Solubility.:This compound is very soluble in hot water, (182 parts per 100 parts solvent by mass), but a lot less soluble in cold water, (32 parts per 100 parts solvent), about the solubility of sodium chloride. It is not appreciably soluble in ethanol or ethanol water mixtures which are more than 50% ethanol by mass. It is somewhat more soluble in water than the corresponding potassium salt.
- Purity/Quality:
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99.0% *data from raw suppliers
Safty Information:
- Pictogram(s):
- Hazard Codes:
- MSDS Files:
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SDS file from LookChem
Useful:
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Description
Sodium ferri oxalate, also known as sodium oxalatoferrate, is a chemical compound with the formula Na3[Fe(C2O4)3], where iron is in the +3 oxidation state. It is an octahedral transition metal complex in which three bidentate oxalate ions act as ligands bound to an iron centre. Sodium acts as a counterion, balancing the -3 charge of the complex. Crystals of the hydrated form of the complex, Na3[Fe(C2O4)x].xH2O, are lime green in colour. In solution the complex dissociates to give the ferrioxalate anion, [Fe(C2O4)3]3-, which appears a deep apple green in colour.
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Physical properties
The bonds to the iron atom are dative covalent bonds where the ligands, (oxalate ions, blue), donate a lone pair into the empty p and d orbitals of the transition metal (iron, red), atom. The three oxalate ions donate 12 electrons in all and Fe-III has three electrons in the d orbitals leaving 13 empty places in the remaining d and p orbitals.
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Uses
Photography, blueprinting. In contemporary times ferrioxalate salts, usually the potassium salt, are used as exampls of a transition metal ligand complexes which can be easily synthesized by high school, college or undergraduate university students to introduce them to transition metal ligand chemistry, as well as to redox chemistry in now-obsolete photographic processes. The process of blueprint making, now also nearly obsolete, makes use of Iron-cyanide ligand complexes such as Ferricyanide and Ferrocyanide and redox reactions related to them. The presence of free Iron-II ions and oxalate ions gives rise to a whole family of Iron centered ligand complexes exhibiting intense blue colours. The best known of these is Prussian Blue, Potassium Ferrous Ferrocyanide.
