Iron(III) nitrate
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| Template:Longitem | Fe(NO3)3 |
| Molar mass | 403.999 g/mol (nonahydrate) 241.86 g/mol (anhydrous) |
| Appearance | Pale violet crystals hygroscopic |
| Density | 1.68 g/cm3 (hexahydrate) 1.6429 g/cm3(nonahydrate) |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Solubility | soluble in alcohol, acetone |
| Template:Longitem | +15,200.0·10−6 cm3/mol |
| Template:Longitem | octahedral |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
| Flash point | Template:Chembox CalcTemperatures |
| Template:Longitem | Iron(III) chloride Iron(III) sulfate |
| Template:Longitem | Iron(II) nitrate |
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Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.
Hydrates
Iron(III) nitrate is deliquescent, and it is commonly found as the nonahydrate Fe(NO3)3·9H2O, which forms colourless to pale violet crystals. This compound is the trinitrate salt of the aquo complex [Fe(H2O)6]3+.[2] Other hydrates Template:Chem/link·xTemplate:Chem/link, include:
- tetrahydrate (x=4), more precisely triaqua dinitratoiron(III) nitrate monohydrate, Template:Chem2, has complex cations wherein Fe3+ is coordinated with two nitrate anions as bidentate ligands and three of the four water molecules, in a pentagonal bipyramid configuration with two water molecules at the poles.[3]
- pentahydrate (x=5), more precisely penta-aqua nitratoiron(III) dinitrate, Template:Chem2, in which the Fe3+ ion is coordinated to five water molecules and a unidentate nitrate anion ligand in octahedral configuration.[3]
- hexahydrate (x=6), more precisely hexaaquairon(III) trinitrate, Template:Chem2, where the Fe3+ ion is coordinated to six water molecules in octahedral configuration.[3]
Reactions
Iron(III) nitrate is a useful precursor to other iron compounds because the nitrate is easily removed or decomposed. It is for example, a standard precursor to potassium ferrate Template:Chem2.[4]
When dissolved, iron(III) nitrate forms yellow solutions. When this solution is heated to near boiling, nitric acid evaporates and a solid precipitate of iron(III) oxide Template:Chem/link appears.[5] Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions.[6]
Preparation
The compound can be prepared by treating iron metal powder with nitric acid, as summarized by the following idealized equation:[7]
Applications
Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of sodium amide from a solution of sodium in ammonia:[8]
Certain clays impregnated with ferric nitrate have been shown to be useful oxidants in organic synthesis. For example, ferric nitrate on Montmorillonite—a reagent called Clayfen—has been employed for the oxidation of alcohols to aldehydes and thiols to disulfides.[9]
Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.
References
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- ↑ a b c H. Schmidt, A. Asztalos, F. Bok and W. Voigt (2012): "New Iron(III) Nitrate Hydrates: Template:Chem2 with x = 4, 5 and 6". Acta Crystallographica Section C - Inorganic Compounds, volume C68, pages i29-i33. Script error: No such module "CS1 identifiers".
- ↑ Script error: No such module "citation/CS1".
- ↑ Egon Matijević and Paul Scheiner (1978): "Ferric Hydrous Oxide Sols: III. Preparation of Uniform Particles by Hydrolysis of Fe(III)-Chloride, -Nitrate, and -Perchlorate solutions". Journal of Colloid and Interface Science, volume 63, issue 3, pages 509-524. Script error: No such module "CS1 identifiers".
- ↑ Script error: No such module "citation/CS1".
- ↑ Script error: No such module "Template wrapper".
- ↑ Script error: No such module "Citation/CS1".; Script error: No such module "citation/CS1".. As of 2007, 22 other entries describe similar preparations in Organic Syntheses
- ↑ Cornélis, A. Laszlo, P.; Zettler, M. W. "Iron(III) Nitrate–K10 Montmorillonite Clay" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. Script error: No such module "CS1 identifiers"..
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