Iron(III) nitrate
Names IUPAC name Other names Identifiers ChemSpider ECHA InfoCard 100.030.805 RTECS number UNII Properties 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 47.2 °C (117.0 °F; 320.3 K) (nonahydrate) Boiling point 125 °C (257 °F; 398 K) (nonahydrate) 150 g/100 mL (hexahydrate) Solubility soluble in alcohol, acetone +15,200.0·10−6 cm3/mol Structure octahedral Hazards[2] GHS labelling: Warning H272, H302, H319 P210, P220, P221, P264, P270, P280, P301+P312, P305+P351+P338, P330, P337+P313, P370+P378, P501 NFPA 704 (fire diamond) Flash point non-flammable NIOSH (US health exposure limits): TWA 1 mg/m3[1] Related compounds Iron(III) chlorideIron(III) sulfate Iron(II) nitrate
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.
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+.[3] Other hydrates Fe(NO3)3·xH2O, include:
- tetrahydrate (x=4), more precisely triaqua dinitratoiron(III) nitrate monohydrate, [Fe(NO3)2(H2O)3]NO3·H2O, 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.[4]
- pentahydrate (x=5), more precisely penta-aqua nitratoiron(III) dinitrate, [Fe(NO3)(H2O)5](NO3)2, in which the Fe3+ ion is coordinated to five water molecules and a unidentate nitrate anion ligand in octahedral configuration.[4]
- hexahydrate (x=6), more precisely hexaaquairon(III) trinitrate, [Fe(H2O)6](NO3)3, where the Fe3+ ion is coordinated to six water molecules in octahedral configuration.[4]
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 K2FeO4.[5]
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 Fe2O3 appears.[6] Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions.[7]
The compound can be prepared by treating iron metal powder with nitric acid, as summarized by the following idealized equation:[8]
Fe + 4 HNO3 + 7 H2O → Fe(NO3)3(H2O)9 + NO
Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of sodium amide from a solution of sodium in ammonia:[9]
2 NH3 + 2Na → 2 NaNH2 + H2
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.[10]
Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.
