Iron(III) nitrate

Iron(III) nitrate
IUPAC name Iron(III) nitrate
Other names Ferric nitrate Nitric acid, iron(3+) salt
Identifiers
CAS number	10421-48-4 Y,  13476-08-9 (hexahydrate) 7782-61-8 (nonahydrate)
PubChem	168014
ChemSpider	10670706 Y
UNII	N8H8402XOB Y
RTECS number	NO7175000
Jmol-3D images	{{#if:[Fe+3].O.O.O.O.O.O.O.O.O.O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O|Image 1
SMILES [Fe+3].O.O.O.O.O.O.O.O.O.O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O
InChI InChI=1S/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;; Y Key: SZQUEWJRBJDHSM-UHFFFAOYSA-N Y InChI=1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;; Key: SZQUEWJRBJDHSM-UHFFFAOYAC
Properties
Molecular formula	Fe(NO3)3
Molar mass	241.86 g/mol (anhydrous) 403.999 g/mol (nonahydrate)
Appearance	Pale violet crystals hygroscopic
Density	1.68 g/cm3 (hexahydrate) 1.6429 g/cm3(nonahydrate)
Melting point	47.2 °C (nonahydrate)
Boiling point	125 °C (nonahydrate)
Solubility in water	150 g/100 mL (hexahydrate)
Solubility	soluble in alcohol, acetone
Structure
Coordination geometry	octahedral
Hazards[1]
GHS pictograms
GHS signal word	WARNING
GHS hazard statements	H272, H302, H319
GHS precautionary statements	P210, P220, P221, P264, P270, P280, P301+312, P305+351+338, P330, P337+313, P370+378, P501
EU Index	not listed
NFPA 704	0 1 0 OX
Flash point	non-flammable
Related compounds
Related compounds	Iron(III) chloride Iron(III) sulfate
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Iron(III) nitrate, or ferric nitrate, is the chemical compound with the formula Fe(NO₃)₃. Since it is deliquescent, it is commonly found in its nonahydrate form Fe(NO₃)₃·9H₂O in which it forms colourless to pale violet crystals.

Preparation

The compound is prepared by treating iron metal powder with nitric acid.

2 Fe + 8 HNO₃ = 2 Fe(NO₃)₃ + 2 NO + 4 H₂O.

Applications

In the chemical laboratory

Ferric nitrate is the catalyst of choice for the synthesis of sodium amide from a solution of sodium in ammonia:^[2]

2 NH₃ + 2 Na → 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.^[3]

Other applications

Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.

References

1. ↑ HSNO Chemical Classification Information Database, New Zealand Environmental Risk Management Authority, retrieved 2010-09-19 .
2. ↑ Hampton, K. G. Harris, T. M.; Hauser, C. R. (1973), "2,4-Nonanedione", Org. Synth. ; Coll. Vol. 5: 848  As of 2007, 22 other entries describe similar preparations in Organic Syntheses
3. ↑ 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. doi:10.1002/047084289.