Iron(III) nitrate

Iron(III) nitrate

Names
IUPAC name Iron(III) nitrate
Other names Ferric nitrate Nitric acid, iron(3+) salt
Identifiers
CAS Number	10421-48-4 13476-08-9 (hexahydrate) 7782-61-8 (nonahydrate)
ChemSpider	10670706
Jmol 3D model	Interactive image
PubChem	168014
RTECS number	NO7175000
UNII	N8H8402XOB
InChI InChI=1S/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;; Key: SZQUEWJRBJDHSM-UHFFFAOYSA-N InChI=1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;; Key: SZQUEWJRBJDHSM-UHFFFAOYAC
SMILES [Fe+3].O.O.O.O.O.O.O.O.O.O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Chemical 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/cm^3 (hexahydrate) 1.6429 g/cm^3(nonahydrate)
Melting point	47.2 °C (117.0 °F; 320.3 K) (nonahydrate)
Boiling point	125 °C (257 °F; 398 K) (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
NFPA 704	0 1 0 OX
Flash point	non-flammable
US health exposure limits (NIOSH):
REL (Recommended)	TWA 1 mg/m^3[2]
Related compounds
Related compounds	Iron(III) chloride Iron(III) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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.

Fe + 4 HNO₃ → Fe(NO₃)₃ + NO + 2 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:^[3]

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.^[4]

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. "NIOSH Pocket Guide to Chemical Hazards #0346". National Institute for Occupational Safety and Health (NIOSH).
3. Hampton, K. G. Harris, T. M.; Hauser, C. R. (1973). "2,4-Nonanedione". Org. Synth.; Coll. Vol. 5, p. 848 As of 2007, 22 other entries describe similar preparations in Organic Syntheses
4. 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.

Salts and covalent derivatives of the Nitrate ion
HNO3																	He
LiNO3	Be(NO3)2											B(NO3)4^−	C	N	O	FNO3	Ne
NaNO3	Mg(NO3)2											Al(NO3)3	Si	P	S	ClONO2	Ar
KNO3	Ca(NO3)2	Sc(NO3)3	Ti(NO3)4	VO(NO3)3	Cr(NO3)3	Mn(NO3)2	Fe(NO3)3	Co(NO3)2, Co(NO3)3	Ni(NO3)2	Cu(NO3)2	Zn(NO3)2	Ga(NO3)3	Ge	As	Se	Br	Kr
RbNO3	Sr(NO3)2	Y	Zr(NO3)4	Nb	Mo	Tc	Ru	Rh	Pd(NO3)2	AgNO3	Cd(NO3)2	In	Sn	Sb	Te	I	Xe(NO3)2
CsNO3	Ba(NO3)2		Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg2(NO3)2, Hg(NO3)2	Tl(NO3)3	Pb(NO3)2	Bi(NO3)3	Po	At	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Uut	Fl	Uup	Lv	Uus	Uuo
		↓
		La	Ce(NO3)3, Ce(NO3)4	Pr	Nd	Pm	Sm	Eu	Gd(NO3)3	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(NO3)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr