|Jmol-3D images||Image 1|
|Molar mass||241.86 g/mol (anhydrous)
403.999 g/mol (nonahydrate)
|Appearance||Pale violet crystals
|Density||1.68 g/cm3 (hexahydrate)
47.2 °C (nonahydrate)
125 °C (nonahydrate)
|Solubility in water||150 g/100 mL (hexahydrate)|
|Solubility||soluble in alcohol, acetone|
|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|
|Related compounds||Iron(III) chloride
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
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.
The compound is prepared by treating iron metal powder with nitric acid.
- 2 Fe + 8 HNO3 = 2 Fe(NO3)3 + 2 NO + 4 H2O.
In the chemical laboratory
- 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.
Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.
- HSNO Chemical Classification Information Database, New Zealand Environmental Risk Management Authority, retrieved 2010-09-19.
- 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
- 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.