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.
Nitric acid, iron(3+) salt
3D model (JSmol)
|Molar mass||403.999 g/mol (nonahydrate) |
241.86 g/mol (anhydrous)
|Appearance||Pale violet crystals |
|Density||1.68 g/cm3 (hexahydrate) |
|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|
|H272, H302, H319|
|P210, P220, P221, P264, P270, P280, P301+P312, P305+P351+P338, P330, P337+P313, P370+P378, P501|
|NFPA 704 (fire diamond)|
|NIOSH (US health exposure limits):|
|TWA 1 mg/m3|
|Safety data sheet (SDS)||External SDS|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
(what is ?)
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+.
Other hydrates Fe(NO
When dissolved, iron(III) nitrate forms yellow solution due to hydrolysis. When heated to near boiling, nitric acid will evaporate from the solution, and all the iron will precipitate as iron(III) oxide Fe
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.