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.
![]() Chemical structure of ferric nitrate aquo complex
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![]() Sample of ferric nitrate nonahydrate
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Names | |
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IUPAC name
Iron(III) nitrate
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Other names
Ferric nitrate
Nitric acid, iron(3+) salt | |
Identifiers | |
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3D model (JSmol)
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ChemSpider |
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ECHA InfoCard | 100.030.805 |
PubChem CID
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RTECS number |
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UNII |
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CompTox Dashboard (EPA)
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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[3] | |
GHS labelling: | |
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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): | |
REL (Recommended)
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TWA 1 mg/m3[2] |
Safety data sheet (SDS) | External SDS |
Related compounds | |
Other anions
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Iron(III) chloride Iron(III) sulfate |
Related compounds
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Iron(II) nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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+.[4]
Other hydrates Fe(NO
3)
3·xH
2O, include:
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.[6]
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 Fe
2O
3 appears.[7] Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions.[8]
The compound can be prepared by treating iron metal powder with nitric acid, as summarized by the following idealized equation:[9]
Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of sodium amide from a solution of sodium in ammonia:[10]
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.[11]
Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.