Iron(III) nitrate

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Iron(III) nitrate
Iron(III) nitrate nonahydrate
Identifiers
CAS number 10421-48-4 YesY
13476-08-9 (hexahydrate)
7782-61-8 (nonahydrate)
PubChem 168014
ChemSpider 10670706 YesY
UNII N8H8402XOB YesY
RTECS number NO7175000
Jmol-3D images Image 1
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 Ox. sol. 3Acute tox. 4 (oral); Eye irrit. 1
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
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point non-flammable
Related compounds
Related compounds Iron(III) chloride
Iron(III) sulfate
Except where noted otherwise, 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[edit]

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[edit]

In the chemical laboratory[edit]

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[edit]

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

References[edit]

  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.
HNO3 He
LiNO3 Be(NO3)2 B(NO3)3 C N O F Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti V 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 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I Xe
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 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