Iron(III) nitrate

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Iron(III) nitrate
Iron(III) nitrate nonahydrate
Names
IUPAC name
Iron(III) nitrate
Other names
Ferric nitrate
Nitric acid, iron(3+) salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.805
RTECS number NO7175000
UNII
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[2]
GHS pictograms Ox. sol. 3Acute tox. 4 (oral); Eye irrit. 1
GHS signal word WARNING
H272, H302, H319
P210, P220, P221, P264, P270, P280, P301+312, P305+351+338, P330, P337+313, P370+378, P501
NFPA 704
Flash point non-flammable
US health exposure limits (NIOSH):
REL (Recommended)
TWA 1 mg/m3[1]
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. When dissolved, it forms yellow solution due to hydrolysis.

Preparation[edit]

The compound is prepared by treating iron metal powder with nitric acid.

Fe + 4 HNO3 → Fe(NO3)3 + NO + 2 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:[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[edit]

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

References[edit]

  1. ^ "NIOSH Pocket Guide to Chemical Hazards #0346". National Institute for Occupational Safety and Health (NIOSH). 
  2. ^ HSNO Chemical Classification Information Database, New Zealand Environmental Risk Management Authority, retrieved 2010-09-19 .
  3. ^ Hampton, K. G. Harris, T. M.; Hauser, C. R. (1973). "2,4-Nonanedione". Organic Syntheses. ; Collective Volume, 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(NO
3
)
4
C NO
3
,
NH4NO3
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,
Fe(NO3)2
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(NO3)3 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,
TlNO3
Pb(NO3)2 Bi(NO3)3
BiO(NO3)
Po At Rn
FrNO3 Ra(NO3)2   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
La(NO3)3 Ce(NO3)3,
Ce(NO3)4
Pr Nd Pm Sm Eu(NO3)3 Gd(NO3)3 Tb Dy Ho Er Tm Yb Lu
Ac(NO3)3 Th(NO3)4 Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr