Msds for 0.200 M Fe No3 3 Solution
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| Names | |
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| IUPAC name Iron(III) nitrate | |
| Other names Ferric nitrate | |
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| ECHA InfoCard | 100.030.805  |
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| Properties | |
| Chemical formula | 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) |
| Solubility in water | 150 g/100 mL (hexahydrate) |
| Solubility | soluble in alcohol, acetone |
| Magnetic susceptibility (χ) | +15,200.0·10−6 cm3/mol |
| Structure | |
| Coordination geometry | octahedral |
| Hazards[3] | |
| Safety data sheet | External SDS |
| GHS pictograms |   [1] |
| GHS Signal word | Warning |
| GHS hazard statements | H272, H302, H319 |
| GHS precautionary statements | P210, P220, P221, P264, P270, P280, P301+P312, P305+P351+P338, P330, P337+P313, P370+P378, P501 |
| NFPA 704 (fire diamond) | 1 0 0 OX |
| Flash point | non-flammable |
| NIOSH (US health exposure limits): | |
| REL (Recommended) | TWA 1 mg/m3 [2] |
| Related compounds | |
| Other anions | Iron(III) chloride Iron(III) sulfate |
| Related compounds | Iron(II) nitrate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 Nverify (what is  Y  N ?) | |
| Infobox references | |
Chemical compound
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.
Hydrates [edit]
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 ·x H
2 O, include:
- tetrahydrate (x=4), more precisely triaqua dinitratoiron(III) nitrate monohydrate, [Fe(NO
3 )
2 (H
2 O) +
3 ] [NO −
3 ]·H
2 O, has complex cations where Fe 3+
atom is coordinated with two nitrate anions as bidentate ligands and three of the four water molecules, in a pentagonal bipyramid configuration with two water molecules at the poles.[5] - pentahydrate (x=5), more precisely penta-aqua nitratoiron(III) dinitrate, [Fe(NO
3 )(H
2 O) 2+
5 ] [NO −
3 ]
2 , in which the Fe 3+
atom is coordinated to five water molecules and a unidentate nitrate anion ligand in octahedral configuration.[5] - hexahydrate (x=6), more precisely hexaaquairon(III) trinitrate, [Fe(H
2 O) 3+
6 ] [NO −
3 ]
3 , where the Fe 3+
atom is coordinated to six water molecules in octahedral configuration.[5]
Chemical properties [edit]
Decomposition [edit]
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
2 O
3 .[6]
The compound will dissolve in molten stearic acid and decompose at about 120 °C to give iron(III) oxide-hydroxide FeO(OH).[7]
Preparation [edit]
The compound can be prepared by treating iron metal powder with nitric acid.
- Fe + 4 HNO3 → Fe(NO3)3 + NO + 2 H2O.
Applications [edit]
Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of sodium amide from a solution of sodium in ammonia:[8]
- 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.[9]
Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.
References [edit]
- ^ "Iron(III) Nitrate Nonahydrate". American Elements. Retrieved June 20, 2019.
- ^ NIOSH Pocket Guide to Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH).
- ^ HSNO Chemical Classification Information Database, New Zealand Environmental Risk Management Authority, retrieved 2010-09-19 .
- ^ Hair, Neil J.; Beattie, James K. (1977). "Structure of Hexaaquairon(III) Nitrate Trihydrate. Comparison of Iron(II) and Iron(III) Bond Lengths in High-Spin Octahedral Environments". Inorganic Chemistry. 16 (2): 245–250. doi:10.1021/ic50168a006.
- ^ a b c H. Schmidt, A. Asztalos, F. Bok and W. Voigt (2012): "New iron(III) nitrate hydrates: Fe(NO
3 )
3 ·x H
2 O with x = 4, 5 and 6". Acta Crystallographica Section C - Inorganic Compounds, volume C68, pages i29-i33. doi:10.1107/S0108270112015855 - ^ Egon Matijević and Paul Scheiner (1978): "Ferric hydrous oxide sols: III. Preparation of uniform particles by hydrolysis of Fe(III)-chloride, -nitrate, and -perchlorate solutions". Journal of Colloid and Interface Science, volume 63, issue 3, pages 509-524. doi:10.1016/S0021-9797(78)80011-3
- ^ Dan Li, Xiaohui Wang, Gang Xiong, Lude Lu, Xujie Yang and Xin Wang (1997): "A novel technique to prepare ultrafine Fe
2 O
3 via hydrated iron(III) nitrate". Journal of Materials Science Letters volume 16, pages 493–495 doi:10.1023/A:1018528713566 - ^ 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
- ^ 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:10.1002/047084289X.
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Salts and covalent derivatives of the nitrate ion
Msds for 0.200 M Fe No3 3 Solution
Source: https://en.wikipedia.org/wiki/Iron%28III%29_nitrate
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