Molar Mass Of Iron Nitrate
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| Names | |
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| IUPAC name Iron(Three) nitrate | |
| Other names Ferric nitrate | |
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| ECHA InfoCard | 100.030.805 |
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| Backdrop | |
| Chemical formula | Fe(NOiii)3 |
| Molar mass | 403.999 thou/mol (nonahydrate) 241.86 g/mol (anhydrous) |
| Appearance | Pale violet crystals hygroscopic |
| Density | i.68 grand/cmthree (hexahydrate) 1.6429 g/cm3(nonahydrate) |
| Melting point | 47.ii °C (117.0 °F; 320.iii K) (nonahydrate) |
| Humid point | 125 °C (257 °F; 398 K) (nonahydrate) |
| Solubility in water | 150 g/100 mL (hexahydrate) |
| Solubility | soluble in booze, acetone |
| Magnetic susceptibility (χ) | +15,200.0·ten−half dozen cmthree/mol |
| Structure | |
| Coordination geometry | octahedral |
| Hazards[three] | |
| GHS labelling: | |
| Pictograms |   [i] |
| Bespeak discussion | Alarm |
| Chance statements | H272, H302, H319 |
| Precautionary statements | P210, P220, P221, P264, P270, P280, P301+P312, P305+P351+P338, P330, P337+P313, P370+P378, P501 |
| NFPA 704 (fire diamond) | ane 0 0 OX |
| Wink point | not-flammable |
| NIOSH (US health exposure limits): | |
| REL (Recommended) | TWA one mg/mthree [2] |
| Safety data sheet (SDS) | External SDS |
| Related compounds | |
| Other anions | Iron(3) chloride Iron(Three) sulfate |
| Related compounds | Iron(2) nitrate |
| Except where otherwise noted, data are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Infobox references | |
Iron(III) nitrate, or ferric nitrate, is the proper noun used for a series of inorganic compounds with the formula Fe(NOthree)3 .(HtwoO)northward. Most common is the nonahydrate Atomic number 26(NOiii)3 .(H2O)9. The hydrates are all stake colored, water-soluble paramagnetic salts.
Hydrates [edit]
Iron(Three) nitrate is deliquescent, and it is commonly found as the nonahydrate Fe(NOthree)3·9H2O, which forms colourless to pale violet crystals. This compound is the trinitrate salt of the aquo complex [Fe(HtwoO)half dozen]three+.[4] Other hydrates Fe(NO
3 )
3 ·x H
two O, include:
- tetrahydrate (x=iv), more precisely triaqua dinitratoiron(III) nitrate monohydrate, [Iron(NO
iii )
ii (H
two O) +
3 ] [NO −
3 ]·H
2 O, has complex cations where Fe 3+
cantlet is coordinated with two nitrate anions every bit bidentate ligands and 3 of the four h2o 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) two+
v ] [NO −
3 ]
2 , in which the Iron iii+
atom is coordinated to five h2o molecules and a unidentate nitrate anion ligand in octahedral configuration.[five] - hexahydrate (x=six), more precisely hexaaquairon(Iii) trinitrate, [Fe(H
2 O) 3+
vi ] [NO −
3 ]
3 , where the Atomic number 26 three+atom is coordinated to six water molecules in octahedral configuration.[5]
Chemical properties [edit]
Decomposition [edit]
When dissolved, fe(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 .[half dozen]
The compound will dissolve in molten stearic acrid and decompose at well-nigh 120 °C to requite iron(Iii) oxide-hydroxide FeO(OH).[seven]
Preparation [edit]
The compound can exist prepared by treating iron metal powder with nitric acrid.
- Fe + 4 HNOthree → Atomic number 26(NO3)3 + NO + ii 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]
- two NH3 + 2 Na → ii NaNH2 + H2
Certain clays impregnated with ferric nitrate have been shown to exist 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.[nine]
Ferric nitrate solutions are used by jewelers and metalsmiths to compose silver and silver alloys.
References [edit]
- ^ "Iron(III) Nitrate Nonahydrate". American Elements. Retrieved June 20, 2019.
- ^ NIOSH Pocket Guide to Chemical Hazards. "#0346". National Found for Occupational Safety and Health (NIOSH).
- ^ HSNO Chemical Nomenclature Information Database, New Zealand Environmental Run a risk Management Authority, retrieved 2010-09-nineteen .
- ^ Hair, Neil J.; Beattie, James Chiliad. (1977). "Structure of Hexaaquairon(III) Nitrate Trihydrate. Comparing of Atomic number 26(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(Three) nitrate hydrates: Fe(NO
3 )
3 ·10 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(Three)-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 atomic number 26(III) nitrate". Periodical of Materials Science Letters volume sixteen, pages 493–495 doi:x.1023/A:1018528713566 - ^ Hampton, K. G.; Harris, T. One thousand.; Hauser, C. R. (1973). "two,4-Nonanedione". Organic Syntheses. ; Collective Volume, vol. five, p. 848 As of 2007, 22 other entries describe similar preparations in Organic Syntheses
- ^ Cornélis, A. Laszlo, P.; Zettler, G. W. "Iron(III) Nitrate–K10 Montmorillonite Dirt" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289X.
Molar Mass Of Iron Nitrate,
Source: https://en.wikipedia.org/wiki/Iron%28III%29_nitrate
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