aluminium nitrate
{{distinguish|Aluminium nitride}}
{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 449203454
| ImageFile = Aluminium nitrate.png
| ImageSize = 150px
| ImageFile1 = Dusičnan hlinitý.JPG
| IUPACName = Aluminium nitrate
| OtherNames = Nitric Aluminum salt
aluminum nitrate
aluminium(III) nitrate
| Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 24267
| ChEBI = 231496
| InChI = 1/Al.3NO3/c;3*2-1(3)4/q+3;3*-1
| SMILES = [Al+3].O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O
| InChIKey = JLDSOYXADOWAKB-UHFFFAOYAJ
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Al.3NO3/c;3*2-1(3)4/q+3;3*-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = JLDSOYXADOWAKB-UHFFFAOYSA-N
| CASNo = 13473-90-0
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo2_Ref = {{cascite|correct|CAS}}
| CASNo2 = 7784-27-2
| CASNo2_Comment = (nonahydrate)
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = HUO854648Y
| UNII2_Ref = {{fdacite|correct|FDA}}
| UNII2 = 8MC6621V1H
| UNII2_Comment = (nonhydrate)
| PubChem = 26053
| RTECS = BD1040000 (anhydrous)
BD1050000 (nonahydrate)
| EC_number = 236-751-8
| UNNumber = 1438
}}
| Section2 = {{Chembox Properties
| Formula = Al(NO3)3
| MolarMass = 212.996 g/mol (anhydrous)
375.134 g/mol (nonahydrate)
| Appearance = White crystals, solid
hygroscopic
| Odor = odorless
| Density = 1.72 g/cm3 (nonahydrate)
| Solubility = anhydrous:
60.0 g/100ml (0°C)
73.9 g/100ml (20 °C)
160 g/100ml (100 °C)
nonahydrate:
67.3 g/100 mL
| Solubility1 = 14.45 g/100ml
| Solvent1 = methanol
| Solubility2 = 8.63 g/100ml
| Solvent2 = ethanol
| Solubility3 = 18.32 g/100ml
| Solvent3 = ethylene glycol
| MeltingPtC = 66
| MeltingPt_notes = (anhydrous){{cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=8810|title=aluminum nitrate}}
{{convert|73.9|C|F K}} (nonahydrate)
| BoilingPtC = 150
| BoilingPt_notes = (nonahydrate) decomposes
| RefractIndex = 1.54
| pKa =
| pKb =
| Viscosity =
}}
| Section7 = {{Chembox Hazards
| ExternalSDS = [https://beta-static.fishersci.com/content/dam/fishersci/en_US/documents/programs/education/regulatory-documents/sds/chemicals/chemicals-a/S25148A.pdf External MSDS]
| MainHazards =
| FlashPtC = 35
| FlashPt_notes = (nonahydrate)
| NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 1 | NFPA-S = OX
| LD50 = 4280 mg/kg, oral (rat)
| IDLH = N.D.{{PGCH|0024}}
| GHSPictograms = {{GHS03}}{{GHS05}}{{GHS06}}{{GHS07}}{{GHS08}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|271|272|301|315|318|319|361}}
| PPhrases = {{P-phrases|201|202|210|220|221|264|270|280|281|283|301+310|302+352|305+351+338|306+360|308+313|310|321|330|332+313|337+313|362|370+378|371+380+375|405|501}}
}}
}}
Aluminium nitrate is a white, water-soluble salt of aluminium and nitric acid, most commonly existing as the crystalline hydrate, aluminium nitrate nonahydrate, Al(NO3)3·9H2O.
Preparation
Aluminium nitrate cannot be synthesized by the reaction of aluminium with concentrated nitric acid, as the aluminium forms a passivation layer.
Aluminium nitrate may instead be prepared by the reaction of nitric acid with aluminium(III) chloride. Nitrosyl chloride is produced as a by-product; it bubbles out of the solution as a gas. More conveniently, the salt can be made by reacting nitric acid with aluminium hydroxide.
Aluminium nitrate may also be prepared a metathesis reaction between aluminium sulfate and a nitrate salt with a suitable cation such as barium, strontium, calcium, silver, or lead. e.g. Al2(SO4)3 + 3 Ba(NO3)2 → 2 Al(NO3)3 + 3 BaSO4.
Uses
Aluminium nitrate is a strong oxidizing agent. It is used in tanning leather, antiperspirants, corrosion inhibitors, extraction of uranium, petroleum refining, and as a nitrating agent.
The nonahydrate and other hydrated aluminium nitrates have many applications. These salts are used to produce alumina for preparation of insulating papers, in cathode ray tube heating elements, and on transformer core laminates. The hydrated salts are also used for the extraction of actinide elements.Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}.
It is used in the laboratory and classroom such as in the reaction
: Al(NO3)3 + 3 NaOH → Al(OH)3 + 3 NaNO3
It is, however, much less often encountered than aluminium chloride and aluminium sulfate.
References
{{reflist}}
External links
- [https://web.archive.org/web/20150704002145/http://avogadro.chem.iastate.edu/MSDS/Al(NO3)3-9H2O.htm MSDS of nonahydrate]
- [http://www.chemicalsubstanceschimiques.gc.ca/fact-fait/alum-salts-sels-eng.php Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts]
{{Aluminium compounds}}
{{nitrates}}
{{Authority control}}