Aluminium nitrate: Difference between revisions
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| Decomposes at |
| Decomposes at 135°C (575 K) |
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Revision as of 18:23, 30 April 2007
| Aluminium nitrate | |
|---|---|
| Aluminium nitrate | |
| General | |
| Systematic name | Aluminium nitrate |
| Molecular formula | Al(NO3)3 |
| Molar mass | 212.9962 g/mol |
| Appearance | colorless to white solid, hygroscopic |
| CAS Number | 13473-90-0 (anhydrous), 7784-27-2 (nonahydrate) |
| Properties | |
| Density and phase | >1 g/cm³ |
| Solubility in water | 60.0 g/100 ml (0°C) |
| Melting point | 73°C |
| Boiling point | Decomposes at 135°C (575 K) |
| Hazards | |
| MSDS | External MSDS |
| Except where noted otherwise, data are given for materials in their standard state (at 25°C, 100 kPa) Infobox disclaimer and references | |
Aluminium nitrate is a salt of aluminium and nitric acid, existing normally as a crystalline hydrate, most commonly as aluminium nitrate nonahydrate, Al(NO3)3·9H2O, with a molecular formula weight of 375.13.
Synthesis
Aluminium nitrate can be easily prepared by the reaction of aluminum hydroxide with nitric acid.
The synthesis from aluminium metal has many problems since aluminium is not attacked by nitric acid because of its protective oxide layer. The process involves an initial basic attack with KOH, followed by partial neutralization with nitric acid to precipitate the hydroxide. The hydroxide is then filtered and washed througly to remove soluble potassium nitrate. After this, the filtered aluminium hydroxide is reacted with excess nitric acid. The crystals are very deliquescent and must be stored in dry conditions.
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. It is used in the laboratory and classroom such as in the reaction Al(NO3)3 + 3NaOH --> Al(OH)3 + 3NaNO3
External links
- http://www.jtbaker.com/msds/englishhtml/a2832.htm
- http://www.eol.ucar.edu/~beaton/ChemWeb/worksheets/rxnws.html
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