Aluminium nitrate
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| Aluminium nitrate | |
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| IUPAC name |
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| Other names | Nitric acid, aluminum salt |
| Identifiers | |
| CAS number | [], 7784-27-2 (nonahydrate) |
| PubChem | |
| RTECS number | BD1040000 (anhydrous) BD1050000 (nonahydrate) |
| Properties | |
| Molecular formula | Al(NO3)3 |
| Molar mass | 212.996 g/mol (anhydrous) 375.134 g/mol (nonahydrate) |
| Appearance | white solid hygroscopic |
| Odor | odorless |
| Density | 1.72 g/cm3 (nonahydrate) |
| Melting point |
72.8 °C (nonahydrate) |
| Boiling point |
135 °C (nonahyrdate, decomp.) |
| Solubility in water | anhydrous: 60.0 g/100 mL (0°C) 73.4 g/100 mL (20 °C) 160 g/100 mL (100 °C) nonahydrate: 67.3 g/100 mL |
| Solubility in methanol | 14.45 g/ 100mL |
| Solubility in ethanol | 8.63 g/ 100mL |
| Solubility in ethylene glycol | 18.32 g/100 mL |
| Refractive index (nD) | 1.54 |
| Hazards | |
| MSDS | External MSDS |
| NFPA 704 |
 0
2
1
OX
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| Flash point | 135 °C (nonahydrate) |
| LD50 | 4280 mg/kg, oral (rat) |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
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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 375.117 g/mol.
Contents |
[edit] Preparation
Aluminum nitrate nonahydrate is made by adding a lead nitrate solution to an aluminum sulfate solution.
[edit] 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 aluminum nitrates have many applications. These salts are used to produce alumina for preparation of insulating papers, in cathode tube heating elements, and on transformer core laminates. The hydrated salts are also used for the extraction of actinide elements. [1]
It is used in the laboratory and classroom such as in the reaction:
Al(NO3)3 + 3NaOH --> Al(OH)3 + 3NaNO3
[edit] References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
[edit] External links
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