Aluminium nitrate

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Aluminium nitrate
Names
IUPAC name
Aluminium nitrate
Other names
Nitric Aluminum salt
aluminum nitrate
aluminium(III) nitrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.396 Edit this at Wikidata
RTECS number
  • BD1040000 (anhydrous)
    BD1050000 (nonahydrate)
  • InChI=1S/Al.3NO3/c;3*2-1(3)4/q+3;3*-1 checkY
    Key: JLDSOYXADOWAKB-UHFFFAOYSA-N checkY
  • InChI=1/Al.3NO3/c;3*2-1(3)4/q+3;3*-1
    Key: JLDSOYXADOWAKB-UHFFFAOYAJ
  • [Al+3].O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Al(NO3)3
Molar mass 212.996 g/mol (anhydrous)
375.134 g/mol (nonahydrate)
Appearance White crystals, solid
hygroscopic
Odor odorless
Density 1.72 g/cm3 (nonahydrate)
Melting point 66 °C (151 °F; 339 K) (anhydrous)[1]
73.9 °C (165.0 °F; 347.0 K) (nonahydrate)
Boiling point 150 °C (302 °F; 423 K) (nonahydrate) decomposes
anhydrous:
60.0 g/100ml (0°C)
73.9 g/100ml (20 °C)
160 g/100ml (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/100ml
1.54
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
0
3
3
OX
Flash point 35 °C (95 °F; 308 K) (nonahydrate)
Lethal dose or concentration (LD, LC):
4280 mg/kg, oral (rat)
NIOSH (US health exposure limits):
PEL (Permissible)
 none[2]
REL (Recommended)
 2 mg/m3[2]
IDLH (Immediate danger)
 N.D.[2]
Safety data sheet (SDS) External MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

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.

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 + 3Ba(NO3)2 → 2Al(NO3)3 + 3BaSO4

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.[3]

It is used in the laboratory and classroom such as in the reaction:

Al(NO3)3 + 3 NaOH → Al(OH)3 + 3 NaNO3

References

  1. ^ "aluminum nitrate".
  2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0024". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8

External links

Retrieved from "https://en.wikipedia.org/w/index.php?title=Aluminium_nitrate&oldid=862925043"