al(no3)3

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Aluminium nitrate
Names
IUPAC name

Aluminium nitrate

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Other names

Nitric Aluminum salt
aluminum nitrate
aluminium(III) nitrate

Identifiers

CAS Number

  • 13473-90-0 check
  • 7784-27-2 (nonahydrate) check

3D model (JSmol)

  • Interactive image
ChemSpider
  • 24267 check
ECHA InfoCard 100.033.396 Edit this at Wikidata
EC Number
  • 236-751-8

PubChem CID

  • 26053
RTECS number
  • BD1040000 (anhydrous)
    BD1050000 (nonahydrate)
UNII
  • HUO854648Y check
  • 8MC6621V1H (nonhydrate) check
UN number 1438

CompTox Dashboard (EPA)

  • DTXSID7040318 Edit this at Wikidata

InChI

  • InChI=1S/Al.3NO3/c;3*2-1(3)4/q+3;3*-1 check

    Key: JLDSOYXADOWAKB-UHFFFAOYSA-N check

  • InChI=1/Al.3NO3/c;3*2-1(3)4/q+3;3*-1

    Key: JLDSOYXADOWAKB-UHFFFAOYAJ

SMILES

  • [Al+3].O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O

Properties

Chemical formula

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

Solubility in water

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

Refractive index (nD)

1.54
Hazards
GHS labelling:

Pictograms

GHS03: OxidizingGHS05: CorrosiveGHS06: ToxicGHS07: Exclamation markGHS08: Health hazard

Signal word

Danger

Hazard statements

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H271, H272, H301, H315, H318, H319, H361

Precautionary statements

P201, P202, P210, P220, P221, P264, P270, P280, P281, P283, P301+P310, P302+P352, P305+P351+P338, P306+P360, P308+P313, P310, P321, P330, P332+P313, P337+P313, P362, P370+P378, P371+P380+P375, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate

2

1

OX

Flash point 35 °C (95 °F; 308 K) (nonahydrate)
Lethal dose or concentration (LD, LC):

LD50 (median dose)

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).

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Infobox references

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[edit]

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[edit]

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.

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The nonahydrate and other hydrated aluminium nitrates have many applications. These salts are used lớn 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

It is, however, much less often encountered kêu ca aluminium chloride and aluminium sulfate.

References[edit]

External links[edit]

  • MSDS of nonahydrate
  • Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts