Aluminium nitrate

Aluminium nitrate
Names
IUPAC name
Aluminium nitrate
Other names
Nitric acid, aluminum salt
aluminum nitrate
aluminium(III) nitrate
Identifiers
13473-90-0 YesY
7784-27-2 (nonahydrate) N
3D model (Jmol) Interactive image
ChemSpider 24267 YesY
ECHA InfoCard 100.033.396
PubChem 26053
RTECS number BD1040000 (anhydrous)
BD1050000 (nonahydrate)
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
Safety data sheet External MSDS
NFPA 704
Flash point 35 °C (95 °F; 308 K) (nonahydrate)
Lethal dose or concentration (LD, LC):
4280 mg/kg, oral (rat)
US health exposure limits (NIOSH):
PEL (Permissible)
 none[2]
REL (Recommended)
 2 mg/m3[2]
IDLH (Immediate danger)
 N.D.[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
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

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. 1 2 3 "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

Salts and covalent derivatives of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4− C N O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Co(NO3)3		 Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I Xe(NO3)2
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2		 Tl(NO3)3 Pb(NO3)2 Bi(NO3)3
BiO(NO3)		 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La Ce(NO3)3,
Ce(NO3)4		 Pr Nd Pm Sm Eu Gd(NO3)3 Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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