Aluminium nitrate

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Aluminium nitrate
Aluminium nitrate.png
Dusičnan hlinitý.JPG
Identifiers
CAS number 13473-90-0 YesY
7784-27-2 (nonahydrate)
PubChem 26053
ChemSpider 24267 YesY
RTECS number BD1040000 (anhydrous)
BD1050000 (nonahydrate)
Jmol-3D images Image 1
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 (163.0 °F; 345.9 K) nonahydrate
Boiling point 135 °C (275 °F; 408 K) nonahydrate, decomposes
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
Flammability code 0: Will not burn. E.g., water Health code 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g., sodium chloride Reactivity code 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., fluorine Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point 35 °C (95 °F; 308 K)
LD50 4280 mg/kg, oral (rat)
Except where noted otherwise, 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 salt of aluminium and nitric acid, existing normally as a crystalline hydrate, most commonly as aluminium nitrate nonahydrate, Al(NO3)3·9H2O.

Preparation[edit]

Aluminium nitrate is not easily made by adding aluminium to nitric acid, as the aluminium forms a passivation layer.

Aluminium nitrate is made by adding nitric acid to aluminium trichloride. Nitrosyl chloride is produced as a by-product; it bubbles out of the solution as a gas.

Aluminium nitrate nonahydrate can also be made by adding a lead nitrate solution to an aluminium sulfate solution. The insoluble lead sulfate is precipitated out of the solution, leaving a solution of aluminium nitrate.

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.

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.[1]

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

Al(NO3)3 + 3NaOH → Al(OH)3 + 3NaNO3

References[edit]

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8

External links[edit]

HNO3 He
LiNO3 Be(NO3)2 B(NO3)3 C N O F Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti V 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 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I Xe
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 Po At Rn
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce 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