Sodium aluminate

Sodium aluminate

Crystal structure with sodium in yellow, aluminium in grey, and oxygen in red[1]

Sodium metaaluminate sample
Names
IUPAC name
Sodium aluminate
Other names
Sodium aluminium oxide,
Sodium metaaluminate
Aluminate, ((AlO2)1−), sodium
Identifiers
3D model (JSmol)
ECHA InfoCard 100.013.728 Edit this at Wikidata
EC Number
  • 215-100-1
UNII
  • InChI=1S/Al.Na.2O/q-1;+1;;
    Key: IYJYQHRNMMNLRH-UHFFFAOYSA-N
  • O=[Al-]=O.[Na+]
Properties
NaAlO2
Molar mass 81.97 g/mol
Appearance white powder (sometimes light-yellowish)
hygroscopic/ when dissolved in water a colloidal black solution is formed
Odor odorless
Density 1.5 g/cm3
Melting point 1,650 °C (3,000 °F; 1,920 K)
highly soluble
Solubility Insoluble in alcohol[2]
1.566
Structure
orthorhombic
Thermochemistry
73.6 J/mol K
70.4 J/mol K
-1133.2 kJ/mol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium aluminate is an inorganic chemical that is used as an effective source of aluminium hydroxide for many industrial and technical applications. Pure sodium aluminate (anhydrous) is a white crystalline solid having a formula variously given as NaAlO2, NaAl(OH)4 (hydrated),[3] Na2O·Al2O3, or Na2Al2O4. Commercial sodium aluminate is available as a solution or a solid.
Other related compounds, sometimes called sodium aluminate, prepared by reaction of Na2O and Al2O3 are Na5AlO4 which contains discrete AlO45− anions, Na7Al3O8 and Na17Al5O16 which contain complex polymeric anions, and NaAl11O17, once mistakenly believed to be β-alumina, a phase of aluminium oxide.[4][5]

  1. ^ Kaduk, James A.; Pei, Shiyou (1995). "The Crystal Structure of Hydrated Sodium Aluminate, NaAlO2•5/4H2O, and Its Dehydration Product". Journal of Solid State Chemistry. 115 (1): 126–139. doi:10.1006/jssc.1995.1111.
  2. ^ The Merck Index. 10th ed. Rahway, New Jersey: Merck Co., Inc., 1983., p. 1229
  3. ^ "Aluminium". chemguide.co.uk.
  4. ^ "Identification and characterisation of three novel compounds in the sodium–aluminium–oxygen system", Marten G. Barker, Paul G. Gadd and Michael J. Begley, J. Chem. Soc., Dalton Trans., 1984, 1139–1146, doi:10.1039/DT9840001139
  5. ^ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5