Hostname: page-component-586b7cd67f-dsjbd Total loading time: 0 Render date: 2024-11-23T03:28:45.536Z Has data issue: false hasContentIssue false
  • English
  • Français

Formation of X-ray amorphous and crystalline aluminium hydroxides1

Published online by Cambridge University Press:  14 March 2018

Pa Ho Hsu  and
Thomas F. Bates
Pa Ho Hsu
Affiliation:
Department of Geochemistry and Mineralogy, The Pennsylvania State University, University Park, Pennsylvania, U.S.A.
Thomas F. Bates
Affiliation:
Department of Geochemistry and Mineralogy, The Pennsylvania State University, University Park, Pennsylvania, U.S.A.
Get access Rights & Permissions [Opens in a new window]

Summary

Various crystalline and X-ray amorphous forms of aluminium hydroxide prepared from sulphate and chloride solutions by varying the mole ratio of NaOH to Al3+ have been characterized by chemical analysis and X-ray diffraction. When the NaOH/Al ratio is 3 or 3·3, crystalline Al(OH)3 in the form of bayerite, nordstrandite, gibbsite, or mixtures is obtained in several hours. When the ratio is 2·75 or below, no Al(OH)3 is evident and the products are X-ray amorphous and remain so even after ageing for six months. Chemical analysis indicates that the amorphous precipitates are basic aluminium sulphates or chlorides. In the 0 to 2·1 range of NaOH/Al, the composition of the products is constant, being approximately Al(OH)2·2X0·8. In the 2·1 to 2·75 range, a continuous series of basic salts, of composition ranging from Al(OH)2·2X0·8 to Al(OH)2·75X0·25, is obtained.

Type
Research Article
Information
Mineralogical magazine and journal of the Mineralogical Society , Volume 33 , Issue 264 , March 1964 , pp. 749 - 768
Copyright
Copyright © 1964, The Mineralogical Society

Access options

Get access to the full version of this content by using one of the access options below. (Log in options will check for institutional or personal access. Content may require purchase if you do not have access.)

Footnotes

1

Contribution No. 62–50 from the College of Mineral Industries, The Pennsylvania State University.

References

Bale, (H.D.) and Scihmidt, (P.W.), 1958. Journ. Phys. Chem., vol. 62, p. 1179..Google Scholar
Bale, (H.D.) Bale, (H.D.) 1959. Ibid., vol. 31, p. 1612.Google Scholar
Brosset, (C.), Biedermann, (G.), and Silleiw, (L.G.), 1954. Acta Chem. Scand., vol. 8, p. 1917.CrossRefGoogle Scholar
Calvet, (E.), Boivinet, (P.), Noel, (M.), Thibo:N, (H.), Maillard, (A.), and Tertian, (R.), 1953. Bull. Soc. Chim. France, p. 99.Google Scholar
Harris, (M.R.) and Sing, (W.K.S..), 1955. Journ. Appl. Chem., vol. 5, p. 223.Google Scholar
Harris, (M.R.). 1957. Ibid., vol. 7, p. 397.Google Scholar
Herrbillon, (A.) and Gastuci∼E, (M.), 1962. Compt. Rend. Acad. Sci. Pari., vol. 254, p. 1105.Google Scholar
Hollingworth, (S.E.) and Bannister, (F.A.), 1950. Min. Mag., vol. 29, p. 1.Google Scholar
Hsu, (Pa Ho) and Rich, (C.I.), 1960. Proc. Soil Sci. Soc. Amer., vol. 24, p. 21.Google Scholar
Hsc, (Pa Ho), 1963. Soil Sci., vol. 96, p. 230.Google Scholar
Kunin, (R.), 1958. Ion exchange resins, 2nd edn. John Wiley & Sons, Inc. New York, 466 pp.Google Scholar
Mackenzie, (R.C.), Meldau, (R.), and Gard, (J.A.), 1962. Min. Mag., vol. 33, p. 145.Google Scholar
Marboe, (E.C.) and Bentur, (S.), 1961. Silicates Industriel., vol. 26, p. 389.Google Scholar
Newsome, (J.W.), Heiser, (H.W.), Russel, (A.S.), and Stumpf, (H.C.), 1960. Alumina properties. Alcoa Research Laboratories, Technical Paper No. 10. Second revision.Google Scholar
Papée, (D.), Tertian, (R.), and Biais, (R.), 1958. Bull. Soc. Chim. France, p. 1301.Google Scholar
U.S.D.Salinity Laboratories, 1954. Diagnosis and improvement of saline and alkali soils. U.S.D.Agr. Handbook 60.Google Scholar
Weiser, (H.B.), Milligan, (W.O.), and Purcell, (W.R.), 1940. Ind. Eng. Chem., vol. 32, p. 1487.Google Scholar
Weiser, (H.B.), Milligan, (W.O.), 1941. Ibid., vol. 33, p. 669.Google Scholar
Williamson, (F.S.), 1923. Journ. Phys. Chem., vol. 27, p. 284.Google Scholar