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Aluminium acetate

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Aluminium acetate or aluminium ethanoate[1] (also "aluminum ~"), sometimes abbreviated AlAc in geochemistry,[2] can refer to a number of different salts of aluminum with acetic acid. In the solid state, three salts exist under this name: basic aluminium monoacetate, (HO)2AlCH3CO2, basic aluminium diacetate, HOAl(CH3CO2)2,[3] and neutral aluminium triacetate, Al(CH3CO2)3.[3] In aqueous solution, aluminium triacetate hydrolyses to form a mixture of the other two,[1] and all solutions of all three can be referred to as "aluminium acetate" as the species formed co-exist and inter-convert in chemical equilibrium.

Aluminium monoacetate

Main article: Aluminium monoacetate

Aluminium monoacetate, also known as dibasic aluminium acetate, forms from Al(OH)3 and dilute aqueous acetic acid. More concentrated acid leads to the di- and triacetate.[4]

Aluminium diacetate

Main article: Aluminium diacetate

Aluminium diacetate, also known as basic aluminium acetate, is prepared from aqueous aluminium acetate solution resulting in a white powder.[5] This basic salt forms from the hydrolysis of the triacetate in water.[1]

Aluminium triacetate

Main article: Aluminium triacetate

Aluminium triacetate is a chemical compound that is prepared by heating aluminium chloride (AlCl3) or Al powder with a mixture of acetic acid (CH3COOH) and acetic anhydride (C4H6O3).[5] It is referred as the normal salt and is only made in the absence of water at a relatively high temperature like 180 °C.[1]

References

  1. ^ a b c d Daintith, John, ed. (2008). "Aluminium ethanoate (aluminium acetate)". A Dictionary of Chemistry (6th ed.). Oxford University Press. ISBN 9780199204632.
  2. ^ Wesolowski, D. J.; Blencoe, J. G.; Cole, D. R.; Bell, J. L. S.; Palmer, D. A. (1992). "Geochemistry of Crustal Processes to High Temperatures and Pressures". Summaries of FY 92 Geosciences Research (PDF). United States Department of Energy. pp. 38–44.
  3. ^ a b Perry, Dale L.; Phillips, Sidney L., eds. (1995). Handbook of Inorganic Compounds. CRC Press. p. 3. ISBN 9780849386718.
  4. ^ Wade, K. (1973). The Chemistry of Aluminium, Gallium, Indium and Thallium : Comprehensive Inorganic Chemistry. Banister, A. J., Bailar, J. C., Emeléus, H. J., Nyholm, Ronald. Saint Louis: Elsevier Science. p. 1047. ISBN 978-1-4831-5322-3. OCLC 953379198.
  5. ^ a b Downs, A. J. (1993). Chemistry of Aluminium, Gallium, Indium, and Thallium. Bishopbriggs, Glasgow: Chapman & Hall. p. 158. ISBN 075140103X.
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