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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 aluminium 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.
Stoichiometry
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]
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]
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
- ^ a b c d Daintith J, ed. (2008). "Aluminium ethanoate (aluminium acetate)". A Dictionary of Chemistry (6th ed.). Oxford University Press. ISBN 978-0-19-920463-2.
- ^ Wesolowski DJ, Blencoe JG, Cole DR, Bell JL, Palmer DA (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.
- ^ a b Perry DL, Phillips SL, eds. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 978-0-8493-8671-8.
- ^ Wade K, Banister AJ, Bailar JA, Emeléus HJ, Nyholm R (1973). The Chemistry of Aluminium, Gallium, Indium and Thallium : Comprehensive Inorganic Chemistry. Saint Louis: Elsevier Science. p. 1047. ISBN 978-1-4831-5322-3. OCLC 953379198.
- ^ a b Taylor MJ, Brothers PJ (1993). "Inorganic derivative of the elements". In Downs AJ (ed.). Chemistry of Aluminium, Gallium, Indium, and Thallium. Bishopbriggs, Glasgow: Chapman & Hall. p. 158. ISBN 978-0-7514-0103-5.
If an internal link led you here, you may wish to change the link to point directly to the intended article.
| Clinical data | |
|---|---|
| AHFS/ Drugs.com | Monograph |
| License data | |
|
Routes of administration | Topical |
| ATC code |
|
Aluminium acetate or aluminium ethanoate [1] (also "aluminum ~"), sometimes abbreviated AlAc in geochemistry, [2] can refer to a number of different salts of aluminium 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.
Stoichiometry
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]
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]
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
- ^ a b c d Daintith J, ed. (2008). "Aluminium ethanoate (aluminium acetate)". A Dictionary of Chemistry (6th ed.). Oxford University Press. ISBN 978-0-19-920463-2.
- ^ Wesolowski DJ, Blencoe JG, Cole DR, Bell JL, Palmer DA (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.
- ^ a b Perry DL, Phillips SL, eds. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 978-0-8493-8671-8.
- ^ Wade K, Banister AJ, Bailar JA, Emeléus HJ, Nyholm R (1973). The Chemistry of Aluminium, Gallium, Indium and Thallium : Comprehensive Inorganic Chemistry. Saint Louis: Elsevier Science. p. 1047. ISBN 978-1-4831-5322-3. OCLC 953379198.
- ^ a b Taylor MJ, Brothers PJ (1993). "Inorganic derivative of the elements". In Downs AJ (ed.). Chemistry of Aluminium, Gallium, Indium, and Thallium. Bishopbriggs, Glasgow: Chapman & Hall. p. 158. ISBN 978-0-7514-0103-5.
If an internal link led you here, you may wish to change the link to point directly to the intended article.