Chemistry:Aluminium acetate
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.
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
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
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
- ↑ 1.0 1.1 1.2 1.3 Daintith, John, ed (2008). "Aluminium ethanoate (aluminium acetate)". A Dictionary of Chemistry (6th ed.). Oxford University Press. ISBN 9780199204632. http://www.oxfordreference.com/view/10.1093/acref/9780199204632.001.0001/acref-9780199204632-e-186?rskey=bytpyG&result=1.
- ↑ 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. United States Department of Energy. pp. 38–44. http://science.energy.gov/~/media/bes/pdf/archives/summaries/geosciences_summary_book_fy1992.pdf.
- ↑ 3.0 3.1 Perry, Dale L.; Phillips, Sidney L., eds (1995). Handbook of Inorganic Compounds. CRC Press. p. 3. ISBN 9780849386718. https://books.google.com/books?id=0fT4wfhF1AsC&q=aluminium+triacetate+decomposes+200+C&pg=PA3.
- ↑ 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. pp. 1047. ISBN 978-1-4831-5322-3. OCLC 953379198. https://www.worldcat.org/oclc/953379198.
- ↑ 5.0 5.1 Downs, A. J. (1993). Chemistry of Aluminium, Gallium, Indium, and Thallium. Bishopbriggs, Glasgow: Chapman & Hall. pp. 158. ISBN 075140103X.
Acetyl halides and salts of the acetate ion
| |||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| AcOH | He | ||||||||||||||||||
| LiOAc | Be(OAc)2 BeAcOH |
B(OAc)3 | AcOAc ROAc |
NH4OAc | AcOOH | FAc | Ne | ||||||||||||
| NaOAc | Mg(OAc)2 | Al(OAc)3 ALSOL Al(OAc)2OH Al2SO4(OAc)4 |
Si | P | S | ClAc | Ar | ||||||||||||
| KOAc | Ca(OAc)2 | Sc(OAc)3 | Ti(OAc)4 | VO(OAc)3 | Cr(OAc)2 Cr(OAc)3 |
Mn(OAc)2 Mn(OAc)3 |
Fe(OAc)2 Fe(OAc)3 |
Co(OAc)2, Co(OAc)3 |
Ni(OAc)2 | Cu(OAc)2 | Zn(OAc)2 | Ga(OAc)3 | Ge | As(OAc)3 | Se | BrAc | Kr | ||
| RbOAc | Sr(OAc)2 | Y(OAc)3 | Zr(OAc)4 | Nb | Mo(OAc)2 | Tc | Ru(OAc)2 Ru(OAc)3 Ru(OAc)4 |
Rh2(OAc)4 | Pd(OAc)2 | AgOAc | Cd(OAc)2 | In | Sn(OAc)2 Sn(OAc)4 |
Sb(OAc)3 | Te | IAc | Xe | ||
| CsOAc | Ba(OAc)2 | Hf | Ta | W | Re | Os | Ir | Pt(OAc)2 | Au | Hg2(OAc)2, Hg(OAc)2 |
TlOAc Tl(OAc)3 |
Pb(OAc)2 Pb(OAc)4 |
Bi(OAc)3 | Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La(OAc)3 | Ce(OAc)x | Pr | Nd | Pm | Sm(OAc)3 | Eu(OAc)3 | Gd(OAc)3 | Tb | Dy(OAc)3 | Ho(OAc)3 | Er | Tm | Yb(OAc)3 | Lu(OAc)3 | |||||
| Ac | Th | Pa | UO2(OAc)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
 |  |
