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 aluminum with acetic acid. In the solid state, three salts exist under this name: basic aluminium monoacetate, (HO)₂AlCH₃CO_2, 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 is prepared by the diformate, Al(OH)(O₂CH)₂ • H₂O, crystallizing from a concentrated solutions of newly precipitated Al(OH)₃ in formic acid. With an excess of the acid, Al(O₂CH)₃ • 3H₂O crystallizes.[4]

Aluminium diacetate

Main article: Aluminium diacetate

Aluminium diacetate, the basic acetates, are prepared from aqueous aluminium acetate solution resulting in white powders.[4] This basic salt forms 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).[4] 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. 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. Perry, Dale L.; Phillips, Sidney L., eds. (1995). Handbook of Inorganic Compounds. CRC Press. p. 3. ISBN 9780849386718.
4. Downs, A. J. (1993). Chemistry of Aluminium, Gallium, Indium, and Thallium. Bishopbriggs, Glasgow: Chapman & Hall. p. 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