Copper(II) acetate

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Copper(II) acetate
Small crystals of copper(II) acetate
Copper(II)acetate crystal 01.jpg
Copper(II) acetate crystals on copper wire
IUPAC name
Other names
Copper(II) ethanoate
Cupric acetate
Copper acetate
3D model (JSmol)
ECHA InfoCard 100.005.049
EC Number
  • 205-553-3
UN number 3077
Molar mass 181.63 g/mol (anhydrous)
199.65 g/mol (hydrate)
Appearance Dark green crystalline solid
Odor Odorless (hydrate)
Density 1.882 g/cm3 (hydrate)
Melting point Undetermined(135-by 中文wikipedia)[1]
Boiling point 240 °C (464 °F; 513 K)
7.2 g/100 mL (cold water)
20 g/100 mL (hot water)
Solubility Soluble in alcohol
Slightly soluble in ether and glycerol
1.545 (hydrate)
Safety data sheet Baker MSDS
GHS pictograms GHS05: CorrosiveGHS06: ToxicGHS07: HarmfulGHS09: Environmental hazard
GHS Signal word Danger
H301, H302, H311, H314, H318, H400, H410, H411, H412
P260, P264, P270, P273, P280, P301+310, P301+312, P301+330+331, P302+352, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P322, P330, P361, P363, P391, P405, P501
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
710 mg/kg oral rat[3]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 1 mg/m3 (as Cu)[2]
REL (Recommended)
TWA 1 mg/m3 (as Cu)[2]
IDLH (Immediate danger)
TWA 100 mg/m3 (as Cu)[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Copper(II) acetate, also referred to as cupric acetate, is the chemical compound with the formula Cu(OAc)2 where AcO is acetate (CH
). The hydrated derivative, which contains one molecule of water for each Cu atom, is available commercially. Anhydrous Cu(OAc)2 is a dark green crystalline solid, whereas Cu2(OAc)4(H2O)2 is more bluish-green. Since ancient times, copper acetates of some form have been used as fungicides and green pigments. Today, copper acetates are used as reagents for the synthesis of various inorganic and organic compounds.[4] Copper acetate, like all copper compounds, emits a blue-green glow in a flame. The mineral hoganite is a naturally occurring form of copper(II) acetate.


The dinuclear structure of dimeric copper(II) acetate hydrate
Copper(II) acetate monohydrate, dichroic

Copper acetate hydrate adopts the paddle wheel structure seen also for related Rh(II) and Cr(II) tetraacetates.[5][6] One oxygen atom on each acetate is bound to one copper at 1.97 Å (197 pm). Completing the coordination sphere are two water ligands, with Cu–O distances of 2.20 Å (220 pm). The two five-coordinate copper atoms are separated by only 2.62 Å (262 pm), which is close to the Cu–Cu separation in metallic copper.[7] The two copper centers interact resulting in a diminishing of the magnetic moment such that near 90 K, Cu2(OAc)4(H2O)2 is essentially diamagnetic due to cancellation of the two opposing spins. Cu2(OAc)4(H2O)2 was a critical step in the development of modern theories for antiferromagnetic coupling.[8]


Copper(II) acetate is prepared industrially by heating copper(II) hydroxide or basic copper(II) carbonate with acetic acid.[4]

Related compounds[edit]

Heating a mixture of anhydrous copper(II) acetate and copper metal affords copper(I) acetate:[9][10]

Cu + Cu(OAc)2 → 2 CuOAc

Unlike the copper(II) derivative, copper(I) acetate is colourless and diamagnetic.

"Basic copper acetate" is prepared by neutralizing an aqueous solution of copper(II) acetate. The basic acetate is poorly soluble. This material is a component of verdigris, the blue-green substance that forms on copper during long exposures to atmosphere.

Uses in chemical synthesis[edit]

Copper(II) acetate has found some use as an oxidizing agent in organic syntheses. In the Eglinton reaction Cu2(OAc)4 is used to couple terminal alkynes to give a 1,3-diyne:[11][12]

Cu2(OAc)4 + 2 RC≡CH → 2 CuOAc + RC≡C−C≡CR + 2 HOAc

The reaction proceeds via the intermediacy of copper(I) acetylides, which are then oxidized by the copper(II) acetate, releasing the acetylide radical. A related reaction involving copper acetylides is the synthesis of ynamines, terminal alkynes with amine groups using Cu2(OAc)4.[13] It has been used for hydroamination of acrylonitrile.[14]

It is also an oxidising agent in Barfoed's test.

It combines with arsenic trioxide to form copper acetoarsenite, a powerful insecticide and fungicide called Paris Green or Schweinfurt Green.

External links[edit]


  1. ^ Trimble, R. F. "Copper(II) acetate monohydrate - An erroneous melting point". Journal of Chemical Education. 53: 397. doi:10.1021/ed053p397.
  2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ "Archived copy" (PDF). Archived from the original (PDF) on 2011-09-28. Retrieved 2011-06-14.CS1 maint: archived copy as title (link)
  4. ^ a b Richardson, H. Wayne. "Copper Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH.
  5. ^ Van Niekerk, J. N.; Schoening, F. R. L. (1953). "X-Ray Evidence for Metal-to-Metal Bonds in Cupric and Chromous Acetate". Nature. 171 (4340): 36–37. doi:10.1038/171036a0.
  6. ^ Wells, A. F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press.[ISBN missing]
  7. ^ Catterick, J.; Thornton, P. (1977). "Structures and physical properties of polynuclear carboxylates". Adv. Inorg. Chem. Radiochem. 20: 291–362. doi:10.1016/s0065-2792(08)60041-2.
  8. ^ Carlin, R. L. (1986). Magnetochemistry. Berlin: Springer.[ISBN missing]
  9. ^ Kirchner, S. J.; Fernando, Q. (1980). "Copper(I) Acetate". Inorg. Synth. 20: 53–55. doi:10.1002/9780470132517.ch16.
  10. ^ Parish, E. J.; Kizito, S. A. (2001). "Copper(I) Acetate". Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rc193.
  11. ^ Stöckel, K.; Sondheimer, F. "[18]Annulene". Organic Syntheses. 54: 1. doi:10.15227/orgsyn.054.0001.; Collective Volume, 6, p. 68
  12. ^ Campbell, I. D.; Eglinton, G. "Diphenyldiacetylene". Organic Syntheses. 45: 39. doi:10.15227/orgsyn.045.0039.; Collective Volume, 5, p. 517
  13. ^ Vogel, P.; Srogl, J. (2005). "Copper(II) Acetate". EROS Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rc194.pub2. ISBN 978-0-470-84289-8..
  14. ^ Heininger, S. A. "3-(o-Chloroanilino)propionitrile". Organic Syntheses. 38: 14. doi:10.15227/orgsyn.038.0014.; Collective Volume, 4, p. 146