| IUPAC names
| Other names
|Molar mass|| 181.63 g/mol (anhydrous)|
199.65 g/mol (hydrate)
|Appearance|| Dark green crystalline solid (anhydrous)|
Blue-green crystalline solid (monohydrated)
|Density||1.882 g/cm3 (hydrate) (at 20 °C)|
|Melting point||Decomposes above 145 °C|
|Boiling point||240 °C (464 °F; 513 K)|
|7.2 g/100 mL (hydrated)|
|Solubility|| Soluble in ethanol|
Slightly soluble in diethyl ether and glycerol
|Safety data sheet||FischerScientific|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|710 mg/kg oral (rat)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Copper(II) acetate or cupric acetate is a salt of copper with the formula Cu(CH3COO)2, sometimes shortened to Cu(OAc)2. Copper(II) acetate is generally encountered as monohydrate. Anhydrous Cu(OAc)2 is a dark green crystalline solid, while the monohydrate is more bluish-green.
Copper(II) acetate can be used to couple terminal alkynes to give a 1,3-diyne, process known as Eglinton reaction:
- Cu2(OAc)4 + 2 RC≡CH → 2 CuOAc + RC≡C−C≡CR + 2 HOAc
- 2 Cu + Cu2(OAc)4 → 4CuOAc
Copper(II) acetate is a dark green (anhydrous) or blue-green (monohydrate) solid, soluble in water.
Copper(II) acetate can be purchased online.
Copper(II) acetate monohydrate can be made by reacting a copper base with acetic acid.
- 2 CH3COOH + CuO → Cu(CH3COO)2 + H2O
- 2 CH3COOH + Cu(OH)2 → Cu(CH3COO)2 + H2O + 2H2O
Common vinegar can be used for this reaction, though impurities will precipitate when the solution is concentrated.
If you want to use copper metal, you will also need to add diluted hydrogen peroxide to the solution.
Anhydrous copper(II) acetate can be made by heating the monohydrate at 100 °C in a vacuum.
- Make glacial acetic acid
- Grow large crystals
Copper(II) acetates is irritant and toxic.
Copper(II) acetate should be stored in closed bottles. The anhydrous form should be kept in air-tight containers.