Copper(II) acetate
 Copper(II) acetate monohydrate
| |
| Names | |
|---|---|
| IUPAC names
Copper(II) acetate
Tetra-μ2-acetatodiaquadicopper(II) (hydrated) | |
| Other names
Copper acetate
Copper(II) ethanoate Copper diacetate Cupric acetate Verdigris | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| CuC4H6O4 Cu(CH3COO)2 | |
| Molar mass | 181.63 g/mol (anhydrous) 199.65 g/mol (hydrate) |
| Appearance | Dark green crystalline solid (anhydrous) Blue-green crystalline solid (monohydrated) |
| Odor | Odorless |
| Density | 1.882 g/cm3 (hydrate) (at 20 °C) |
| Melting point | Decomposes above 145 °C[1] |
| 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 |
| Hazards | |
| Safety data sheet | FischerScientific |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
710 mg/kg oral (rat) |
| Related compounds | |
| Related compounds
|
Copper(I) acetate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
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.
Contents
Properties
Chemical
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
Heating a mixture of anhydrous copper(II) acetate and copper metal yields copper(I) acetate:
- 2 Cu + Cu2(OAc)4 → 4CuOAc
Physical
Copper(II) acetate is a dark green (anhydrous) or blue-green (monohydrate) solid, soluble in water.[2] Copper(II) acetate has a color that is slightly difficult to properly capture on camera.
Availability
Copper(II) acetate can be purchased online.
Preparation
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.
Copper(II) acetate can also be prepared from copper(II) hydroxide or basic copper carbonate by the addition of acetic acid followed by evaporation of the solution.[3]
Projects
- Make glacial acetic acid
- Grow large crystals
- Pigment
- Preparation of cis- and trans-Bis(glycinato)copper(II) Monohydrate[4]
Handling
Safety
Copper(II) acetates is irritant and toxic.
Storage
Copper(II) acetate should be stored in closed bottles. The anhydrous form should be kept in air-tight containers.
Disposal
Can be reduced with a metal such as zinc or iron to metallic copper which can be recycled.
References
- ↑ http://pubs.acs.org/doi/pdf/10.1021/ed053p397
- ↑ http://woelen.homescience.net/science/chem/exps/copper_acetates/index.html
- ↑ https://en.crystalls.info/Copper(II)_acetate
- ↑ https://webs.wofford.edu/hilljb/Chem%20323/CopperGlycine.pdf
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- Chemical compounds
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