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Cupric acetate

Basic information Physical Properties Uses Preparation Toxicity Safety Related Supplier
Cupric acetate Basic information
Cupric acetate Chemical Properties
  • Melting point:115°C
  • vapor density 6.9 (vs air)
  • form Powder
  • color Green to blue
  • Water Solubility Soluble in water and alcohol. Slightly soluble in ether and glycerol.
  • Sensitive Hygroscopic
  • Merck 14,2624
  • BRN 3595638
  • Stability:hygroscopic
  • CAS DataBase Reference142-71-2(CAS DataBase Reference)
  • EPA Substance Registry SystemCupric acetate (142-71-2)
Safety Information
Cupric acetate Usage And Synthesis
  • Physical PropertiesBluish-green fine powder; hygroscopic. The monohydrate is dimeric; density 1.88 g/cm3; melts at 115°C; decomposes at 240°C; soluble in water and ethanol; and slightly soluble in ether.
  • UsesCopper(II) acetate is used as a pigment for ceramics; in the manufacture of Paris green; in textile dyeing; as a fungicide; and as a catalyst.
  • PreparationCopper(II) acetate is prepared by treatment of copper(II) oxide, CuO, or copper(II) carbonate, CuCO3, with acetic acid, followed by crystallization:
    CuO + 2CH3COOH → (CH3COO)2Cu + H2O
  • ToxicityCopper(II) acetate is moderately toxic by ingestion and possibly other routes of administration.
    LD50 oral (rat): c. 600 mg/kg
  • DescriptionCopper (II) acetate, also referred to as cupric acetate, is the chemical compound with the formula Cu(OAc)22 where OAc- is acetate (CH3CO2-). 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. Copper acetate, like all copper compounds, emits a blue-green glow in a flame.
  • Chemical PropertiesGreen crystalline powder
  • Chemical PropertiesCupric acetate is a greenish Blue powder or small crystals.
  • HistoryCopper (II) acetate was historically prepared in vineyards, since acetic acid is a byproduct of fermentation. Copper sheets were alternately layered with fermented grape skins and dregs left over from wine production and exposed to air. This would leave a blue substance on the outside of the sheet. This was then scraped off and dissolved in water. The resulting solid was used as a pigment, or combined with arsenic trioxide to form copper acetoarsenite, a powerful insecticide and fungicide called Paris Green or Schweinfurt Green.
    During the Second World War copper acetate was used as shark repellent . Under war conditions, before adoption it has been tested only very briefly (while in general successfully). The source says copper acetate does repel sharks in some situations but not in all.
  • UsesUsed as a catalyst or oxidizing agent in organic syntheses
  • UsesUsed in biochemical applications such as DNA extraction
  • ApplicationThe uses for copper (II) acetate are more plentiful as a catalyst or oxidizing agent in organic syntheses. For example, Cu2(OAc)4 is used to couple two terminal alkynes to make a 1,3-diyne:
    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.
  • General DescriptionA blue-green crystalline solid. The primary hazard is the threat to the environment. Immediate steps should be taken to limit its spread to the environment. Cupric acetate is used as an insecticide, in the preparation of other chemicals, as a fungicide, and mildew preventive.
  • Air & Water ReactionsWater soluble.
  • Reactivity ProfileSalts, basic, such as Cupric acetate, are generally soluble in water. The resulting solutions contain moderate concentrations of hydroxide ions and have pH's greater than 7.0. They react as bases to neutralize acids. These neutralizations generate heat, but less or far less than is generated by neutralization of the bases in reactivity group 10 (Bases) and the neutralization of amines. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible.
  • Health HazardInhalation of dust causes irritation of throat and lungs. Ingestion of large amounts causes violent vomiting and purging, intense pain, collapse, coma, convulsions, and paralysis. Contact with solutions irritates eyes; contact with solid causes severe eye surface injury and irritation of skin.
  • Fire HazardSpecial Hazards of Combustion Products: Irritating vapors of acetic acid may form in fires.
  • Safety ProfilePoison by subcutaneous and intraperitoneal routes. Moderately toxic by ingestion. Experimental reproductive effects. When heated to decomposition it emits acrid smoke and irritating fumes. See also COPPER COMPOUNDS.
  • Chemical SynthesisCopper (II) acetate synthesized by the method described in the history section leads to impure samples. It is prepared industrially by heating copper (II) hydroxide or copper (II) carbonate with acetic acid. A second method of copper acetate production is to electrolyze a concentrated aqueous solution of calcium acetate with copper electrodes. As the reaction proceeds the anode oxidizes to produce copper acetate which adheres to its surface and can be removed as crystals. At the cathode calcium ions are reduced to calcium atoms and would be deposited, but due to the water content of the solution the calcium is converted to insoluble calcium hydroxide. The drawback with this setup is that the cathode gets coated with an insulating layer of calcium hydroxide, which gradually slows the process. To negate this hydroxide buildup mercury is utilized as the cathode; therefore as the process takes place the calcium formed immediately reacts with the mercury to make a calcium-mercury amalgam and the copper acetate formed at the anode is removed periodically. This process generally yields suitably pure copper acetate, on a small scale, with slight traces of calcium acetate.
    Copper (II) acetate also forms by treating copper metal with a solution of acetic acid and hydrogen peroxide.
  • Potential ExposureCupric acetate is used as a fungicide, as a catalyst for organic reactions; in textile dyeing and as a pigment for ceramics.
  • ShippingUN3077 Environmentally hazardous substances, solid, n.o.s., Hazard class: 9; Labels: 9-Miscellaneous hazardous material, Technical Name Required.
  • Purification MethodsRecystallise it twice from warm dilute acetic acid solutions (5mL/g) by cooling. [Beilstein 2 IV 111.]
  • IncompatibilitiesForms explosive materials with acetylene gas, ammonia, caustic solutions; sodium hypobromite; notromethane. Keep away from chemically active metals; strong acids; nitrates. Decomposes above 240C forming acetic acid fumes
  • Waste DisposalCopper-containing soluble wastes can be concentrated through the use of ion exchange, reverse osmosis, or evaporators to the point where copper can be electrolytically removed and sent to a reclaiming firm. If recovery is not feasible, the copper can be precipitated through the use of caustics and the sludge deposited in a chemical waste landfill.
Cupric acetate Preparation Products And Raw materials
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