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Aqueous solutions prepared from copper(II) chloride contain a range of copper(II) complexes depending on concentration, temperature, and the presence of additional chloride ions. These species include the blue color of [Cu(H 2 O) 6 ] 2+ and the yellow or red color of the halide complexes of the formula [CuCl 2+ x ] x − .
The same hydrochloric acid solutions also react with acetylene gas to form [CuCl(C 2 H 2)]. Ammoniacal solutions of CuCl react with acetylenes to form the explosive copper(I) acetylide, Cu 2 C 2. Alkene complexes of CuCl can be prepared by reduction of CuCl 2 by sulfur dioxide in the presence of the alkene in alcohol solution.
Cu 2 (OH) 3 Cl can be prepared by air oxidation of CuCl in brine solution. The CuCl solution is usually made by the reduction of CuCl 2 solutions over copper metal. A CuCl 2 solution with concentrated brine is contacted with copper metal until the Cu(II) is completely reduced. The resulting CuCl is then heated to 60–90 °C (140–194 °F) and ...
Copper(II) acetate, also referred to as cupric acetate, is the chemical compound with the formula Cu(OAc) 2 where AcO − is acetate (CH 3 CO − 2).The hydrated derivative, Cu 2 (OAc) 4 (H 2 O) 2, which contains one molecule of water for each copper atom, is available commercially.
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
Legend: (g)—gas; (l)—liquid; (aq)—aqueous solution; the balance of the species are in a solid phase. Atomic Energy of Canada Limited has demonstrated experimentally a CuCl electrolyzer in which hydrogen is produced electrolytically at the cathode and Cu(I) is oxidized to Cu(II) at the anode, thereby combining above steps 1 and 4 to ...
4 CuI + Hg → (Cu +) 2 [HgI 4] 2− + 2 Cu. This reaction can be used for the detection of mercury since the white CuI to brown Cu 2 [HgI 4] color change is dramatic. Copper(I) iodide is used in the synthesis of Cu(I) clusters such as [Cu 6 I 7] −. [10] Copper(I) iodide dissolves in acetonitrile, yielding diverse complexes.
Copper(II) thiocyanate can be prepared from the reaction of concentrated solutions of copper(II) and a soluble thiocyanate salt in water, precipitating as a black powder. [2] [3] With rapid drying, pure Cu(SCN) 2 can be isolated. Reaction at lower concentrations and for longer periods of time generates instead copper(I) thiocyanate. [4]