| IUPAC name
| Other names
|Molar mass||98.999 g/mol|
|Melting point||423 °C (793 °F; 696 K)|
|Boiling point||1,490 °C (2,710 °F; 1,760 K) (decomposes)|
|0.47 g/100 ml (20 °C)|
|Solubility|| Soluble in aq. ammonia, conc. HCl|
Insoluble in acetone, ethanol
|Vapor pressure||~0 mmHg|
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Copper(I) chloride, also called cuprous chloride, has the chemical formula CuCl. It is a white, almost insoluble salt which is slowly oxidized by air to Cu(II).
Pure samples of copper(I) chloride appear as white, dense, cubical crystals. As it is slowly oxidized in air, older samples may appear dirty green or brown.
Copper(I) chloride can be prepared by reduction of copper(II) ions in presence of chloride ions. Possible methods include bubbling sulfur dioxide through an aqueous solution of copper(II) chloride, or heating a solution of copper sulfate, sodium chloride and ascorbic acid. It can also be produced by boiling copper(II) chloride and copper metal in hydrochloric acid.
Copper(I) chloride can be used to make copper oxychloride by oxidation in air.
Cuprous chloride is irritant and corrosive to eyes and skin. Protection clothing should be worn when handling it.
CuCl should be kept in sealed containers, away from oxygen. Schlenk flasks are a good storage container.
CuCl can be oxidized with oxygen or hydrogen peroxide to the more soluble CuCl2, which can be reduced to metallic copper with a more reactive metal, such as iron or zinc.
Copper(I) chloride, Wikipedia (http://en.wikipedia.org/wiki/Copper%28I%29_chloride).