Copper(II) Chloride

{{Chemical|related_anions=|solubility=70.6 g/100mL (0 °C) 107.9 g/100mL (100 °C)|solubility_in_water=Soluble in methanol, ethanol, hot sulfuric acid, and acetone|boiling_point=990 °C (decomposes)|melting_point=620 °C|density=2.54 g/cm^3 (20 °C)|appearance=Brown crystalline powder (anhydrous) Greeen crystalline solid (dihydrate)|chemical_formula=CuCl2|molar_mass=134.45 g/mol|smiles=Cl[Cu]Cl|inchl=InChI=1S/2ClH.Cu/h2*1H;/q;;+2/p-2 KEY= ORTQZVOHEJQUHG-UHFFFAOYSA-L|pubchem_cid=24014|chemspider=148734|cas_number=7447-39-4 (anhydrous} 10125-13-0 (dihydrate)|other_names=Cupric chloride, copper dichloride,|iupac_name=Dichlorocopper|image1=}}

Copper(II) chloride is an inorganic salt with the formula CuCl 2. Copper(II) chloride can be found naturally as the minerals eriochalcite (dihydrate) and tolbachnite (anhydrous). Copper(II) It has been shown to have paramagnetic properties, and was used in the first electron paramagnetic resonance measurements by Yevgeny Zavoisky in 1944.

Synthesis
Copper(II) chloride is prepared industrially by bringing copper metal to 400 °C in a chlorine atmosphere.

Another method of creating it commercially is mixing copper(II) oxide and an excess of ammonium chloride.

A method that is not common in industry is the reaction of a copper salt like basic copper carbonate with hydrochloric acid. Copper metal cannot be used in this method to create copper(II) chloride. this method could produce copper(I) chloride but this problem can be easily fixed by air through the solution.

A fourth, mostly unknown method is using copper(II) sulfate and calcium chloride in a solution and heating it. this will precipitate out calcium sulfate and will leave a neutral copper chloride solution that can be filtered and evaporated.

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