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Names | |
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Other names Copper (II) oxalate, cupric oxalate, copper(2+) ethanedioate | |
Identifiers | |
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3D model (JSmol) | |
ChemSpider | |
ECHA InfoCard | 100.011.283 |
EC Number |
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PubChem CID | |
UNII | |
UN number | 3077 |
CompTox Dashboard (EPA) | |
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Properties | |
CuC 2O 4 | |
Molar mass | 151.56 |
Appearance | blue solid |
Density | 6.57 g/cm3 |
insoluble | |
Solubility product (Ksp) | 4.43×10−10 [1] |
Hazards | |
GHS labelling: | |
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Warning | |
H302, H302+H312, H312 | |
P264, P270, P280, P301+P312, P302+P352, P312, P322, P330, P363, P501 | |
Thermochemistry | |
Std enthalpy of formation (ΔfH⦵298) | −751.3 kJ/mol [3] |
Related compounds | |
Related compounds | Calcium oxalate Sodium oxalate Magnesium oxalate Strontium oxalate Barium oxalate Iron(II) oxalate Iron(III) oxalate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
Copper(II) oxalate is an inorganic compound with the chemical formula CuC2O4•(H2O)x. The value of x lies between 0 (anhydrous form) and 0.44. One of these species is found as the secondary mineral moolooite (0.44 hydrate). [4] The anhydrous compound has been characterized by X-ray crystallography. [5] Many transition metal oxalate complexes are known.
Copper(II) oxalate, whether anhydrous or hydrated, is practically insoluble in all solvents, as it is a coordination polymer. [6]
Copper(II) oxalate can be produced by precipitation from acidified aqueous copper(II) salts and oxalic acid or an alkali metal oxalate. [7] [8]
Upon heating to 130 °C, the hydrated copper(II) oxalates convert to the anhydrous cupric oxalate. Further heating at higher temperatures under an atmosphere of hydrogen gives copper metal, suitable as a reagent. [7]
The hydrates bind Lewis bases.
Hydrated copper(II) oxalate reacts with alkali metal oxalates and ammonium oxalate to give bis(oxalato)cuprate: [9]
Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylated polyformaldehyde. [10] [11]
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