Copper oxalate
_Oxalate_Structural_Formula_V1.svg)
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| Names | |
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| Other names
Copper (II) oxalate, cupric oxalate, copper(2+) ethanedioate
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider |
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| ECHA InfoCard | 100.011.283 |
| EC Number |
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PubChem CID
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| UNII |
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| UN number | 3077 |
CompTox Dashboard (EPA)
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| Properties | |
| CuC 2O 4 | |
| Molar mass | 151.56 |
| Appearance | blue-white solid (as a hemihydrate) |
| Melting point | 310 °C (590 °F; 583 K) |
| insoluble | |
Solubility product (Ksp)
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4.43×10−10[1] |
| Hazards | |
| GHS labelling: | |
 [2]
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| Warning | |
| H302, H302+H312, H312 | |
| P264, P270, P280, P301+P312, P302+P352, P312, P322, P330, P363, P501 | |
| Related compounds | |
Related compounds
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Calcium oxalate Sodium oxalate Magnesium oxalate Strontium oxalate Barium oxalate Iron(II) oxalate Iron(III) oxalate Lithium oxalate Praseodymium oxalate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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-oxalat.jpg/1280px-Kupfer(II)-oxalat.jpg)
Copper oxalate is an inorganic compound, a salt of copper metal and oxalic acid with the chemical formula CuC
2O
4.[3] The compound is practically insoluble in water, alcohol, ether, and acetic acid but soluble in ammonium hydroxide.[4] Copper oxalate forms a hydrate, which forms acid-blue crystals.
Synthesis
Copper oxalate can be produced by precipitation from a mixture of a copper (II) salt and a sodium oxalate solution or by reacting copper sulfate with oxalic acid.[5]
Properties
As a hemihydrate, copper oxalate is a blue-white solid that is practically insoluble in water. At 200 °C, it loses its water of crystallization.
The compound also forms complex salts with alkali metal oxalates and ammonium oxalate:
![{\displaystyle {\mathsf {CuC_{2}O_{4}+K_{2}C_{2}O_{4}+2H_{2}O\ {\xrightarrow {}}\ K_{2}[Cu(C_{2}O_{4})_{2}]\cdot 2H_{2}O}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/f0b02cf2d9c1eaa651423be5849f913d57b428f4)
-oxalat.jpg){kind=link}
Uses
Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylated polyformaldehyde[6] and in seed treatment (to repel birds and rodents).[citation needed]
See also
References
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
- ^ "Copper oxalate - Substance Information - ECHA". European Chemical Agency. Retrieved 17 June 2021.
- ^ Royappa, A. Timothy; Royappa, Andrew D.; Moral, Raphael F.; Rheingold, Arnold L.; Papoular, Robert J.; Blum, Deke M.; Duong, Tien Q.; Stepherson, Jacob R.; Vu, Oliver D.; Chen, Banghao; Suchomel, Matthew R.; Golen, James A.; André, Gilles; Kourkoumelis, Nikolaos; Mercer, Andrew D.; Pekarek, Allegra M.; Kelly, Dylan C. (November 2016). "Copper(I) oxalate complexes: Synthesis, structures and surprises". Polyhedron. 119: 563–574. doi:10.1016/j.poly.2016.09.043.
- ^ "Hazardous Substances Data Bank (HSDB) : 265". National Library of Medicine. Retrieved 17 June 2021.
- ^ Gooch, Frank Austin (1909). The precipitation of copper oxalate in analysis. p. 448. OCLC 890741677.
- ^ Richardson, H. Wayne (1997). Handbook of Copper Compounds and Applications. CRC Press. p. 84. ISBN 978-0-8247-8998-5.