Copper(II) oxalate
_Oxalate_Structural_Formula_V1.svg.png) | |
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| Names | |
|---|---|
| Other names
Copper (II) oxalate, cupric oxalate, copper(2+) ethanedioate
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| Identifiers | |
CAS Number
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.011.283 |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 3077 |
CompTox Dashboard (EPA)
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InChI
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SMILES
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| Properties | |
Chemical formula
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CuC 2O 4 |
| Molar mass | 151.56 |
| Appearance | blue solid |
| Density | 6.57 g/cm3 |
Solubility in water
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insoluble |
Solubility product (Ksp)
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4.43×10−10[1] |
| Hazards | |
| GHS labelling: | |
Pictograms
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 [2]
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Signal word
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Warning |
Hazard statements
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H302, H302+H312, H312 |
Precautionary statements
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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
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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).
Infobox references
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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]
Synthesis
Copper(II) oxalate can be produced by precipitation from acidified aqueous copper(II) salts and oxalic acid or an alkali metal oxalate.[7][8]
- CuSO4 + H2C2O4 + H2O → CuC2O4·H2O + H2SO4
Reactions
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]
- (CuC2O4)(H2O)x + C2O2−4 → [Cu(C2O4)2]2− + x H2O
Uses
Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylated polyformaldehyde.[10][11]
Related compounds
- Cuprous oxalates.[12]
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.
- ^ Lamprecht, Emmanuel; Watkins, Gareth M.; Brown, Michael E. (July 2006). "The thermal decomposition of copper(II) oxalate revisited". Thermochimica Acta. 446 (1–2): 91–100. Bibcode:2006TcAc..446...91L. doi:10.1016/j.tca.2006.03.008.
- ^ Christensen, Axel Nørlund; Lebech, Bente; Andersen, Niels Hessel; Grivel, Jean-Claude (2014). "The Crystal structure of paramagnetic copper(<SCP>ii</SCP>) oxalate (CuC2O4): Formation and thermal decomposition of randomly stacked anisotropic nano-sized crystallites" (PDF). Dalton Trans. 43 (44): 16754–16768. doi:10.1039/C4DT01689K. PMID 25278188.
- ^ Schmittler, H. (1968). "Zum Strukturprinzip des fehlgeordneten Kupfer(II)-Oxalats CuC2O4·nH2O". Monatsberichte der Deutschen Akademie der Wissenschaften zu Berlin. 10: 581–604.
- ^ "Hazardous Substances Data Bank (HSDB) : 265". National Library of Medicine. Retrieved 17 June 2021.
- ^ a b O. Glemser; R. Sauer (1963). "Copper(II) Sulfide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1017-1018. NY, NY: Academic Press.
- ^ Gooch, Frank Austin (1909). The precipitation of copper oxalate in analysis. p. 448. OCLC 890741677.
- ^ Kirschner, Stanley; McLean, John A.; Meerman, Gerardine (1960). "Potassium Dioxalatocuprate(II) 2-Hydrate". Inorganic Syntheses. Vol. 6. pp. 1–2. doi:10.1002/9780470132371.ch1. ISBN 978-0-470-13165-7.
{{cite book}}: ISBN / Date incompatibility (help) - ^ Richardson, H. Wayne (1997). Handbook of Copper Compounds and Applications. CRC Press. p. 84. ISBN 978-0-8247-8998-5.
- ^ Richardson, H. Wayne (2000). "Copper Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a07_567. ISBN 978-3-527-30385-4.
- ^ 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.