Copper(II) oxalate
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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 | |
ECHA InfoCard | 100.011.283 |
EC Number |
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PubChemCID
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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)
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4.43×10−10[1] |
Hazards | |
GHSlabelling: | |
[2] | |
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 |
Except where otherwise noted, data are given for materials in theirstandard state(at 25 °C [77 °F], 100 kPa).
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Copper(II) oxalateareinorganic compoundswith the chemical formulaCuC2O4(H2O)x.The value of x can be 0, 0.44, and 1. Two of these species are found as secondary minerals (degradation of minerals),whewellite(monohydrate andmoolooite(0.44 hydrate).[3]The anhydrous compound has been characterized byX-ray crystallography.[4]Manytransition metal oxalate complexesare known.
Copper(II) monooxalates are practically insoluble in all solvents. They arecoordination polymers.[5]
Synthesis
[edit]Copper(II) oxalate can be produced by precipitation from acidified aqueous copper(II) salts andoxalic acid.[6][7]
- CuSO4+ H2C2O4+ H2O → CuC2O4·H2O + H2SO4
Reactions
[edit]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.[6]
The hydrates bindLewis bases.
Hydrated copper(II) oxalate reacts with alkali metal oxalates andammonium oxalateto give bis(oxalato)cuprate:[8]
- CuC2O4)(H2O)x+ C2O2−4→ [Cu(C2O4)2]2−+ x H2O
Uses
[edit]Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylatedpolyformaldehyde.[9][10]
Related compounds
[edit]- Cuprous oxalates.[11]
References
[edit]- ^John Rumble (June 18, 2018).CRC Handbook of Chemistry and Physics(99 ed.). CRC Press. pp. 5–188.ISBN978-1138561632.
- ^"Copper oxalate - Substance Information - ECHA".European Chemical Agency.Retrieved17 June2021.
- ^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.
- ^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.Retrieved17 June2021.
- ^abO. 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.OCLC890741677.
- ^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.ISBN978-0-470-13165-7.
- ^Richardson, H. Wayne (1997).Handbook of Copper Compounds and Applications.CRC Press. p. 84.ISBN978-0-8247-8998-5.
- ^Richardson, H. Wayne (2000). "Copper Compounds".Ullmann's Encyclopedia of Industrial Chemistry.doi:10.1002/14356007.a07_567.ISBN978-3-527-30385-4.
- ^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.