Difference between revisions of "Copper(II) perchlorate"
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If perchloric acid is not available but other perchlorate salts are, addition of aq. copper(II) sulfate to aq. [[barium perchlorate]] can work: | If perchloric acid is not available but other perchlorate salts are, addition of aq. copper(II) sulfate to aq. [[barium perchlorate]] can work: | ||
| − | : | + | : CuSO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → Cu(ClO<sub>4</sub>)<sub>2</sub> + BaSO<sub>4</sub> |
According to one source in literature, anhydrous copper(II) perchlorate can be prepared by [[silver perchlorate]] in [[diethyl ether]], followed by addition of copper(II)bromide. Silver bromide precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.<ref>Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)</ref> A different source indicates that [[copper(II) chloride]] can also be used, but no product is given.<ref>Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324</ref> | According to one source in literature, anhydrous copper(II) perchlorate can be prepared by [[silver perchlorate]] in [[diethyl ether]], followed by addition of copper(II)bromide. Silver bromide precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.<ref>Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)</ref> A different source indicates that [[copper(II) chloride]] can also be used, but no product is given.<ref>Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324</ref> | ||
Revision as of 18:35, 9 September 2023
| Names | |
|---|---|
| IUPAC name
Copper(II) perchlorate
| |
| Other names
Copper diperchlorate
Cupric perchlorate | |
| Properties | |
| Cu(ClO4)2 (anhydrous) Cu(ClO4)2·6 H2O (hexahydrate) | |
| Molar mass | 262.447 g/mol (anhydrous) 370.539 g/mol (hexahydrate) |
| Appearance | Blue crystalline solid |
| Odor | Odorless |
| Density | 2.225 g/cm3 (25 °C) |
| Melting point | 82 °C (180 °F; 355 K) |
| Boiling point | 100–102 °C (212–216 °F; 373–375 K) (decomposes) |
| 146 g/100 ml (30 °C) | |
| Solubility | Soluble in acetic acid, acetone, diethyl ether, ethanol, methanol |
| Solubility in furfural | 69 g/100 ml (20 °C)[1] |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
-1,915 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (hexahydrate) |
| Related compounds | |
| Related compounds
|
Silver perchlorate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(II) perchlorate is an inorganic chemical compound, a salt of copper and perchloric acid. It has the formula Cu(ClO4)2, though it is more commonly encountered as hexahydrate, Cu(ClO4)2·6 H2O.
Contents
Properties
Chemical
Copper(II) perchlorate decomposes when heated.
Physical
Copper(II) perchlorate is a hygroscopic blueish solid, soluble in water.
Availability
Copper(II) perchlorate is sold by chemical suppliers.
Preparation
Copper(II) perchlorate can be prepared by dissolving copper(II) oxide with perchloric acid.[2]
- CuO + 2 HClO4 → Cu(ClO4)2 + H2O
Copper metal must not be used as the reaction is claimed to be dangerous.
If perchloric acid is not available but other perchlorate salts are, addition of aq. copper(II) sulfate to aq. barium perchlorate can work:
- CuSO4 + Ba(ClO4)2 → Cu(ClO4)2 + BaSO4
According to one source in literature, anhydrous copper(II) perchlorate can be prepared by silver perchlorate in diethyl ether, followed by addition of copper(II)bromide. Silver bromide precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.[3] A different source indicates that copper(II) chloride can also be used, but no product is given.[4]
Projects
Handling
Safety
Copper(II) perchlorate is a powerful oxidizer. Perchlorates are toxic.
Storage
Should be kept in a clean bottle, away from any reducing agents or combustible materials.
Disposal
Copper(II) perchlorate should be reduced to chloride and the copper recycled.
References
- ↑ Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961 (Solubility Handbook. - T.1, Book.1. - M.-L.: IAN USSR, 1961)
- ↑ Nagy, L.; Zsikla, L.; Burger, K.; Rockenbauer, A.; Kiss, J. T.; Journal of Crystallographic and Spectroscopic Research; vol. 19; nb. 5; (1989); p. 911 - 918
- ↑ Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)
- ↑ Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324
