Difference between revisions of "Copper citrate"
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==Preparation== | ==Preparation== | ||
Copper citrate can be made by reacting copper oxide or hydroxide with citric acid. | Copper citrate can be made by reacting copper oxide or hydroxide with citric acid. | ||
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| + | Copper citrate has a low solubility in water, and can be prepared by precipitation from aqueous solution containing copper and citrate ions. A procedure is available from the Royal Society for Chemistry<ref> | ||
| + | Preparation of copper(II) citrate. RSC Student worksheet, http://www.rsc.org/learn-chemistry/resource/download/res00000903/cmp00001141/pdf</ref> describing its preparation from trisodium citrate and copper acetate or sulfate. However, when followed, the reaction proceeds only very slowly, and deposits the product as a crust. Heating the mixture will accelerate the reaction and give a finely-divided product. | ||
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| + | Magnesium citrate, available in solution as a laxative, can also be used in place of trisodium citrate. | ||
==Projects== | ==Projects== | ||
Revision as of 17:14, 28 March 2016
| Properties | |
|---|---|
| Molar mass | Cu3C12H10O14 |
| Soluble | |
| Related compounds | |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(II) citrate, also known as cuprocitrol, is an ionic compound of copper and citric acid with the formula Cu3(C6H5O7)2 or Cu3C12H10O14, with a molecular weight of 568.85 g/mol. Some resources incorrectly list its formula as Cu2C6H4O7 and a molecular weight of 360.2 g/mol, but this formulation would require the citric acid molecule to lose more protons than it has carboxylic groups. It exists as a seafoam green hemipentahydrate and a sky-blue anhydrous solid.
Contents
Properties
Chemical
Physical
Availability
Delete this section if not applicable
Preparation
Copper citrate can be made by reacting copper oxide or hydroxide with citric acid.
Copper citrate has a low solubility in water, and can be prepared by precipitation from aqueous solution containing copper and citrate ions. A procedure is available from the Royal Society for Chemistry[1] describing its preparation from trisodium citrate and copper acetate or sulfate. However, when followed, the reaction proceeds only very slowly, and deposits the product as a crust. Heating the mixture will accelerate the reaction and give a finely-divided product.
Magnesium citrate, available in solution as a laxative, can also be used in place of trisodium citrate.
Projects
Handling
Safety
Storage
In closed bottles, or sealed if you want the anhydrous form.
Disposal
Copper citrate should be disposed of just any other copper compound.
References
- ↑ Preparation of copper(II) citrate. RSC Student worksheet, http://www.rsc.org/learn-chemistry/resource/download/res00000903/cmp00001141/pdf
