Copper(II) sulfate: Difference between revisions
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| Name = Copper(II) |
| Name = Copper(II) sulphate |
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| ImageFile = CuSO4.5H2O.jpg |
| ImageFile = CuSO4.5H2O.jpg |
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| ImageSize = 150px |
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| ImageFile1 = Copper(II)-sulfate-pentahydrate-sample.jpg |
| ImageFile1 = Copper(II)-sulfate-pentahydrate-sample.jpg |
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| ImageName1 = Photo of powdered copper(II) |
| ImageName1 = Photo of powdered copper(II) sulphate pentahydrate |
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| ImageFile2 = Copper(II)- |
| ImageFile2 = Copper(II)-sulphate-unit-cell-3D-balls.png |
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| ImageName2 = Ball-and-stick model of the unit cell of anhydrous copper(II) |
| ImageName2 = Ball-and-stick model of the unit cell of anhydrous copper(II) sulphate |
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| ImageFile3 = Copper(II)-sulfate-3D-vdW.png |
| ImageFile3 = Copper(II)-sulfate-3D-vdW.png |
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| ImageSize3 = 120px |
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| ImageName3 = Space-filling model of part of the crystal structure of anhydrous copper(II) |
| ImageName3 = Space-filling model of part of the crystal structure of anhydrous copper(II) sulphate |
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| IUPACName = Copper(II) |
| IUPACName = Copper(II) sulphate<br />pentahydrate |
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| OtherNames = Copper(II) |
| OtherNames = Copper(II) sulphate<br />Copper(II)sulphate<br />Cupric sulphate<br />Blue vitriol<br />Bluestone<br />[[Chalcanthite]] |
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| Name = Properties |
| Name = Properties |
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| Name = Safety data |
| Name = Safety data |
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Revision as of 02:51, 22 October 2007
Template:Chembox new Copper(II) sulfate ("sulphate" in most Commonwealth nations) is the chemical compound with the formula CuSO4. This salt exists as a series of compounds that differ in their degree of hydration. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. This hydrated copper sulfate occurs in nature as the mineral called chalcanthite. Archaic names for copper(II) sulfate are "blue vitriol" and "bluestone"[1]
Structure
In the pentahydrate, copper(II) is bonded to four molecules of water and to the oxygen atoms of two sulfate anions. The fifth water is not coordinated, but links the sulfate anions via hydrogen bonding. In the trihydrate, all three water molecules are bonded as well as one oxygen atom of the sulfate, to define a distorted square planar arrangement, two more oxygen ligands are ca. 2.4 Å distant from copper. In the anhydrous form, copper is bound to four oxygen atoms of sulfate (rCu-O = 1.9-2.0Å) and more weakly bonded to two other oxygen atoms (2.4 Å).[2] A monohydrate is also known. hi
=
Uses
In organic synthesis
Copper sulfate is employed in organic synthesis.[3] The anhydrous salt catalyses the transacetalization in organic synthesis.[4] The hydrated salt reacts with potassium permanganate to give an oxidant for the conversion of primary alcohols.[5]
In school chemistry demonstrations
Copper sulfate is a commonly included chemical in children's chemistry sets and is often used in high school crystal growing.[6] and copper plating experiments. Due to its toxicity, it is not recommended for small children. Copper sulfate is often used to demonstrate an exothermic reaction, in which steel wool or magnesium ribbon is placed in an aqueous solution of CuSO4. It is used in school chemistry courses to demonstrate the principle of mineral hydration. The pentahydrate form, which is blue, is heated, turning the copper sulfate into the anhydrous form which is white, while the water that was present in the pentahydrate form evaporates. When water is then added to the anhydrous compound, it turns back into the pentahydrate form, regaining its blue colour.
In an illustration of a "single metal replacement reaction," iron is submerged in a solution of copper sulfate. Upon standing, iron dissolves and copper precipitates.
As an herbicide, fungicide, pesticide
Copper sulfate pentahydrate is a fungicide. Mixed with lime it is called Bordeaux mixture to control fungus on grapes and other berries[7], another application is Cheshunt compound, a mixture of copper sulphate and ammonium carbonate used in horticulture to prevent damping off in seedlings. Its use as an herbicide is not agricultural, but instead for control of invasive exotic aquatic plants and the roots of other invasive plants near various pipes that contain water. A dilute solution of copper sulfate is used to treat aquarium fish of various parasitic infections[8], and is also used to remove snails from aquariums. However, as the copper ions are also highly toxic to the fish, care must be taken with the dosage. Most species of algae can be controlled with very low concentrations of copper sulfate. Copper sulfate inhibits growth of bacteria such as E. coli.
Analytical reagent
Several chemical tests utilize copper sulfate. It is used in Fehling's solution and Benedict's solution to test for reducing sugars, which reduce the soluble blue copper(II) sulfate to insoluble red copper(I) oxide. Copper(II) sulfate is also used in the Biuret reagent to test for proteins.
Copper sulfate is also used to test blood for anemia[9]. A drop of the patient's blood is dropped into an aqueous solution of copper sulfate solution: if it sinks within a certain time, then the patient has sufficient hemoglobin levels and is not anemic. If the blood drop floats or sinks slowly, then the patient is iron-deficient and may be anemic.
In a flame test, its copper ions emit a deep blue-green light, much more blue than the flame test for barium.
Other uses
Other applications include hair dyes, coloring glass, processing of leather and textiles, and in pyrotechnics as a green colorant.[10] A full list of uses can be seen here.
Safety
Copper salts are toxic in large amounts.[11]
References
- ^ http://ptcl.chem.ox.ac.uk/MSDS/CO/copper_II_sulfate.html
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ Hoffman, R. V. "Copper(II) Sulfate" Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley & Sons. DOI: 10.1002/047084289X.rc247
- ^ Hulce, M. Mallomo, J. P.; Frye, L. L.; Kogan, T. P.; Posner, G. H. “(S)-( + )-2-(p-Toluenesulfinyl)-2-Cyclopentanone: Precursor for Enantioselective Synthesis of 3-Substituted Cyclopentanones” Organic Syntheses, Collected Volume 7, p.495 (1990).
- ^ Jefford, C. W.; Li, Y.; Wang, Y. “A Selective, Heterogeneous Oxidation using a Mixture of Potassium Permanganate and Cupric Sulfate: (3aS,7aR)-Hexahydro-(3S,6R)-Dimethyl-2(3H)-Benzofuranone” Collective Volume 9, page 462.
- ^ http://www.newton.dep.anl.gov/askasci/chem03/chem03203.htm
- ^ http://www.copper.org/applications/compounds/copper_sulfate02.html
- ^ http://www.fishdoc.co.uk/treatments/copper.htm
- ^ http://cat.inist.fr/?aModele=afficheN&cpsidt=2686293
- ^ http://www.copper.org/applications/compounds/table_a.html
- ^ http://ptcl.chem.ox.ac.uk/MSDS/CO/copper_II_sulfate.html