Copper(II) sulfate 477292 223114253 2008-07-02T17:09:59Z Rifleman 82 1255637 /* Chemical properties */ add line break {{Chembox new | Name = Copper(II) sulfate | ImageFile = CuSO4.5H2O.jpg | ImageSize = 150px | ImageName = Crystal of copper(II)sulfate<sub>4</sub>&nbsp;·&nbsp;5H<sub>2</sub>O | ImageFile1 = Copper(II)-sulfate-pentahydrate-sample.jpg | ImageSize1 = 150px | ImageName1 = Photo of powdered copper(II) sulfate pentahydrate | ImageFile2 = Copper(II)-sulfate-unit-cell-3D-balls.png | ImageSize2 = 150px | ImageName2 = Ball-and-stick model of the unit cell of anhydrous copper(II) sulfate | ImageFile3 = Copper(II)-sulfate-3D-vdW.png | ImageSize3 = 120px | ImageName3 = Space-filling model of part of the crystal structure of anhydrous copper(II) sulfate | IUPACName = Copper(II) sulfate<br />pentahydrate | OtherNames = Copper(II) sulfate<br />Copper(II)sulfate<br />Cupric sulfate<br />Blue vitriol<br />Bluestone<br />[[Chalcanthite]] | Section1 = {{Chembox Identifiers | CASNo = 7758-98-7 | EINECS = 231-847-6 | RTECS = GL8800000 }} | Section2 = {{Chembox Properties | Formula = CuSO<sub>4</sub>·5H<sub>2</sub>O (pentahydrate)<br /> CuSO<sub>4</sub> (anhydrous) | MolarMass = 249.684 g/mol (pentahydrate)<br /> 159.608 g/mol (anhydrous) | Appearance = blue crystalline solid (pentahydrate)<br /> gray-white powder (anhydrous) | Solubility = 31.6 g/100 ml (0 °C) | MeltingPt = 110 °C (− 4H<sub>2</sub>O)<br />150 °C (423 K) (− 5H<sub>2</sub>O)<br />650 °C ''decomp.'' }} | Section3 = {{Chembox Structure | Coordination = Octahedral | CrystalStruct = [[Triclinic]] }} | Section4 = {{Chembox Thermochemistry | DeltaHf = -769.98 kJ/mol }} | Section4 = {{Chembox Thermochemistry | Entropy = 109.05 J.K<sup>−1</sup>.mol<sup>−1</sup> }} | Section7 = {{Chembox Hazards | EUClass = Harmful ('''Xn''') <br />Dangerous for the environment ('''N''') | NFPA-H = 2 | NFPA-F = | NFPA-R = | FlashPt = non flammable }} | Section8 = {{Chembox Related | OtherCations = [[Nickel(II) sulfate]]<br />[[Zinc sulfate]]}} }} '''Copper(II) sulfate''' is the [[chemical compound]] with the [[chemical formula|formula]] [[Copper|Cu]][[Sulfur|S]][[Oxygen|O]]<sub>4</sub>. This salt exists as a series of compounds that differ in their degree of [[water of crystallization|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".<ref>{{Cite web | publisher = [[Oxford University]] | title = Copper(II) sulfate MSDS | url = http://ptcl.chem.ox.ac.uk/MSDS/CO/copper_II_sulfate.html | accessdate = 2007-12-31}}</ref> ==Preparation== [[Image:Synthesizing Copper Sulfate.jpg|left|thumb|Preparation of copper(II) sulfate by electrolyzing sulfuric acid, using copper electrodes]] Since it is available commercially, a copper sulfate is usually purchased, not prepared in the laboratory. It can be made by the action of [[sulfuric acid]] on a variety of copper(II) compounds, for example [[copper(II) oxide]]. It may also be prepared by electrolyzing sulfuric acid, using copper electrodes. <br clear = left/> ==Chemical properties== Copper(II) sulfate pentahydrate [[chemical decomposition|decomposes]] before melting, losing four water molecules at 110 °C and all five at 150 °C. At 650 °C, copper(II) sulfate decomposes into copper(II) oxide (CuO) and [[sulfur trioxide]] (SO<sub>3</sub>). When heated in an open flame the crystals are dehydrated and turn grayish-white.<ref>Holleman, A. F.; Wiberg, E. ''Inorganic Chemistry'' Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> ==Uses== ===As an herbicide, fungicide, pesticide=== Copper sulfate pentahydrate is a [[fungicide]]. Mixed with [[lime (mineral)|lime]] it is called [[Bordeaux mixture]] to control fungus on grapes, melons, and other berries<ref>{{cite web | title = Uses of Copper Compounds: Copper Sulfate's Role in Agriculture | publisher = Copper.org | accessdate = 2007-12-31 | url = http://www.copper.org/applications/compounds/copper_sulfate02.html}}</ref>. Another application is [[Cheshunt compound]], a mixture of copper sulfate 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,<ref>{{cite web | title = All About Copper Sulfate | publisher = National Fish Pharmaceuticals | url = http://www.fishyfarmacy.com/Q&A/all_about_copper.html | accessdate = 2007-12-31}}</ref> 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 sugar]]s, 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]]. The blood is tested by dropping it into a solution of copper sulfate of known [[specific gravity]] &mdash; blood which contains sufficient [[hemoglobin]] sinks rapidly due to its density, whereas blood which does not, floats or sinks slowly.<ref>{{cite book | title = Basic Medical Laboratory Techniques | author = Barbara H. Estridge, Anna P. Reynolds, Norma J. Walters | pages = 166 | publisher = Thomson Delmar Learning | year = 2000 | isbn = 0766812065}}</ref> In a [[flame test]], its copper [[ion]]s emit a deep blue-green light, much more blue than the flame test for [[barium]]. ===Organic synthesis=== Copper sulfate is employed in [[organic synthesis]].<ref>Hoffman, R. V. "Copper(II) Sulfate" ''Encyclopedia of Reagents for Organic Synthesis'', 2001 John Wiley & Sons. DOI: 10.1002/047084289X.rc247</ref> The anhydrous salt catalyses the trans[[acetal]]ization in organic synthesis.<ref>{{OrgSynth | author = Hulce, M. Mallomo, J. P.; Frye, L. L.; Kogan, T. P.; Posner, G. H. | prep = CV7P0495 | title = (S)-( + )-2-(p-Toluenesulfinyl)-2-Cyclopentanone: Precursor for Enantioselective Synthesis of 3-Substituted Cyclopentanones | collvol = 7 | collvolpages = 495 | year = 1990}}</ref> The hydrated salt reacts with [[potassium permanganate]] to give an oxidant for the conversion of primary alcohols.<ref>{{OrgSynth | author = Jefford, C. W.; Li, Y.; Wang, Y. | prep = cv9p0462 | title = A Selective, Heterogeneous Oxidation using a Mixture of Potassium Permanganate and Cupric Sulfate: (3aS,7aR)-Hexahydro-(3S,6R)-Dimethyl-2(3H)-Benzofuranone | collvol = 9 | collvolpages = 462}}</ref> ===Chemistry education=== Copper sulfate is a commonly included chemical in children's [[chemistry set]]s and is often used to grow crystals in [[school]]s and in [[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 CuSO<sub>4</sub>. 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 color, and is known as blue copperas.<ref>http://66.102.9.104/search?q=cache:Jj02FqBkPCAJ:www.freepatentsonline.com/4315915.html+Blue+copperas&hl=en&ct=clnk&cd=3&gl=uk</ref> 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. :Fe + CuSO<sub>4</sub> → FeSO<sub>4</sub> + Cu The copper can also be electroplated to the iron. ===Other uses=== Other applications include hair [[dye]]s, coloring glass, processing of [[leather]] and [[textiles]] and in pyrotechnics as a green colorant.<ref>{{cite web | title = Uses of Copper Compounds: Table A - Uses of Copper Sulfate | publisher = Copper.org | accessdate = 2007-12-31 | url = http://www.copper.org/applications/compounds/table_a.html}}</ref> ==References== {{reflist|2}} ==External links== <!-- Image with unknown copyright status removed:[[Image:Cu_3.jpg|thumb|left|Flame test for copper ions]] --> *{{ICSC|0751|07}} (anhydrous) *{{ICSC|1416|14}} (pentahydrate) *[http://www.npi.gov.au/database/substance-info/profiles/27.html National Pollutant Inventory - Copper and compounds fact sheet] * [http://www.uncp.edu/home/mcclurem/ptable/copper/cu.htm UNCP Copper] {{Antidotes}} [[Category:Copper compounds]] [[Category:Sulfates]] [[Category:Desiccants]] [[Category:Herbicides]] [[ar:كبريتات نحاس ثنائي]] [[cs:Síran měďnatý]] [[da:Kobber(II)sulfat]] [[de:Kupfersulfat]] [[es:Sulfato de cobre (II)]] [[fr:Sulfate de cuivre]] [[hr:Modra galica]] [[it:Solfato rameico]] [[he:נחושת גופרתית]] [[lv:Vara sulfāts]] [[hu:Réz-szulfát]] [[ms:Kuprum(II) sulfat]] [[nl:Koper(II)sulfaat]] [[ja:硫酸銅(II)]] [[nds:Koppersulfat]] [[pl:Siarczan miedzi]] [[pt:Sulfato de cobre (II)]] [[ru:Сульфат меди]] [[sk:Síran meďnatý]] [[sl:Bakrov(II) sulfat]] [[fi:Kuparisulfaatti]] [[sv:Kopparsulfat]] [[uk:Сульфат міді]] [[zh:硫酸铜]]