Copper(II) sulfate
Crystals of CuSO4·5H2O
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Names | |
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IUPAC name
Copper(II) sulfate
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Other names
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Identifiers | |
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3D model (
JSmol ) |
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ChEBI | |
ChEMBL | |
ChemSpider | |
ECHA InfoCard
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100.028.952 |
EC Number |
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8294 | |
KEGG | |
PubChem CID
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RTECS number
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UNII |
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CompTox Dashboard (EPA)
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Properties | |
CuSO4 (anhydrous) CuSO4·5H2O (pentahydrate) | |
Molar mass | 159.60 g/mol (anhydrous)[2] 249.685 g/mol (pentahydrate)[2] |
Appearance | gray-white (anhydrous) blue (pentahydrate) |
Density | 3.60 g/cm3 (anhydrous)[2] 2.286 g/cm3 (pentahydrate)[2] |
Melting point | 110 °C (230 °F; 383 K) decomposes
560 °C decomposes[2](pentahydrate) Fully decomposes at 590 °C (anhydrous) |
Boiling point | decomposes to cupric oxide at 650 °C
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pentahydrate 316 g/L (0 °C) 2033 g/L (100 °C) anhydrous 168 g/L (10 °C) 201 g/L (20 °C) 404 g/L (60 °C) 770 g/L (100 °C)[3] | |
Solubility | anhydrous insoluble in ethanol[2] pentahydrate soluble in methanol[2] 10.4 g/L (18 °C) insoluble in ethanol and acetone |
1330·10−6 cm3/mol | |
Refractive index (nD)
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1.724–1.739 (anhydrous)[4] 1.514–1.544 (pentahydrate)[5] |
Structure | |
Triclinic (pentahydrate), space group P1, aP22, a = 0.5986 nm, b = 0.6141 nm, c = 1.0736 nm, α = 77.333°, β = 82.267°, γ = 72.567°[7]
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Thermochemistry | |
Std molar
entropy (S⦵298) |
5 J/(K·mol) |
Std enthalpy of (ΔfH⦵298)formation |
−769.98 kJ/mol |
Pharmacology | |
V03AB20 (WHO) | |
Hazards | |
GHS labelling: | |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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300 mg/kg (oral, rat)[9]
87 mg/kg (oral, mouse) |
NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3 (as Cu)[8] |
REL (Recommended)
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TWA 1 mg/m3 (as Cu)[8] |
IDLH (Immediate danger) |
TWA 100 mg/m3 (as Cu)[8] |
Safety data sheet (SDS) | anhydrous pentahydrate |
Related compounds | |
Other cations
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Copper(II) sulfate, also known as copper sulphate, is an inorganic compound with the chemical formula CuSO4. It forms hydrates CuSO4·nH2O, where n can range from 1 to 7. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate,[10] while its anhydrous form is white.[11] Older names for the pentahydrate include blue vitriol, bluestone,[12] vitriol of copper,[13] and Roman vitriol.[14] It exothermically dissolves in water to give the aquo complex [Cu(H2O)6]2+, which has octahedral molecular geometry. The structure of the solid pentahydrate reveals a polymeric structure wherein copper is again octahedral but bound to four water ligands. The Cu(II)(H2O)4 centers are interconnected by sulfate anions to form chains.[15]
Preparation and occurrence
Copper sulfate is produced industrially by treating copper metal with hot concentrated
Commercial copper sulfate is usually about 98% pure copper sulfate, and may contain traces of water. Anhydrous copper sulfate is 39.81% copper and 60.19% sulfate by mass, and in its blue, hydrous form, it is 25.47% copper, 38.47% sulfate (12.82% sulfur) and 36.06% water by mass. Four types of
Chemical properties
Copper(II) sulfate pentahydrate decomposes before melting. It loses two water molecules upon heating at 63 °C (145 °F), followed by two more at 109 °C (228 °F) and the final water molecule at 200 °C (392 °F).[17][18]
The chemistry of aqueous copper sulfate is simply that of copper
- Cu2+ + 4 Cl− → [CuCl4]2−
Similarly treatment of such solutions with zinc gives metallic copper, as described by this simplified equation:[19]
- CuSO4 + Zn → Cu + ZnSO4
A further illustration of such single metal replacement reactions occurs when a piece of iron is submerged in a solution of copper sulfate:
- Fe + CuSO4 → FeSO4 + Cu
In high school and general chemistry education, copper sulfate is used as an electrolyte for galvanic cells, usually as a cathode solution. For example, in a zinc/copper cell, copper ion in copper sulfate solution absorbs electron from zinc and forms metallic copper.[20]
- Cu2+ + 2e− → Cu (cathode), E°cell = 0.34 V
Copper sulfate is commonly included in teenager
Uses
As a fungicide and herbicide
Copper sulfate has been used for control of algae in lakes and related fresh waters subject to eutrophication. It "remains the most effective algicidal treatment".[23][24]
A dilute solution of copper sulfate is used to treat aquarium fishes for parasitic infections,[26] and is also used to remove snails from aquariums and zebra mussels from water pipes.[27] Copper ions are highly toxic to fish. Most species of algae can be controlled with very low concentrations of copper sulfate.
Analytical reagent
Several chemical tests utilize copper sulfate. It is used in
Copper sulfate is used to test blood for
In a flame test, the copper ions of copper sulfate emit a deep green light, a much deeper green than the flame test for barium.
Organic synthesis
Copper sulfate is employed at a limited level in organic synthesis.[29] The anhydrous salt is used as a dehydrating agent for forming and manipulating acetal groups.[30] The hydrated salt can be intimately mingled with potassium permanganate to give an oxidant for the conversion of primary alcohols.[31]
Rayon production
Reaction with
Niche uses
Copper(II) sulfate has attracted many niche applications over the centuries. In industry copper sulfate has multiple applications. In printing it is an additive to book-binding pastes and glues to protect paper from insect bites; in building it is used as an additive to concrete to improve water resistance and discourage anything from growing on it. Copper sulfate can be used as a coloring ingredient in artworks, especially glasses and potteries.[32] Copper sulfate is also used in firework manufacture as a blue coloring agent, but it is not safe to mix copper sulfate with chlorates when mixing firework powders.[33]
Copper sulfate was once used to kill
Art
In 2008, the artist
Etching
Copper(II) sulfate is used to etch zinc, aluminium, or copper plates for intaglio printmaking.[37][38] It is also used to etch designs into copper for jewelry, such as for Champlevé.[39]
Dyeing
Copper(II) sulfate can be used as a mordant in vegetable dyeing. It often highlights the green tints of the specific dyes.[citation needed]
Electronics
An aqueous solution of copper(II) sulfate is often used as the resistive element in liquid resistors.[citation needed]
In electronic and microelectronic industry a bath of CuSO4·5H2O and sulfuric acid (H2SO4) is often used for electrodeposition of copper.[40]
Other forms of copper sulfate
Anhydrous copper(II) sulfate can be produced by dehydration of the commonly available pentahydrate copper sulfate. In nature, it is found as the very rare mineral known as chalcocyanite.[41] The pentahydrate also occurs in nature as chalcanthite. Other rare copper sulfate minerals include bonattite (trihydrate),[42] boothite (heptahydrate),[43] and the monohydrate compound poitevinite.[44][45] There are numerous other, more complex, copper(II) sulfate minerals known, with environmentally important basic copper(II) sulfates like langite and posnjakite.[45][46][47]
Toxicological effects
Copper(II) salts have an
It is harmless enough to be a routine component of high school experiments and to be used widely in swimming lakes to control algae.Copper(II) sulfate was used in the past as an
See also
References
- .
- ^ a b c d e f g Haynes, p. 4.62
- ISBN 9781138561632.
- ISBN 978-0962209741.
- ^ Haynes, p. 10.240
- .
- .
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ Cupric sulfate. US National Institutes of Health
- ^ Connor, Nick (2023-07-24). "Copper (II) Sulfate | Formula, Properties & Application". Material Properties. Retrieved 2024-02-03.
- ^ Foundation, In association with Nuffield. "A reversible reaction of hydrated copper(II) sulfate". RSC Education. Retrieved 2024-02-03.
- Oxford University. Archived from the originalon 2007-10-11. Retrieved 2007-12-31.
- ^ Antoine-François de Fourcroy, tr. by Robert Heron (1796) "Elements of Chemistry, and Natural History: To which is Prefixed the Philosophy of Chemistry". J. Murray and others, Edinburgh. Page 348.
- ^ Oxford University Press, "Roman vitriol", Oxford Living Dictionaries. Accessed on 2016-11-13
- PMID 20024268.
- ^ a b "Uses of Copper Compounds: Copper Sulphate". copper.org. Copper Development Association Inc. Retrieved 10 May 2015.
- ISBN 978-0-444-82437-0.
- ISBN 978-0-12-352651-9.
- .
- ISBN 978-1-285-13370-6.
- .
- ^ "Process for the preparation of stable copper(II) sulfate monohydrate applicable as trace element additive in animal fodders". Retrieved 2009-07-07.
- .
- .
- . Retrieved 2007-12-31.
- ^ "All About Copper Sulfate". National Fish Pharmaceuticals. Retrieved 2007-12-31.
- ^ "With Zebra mussels here to stay, Austin has a plan to avoid stinky drinking water". KXAN Austin. 2020-10-26. Retrieved 2020-10-28.
- ISBN 978-0-7668-1206-2.
- ISBN 978-0471936237.
- ISBN 978-1-58890-376-1.
- ^ 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". Organic Syntheses; Collected Volumes, vol. 9, p. 462.
- ^ a b Copper Development Association. "Uses of Copper Compounds: Table A - Uses of Copper Sulphate". copper. Copper Development Association Inc. Retrieved 12 May 2015.
- ^ Partin, Lee. "The Blues: Part 2". skylighter. Skylighter.Inc. Archived from the original on 21 December 2010. Retrieved 12 May 2015.
- ISBN 978-0970002778. Retrieved 12 May 2015.
- ^ "Seizure". Artangel.org.uk. Retrieved 2021-10-05.
- ^ "Roger Hiorns: Seizure". Yorkshire Sculpture Park. Archived from the original on 2015-02-22. Retrieved 2015-02-22.
- ^ greenart.info, Bordeau etch, 2009-01-18, retrieved 2011-06-02.
- ^ ndiprintmaking.ca, The Chemistry of using Copper Sulfate Mordant, 2009-04-12, retrieved 2011-06-02.
- ^ http://mordent.com/etch-howto/, How to Electrolytically etch in copper, brass, steel, nickel silver or silver, retrieved 2015-05-2015.
- )
- ^ "Chalcocyanite". www.mindat.org.
- ^ "Bonattite". www.mindat.org.
- ^ "Boothite". www.mindat.org.
- ^ "Poitevinite". www.mindat.org.
- ^ a b "List of Minerals". www.ima-mineralogy.org. March 21, 2011.
- ^ "Langite". www.mindat.org.
- ^ "Posnjakite". www.mindat.org.
- ^ Windholz, M., ed. 1983. The Merck Index. Tenth edition. Rahway, NJ: Merck and Company.
- ^ Guidance for reregistration of pesticide products containing copper sulfate. Fact sheet no. 100., Washington, DC: U.S. Environmental Protection Agency, Office of Pesticide Programs, 1986
- S2CID 32740524.
- ISBN 978-0-8385-8172-8.
- ^ V03AB20 (WHO)
Bibliography
- Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. ISBN 978-1439855119.
External links
- Media related to Copper(II) sulfate at Wikimedia Commons
- International Chemical Safety Card 0751
- International Chemical Safety Card 1416
- National Pollutant Inventory – Copper and compounds fact sheet