Copper(II) Sulfate - Wikipedia

Copper(II) sulfate

Crystals of CuSO4·5H2O
Copper, Cu  Sulfur, S  Oxygen, O  Hydrogen, HPortion of the structure of the pentahydrate(sulfate links Cu(H2O)2+4 centers)
Unit cell of the crystal structure of CuSO4·5H2Owith hydrogen bonds in black[1]
Names
IUPAC name Copper(II) sulfate
Other names Cupric sulphate Blue vitriol (pentahydrate) Bluestone (pentahydrate) Bonattite (trihydrate mineral) Boothite (heptahydrate mineral) Chalcanthite (pentahydrate mineral) Chalcocyanite (mineral) Copper Sulphate pentahydrate
Identifiers
CAS Number	7758-98-7 (anhydrous) Y 7758-99-8 (pentahydrate) Y 16448-28-5 (trihydrate) N 19086-18-1 (heptahydrate) N
3D model (JSmol)	Interactive image
ChEBI	CHEBI:23414 Y
ChEMBL	ChEMBL604 Y
ChemSpider	22870 Y
ECHA InfoCard	100.028.952
EC Number	231-847-6
Gmelin Reference	8294
KEGG	C18713 Y
PubChem CID	24462
RTECS number	GL8800000 (anhydrous)GL8900000 (pentahydrate)
UNII	KUW2Q3U1VV (anhydrous) Y LRX7AJ16DT (pentahydrate) Y
CompTox Dashboard (EPA)	DTXSID6034479
InChI InChI=1S/Cu.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 YKey: ARUVKPQLZAKDPS-UHFFFAOYSA-L Y InChI=1/Cu.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2Key: ARUVKPQLZAKDPS-NUQVWONBAI
SMILES [O-]S(=O)(=O)[O-].[Cu+2]
Properties
Chemical formula	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
Solubility in water	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	anhydrousinsoluble in ethanol[2] pentahydratesoluble in methanol[2]10.4 g/L (18 °C)insoluble in ethanol and acetone
Magnetic susceptibility (χ)	1330·10−6 cm3/mol
Refractive index (nD)	1.724–1.739 (anhydrous)[4]1.514–1.544 (pentahydrate)[5]
Structure
Crystal structure	Orthorhombic (anhydrous, chalcocyanite), space group Pnma, oP24, a = 0.839 nm, b = 0.669 nm, c = 0.483 nm.[6]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]
Thermochemistry
Std molarentropy (S⦵298)	5 J/(K·mol)
Std enthalpy offormation (ΔfH⦵298)	−769.98 kJ/mol
Pharmacology
ATC code	V03AB20 (WHO)
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H315, H318, H319, H410
Precautionary statements	P264, P264+P265, P270, P273, P280, P301+P317, P302+P352, P305+P351+P338, P305+P354+P338, P317, P321, P330, P332+P317, P337+P317, P362+P364, P391, P501
NFPA 704 (fire diamond)	2 0 1
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	300 mg/kg (oral, rat)[9] 87 mg/kg (oral, mouse)
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3 (as Cu)[8]
REL (Recommended)	TWA 1 mg/m3 (as Cu)[8]
IDLH (Immediate danger)	TWA 100 mg/m3 (as Cu)[8]
Safety data sheet (SDS)	anhydrouspentahydrate
Related compounds
Other cations	Iron(II) sulfate Manganese(II) sulfate Nickel(II) sulfate Zinc sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Chemical compound

Copper(II) sulfate 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

[edit]

Copper sulfate is produced industrially by treating copper metal with hot concentrated sulfuric acid or copper oxides with dilute sulfuric acid. For laboratory use, copper sulfate is usually purchased. Copper sulfate can also be produced by slowly leaching low-grade copper ore in air; bacteria may be used to hasten the process.[16]

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 crystal size are provided based on its usage: large crystals (10–40 mm), small crystals (2–10 mm), snow crystals (less than 2 mm), and windswept powder (less than 0.15 mm).[16]

Chemical properties

[edit]

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 aquo complex, since the sulfate is not bound to copper in such solutions. Thus, such solutions react with concentrated hydrochloric acid to give tetrachlorocuprate(II):

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 teenage chemistry sets and undergraduate experiments.[21] It is often used to grow crystals in schools and in Copper electroplating experiments despite its toxicity. 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 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.[citation needed] Copper(II) sulfate pentahydrate can easily be produced by crystallization from solution as copper(II) sulfate, which is hygroscopic.

Uses

[edit]

As a fungicide and herbicide

[edit]

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".[22][23]

Bordeaux mixture, a suspension of copper(II) sulfate (CuSO4) and calcium hydroxide (Ca(OH)2), is used to control fungus on grapes, melons, and other berries.[24] It is produced by mixing a water solution of copper sulfate and a suspension of slaked lime.

A dilute solution of copper sulfate is used to treat aquarium fishes for parasitic infections,[25] and is also used to remove snails from aquariums and zebra mussels from water pipes.[26] Copper ions are highly toxic to fish. Most species of algae can be controlled with very low concentrations of copper sulfate.

Analytical reagent

[edit]

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 used to test blood for anemia. The blood is dropped into a solution of copper sulfate of known specific gravity—blood with sufficient hemoglobin sinks rapidly due to its density, whereas blood which sinks slowly or not at all has an insufficient amount of hemoglobin.[27] Clinically relevant, however, modern laboratories utilize automated blood analyzers for accurate quantitative hemoglobin determinations, as opposed to older qualitative means.[citation needed]

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

[edit]

Copper sulfate is employed at a limited level in organic synthesis.[28] The anhydrous salt is used as a dehydrating agent for forming and manipulating acetal groups.[29] The hydrated salt can be intimately mingled with potassium permanganate to give an oxidant for the conversion of primary alcohols.[30]

Rayon production

[edit]

Reaction with ammonium hydroxide can yield tetraamminecopper(II) sulfate and Schweizer's reagent (nonsulphurous), which is used to dissolve cellulose in the industrial production of Rayon.

Niche uses

[edit]

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 prevent plant and mushroom growth. Copper sulfate can be used as a coloring ingredient in artworks, especially glasses and potteries.[31] Copper sulfate is also rarely used in firework manufacture as a blue coloring agent, but it is not safe to mix copper(II) sulfate with metal powders, or it or any copper(II) compound with chlorates; the sulfate and other copper(II) compounds are not allowed in chlorate containing mixtures in the US.[32][33]

Copper sulfate was once used to kill bromeliads, which serve as mosquito breeding sites.[34] Copper sulfate is used as a molluscicide to treat bilharzia in tropical countries.[31]

Art

[edit]

In 2008, the artist Roger Hiorns filled an abandoned waterproofed council flat in London with 75,000 liters of copper(II) sulfate water solution. The solution was left to crystallize for several weeks before the flat was drained, leaving crystal-covered walls, floors and ceilings. The work is titled Seizure.[35] Since 2011, it has been on exhibition at the Yorkshire Sculpture Park.[36]

Etching

[edit]

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

[edit]

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

[edit]

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

[edit]

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]

Forms of copper(II) sulfate

• Anhydrous CuSO4
• Copper(II) sulfate monohydrate
• Copper(II) sulfate pentahydrate
• The rare mineral boothite (CuSO4·7H2O)

Toxicological effects

[edit] See also: Copper toxicity

Copper(II) salts have an LD50 of 100 mg/kg.[48][49]

Copper(II) sulfate was used in the past as an emetic.[50] It is now considered too toxic for this use.[51] It is still listed as an antidote in the World Health Organization's Anatomical Therapeutic Chemical Classification System.[52]

See also

[edit]

• Chalcanthum
• Vitriol

References

[edit]

1. ^ Varghese, J. N.; Maslen, E. N. (1985). "Electron density in non-ideal metal complexes. I. Copper sulphate pentahydrate". Acta Crystallographica Section B. 41 (3): 184–190. doi:10.1107/S0108768185001914.
2. ^ a b c d e f g Haynes, p. 4.62
3. ^ Rumble, John, ed. (2018). CRC Handbook of Chemistry and Physics (99th ed.). CRC Press, Taylor & Francis Group. pp. 5–179. ISBN 9781138561632.
4. ^ Anthony, John W.; Bideaux, Richard A.; Bladh, Kenneth W.; Nichols, Monte C., eds. (2003). "Chalcocyanite" (PDF). Handbook of Mineralogy. Vol. V. Borates, Carbonates, Sulfates. Chantilly, VA, US: Mineralogical Society of America. ISBN 978-0962209741.
5. ^ Haynes, p. 10.240
6. ^ Kokkoros, P. A.; Rentzeperis, P. J. (1958). "The crystal structure of the anhydrous sulphates of copper and zinc". Acta Crystallographica. 11 (5): 361–364. doi:10.1107/S0365110X58000955.
7. ^ Bacon, G. E.; Titterton, D. H. (1975). "Neutron-diffraction studies of CuSO4 · 5H2O and CuSO4 · 5D2O". Z. Kristallogr. 141 (5–6): 330–341. Bibcode:1975ZK....141..330B. doi:10.1524/zkri.1975.141.5-6.330.
8. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
9. ^ Cupric sulfate. US National Institutes of Health
10. ^ Connor, Nick (2023-07-24). "Copper (II) Sulfate | Formula, Properties & Application". Material Properties. Retrieved 2024-02-03.
11. ^ Foundation, In association with Nuffield. "A reversible reaction of hydrated copper(II) sulfate". RSC Education. Retrieved 2024-02-03.
12. ^ "Copper (II) sulfate MSDS". Oxford University. Archived from the original on 2007-10-11. Retrieved 2007-12-31.
13. ^ 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.
14. ^ Oxford University Press, "Roman vitriol", Oxford Living Dictionaries. Accessed on 2016-11-13
15. ^ Ting, V. P.; Henry, P. F.; Schmidtmann, M.; Wilson, C. C.; Weller, M. T. (2009). "In situ neutron powder diffraction and structure determination in controlled humidities". Chem. Commun. 2009 (48): 7527–7529. doi:10.1039/B918702B. PMID 20024268.
16. ^ a b "Uses of Copper Compounds: Copper Sulphate". copper.org. Copper Development Association Inc. Retrieved 10 May 2015.
17. ^ Andrew Knox Galwey; Michael E. Green (1999). Thermal decomposition of ionic solids. Elsevier. pp. 228–229. ISBN 978-0-444-82437-0.
18. ^ Wiberg, Egon; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. p. 1263. ISBN 978-0-12-352651-9.
19. ^ Ray Q. Brewster, Theodore Groening (1934). "P-Nitrophenyl Ether". Organic Syntheses. 14: 66. doi:10.15227/orgsyn.014.0066.
20. ^ Zumdahl, Steven; DeCoste, Donald (2013). Chemical Principles. Cengage Learning. pp. 506–507. ISBN 978-1-285-13370-6.
21. ^ Rodríguez, Emilio; Vicente, Miguel Angel (2002). "A Copper-Sulfate-Based Inorganic Chemistry Laboratory for First-Year University Students That Teaches Basic Operations and Concepts". Journal of Chemical Education. 79 (4): 486. Bibcode:2002JChEd..79..486R. doi:10.1021/ed079p486.
22. ^ Van Hullebusch, E.; Chatenet, P.; Deluchat, V.; Chazal, P. M.; Froissard, D.; Lens, P. N.L.; Baudu, M. (2003). "Fate and forms of Cu in a reservoir ecosystem following copper sulfate treatment (Saint Germain les Belles, France)". Journal de Physique IV (Proceedings). 107: 1333–1336. doi:10.1051/jp4:20030547.
23. ^ Haughey, M. (2000). "Forms and fate of Cu in a source drinking water reservoir following CuSO4 treatment". Water Research. 34 (13): 3440–3452. doi:10.1016/S0043-1354(00)00054-3.
24. ^ Martin, Hubert (1933). "Uses of Copper Compounds: Copper Sulfate's Role in Agriculture". Annals of Applied Biology. 20 (2): 342–363. doi:10.1111/j.1744-7348.1933.tb07770.x.
25. ^ "All About Copper Sulfate". National Fish Pharmaceuticals. Retrieved 2007-12-31.
26. ^ "With Zebra mussels here to stay, Austin has a plan to avoid stinky drinking water". KXAN Austin. 2020-10-26. Retrieved 2020-10-28.
27. ^ Estridge, Barbara H.; Anna P. Reynolds; Norma J. Walters (2000). Basic Medical Laboratory Techniques. Thomson Delmar Learning. p. 166. ISBN 978-0-7668-1206-2.
28. ^ Hoffman, R. V. (2001). "Copper(II) Sulfate". Copper(II) Sulfate, in Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289X.rc247. ISBN 978-0471936237.
29. ^ Philip J. Kocienski (2005). Protecting Groups. Thieme. p. 58. ISBN 978-1-58890-376-1.
30. ^ 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.
31. ^ a b Copper Development Association. "Uses of Copper Compounds: Table A - Uses of Copper Sulphate". copper. Copper Development Association Inc. Retrieved 12 May 2015.
32. ^ Partin, Lee. "The Blues: Part 2". skylighter. Skylighter.Inc. Retrieved 12 May 2015.
33. ^ "Approved and Prohibited Fireworks Chemicals, v2" (PDF). phmsa.dot.gov. US Department of Transportation - Pipeline and Hazardous Materials Safety Administration. 5 November 2019. p. 1. Retrieved 3 August 2025. Copper Sulfate...Color Agent...Prohibited if mixed with a chlorate
34. ^ Despommier; Gwadz; Hotez; Knirsch (June 2005). Parasitic Disease (5 ed.). NY: Apple Tree Production L.L.C. pp. Section 4.2. ISBN 978-0970002778. Retrieved 12 May 2015.
35. ^ "Seizure". Artangel.org.uk. Retrieved 2021-10-05.
36. ^ "Roger Hiorns: Seizure". Yorkshire Sculpture Park. Archived from the original on 2015-02-22. Retrieved 2015-02-22.
37. ^ Cedric Green (10 August 2014). "Bordeaux Etch: etching zinc and steel plates safely (Extract from GREEN PRINTS)". www.greenart.info. Cedric Green. Retrieved 3 August 2025.
38. ^ Semenoff, Nik (12 April 2009). "The Chemistry of using Copper Sulfate Mordant | New Directions in Printmaking". www.ndiprintmaking.ca. Nik Semenoff. Retrieved 3 August 2025.
39. ^ Moretti, Nick (2015). "How to Electrolytically Etch in Copper, Brass, Steel, Nickel Silver, or Silver". mordent.com. Mordent Design. Retrieved 3 August 2025.
40. ^ K. Kondo; Rohan N. Akolkar; Dale P. Barkey; Masayuki Yokoi (2014). Copper Electrodeposition for Nanofabrication of Electronics Devices. New York. ISBN 978-1-4614-9176-7. OCLC 868688018.{{cite book}}: CS1 maint: location missing publisher (link)
41. ^ "Chalcocyanite". www.mindat.org.
42. ^ "Bonattite". www.mindat.org.
43. ^ "Boothite". www.mindat.org.
44. ^ "Poitevinite". www.mindat.org.
45. ^ a b "List of Minerals". www.ima-mineralogy.org. March 21, 2011.
46. ^ "Langite". www.mindat.org.
47. ^ "Posnjakite". www.mindat.org.
48. ^ Windholz, M., ed. 1983. The Merck Index. Tenth edition. Rahway, NJ: Merck and Company.
49. ^ 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
50. ^ Holtzmann, N. A.; Haslam, R. H. (July 1968). "Elevation of serum copper following copper sulfate as an emetic". Pediatrics. 42 (1): 189–93. doi:10.1542/peds.42.1.189. PMID 4385403. S2CID 32740524.
51. ^ Olson, Kent C. (2004). Poisoning & drug overdose. New York: Lange Medical Mooks/McGraw-Hill. p. 175. ISBN 978-0-8385-8172-8.
52. ^ V03AB20 (WHO)

Bibliography

[edit]

• Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. ISBN 978-1439855119.

External links

[edit]

• 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

v t e Copper compounds
Cu(0,I)	Cu5Si
Cu(I)	CuBr CuCN CuCl CuF CuH CuI Cu2C2 Cu2Cr2O5 Cu2O CuOH CuNO3 Cu3P Cu2S CuS CuSCN C6H5Cu
Cu(I,II)	Cu4O3 Cu3H4O8S2
Cu(II)	Cu(BF4)2 CuBr2 CuC2 Cu(CH3COO)2 Cu(CF3COO)2 Cu(C3H5O3)2 CuCO3 Cu2CO3(OH)2 Cu(CN)2 CuCl2 / KCuCl3 / K2CuCl4 Cu(ClO3)2 Cu(ClO4)2 CuF2 Cu(NO3)2 Cu3(PO4)2 Cu3(BO3)2 Cu(N3)2 CuC2O4 CuO CuO2 Cu(OH)2 Cu(SCN)2 CuSO4 Cu3(AsO4)2 Cu(C11H23COO)2 Cu(C17H35COO)2 Cu(O2CC6H5)2 CuTe CuTe2 [Cu(NH3)4(H2O)]SO4
Cu(III)	K3CuF6 CuO−2
Cu(IV)	CuO2 Cs2CuF6

v t e Compounds containing the sulfate group (SO2−4)

H2SO4 He Li2SO4 BeSO4 B2S2O9-BO3+BO3 estersROSO−3(RO)2SO2+CO3+C2O4 (NH4)2SO4[N2H5]HSO4(NH3OH)2SO4NOHSO4+NO3 H2OSO4 +F Ne Na2SO4NaHSO4 MgSO4 Al2(SO4)3Al2SO4(OAc)4 Si +PO4 SO2−4HSO3HSO4(HSO4)2+SO3 +Cl Ar K2SO4KHSO4 CaSO4 Sc2(SO4)3 TiOSO4 VSO4V2(SO4)3VOSO4 CrSO4Cr2(SO4)3 MnSO4 FeSO4Fe2(SO4)3 CoSO4Co2(SO4)3 NiSO4Ni2(SO4)3 CuSO4Cu2SO4[Cu(NH3)4(H2O)]SO4 ZnSO4 Ga2(SO4)3 Ge(SO4)2 +AsO4 +SeO3 +Br Kr RbHSO4Rb2SO4 SrSO4 Y2(SO4)3 Zr(SO4)2 Nb2O2(SO4)3 MoO(SO4)2MoO2(SO4) Tc Ru(SO4)2 Rh2(SO4)3 PdSO4 Ag2SO4AgSO4 CdSO4 In2(SO4)3 SnSO4Sn(SO4)2 Sb2(SO4)3 TeOSO4 I2(SO4)3(IO)2SO4+IO3 Xe Cs2SO4CsHSO4 BaSO4 * Lu2(SO4)3 Hf(SO4)2 Ta(SO4)67– WO(SO4)2 Re2O5(SO4)2 OsSO4Os2(SO4)3Os(SO4)2 IrSO4Ir2(SO4)3 Pt2(SO4)54– AuSO4Au2(SO4)3 Hg2SO4HgSO4 Tl2SO4Tl2(SO4)3 PbSO4Pb(SO4)2 Bi2(SO4)3 PoSO4Po(SO4)2 At Rn Fr RaSO4 ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og   * La2(SO4)3 Ce2(SO4)3Ce(SO4)2 Pr2(SO4)3 Nd2(SO4)3 Pm2(SO4)3 Sm2(SO4)3 EuSO4Eu2(SO4)3 Gd2(SO4)3 Tb2(SO4)3 Dy2(SO4)3 Ho2(SO4)3 Er2(SO4)3 Tm2(SO4)3 Yb2(SO4)3 ** Ac2(SO4)3 Th(SO4)2 (PaO)2(SO4)3H3PaO(SO4)3 U2(SO4)3U(SO4)2UO2SO4 Np(SO4)2(NpO2)2SO4NpO2SO4 Pu(SO4)2PuO2SO4 Am2(SO4)3Am2O2SO4 Cm2(SO4)3Cm2O2SO4 Bk2O2SO4 Cf2(SO4)3Cf2O2SO4 Es Fm Md No

v t e Antidotes (V03AB)
Nervous system	Alcohol intoxication Metadoxine Thiamine Barbiturate overdose Bemegride Ethamivan Benzodiazepine overdose Cyprodenate Flumazenil GHB overdose Physostigmine SCH-50911 Nerve agent / Organophosphate poisoning Atropine# Biperiden Diazepam# Oximes Obidoxime Pralidoxime see also: Cholinesterase Opioid overdose Diprenorphine Doxapram Nalmefene Nalorphine Naloxone# Naltrexone Reversal of neuromuscular blockade Sugammadex
Circulatory system	Beta blocker Glucagon Digoxin toxicity Digoxin immune fab Anticoagulants against direct Xa inhibitors (Andexanet alfa) against heparin (Protamine#)
Other	Arsenic poisoning Dimercaprol# Succimer Cyanide poisoning 4-Dimethylaminophenol Hydroxocobalamin nitrite Amyl nitrite Sodium nitrite# Sodium thiosulfate# Hydrofluoric acid Calcium gluconate# Methanol / Ethylene glycol poisoning Primary alcohols: Ethanol Fomepizole Paracetamol toxicity (Acetaminophen) Acetylcysteine# Glutathione Methionine# Toxic metals (cadmium lead mercury thallium) Dimercaprol# Edetates Prussian blue# Other iodine-131 Potassium iodide Methylthioninium chloride# oxidizing agent Potassium permanganate Prednisolone/promethazine
Emetic	Copper sulfate Ipecacuanha Syrup of ipecac
#WHO-EM ‡Withdrawn from market Clinical trials: †Phase III §Never to phase III

v t e Sulfur compounds
Sulfides and disulfides	Al2S3 As2S2 As2S3 As2S5 As4S4 Au2S Au2S3 B2S3 BaS BeS Bi2S3 CS2 C3S2 C6S6 CaS CdS CeS CoS Cr2S3 CSSe CSTe CuFeS2 CuS D2S Dy2S3 Er2S3 EuS FeS2 GaS H2S HfS2 HgS In2S3 K2S LaS LiS MgS MoS2 MoS3 NaHS Na2S NH4HS NiS P4Sx PbS PbS2 PSCl3 PSI3 PtS ReS2 Re2S7 SiS SrS TlS VS SeS2 S2U WS2 WS3 Sb2S3 Sb2S5 Sb4S3O3 Sm2S3 Y2S3 ZrS2 La2O2S Gd2O2S
Sulfur halides	S2Br2 SBr2 S2Cl2 SCl2 SCl4 S2F2 SF2 SF4 S2F10 SF6 S2I2
Sulfur oxides and oxyhalides	BrSO3F S2O5Cl2 F2S5O2 FClO5S2 F2OS3 ISO3F F2O6S2 SO2 SO3 SOBr2 SOCl2 SOF2 SOF4 H2S3O6 I3SO3F S3O8Cl2 S3O8F2 H2SO3 H2SO4 H2S2O7 H2SO5 Sulfites CdSO3 K2SO3 Sulfates Ag2SO4 CaSO4 CuSO4 Cs2SO4 Er2(SO4)3 Eu2(SO4)3 HgSO4 K2SO4 KAl(SO4)2 NaAl(SO4)2 RaSO4 SnSO4 SrSO4 Ti(SO4)2 Tm2(SO4)3 Yb2(SO4)3 Zr(SO4)2
Sulfur nitrides	SN S2N2 S4N4
Thiocyanates	HSCN KSCN Co(SCN)2
Organic compounds	C2H4S C2H6S3 C4H4S C32H66S2 CHCl3S C2H3SN

Authority control databases
International	GND FAST
National	United States Israel
Other	Yale LUX