3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||161.47 g/mol (anhydrous) |
179.47 g/mol (monohydrate)
287.53 g/mol (heptahydrate)
|Density||3.54 g/cm3 (anhydrous) |
2.072 g/cm3 (hexahydrate)
|Melting point|| 680 °C (1,256 °F; 953 K) decomposes (anhydrous) |
100 °C (heptahydrate)
70 °C, decomposes (hexahydrate)
|Boiling point|| 740 °C (1,360 °F; 1,010 K) (anhydrous) |
280 °C, decomposes (heptahydrate)
|57.7 g/100 mL, anhydrous (20 °C) (In aqueous solutions with a pH < 5)|
Refractive index (nD)
|1.658 (anhydrous), 1.4357 (heptahydrate)|
Std enthalpy of
|Safety data sheet||ICSC 1698|
Dangerous for the environment (N)
|R-phrases (outdated)||R22, R41, R50/53|
|S-phrases (outdated)||(S2), S22, S26, S39, S46, S60, S61|
|NFPA 704 (fire diamond)|
|Cadmium sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Zinc sulfate is an inorganic compound. It is used as a dietary supplement to treat zinc deficiency and to prevent the condition in those at high risk. Side effects of excess supplementation may include abdominal pain, vomiting, headache, and tiredness.
The most common form includes water of crystallization as the heptahydrate, with the formula ZnSO4•7H2O. It was historically known as "white vitriol". Zinc sulfate and its hydrates are colourless solids.
Zinc sulfate is used to supply zinc in animal feeds, fertilizers, toothpaste, and agricultural sprays. Zinc sulfate, like many zinc compounds, can be used to control moss growth on roofs.
Zinc sulfate can be used to supplement zinc in the brewing process. Zinc is a necessary nutrient for optimal yeast health and performance, although it is not a necessary supplement for low-gravity beers, as the grains commonly used in brewing already provide adequate zinc. It is a more common practice when pushing yeast to their limit by increasing alcohol content beyond their comfort zone. Before modern stainless steel, brew Kettles, fermenting vessels and after wood, zinc was slowly leached by the use of copper kettles. A modern copper immersion chiller is speculated to provide trace elements of zinc; thus care must be taken when adding supplemental zinc so as not to cause excess. Side effects include "...increased acetaldehyde and fusel alcohol production due to high yeast growth when zinc concentrations exceed 5 ppm. Excess zinc can also cause soapy or goaty flavors." 
Zinc sulfate powder is an eye irritant. Ingestion of trace amounts is considered safe, and zinc sulfate is added to animal feed as a source of essential zinc, at rates of up to several hundred milligrams per kilogram of feed. Excess ingestion results in acute stomach distress, with nausea and vomiting appearing at 2–8 mg/Kg of body weight.
Production and reactivity
Zinc sulfate is produced by treating virtually any zinc-containing material (metal, minerals, oxides) with sulfuric acid.
Specific reactions include the reaction of the metal with aqueous sulfuric acid:
- Zn + H2SO4 + 7 H2O → ZnSO4•7H2O + H2
Pharmaceutical-grade zinc sulfate is produced by treating high-purity zinc oxide with sulfuric acid:
- ZnO + H2SO4 + 6 H2O → ZnSO4•7H2O
In aqueous solution, all forms of zinc sulfate behave identically. These aqueous solutions consist of the metal aquo complex [Zn(H2O)6]2+ and SO42− ions. Barium sulfate forms when these solutions are treated with solutions of barium ions:
- ZnSO4 + BaCl2 → BaSO4 + ZnCl2
With a reduction potential of -0.76, zinc(II) reduces only with difficulty.
As a mineral, ZnSO4•7H2O is known as goslarite. Zinc sulfate occurs as several other minor minerals, such as zincmelanterite, (Zn,Cu,Fe)SO4•7H2O (structurally different from goslarite). Lower hydrates of zinc sulfate are rarely found in nature: (Zn,Fe)SO4•6H2O (bianchite), (Zn,Mg)SO4•4H2O (boyleite), and (Zn,Mn)SO4•H2O (gunningite).
- Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
- British national formulary : BNF 69 (69 ed.). British Medical Association. 2015. p. 700. ISBN 9780857111562.
- World Health Organization (2009). Stuart MC, Kouimtzi M, Hill SR (eds.). WHO Model Formulary 2008. World Health Organization. p. 351. hdl:10665/44053. ISBN 9789241547659.
- Dieter M. M. Rohe; Hans Uwe Wolf (2005). "Zinc Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: John Wiley & Sons. doi:10.1002/14356007.a28_537. ISBN 978-3527306732.
- "Moss on Roofs" (PDF). Community Horticultural Fact Sheet #97. Washington State University King County Extension. Archived from the original (PDF) on 22 December 2015.
- "Metallurgy for Homebrewers". Brew Your Own Magazine.
- "The Effect of Zinc on Fermentation Performance". Braukaiser blog.
- Šillerová, Silvia; Lavová, Blažena; Urminská, Dana; Poláková, Anežka; Vollmannová, Alena; Harangozo, Ľuboš (February 2012). "Preparation of Zinc Enriched Yeast (Saccharomyces cerevisiae) by Cultivation With Different Zinc Salts". Journal of Microbiology, Biotechnology and Food Sciences. 1 (Special issue): 689–695. ISSN 1338-5178.
- "Scientific Opinion on safety and efficacy of zinc compounds (E6) as feed additives for all animal species: Zinc sulphate monohydrate". EFSA Journal. European Food Safety Authority (EFSA). 10 (2): 2572. February 2012. doi:10.2903/j.efsa.2012.2572.
- "Zinc Sulphate Zinc Sulfate MSDS Sheet of Manufacturers". Mubychem.com. 5 May 2013. Retrieved 8 June 2013.