3D model (Jmol)
|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|R-phrases (outdated)||R22, R41, R50/53|
|S-phrases (outdated)||(S2), S22, S26, S39, S46, S60, S61|
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 and dietary supplement. As a supplement it is used to treat zinc deficiency and to prevention the conditions in those at high risk. Side effects may include abdominal pain, vomiting, headache, and feeling tired.
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 not necessary 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 and fermenting vessels and after wood, zinc was slowly leeched by the use of copper kettles. A modern copper immersion chiller is speculated to provide trace elements of zinc. Be careful when adding supplemental zinc to not overdo it. 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."   [Sillerova et al. (2012) Journal of Microbiology, Biotechnolgy and Food Sciences 1 (February special issue): 689-695]
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 the reaction of the metal with aqueous sulfuric acid:
- Zn + H2SO4 + 7 H2O → ZnSO4(H2O)7 + H2
Pharmaceutical grade zinc sulfate is produced by treating high purity zinc oxide with sulfuric acid:
- ZnO + H2SO4 + 6 H2O → ZnSO4(H2O)7
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 Zinc-melanterite (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 0-618-94690-X.
- British national formulary : BNF 69 (69 ed.). British Medical Association. 2015. p. 700. ISBN 9780857111562.
- WHO Model Formulary 2008 (PDF). World Health Organization. 2009. p. 351. ISBN 9789241547659. Retrieved 8 January 2017.
- Dieter M. M. Rohe, Hans Uwe Wolf "Zinc Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a28 537
- "Moss on Roofs," .Community Horticultural Fact Sheet #97, Washington State University King County Extension, 
- "Metallurgy for Homebrewers" Brew Your Own Magazine 
- "The Effect of Zinc on Fermentation Performance" Braukaiser blog.
- European Food Safety Authority (EFSA), "Scientific Opinion on safety and efficacy of zinc compounds (E6) as feed additives for all animal species: Zinc sulphate monohydrate", Feb 2012 
- "Zinc Sulphate Zinc Sulfate MSDS Sheet of Manufacturers". Mubychem.com. 2013-05-05. Retrieved 2013-06-08.
Salts and esters of the sulfate ion