Zinc sulfate

Chemical compound
Zinc sulfate
Names
IUPAC name
Zinc sulfate
Other names
White vitriol
Goslarite
Identifiers
CAS Number
  • 7733-02-0 checkY
  • 7446-19-7 (monohydrate) checkY
  • 13986-24-8 (hexahydrate) ☒N
  • 7446-20-0 (heptahydrate) checkY
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:35176 checkY
ChEMBL
  • ChEMBL1200929 checkY
ChemSpider
  • 22833 checkY
DrugBank
  • DB09322
ECHA InfoCard 100.028.904 Edit this at Wikidata
EC Number
  • 231-793-3
PubChem CID
  • 24424
RTECS number
  • ZH5260000
UNII
  • 0J6Z13X3WO checkY
  • PTX099XSF1 (monohydrate) checkY
  • N57JI2K7WP (heptahydrate) checkY
UN number 3077
CompTox Dashboard (EPA)
  • DTXSID2040315 Edit this at Wikidata
InChI
  • InChI=1S/H2O4S.Zn/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 checkY
    Key: NWONKYPBYAMBJT-UHFFFAOYSA-L checkY
  • InChI=1/H2O4S.Zn/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2
    Key: NWONKYPBYAMBJT-NUQVWONBAU
  • [Zn+2].[O-]S([O-])(=O)=O
Properties
Chemical formula
 ZnSO4
Molar mass 161.44[1] g/mol (anhydrous)
179.47 g/mol (monohydrate)
287.53 g/mol (heptahydrate)
Appearance white powder
Odor odorless
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)[2]
Solubility alcohols
−45.0·10−6 cm3/mol
1.658 (anhydrous), 1.4357 (heptahydrate)
Thermochemistry
Std molar
entropy (S⦵298)
 120 J·mol−1·K−1[3]
Std enthalpy of
formation (ΔfH⦵298)
 −983 kJ·mol−1[3]
Hazards
GHS labelling:
GHS05: CorrosiveGHS07: Exclamation markGHS09: Environmental hazard
Danger
H302, H318, H410
P264, P270, P273, P280, P301+P312, P305+P351+P338, P310, P330, P391, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Flash point Non-flammable
Safety data sheet (SDS) ICSC 1698
Related compounds
Other cations
 Cadmium sulfate
Manganese sulfate
Related compounds
 Copper(II) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
Chemical compound

Zinc sulfate describes a family of inorganic compounds with the formula ZnSO4(H2O)x. All are colorless solids. The most common form includes water of crystallization as the heptahydrate,[4] with the formula ZnSO4·7H2O. As early as the 16th century it was prepared on the large scale, and was historically known as "white vitriol"[5] (the name was used, for example, in 1620s by the collective writing under the pseudonym of Basil Valentine). Zinc sulfate and its hydrates are colourless solids.

Uses

Manufacturing

The main application of the heptahydrate is as a coagulant in the production of rayon. It is also a precursor to the pigment lithopone. It is also used as an electrolyte for zinc electroplating, as a mordant in dyeing, and as a preservative for skins and leather.

Nutrition

Zinc sulfate is used to supply zinc in animal feeds, fertilizers, toothpaste, and agricultural sprays. Zinc sulfate,[6] like many zinc compounds, can be used to control moss growth on roofs.[7]

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 amounts 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."[8][9][10]

Zinc sulfate is a potent inhibitor of sweetness perception for most sweet-tasting substances.[11]

Medicine

It is used as a dietary supplement to treat zinc deficiency and to prevent the condition in those at high risk.[12] Side effects of excess supplementation may include abdominal pain, vomiting, headache, and tiredness.[13] it is also used together with oral rehydration therapy (ORT) and an astringent.[4]

Production, reactions, structure

Aqueous solutions of zinc sulfate consist of the aquo complex [Zn(H2O)6]2+.

Zinc sulfate is produced by treating virtually any zinc-containing material (metal, minerals, oxides) with sulfuric acid.[4]

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 SO2−
4 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 V, zinc(II) reduces only with difficulty.

When heated above 680 °C, zinc sulfate decomposes into sulfur dioxide gas and zinc oxide fume, both of which are hazardous.[14]

The heptahydrate is isostructural with ferrous sulfate heptahydrate. The solid consists of [Zn(H2O)6]2+ ions interacting with sulfate and one water of crystallization by hydrogen bonds. Anhydrous zinc sulfate is isomorphous with anhydrous copper(II) sulfate. It exists as the mineral zincosite.[15] A monohydrate is known.[16] The hexahydrate is also recognized.[17]

Minerals

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).

Safety

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.[18] Nasal irrigation with a solution of zinc sulfate has been found to be able to damage the olfactory sense nerves and induce anosmia in a number of different species, including humans.[19]

References

  1. ^ "Zinc sulphate".
  2. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  3. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
  4. ^ a b c 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.
  5. ^ Roscoe, Henry Enfield; Schorlemmer, Carl (1889). A Treatise on Chemistry: Metals. Appleton.
  6. ^ "Zinc Sulphate". Chemical & Fertilizer Expert. Archived from the original on 15 September 2021. Retrieved 15 September 2021.
  7. ^ "Moss on Roofs" (PDF). Community Horticultural Fact Sheet #97. Washington State University King County Extension. Archived from the original (PDF) on 22 December 2015.
  8. ^ "Metallurgy for Homebrewers". Brew Your Own Magazine.
  9. ^ "The Effect of Zinc on Fermentation Performance". Braukaiser blog.
  10. ^ 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.
  11. ^ Keast, R. S.J.; Canty, T. M.; Breslin, P. A. (2004). "Oral Zinc Sulfate Solutions Inhibit Sweet Taste Perception". Chemical Senses. 29 (6): 513–521. doi:10.1093/chemse/bjh053. PMID 15269123.
  12. ^ British national formulary : BNF 69 (69 ed.). British Medical Association. 2015. p. 700. ISBN 9780857111562.
  13. ^ 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.
  14. ^ "Zinc Sulphate Zinc Sulfate MSDS Sheet of Manufacturers". Mubychem.com. 5 May 2013. Retrieved 8 June 2013.
  15. ^ Wildner, M.; Giester, G. (1988). "Crystal Structure refinements of synthetic chalcocyanite (CUSO4) and zincosite (ZnSO4)". Mineralogy and Petrology. 39 (3–4): 201–209. Bibcode:1988MinPe..39..201W. doi:10.1007/BF01163035. S2CID 93701665.
  16. ^ Wildner, M.; Giester, G. (1991). "The Crystal Structures of Kieserite-Type Compounds. I. Crystal Structures of Me(II)SO4*H2O (Me = Mn, Fe, Co, Ni, Zn)". Neues Jahrbuch für Mineralogie - Monatshefte. 1991: 296–306.
  17. ^ Spiess, M.; Gruehn, R. (1979). "Beiträge zum thermischen Verhalten von Sulfaten. II. Zur thermischen Dehydratisierung des ZnSO4•7H2O und zum Hochtemperaturverhalten von wasserfreiem ZnSO4". Zeitschrift für Anorganische und Allgemeine Chemie. 456: 222–240. doi:10.1002/zaac.19794560124.
  18. ^ "Scientific Opinion on safety and efficacy of zinc compounds (E6) as feed additives for all animal species: Zinc sulphate monohydrate". EFSA Journal. 10 (2). European Food Safety Authority (EFSA): 2572. February 2012. doi:10.2903/j.efsa.2012.2572.
  19. ^ Davidson, Terence M.; Smith, Wendy M. (19 July 2010). "The Bradford Hill Criteria and Zinc-Induced Anosmia: A Causality Analysis". Archives of Otolaryngology–Head & Neck Surgery. 136 (7): 673–676. doi:10.1001/archoto.2010.111. PMID 20644061.
  • v
  • t
  • e
Zinc(I)
Organozinc(I) compounds
  • Zn2(C5(CH3)5)2
Zinc(II)
  • Zn(acac)2
  • Zn(N3)2
  • ZnBr2
  • ZnCO3
  • Zn(CN)2
  • ZnCl2
  • Zn(ClO3)2
  • ZnCrO4
  • ZnF2
  • ZnH2
  • ZnI2
  • ZnMoO4
  • Zn(NO3)2
  • ZnO
  • ZnO2
  • Zn(ClO
    4    )
    2
  • Zn(OH)2
  • ZnS
  • ZnSO4
  • ZnSe
  • ZnTe
  • Zn2P2O7
  • Zn3Sb2
  • Zn3As2
  • Zn3N2
  • Zn3P2
  • ZnP2
  • Zn3(PO4)2
Organozinc(II) compounds
  • Zn(CH3)2
  • Zn(C2H5)2
  • Zn(CH3COO)2
  • Zn(CH(CH3)2)2
  • Zn(C(CH3)3)2
  • Zn(C6H5)2
  • Zn(C3H5O3)2
  • ZnICH2I
    • C
      24      H
      46      ZnO
      4
    • v
    • t
    • e
    Compounds containing the sulfate group (SO2−4)
    H2SO4 He
    Li2SO4 BeSO4 B2S2O9
    -BO3
    +BO3     		esters
    ROSO−3
    (RO)2SO2
    +CO3
    +C2O4     		(NH4)2SO4
    [N2H5]HSO4
    (NH3OH)2SO4
    NOHSO4
    +NO3     		HOSO4 +F Ne
    Na2SO4
    NaHSO4     		MgSO4 Al2(SO4)3
    Al2SO4(OAc)4     		Si +PO4 SO2−4
    HSO3HSO4
    (HSO4)2
    +SO3     		+Cl Ar
    K2SO4
    KHSO4     		CaSO4 Sc2(SO4)3 TiOSO4 VSO4
    V2(SO4)3
    VOSO4     		CrSO4
    Cr2(SO4)3     		MnSO4 FeSO4
    Fe2(SO4)3     		CoSO4
    Co2(SO4)3     		NiSO4
    Ni2(SO4)3     		CuSO4
    Cu2SO4
    [Cu(NH3)4(H2O)]SO4     		ZnSO4 Ga2(SO4)3 Ge As +SeO3 Br Kr
    RbHSO4
    Rb2SO4     		SrSO4 Y2(SO4)3 Zr(SO4)2 Nb2O2(SO4)3 MoO(SO4)2
    MoO2(SO4)     		Tc Ru(SO4)2 Rh2(SO4)3 PdSO4 Ag2SO4
    AgSO4     		CdSO4 In2(SO4)3 SnSO4
    Sn(SO4)2     		Sb2(SO4)3 Te +IO3 Xe
    Cs2SO4
    CsHSO4     		BaSO4 * Lu2(SO4)3 Hf Ta WO(SO4)2 Re2O5(SO4)2 OsSO4
    Os2(SO4)3
    Os(SO4)2     		IrSO4
    Ir2(SO4)3     		Pt2(SO4)54– AuSO4
    Au2(SO4)3     		Hg2SO4
    HgSO4     		Tl2SO4
    Tl2(SO4)3     		PbSO4
    Pb(SO4)2     		Bi2(SO4)3 PoSO4
    Po(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)3
    Ce(SO4)2     		Pr2(SO4)3 Nd2(SO4)3 Pm2(SO4)3 Sm2(SO4)3 EuSO4
    Eu2(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 Pa U2(SO4)3
    U(SO4)2
    UO2SO4     		Np(SO4)2 Pu(SO4)2 Am2(SO4)3 Cm2(SO4)3 Bk Cf2(SO4)3 Es Fm Md No
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