Zinc sulfate

Short description: Chemical compound

Zinc sulfate

Names
IUPAC name

Zinc sulfate

Other names

* White vitriol
* Goslarite

Identifiers

CAS Number

* 7733-02-0 Y
* 7446-19-7 (monohydrate) Y
* 13986-24-8 (hexahydrate) N
* 7446-20-0 (heptahydrate) Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:35176 Y

ChEMBL |

* ChEMBL1200929 Y

ChemSpider |

* 22833 Y

DrugBank |

* DB09322

EC Number |

* 231-793-3

KEGG |

* D06371

PubChem CID

* 24424

RTECS number |

* ZH5260000

UNII |

* 0J6Z13X3WO Y
* PTX099XSF1 (monohydrate) Y
* N57JI2K7WP (heptahydrate) Y

UN number | 3077

InChI

* InChI=1S/H2O4S.Zn/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 Y

Key: NWONKYPBYAMBJT-UHFFFAOYSA-L Y

* InChI=1/H2O4S.Zn/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2

Key: NWONKYPBYAMBJT-NUQVWONBAU

SMILES

* [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)

Solubility in water

| 57.7 g/100 mL, anhydrous (20 °C) (in aqueous solutions with a pH < 5)[2]
Solubility | alcohols

Magnetic susceptibility (χ)

| −45.0·10−6 cm3/mol

Refractive index (nD)

| 1.658 (anhydrous), 1.4357 (heptahydrate)
Thermochemistry

Std molar
entropy (S ~~o~~ 298)

| 120 J·mol−1·K−1[3]

Std enthalpy of
formation (ΔfH⦵298)

| −983 kJ·mol−1[3]
Hazards
Safety data sheet | ICSC 1698
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H302, H318, H410

GHS precautionary statements

| P264, P270, P273, P280, P301+312, P305+351+338, P310, P330, P391, P501
NFPA 704 (fire diamond)  |

Flash point | Non-flammable
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).

N verify (what is YN ?)
Infobox references

Zinc sulfate is an inorganic compound with the formula ZnSO4. It forms hydrates ZnSO4·nH2O, where n can range from 0 to 7. All are colorless solids. The most common form includes water of crystallization as the heptahydrate,[4] with the formula ZnSO
4 * 7H2O. As early as the 16th century it was prepared on a 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).[citation needed] Zinc sulfate and its hydrates are colourless solids.

## Contents

* 1 Uses
* 1.1 Manufacturing
* 1.2 Nutrition
* 1.3 Medicine
* 2 Production, reactions, structure
* 3 Minerals
* 4 Safety
* 5 References

## 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

Main article: Medicine:Zinc sulfate (medical use)

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 + H
2SO
4 \+ 7 H
2O → ZnSO
4 * 7H2O + H

Pharmaceutical-grade zinc sulfate is produced by treating high-purity zinc oxide with sulfuric acid:

ZnO + H
2SO
4 \+ 6 H
2O → ZnSO
4 * 7H2O

In aqueous solution, all forms of zinc sulfate behave identically. These aqueous solutions consist of the metal aquo complex [Zn(H
2O)
6]2+ and SO2−4 ions. Barium sulfate forms when these solutions are treated with solutions of barium ions:

ZnSO
4 \+ BaCl
2 → BaSO
4 \+ ZnCl

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)SO
4 * 7H2O (structurally different from goslarite). Lower hydrates of zinc sulfate are rarely found in nature: (Zn,Fe)SO
4 * 6H2O (bianchite), (Zn,Mg)SO
4 * 4H2O (boyleite), and (Zn,Mn)SO
4 * 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". https://webbook.nist.gov/cgi/cbook.cgi?ID=C7733020&Mask=8.
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. ↑ 3.0 3.1 Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin. p. A23. ISBN 978-0-618-94690-7.
4. ↑ 4.0 4.1 4.2 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) (in en). A Treatise on Chemistry: Metals. Appleton. https://books.google.com/books?id=yNbnAAAAMAAJ&pg=PA261.
6. ↑ "Zinc Sulphate" (in en). http://cleanagro.com/zinc-sulphate-manufacturer-in-india.html.
7. ↑ "Moss on Roofs". Community Horticultural Fact Sheet #97. Washington State University King County Extension. http://county.wsu.edu/king/gardening/mg/factsheets/Fact Sheets/Moss on Roofs.pdf.
8. ↑ "Metallurgy for Homebrewers". Brew Your Own Magazine. http://byo.com/malt/item/1144-metallurgy-for-homebrewers.
9. ↑ "The Effect of Zinc on Fermentation Performance". Braukaiser blog. http://braukaiser.com/blog/blog/2012/06/22/the-effect-of-zinc-on-fermentation-performance/.
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. https://www.jmbfs.org/issue/february-2012-vol-1-special-issue/sillerova1/?issue_id=908&article_id=45. Retrieved 15 October 2018.
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. https://academic.oup.com/chemse/article/29/6/513/295743.
12. ↑ British national formulary : BNF 69 (69 ed.). British Medical Association. 2015. p. 700. ISBN 9780857111562.
13. ↑ WHO Model Formulary 2008. World Health Organization. 2009. p. 351. ISBN 9789241547659.
14. ↑ "Zinc Sulphate Zinc Sulfate MSDS Sheet of Manufacturers". Mubychem.com. 2013-05-05. http://mubychem.com/MSDS/Zinc Sulphate MSDS.htm.
15. ↑ Wildner, M.; Giester, G. (1988). "Crystal Structure refinements of synthetic chalcocyanite (CUSO4) and zincosite (ZnSO4)". Mineralogy and Petrology 39 (3–4): 201–209. doi:10.1007/BF01163035. Bibcode: 1988MinPe..39..201W.
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 (European Food Safety Authority (EFSA)) 10 (2): 2572. Feb 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. https://jamanetwork.com/journals/jamaotolaryngology/fullarticle/496489.

* v
* t
* e

Zinc compounds

Zinc(I)|

| Organozinc(I) compounds|

* Zn2(C5(CH3)5)2

|

Zinc(II)|

* Zn(N3)2
* ZnBr2
* Zn(CN)2
* ZnCl2
* Zn(ClO3)2
* ZnCrO4
* ZnF2
* ZnH2
* ZnI2
* ZnMoO4
* Zn(NO3)2
* ZnO
* ZnO2
* Zn(OH)2
* ZnS
* ZnSO4
* ZnSe
* ZnTe
* Zn2P2O7
* Zn3Sb2
* Zn3As2
* Zn3N2
* Zn3P2
* Zn3(PO4)2

| Organozinc(II) compounds|

* Zn(CH3)2
* Zn(C2H5)2
* Zn(CH(CH3)2)2
* Zn(C(CH3)3)2
* Zn(C6H5)2
* ZnCIH2I

|

* v
* t
* e

Compounds containing the sulfate group

H2SO4 |  |  |  | He

|
|
|
|

Li2SO4 | BeSO4 | B  | esters
ROSO3−
(RO)2SO2 | (NH4)2SO4
[N2H5]HSO4
(NH3OH)2SO4
NOHSO4 | HOSO4 | F  | Ne
Na2SO4
NaHSO4 | MgSO4 | Al2(SO4)3
Al2SO4(OAc)4 | Si  | P  | SO42−
HSO3HSO4
(HSO4)2 | Cl  | Ar
K2SO4
KHSO4 | CaSO4 | Sc2(SO4)3 | TiOSO4 | VSO4
V2(SO4)3
VOSO4 | CrSO4
Cr2(SO4)3 | MnSO4 | FeSO4
Fe2(SO4)3 | CoSO4 | NiSO4 | CuSO4
Cu2SO4
[Cu(NH3)4(H2O)]SO4 | ZnSO4 | Ga2(SO4)3 | Ge  | As  | Se  | Br  | Kr
RbHSO4
Rb2SO4 | SrSO4 | Y2(SO4)3 | Zr(SO4)2 | Nb  | Mo  | Tc  | Ru  | Rh2(SO4)3 | PdSO4 | Ag2SO4 | CdSO4 | In2(SO4)3 | SnSO4
Sn(SO4)2 | Sb2(SO4)3 | Te  | I  | Xe
Cs2SO4
CsHSO4 | BaSO4 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt  | AuSO4
Au2(SO4)3 | Hg2SO4
HgSO4 | Tl2SO4
Tl2(SO4)3 | PbSO4 | Bi2(SO4)3 | Po  | At  | Rn
Fr  | Ra  |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce2(SO4)3
Ce(SO4)2 | Pr2(SO4)3 | Nd  | Pm  | Sm  | Eu  | Gd  | Tb  | Dy  | Ho  | Er  | Tm  | Yb2(SO4)3 | Lu
Ac  | Th  | Pa  | U(SO4)2
UO2SO4 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Zinc sulfate. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Zinc_sulfate&oldid=4310329"
*[CID]: Compound ID
*[H302]: Harmful if swallowed
*[H318]: Causes serious eye damage
*[H410]: Very toxic to aquatic life with long lasting effects
*[P264]: Wash … thoroughly after handling
*[P270]: Do not eat, drink or smoke when using this product
*[P273]: Avoid release to the environment
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P301+312]: IF SWALLOWED: Call a POISON CENTER or doctor/physician if you feel unwell
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P310]: Immediately call a POISON CENTER or doctor/physician
*[P330]: Rinse mouth
*[P391]: Collect spillage
*[P501]: Dispose of contents/container to …
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template