Zinc sulfate

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Zinc sulfate
Zinc Sulfate.jpg
Zinc sulfate.png
Names
IUPAC name
Zinc sulfate
Other names
White vitriol
Goslarite
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.028.904 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 231-793-3
PubChem CID
RTECS number
  • ZH5260000
UNII
UN number 3077
  • InChI=1S/H2O4S.Zn/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 Yes check.svgY
    Key: NWONKYPBYAMBJT-UHFFFAOYSA-L Yes check.svgY
  • 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
ZnSO4
Molar mass 161.44 [1] g/mol (anhydrous)
179.47 g/mol (monohydrate)
287.53 g/mol (heptahydrate)
Appearancewhite 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]
−983 kJ·mol−1 [3]
Hazards
GHS labelling:
GHS-pictogram-acid.svg GHS-pictogram-exclam.svg GHS-pictogram-pollu.svg
Danger
H302, H318, H410
P264, P270, P273, P280, P301+P312, P305+P351+P338, P310, P330, P391, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

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 Zn SO4·7H2O . 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.

Contents

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] . Zn(aq)6SO4.svg
Aqueous solutions of zinc sulfate consist of the aquo complex [Zn(H2O)6] .

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]

Related Research Articles

<span class="mw-page-title-main">Sulfate</span> Oxyanion with a central atom of sulfur surrounded by 4 oxygen atoms

The sulfate or sulphate ion is a polyatomic anion with the empirical formula SO2−4. Salts, acid derivatives, and peroxides of sulfate are widely used in industry. Sulfates occur widely in everyday life. Sulfates are salts of sulfuric acid and many are prepared from that acid.

<span class="mw-page-title-main">Iron(II) sulfate</span> Chemical compound

Iron(II) sulfate (British English: iron(II) sulphate) or ferrous sulfate denotes a range of salts with the formula Fe SO4·xH2O. These compounds exist most commonly as the heptahydrate (x = 7) but several values for x are known. The hydrated form is used medically to treat or prevent iron deficiency, and also for industrial applications. Known since ancient times as copperas and as green vitriol (vitriol is an archaic name for sulfate), the blue-green heptahydrate (hydrate with 7 molecules of water) is the most common form of this material. All the iron(II) sulfates dissolve in water to give the same aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic. The name copperas dates from times when the copper(II) sulfate was known as blue copperas, and perhaps in analogy, iron(II) and zinc sulfate were known respectively as green and white copperas.

<span class="mw-page-title-main">Magnesium sulfate</span> Chemical compound with formula MgSO4

Magnesium sulfate or Magnesium sulphate is a chemical compound, a salt with the formula MgSO4, consisting of magnesium cations Mg2+ (20.19% by mass) and sulfate anions SO2−4. It is a white crystalline solid, soluble in water but not in ethanol.

<span class="mw-page-title-main">Copper(II) sulfate</span> Chemical compound

Copper(II) sulfate, also known as copper sulphate, 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. Older names for the pentahydrate include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. 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. Anhydrous copper sulfate is a light grey powder.

<span class="mw-page-title-main">Calcium sulfate</span> Laboratory and industrial chemical

Calcium sulfate (or calcium sulphate) is the inorganic compound with the formula CaSO4 and related hydrates. In the form of γ-anhydrite (the anhydrous form), it is used as a desiccant. One particular hydrate is better known as plaster of Paris, and another occurs naturally as the mineral gypsum. It has many uses in industry. All forms are white solids that are poorly soluble in water. Calcium sulfate causes permanent hardness in water.

<span class="mw-page-title-main">Goslarite</span>

Goslarite is a hydrated zinc sulfate mineral which was first found in the Rammelsberg mine, Goslar, Harz, Germany. It was described in 1847. Goslarite belongs to the epsomite group which also includes epsomite and morenosite. Goslarite is an unstable mineral at the surface and will dehydrate to other minerals like bianchite, boyleite and gunningite.

<span class="mw-page-title-main">Potassium sulfate</span> Chemical compound

Potassium sulfate (US) or potassium sulphate (UK), also called sulphate of potash (SOP), arcanite, or archaically potash of sulfur, is the inorganic compound with formula K2SO4, a white water-soluble solid. It is commonly used in fertilizers, providing both potassium and sulfur.

In chemistry, water(s) of crystallization or water(s) of hydration are water molecules that are present inside crystals. Water is often incorporated in the formation of crystals from aqueous solutions. In some contexts, water of crystallization is the total mass of water in a substance at a given temperature and is mostly present in a definite (stoichiometric) ratio. Classically, "water of crystallization" refers to water that is found in the crystalline framework of a metal complex or a salt, which is not directly bonded to the metal cation.

Uranium(IV) sulfate (U(SO4)2) is a water-soluble salt of uranium. It is a very toxic compound. Uranium sulfate minerals commonly are widespread around uranium bearing mine sites, where they usually form during the evaporation of acid sulfate-rich mine tailings which have been leached by oxygen-bearing waters. Uranium sulfate is a transitional compound in the production of uranium hexafluoride. It was also used to fuel aqueous homogeneous reactors.

<span class="mw-page-title-main">Mercury(II) sulfate</span> Chemical compound

Mercury(II) sulfate, commonly called mercuric sulfate, is the chemical compound HgSO4. It is an odorless salt that forms white granules or crystalline powder. In water, it separates into an insoluble basic sulfate with a yellow color and sulfuric acid.

<span class="mw-page-title-main">Nickel(II) sulfate</span> Chemical compound

Nickel(II) sulfate, or just nickel sulfate, usually refers to the inorganic compound with the formula NiSO4(H2O)6. This highly soluble blue green coloured salt is a common source of the Ni2+ ion for electroplating.

In ore deposit geology, supergene processes or enrichment are those that occur relatively near the surface as opposed to deep hypogene processes. Supergene processes include the predominance of meteoric water circulation (i.e. water derived from precipitation) with concomitant oxidation and chemical weathering. The descending meteoric waters oxidize the primary (hypogene) sulfide ore minerals and redistribute the metallic ore elements. Supergene enrichment occurs at the base of the oxidized portion of an ore deposit. Metals that have been leached from the oxidized ore are carried downward by percolating groundwater, and react with hypogene sulfides at the supergene-hypogene boundary. The reaction produces secondary sulfides with metal contents higher than those of the primary ore. This is particularly noted in copper ore deposits where the copper sulfide minerals chalcocite (Cu2S), covellite (CuS), digenite (Cu18S10), and djurleite (Cu31S16) are deposited by the descending surface waters.

<span class="mw-page-title-main">Manganese(II) sulfate</span> Chemical compound

Manganese(II) sulfate usually refers to the inorganic compound with the formula MnSO4·H2O. This pale pink deliquescent solid is a commercially significant manganese(II) salt. Approximately 260,000 tonnes of manganese(II) sulfate were produced worldwide in 2005. It is the precursor to manganese metal and many other chemical compounds. Manganese-deficient soil is remediated with this salt.

<span class="mw-page-title-main">Mercury(I) sulfate</span> Chemical compound

Mercury(I) sulfate, commonly called mercurous sulphate (UK) or mercurous sulfate (US) is the chemical compound Hg2SO4. Mercury(I) sulfate is a metallic compound that is a white, pale yellow or beige powder. It is a metallic salt of sulfuric acid formed by replacing both hydrogen atoms with mercury(I). It is highly toxic; it could be fatal if inhaled, ingested, or absorbed by skin.

<span class="mw-page-title-main">Szomolnokite</span>

Szomolnokite (Fe2+SO4·H2O) is a monoclinic iron sulfate mineral forming a complete solid solution with magnesium end-member kieserite (MgSO4·H2O). In 1877 szomolnokite's name was derived by Joseph Krenner from its type locality of oxidized sulfide ore containing iron in Szomolnok, Slovakia (Hungary at the time).

<span class="mw-page-title-main">Iron(III) sulfate</span> Chemical compound

Iron(III) sulfate (or ferric sulfate), is a family of inorganic compounds with the formula Fe2(SO4)3(H2O)n. A variety of hydrates are known, including the most commonly encountered form of "ferric sulfate". Solutions are used in dyeing as a mordant, and as a coagulant for industrial wastes. Solutions of ferric sulfate are also used in the processing of aluminum and steel.

<span class="mw-page-title-main">Cobalt(II) sulfate</span> Inorganic compound

Cobalt(II) sulfate is any of the inorganic compounds with the formula CoSO4(H2O)x. Usually cobalt sulfate refers to the hexa- or heptahydrates CoSO4.6H2O or CoSO4.7H2O, respectively. The heptahydrate is a red solid that is soluble in water and methanol. Since cobalt(II) has an odd number of electrons, its salts are paramagnetic.

<span class="mw-page-title-main">Chromium(II) sulfate</span> Chemical compound

Chromium(II) sulfate refers to inorganic compounds with the chemical formula CrSO4·n H2O. Several closely related hydrated salts are known. The pentahydrate is a blue solid that dissolves readily in water. Solutions of chromium(II) are easily oxidized by air to Cr(III) species. Solutions of Cr(II) are used as specialized reducing agents of value in organic synthesis.

<span class="mw-page-title-main">Vanadium(II) sulfate</span> Chemical compound

Vanadium(II) sulfate describes a family of inorganic compounds with the formula VSO4(H2O)x where 0 ≤ x ≤ 7. The hexahydrate is most commonly encountered. It is a violet solid that dissolves in water to give air-sensitive solutions of the aquo complex. The salt is isomorphous with [Mg(H2O)6]SO4. Compared to the V–O bond length of 191 pm in [V(H2O)6]3+, the V–O distance is 212 pm in the [V(H2O)6]SO4. This nearly 10% elongation reflects the effect of the lower charge, hence weakened electrostatic attraction.

Gallium(III) sulfate refers to the chemical compound, a salt, with the formula Ga2(SO4)3, or its hydrates Ga2(SO4)3·xH2O. Gallium metal dissolves in sulfuric acid to form solutions containing [Ga(OH2)6]3+ and SO42− ions. The octadecahydrate Ga2(SO4)3·18H2O crystallises from these solutions at room temperature. This hydrate loses water in stages when heated, forming the anhydrate Ga2(SO4)3 above 150 °C and completely above 310 °C. Anhydrous Ga2(SO4)3 is isostructural with iron(III) sulfate, crystallizing in the rhombohedral space group R3.

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. 1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN   978-0-618-94690-7.
  4. 1 2 3 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. European Food Safety Authority (EFSA). 10 (2): 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.

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