Zinc sulfate

Zinc sulfate
Zinc sulfate
Identifiers
CAS number 7733-02-0 YesY
7446-19-7 (monohydrate)
13986-24-8 (hexahydrate)
7446-20-0 (heptahydrate)
PubChem 24424
ChemSpider 22833 YesY
UNII 0J6Z13X3WO YesY
EC number 231-793-3
UN number 3077
ChEBI CHEBI:35176
ChEMBL CHEMBL1200929
RTECS number ZH5260000
Jmol-3D images Image 1
Properties
Molecular formula ZnSO4
Molar mass 161.47 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 ºC decomp. (anhydrous)
100 °C (heptahydrate)
70 °C, decomp (hexahydrate)

Boiling point

740 °C (anhydrous)
280 °C, decomp (heptahydrate)

Solubility in water 57.7 g/100 mL, anhydrous (20 °C)[1]
Solubility alcohols
Refractive index (nD) 1.658 (anhydrous), 1.4357 (heptahydrate)
Hazards
MSDS ICSC 1698
EU Index 030-006-00-9
EU classification Harmful (Xn)
Dangerous for the environment (N)
R-phrases R22, R41, R50/53
S-phrases (S2), S22, S26, S39, S46, S60, S61
Flash point Non-flammable
Related compounds
Other cations Cadmium sulfate
Related compounds Copper(II) sulfate
 YesY (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Zinc sulfate is the inorganic compound with the formula ZnSO4 as well as any of three hydrates. It was historically known as "white vitriol". It is a colorless solid that is a common source of soluble zinc ions.[2]

Contents

Production and reactivity

Zinc sulfate is produced by treating zinc with aqueous sulfuric acid:

Zn + H2SO4 + 7 H2O → ZnSO4(H2O)7 + H2

Pharmaceutical grade zinc sulfate is produced from high purity zinc oxide:

ZnO + H2SO4 + 6 H2O → ZnSO4(H2O)7

In the laboratory, it can also be prepared by adding solid zinc to a copper(II) sulfate solution:

Zn + CuSO4 → ZnSO4 + Cu

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.

Applications

The hydrates, especially the heptahydrate, are the primary forms used commercially. The main application is as a coagulant in the production of rayon. It is also a precursor to the pigment lithopone. Zinc sulfate is used to supply zinc in animal feeds, fertilizers, and agricultural sprays. It is used as in electrolytes for zinc plating, as a mordant in dyeing, as a preservative for skins and leather and in medicine as an astringent and emetic.[2]

Minerals

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).

References

  1. ^ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3. 
  2. ^ a b 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

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Look at other dictionaries:

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