Zinc sulfate
| Zinc sulfate | |
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Zinc sulfate |
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Other names
White vitriol |
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| Identifiers | |
| CAS number | 7733-02-0  , 7446-19-7 (monohydrate) 13986-24-8 (hexahydrate) 7446-20-0 (heptahydrate) |
| PubChem | 24424 |
| ChemSpider | 22833 |
| UNII | 0J6Z13X3WO |
| EC number | 231-793-3 |
| UN number | 3077 |
| ChEBI | CHEBI:35176 |
| ChEMBL | CHEMBL1200929  |
| RTECS number | ZH5260000 |
| ATC code | A12 |
| Jmol-3D images | Image 1 |
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| 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 °C decomp. (anhydrous) |
| Boiling point |
740 °C (anhydrous) |
| Solubility in water | 57.7 g/100 mL, anhydrous (20 °C)[1] |
| Solubility | alcohols |
| Refractive index (nD) | 1.658 (anhydrous), 1.4357 (heptahydrate) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−983 kJ·mol−1[2] |
| Standard molar entropy S |
120 J·mol−1·K−1[2] |
| 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 sulfateManganese sulfate |
| Related compounds | Copper(II) sulfate |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| 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.[3]
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[edit] 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.
[edit] 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.[3]
[edit] 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).
[edit] References
- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A23. ISBN 061894690X.
- ^ 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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