Potassium selenate, K
2SeO
4, is an odorless, white solid that forms as the potassium salt of selenic acid.
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3D model (JSmol)
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| ECHA InfoCard | 100.029.286 |
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CompTox Dashboard (EPA)
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| Properties | |
| K 2SeO 4 | |
| Molar mass | 221.2 g/mol[1] |
| Appearance | colorless crystals hygroscopic |
| Odor | odorless |
| Density | 3.07 g/cm3[2] |
| 1.07 g/ml (0 °C) 1.11 g/ml (20 °C) 1.22 g/ml (100 °C) | |
Refractive index (nD)
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1.539 |
| Structure | |
| orthorhombic | |
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Other anions
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Potassium sulfate |
Other cations
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Sodium selenate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
editPotassium selenate is produced by the reaction of selenium trioxide and potassium hydroxide.
- SeO3 + 2 KOH → K2SeO4 + H2O
Alternatively, it can be made by treating selenous acid with potassium hydroxide, followed by oxidation of the resulting potassium selenite with bromine water.[3]
- H2SeO3 + 2 KOH → K2SeO3 + 2 H2O
- K2SeO3 + 2 KOH + Br2 → K2SeO4 + 2 KBr + H2O
Uses
editPotassium selenate can be used to produce selenium trioxide.[4] It can also use to treat selenium deficiency in livestock.[5]
References
edit- ^ "Potassium Selenate K2SeO4 Molecular Weight". EndMemo. Retrieved 2019-09-03.
- ^ "Potassium Selenate". American Elements. Retrieved 2019-09-03.
- ^ Rosenfeld, Irene; Beath, Orville A. (2013). Selenium: Geobotany, Biochemistry, Toxicity, and Nutrition. Elsevier Science. p. 305. ISBN 978-1-4832-7590-1.
- ^ Sicius, Hermann (2015). Chalkogene : elemente der sechsten hauptgruppe (in German). Springer. p. 28. ISBN 978-3-658-10522-8. OCLC 919684689.
- ^ Wolfgang Löscher, Angelika Richter, Heidrun Potschka (2014). Pharmakotherapie bei Haus- und Nutztieren (in German). Stuttgart: Enke. ISBN 978-3-8304-1250-2. OCLC 891036290.
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