Potassium selenate

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Potassium selenate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.029.286 Edit this at Wikidata
EC Number
  • 232-214-7
RTECS number
  • VS6600000
UNII
  • InChI=1S/2K.H2O4Se/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
    Key: YAZJAPBTUDGMKO-UHFFFAOYSA-L
  • [K+].[K+].[O-][Se]([O-])(=O)=O
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)
1.539
Structure
orthorhombic
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
1
0
Related compounds
Other anions
 Potassium sulfate
Other cations
 Sodium selenate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Potassium selenate, K
2SeO
4, is an odorless, white solid that forms as the potassium salt of selenic acid.

Preparation[edit]

Potassium 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[edit]

Potassium selenate can be used to produce selenium trioxide.[4] It can also use to treat selenium deficiency in livestock.[5]

References[edit]

  1. ^ "Potassium Selenate K2SeO4 Molecular Weight". EndMemo. Retrieved 2019-09-03.
  2. ^ "Potassium Selenate". American Elements. Retrieved 2019-09-03.
  3. ^ Rosenfeld, Irene; Beath, Orville A. (2013). Selenium: Geobotany, Biochemistry, Toxicity, and Nutrition. Elsevier Science. p. 305. ISBN 978-1-4832-7590-1.
  4. ^ Sicius, Hermann (2015). Chalkogene : elemente der sechsten hauptgruppe (in German). Springer. p. 28. ISBN 978-3-658-10522-8. OCLC 919684689.
  5. ^ Wolfgang Löscher, Angelika Richter, Heidrun Potschka (2014). Pharmakotherapie bei Haus- und Nutztieren (in German). Stuttgart: Enke. ISBN 978-3-8304-1250-2. OCLC 891036290.{{cite book}}: CS1 maint: multiple names: authors list (link)
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