Potassium ferrate
Names | |
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IUPAC name
Potassium ferrate(VI)
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Other names
Potassium ferrate
Dipotassium ferrate | |
Identifiers | |
3D model (
JSmol ) |
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PubChem CID
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Properties | |
K2FeO4 | |
Molar mass | 198.0392 g/mol |
Appearance | Dark purple solid |
Density | 2.829 g/cm3 |
Melting point | >198 °C (decomposes) |
soluble in 1M KOH | |
which? ]
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reacts with most solvents |
Structure | |
K2SO4 motif | |
Tetrahedral | |
0 D | |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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Oxidizer |
GHS labelling: | |
[1] | |
Danger[1] | |
H272[1] | |
P210, P220, P221, P280, P370+P378, P501[1] | |
Flash point | non-combustible |
Safety data sheet (SDS) | External SDS |
Related compounds | |
Other anions
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K2MnO4 K2CrO4 K2RuO4 |
Other cations
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BaFeO4 Na2FeO4 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Potassium
Synthesis and structure
Georg Ernst Stahl (1660 – 1734) first discovered that the residue formed by igniting a mixture of potassium nitrate (saltpetre) and iron powder dissolved in water to give a purple solution. Edmond Frémy (1814 – 1894) later discovered that fusion of potassium hydroxide and iron(III) oxide in air produced a compound that was soluble in water:
- 8 KOH + 2 Fe2O3 + 3 O2 → 4 K2FeO4 + 4 H2O
The composition corresponded to that of
- 3 ClO− + 3 Fe(OH)3(H2O)3 + 4 K+ + 4 OH− → 3 Cl− + 2 K2FeO4 + 11 H2O
The salt is isostructural with K2MnO4, K2SO4, and K2CrO4. The solid consists of K+ and the tetrahedral FeO2−4 anion, with Fe-O distances of 1.66 Å.[3] The poorly soluble barium salt, BaFeO4, is also known.
Properties and applications
The main difficulty with the use of K2FeO4 is that it is often too reactive, as indicated by the fact that it decomposes in contact with water, especially in acidic water:[4]
- 4 K2FeO4 + 4 H2O → 3 O2 + 2 Fe2O3 + 8 KOH
At high pH, aqueous solutions are stable. The deep purple solutions are similar in appearance to potassium permanganate (KMnO4). It is stronger oxidizing agent than the latter. As a dry solid, K2FeO4 is stable.
Because the side products of its redox reactions are rust-like iron oxides, K2FeO4 has been described as a "
K2FeO4 has also attracted attention as a potential
Stabilised forms of potassium ferrate have been proposed for the removal of transuranic species, both dissolved and suspended, from aqueous solutions. Tonnage quantities were proposed to help remediate the effects of the Chernobyl disaster in Belarus. This new technique was successfully applied for the removal of a broad range of heavy metals.[citation needed]
Work on the use of potassium ferrate precipitation of transuranics and heavy metals was carried out in the Laboratories of IC Technologies Inc. in partnership with ADC Laboratories, in 1987 though 1992. The removal of the transuranic species were done on samples from various Dept. of Energy nuclear sites in the USA.[citation needed]
It has been proposed as a bleeding stopper for fresh wounds.[7][8]
References
- ^ a b c d "Potassium Ferrate". American Elements. Retrieved June 13, 2019.
- ^ Schreyer, J. M.; Thompson, G. W.; Ockerman, L. T. (1953). "Potassium Ferrate(VI)" (PDF). In Bailar, John C. (ed.). Inorganic Syntheses. Vol. IV. pp. 164–168.
- .
- ISBN 0-12-352651-5.
- .
- ISSN 1093-0191.
- ^ "How WoundSeal Works". WoundSeal. 2016.
- ^ WO application 2014153566, John Hen; Talmadge Kelly Keene & Mark Travi, "Hemostatic device and method", published 2014-09-25, assigned to Biolife, LLC