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Potassium ferrate
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Potassium ferrate
Potassium ferrate is an inorganic compound with the formula K2FeO4. It is the potassium salt of ferric acid. Potassium ferrate is a powerful oxidizing agent with applications in green chemistry, organic synthesis, and cathode technology.
Generally, there are three ways to produce hexavalent iron: dry oxidation, wet oxidation, and electrochemical synthesis.[citation needed] The methods used to produce potassium ferrate are similar to those used to produce sodium ferrate and barium ferrate.
The dry oxidation method entails heating or melting iron oxides in an alkaline, oxidizing environment, most commonly created with potassium nitrate or potassium peroxide and potassium hydroxide. The combination of high temperature (200–800 °C) and oxidizing agents presents an explosion hazard that has led many researchers to believe this method of production is not suitable from a safety viewpoint, although many attempts have been made to overcome this problem.
In the wet oxidation method, K2FeO4 is prepared by oxidizing an alkaline solution of an iron(III) salt. Generally, this method employs ferric (FeIII) salts such as iron(III) hydroxide as the source of iron ions, an oxidizing agent such as hypochlorite (in the form of Ca(ClO)2 or NaClO) or chlorine (Cl2) and a strong alkali such as sodium hydroxide, sodium carbonate (NaOH, Na2CO3) or potassium hydroxide (KOH) to increase the pH of the solution.
Electrochemical methods used to synthesize potassium ferrate usually consist of an iron anode which electrolyzes a KOH solution.
Potassium ferrate is a dark purple crystalline solid that dissolves in water to form a reddish-purple solution. The salt is paramagnetic and 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. Potassium ferrate decomposes rapidly in neutral and acidic water, e.g.:
In alkaline solution and as a dry solid, K2FeO4 is stable. Under the acidic conditions, the oxidation–reduction potential of the ferrate(VI) ions (2.2 V) is greater than that of ozone (2.0 V).
Like sodium ferrate, K2FeO4 generally does not generate environmentally toxic by-products and can be used in water treatment processes.[citation needed] It can act as:
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Potassium ferrate
Potassium ferrate is an inorganic compound with the formula K2FeO4. It is the potassium salt of ferric acid. Potassium ferrate is a powerful oxidizing agent with applications in green chemistry, organic synthesis, and cathode technology.
Generally, there are three ways to produce hexavalent iron: dry oxidation, wet oxidation, and electrochemical synthesis.[citation needed] The methods used to produce potassium ferrate are similar to those used to produce sodium ferrate and barium ferrate.
The dry oxidation method entails heating or melting iron oxides in an alkaline, oxidizing environment, most commonly created with potassium nitrate or potassium peroxide and potassium hydroxide. The combination of high temperature (200–800 °C) and oxidizing agents presents an explosion hazard that has led many researchers to believe this method of production is not suitable from a safety viewpoint, although many attempts have been made to overcome this problem.
In the wet oxidation method, K2FeO4 is prepared by oxidizing an alkaline solution of an iron(III) salt. Generally, this method employs ferric (FeIII) salts such as iron(III) hydroxide as the source of iron ions, an oxidizing agent such as hypochlorite (in the form of Ca(ClO)2 or NaClO) or chlorine (Cl2) and a strong alkali such as sodium hydroxide, sodium carbonate (NaOH, Na2CO3) or potassium hydroxide (KOH) to increase the pH of the solution.
Electrochemical methods used to synthesize potassium ferrate usually consist of an iron anode which electrolyzes a KOH solution.
Potassium ferrate is a dark purple crystalline solid that dissolves in water to form a reddish-purple solution. The salt is paramagnetic and 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. Potassium ferrate decomposes rapidly in neutral and acidic water, e.g.:
In alkaline solution and as a dry solid, K2FeO4 is stable. Under the acidic conditions, the oxidation–reduction potential of the ferrate(VI) ions (2.2 V) is greater than that of ozone (2.0 V).
Like sodium ferrate, K2FeO4 generally does not generate environmentally toxic by-products and can be used in water treatment processes.[citation needed] It can act as:
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