Potassium hypomanganate
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Potassium hypomanganate
| Potassium hypomanganate | |
|---|---|
|
potassium manganate(V) |
|
| Properties[1] | |
| Molecular formula | K3MnO4 |
| Molar mass | 236.23 g mol−1 |
| Appearance | bright blue solid |
| λmax | 670 nm (ε = 900 dm3 mol−1 cm−1) |
| Related compounds | |
| Other anions | Potassium manganate Potassium permanganate |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
|
| Infobox references | |
Potassium hypomanganate, K3MnO4, also known as potassium manganate(V), is a bright blue salt and a rare example of a manganese(V) compound. It is formed:
- by the reduction of potassium permanganate with excess potassium sulfite;[2][3]
-
- MnO−
4 + SO2−
3 + H2O → MnO3−
4 + SO2−
4 + 2 H+
- MnO−
- by the reduction of potassium manganate with hydrogen peroxide in 10 M potassium hydroxide solution;[4]
-
- 2 MnO2−
4 + H2O2 + 2 OH− → 2 MnO3−
4 + O2 + 2 H2O
- 2 MnO2−
-
- 2 MnO2−
4 + C
8H
7O−
3 + 2 OH− → 2 MnO3−
4 + C
8H
5O−
3 + 2 H2O
- 2 MnO2−
- by disproportionation when manganese dioxide is dissolved in a concentrated solution of potassium hydroxide;[2]
-
- 2 MnO2 + 3 OH− → MnO3−
4 + MnO(OH) + H2O
- 2 MnO2 + 3 OH− → MnO3−
The hypomanganate anion is unstable with respect to disproportionation in all but the most alkaline of solutions:[2][3] estimated electrode potentials at pH 14 are[5][6][7]
- MnO2−
4 + e−
MnO3−
4 E = +0.27 V - MnO3−
4 + e− + 4 H2O MnO2 + 6 OH− E = +0.96 V
The disproportionation is believed to pass through a protonated intermediate,[7] with the acid dissociation constant for the reaction HMnO2−
4 MnO3−
4 + H+ being estimated as pKa = 13.7 ± 0.2.[8] However, K3MnO4 has been cocrystallized with Ca2Cl(PO4), allowing the study of the UV–visible spectrum of the hypomanganate ion.[2][9]
References
- ^ a b Lee, Donald G.; Chen, Tao (1993), "Reduction of manganate(VI) by mandelic acid and its significance for development of a general mechanism of oxidation of organic compounds by high-valent transition metal oxides", J. Am. Chem. Soc. 115 (24): 11231–36, doi:10.1021/ja00077a023.
- ^ a b c d Cotton, F. Albert; Wilkinson, Geoffrey (1980), Advanced Inorganic Chemistry (4th ed.), New York: Wiley, p. 746, ISBN 0-471-02775-8.
- ^ a b Greenwood, Norman N.; Earnshaw, A. (1984). Chemistry of the Elements. Oxford: Pergamon. pp. 1221–22. ISBN 0-08-022057-6..
- ^ Lee, Donald G.; Chen, Tao (1989), "Oxidation of hydrocarbons. 18. Mechanism of the reaction between permanganate and carbon-carbon double bonds", J. Am. Chem. Soc. 111 (19): 7534–38, doi:10.1021/ja00201a039.
- ^ Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. D-134. ISBN 0-8493-0462-8..
- ^ Manganese – compounds – standard reduction potentials, WebElements, http://www.webelements.com/manganese/compounds.html, retrieved 2010-06-26.
- ^ a b Sekula-Brzezińska, K.; Wrona, P. K.; Galus, Z. (1979), "Rate of the MnO4−/MnO42− and MnO42−/MnO43− electrode reactions in alkaline solutions at solid electrodes", Electrochim. Acta 24 (5): 555–63, doi:10.1016/0013-4686(79)85032-X.
- ^ Rush, J. D.; Bielski, B. H. J. (1995), "Studies of Manganate(V), -(VI), and -(VII) Tetraoxyanions by Pulse Radiolysis. Optical Spectra of Protonated Forms", Inorg. Chem. 34 (23): 5832–38, doi:10.1021/ic00127a022.
- ^ Carrington, A.; Symons, M. C. R. (1956), "Structure and reactivity of the oxy-anions of transition metals. Part I. The manganese oxy-anions", J. Chem. Soc.: 3373–80, doi:10.1039/JR9560003373.
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