Talk:Potassium manganate

Article structure[edit]

This article resulted from my subdividing Manganate so that we had a real data table on a real compound vs just an anion. So the writing might be a little redundant between the two reports - feel free to revise and parse as you see fit. --Smokefoot 02:41, 20 May 2006 (UTC)[reply]

Dubious comment[edit]

I removed the bold sentence below (my boldening):

In the laboratory, K₂MnO₄ can be synthesized by heating a solution of KMnO₄ in concentrated KOH solution followed by cooling to give green crystals:^[1]

4 KMnO₄ + 4 KOH → 4 K₂MnO₄ + O₂ + 2 H₂O

This reaction illustrates the relatively rare role of hydroxide as a reducing agent. Solutions of K₂MnO₄ are generated by allowing a solution of KMnO₄ in 5–10 M KOH to stir for a day at room temperature followed by removal of MnO₂, which is insoluble.

The bold comment does not make sense given the equation above. Perhaps it was meant for the "opposite" reaction, the disproportionation of K₂MnO₄ into KMnO₄ + MnO₂? --Jorge Stolfi (talk) 19:50, 3 June 2019 (UTC)[reply]

References

^ Nyholm, R. S.; Woolliams, P. R. (1968). "Manganates(VI)". Inorg. Synth. Inorganic Syntheses. 11: 56–61. doi:10.1002/9780470132425.ch11. ISBN 978-0-470-13242-5.

[1] Nyholm, R. S.; Woolliams, P. R. (1968). "Manganates(VI)". Inorg. Synth. Inorganic Syntheses. 11: 56–61. doi:10.1002/9780470132425.ch11. ISBN 978-0-470-13242-5.

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