Talk:Caesium carbonate

Formulation

"This may be used as a way to produce soluble caesium salts." (This Article, regarding the reaction with acids) Caesium carbonate is, on its own, shockingly soluble, as many other caesium salts. Mind you, the only compounds of caesium which are insoluble are very rare complexes with even more rare ligands. I think it would be better to replace the word soluble to other, seeing as Cs₂CO₃ is already soluble like 99% of its salts. --94.189.216.214 (talk) 15:14, 25 June 2010 (UTC)

Agree and changed. Materialscientist (talk) 00:01, 26 June 2010 (UTC)

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Solubilities

The solubilities given for Cesium carbonate in dipolar aprotic solvents (110-723 g / L) are simply wrong. They are taken from a 1984 JOC article (https://pubs.acs.org/doi/pdf/10.1021/jo00180a033), where the data was given in units of "g/10 mL", i.e., the entry for DMSO reads "3.625". A footnote states "Solubilities in g/10 mL determined at ambient temperature by flame photometry". And that is the only experimental detail given on how those numbers were obtained, no procedure, no details of the measurement. In reality the numbers may be 1000 times lower, maybe there was a mixup of units. The fact is that Cs2CO3 is not really soluble in those solvents, except in traces.