Editing Lithium carbonate (section)

==Properties and reactions ==
Unlike [[sodium carbonate]], which forms at least three [[water of crystallization|hydrates]], lithium carbonate exists only in the anhydrous form. Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithium [[ore]]s capitalizes on this poor solubility. Its apparent solubility increases 10-fold under a mild pressure of [[carbon dioxide]]; this effect is due to the formation of the [[Metastability|metastable]] [[lithium bicarbonate]], which is more soluble:<ref name=Ullmann/><ref>Spellman, F. R. (2023). ''The Science of Lithium''. CRC Press.</ref>
:{{chem|Li|2|CO|3}} + {{chem|CO|2}} + {{chem|H|2|O}}   {{eqm}}   2 {{chem|LiHCO|3}}
The extraction of lithium carbonate at high pressures of {{chem|CO|2}} and its precipitation upon depressurizing is the basis of the Quebec process.

Lithium carbonate can also be purified by exploiting its diminished solubility in hot water.  Thus, heating a saturated aqueous solution causes crystallization of {{chem|Li|2|CO|3}}.<ref>{{cite book | last1 = Caley | first1 = E. R. | last2 = Elving | first2 = P. J. | title = Inorganic Syntheses | year = 1939 | chapter = Purification of Lithium Carbonate | volume = 1 | pages = 1–2 | doi = 10.1002/9780470132326.ch1 | isbn = 978-0-470-13232-6 }}</ref>

Lithium carbonate, and other carbonates of [[alkali metal|group 1]], do not [[decarboxylate]] readily. {{chem|Li|2|CO|3}} decomposes at temperatures around 1300&nbsp;°C.