Talk:Lithium: Difference between revisions

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==Chemistry==

Unlike sodium carbonate, which forms at least three hydrates, lithium carbonate exists only in the anhydrous form.[13] Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithium ores 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 metastable bicarbonate, which is more soluble: ~~Li2CO3~~ + ~~CO2~~ + ~~H2O~~ ⇌ 2 ~~LiHCO3~~

Unlike sodium carbonate, which forms at least three hydrates, lithium carbonate exists only in the anhydrous form.[13] Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithium ores 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 metastable bicarbonate, which is more soluble: Li2CO3 + CO2 + H2O ⇌ 2 LiHCO3

The extraction of lithium carbonate at high pressures of CO2 and its precipitation upon depressuring 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 ~~Li2CO3~~.

Lithium carbonate can also be purified by exploiting its diminished solubility in hot water. Thus, heating a saturated aqueous solution causes crystallization of Li2CO3.

Lithium carbonate, and other carbonates of group 1, do not decarboxylate readily. ~~Li2CO3~~ decomposes at temperatures around 1300 °C.

Lithium carbonate, and other carbonates of group 1, do not decarboxylate readily. Li2CO3 decomposes at temperatures around 1300 °C.

==Pharmacology==

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 ==Chemistry==
 {{chemistry}}
-Unlike sodium carbonate, which forms at least three hydrates, lithium carbonate exists only in the anhydrous form.[13] Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithium ores 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 metastable bicarbonate, which is more soluble: Li2CO3 + CO2 + H2O ⇌ 2 LiHCO3
+Unlike sodium carbonate, which forms at least three hydrates, lithium carbonate exists only in the anhydrous form.[13] Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithium ores 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 metastable bicarbonate, which is more soluble: Li<sub>2</sub>CO<sub>3</sub>  + CO<sub>2</sub> + H<sub>2</sub>O ⇌ 2 LiHCO<sub>3</sub>
 The extraction of lithium carbonate at high pressures of CO2 and its precipitation upon depressuring 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 Li2CO3.
+Lithium carbonate can also be purified by exploiting its diminished solubility in hot water. Thus, heating a saturated aqueous solution causes crystallization of Li<sub>2</sub>CO<sub>3</sub>.
-Lithium carbonate, and other carbonates of group 1, do not decarboxylate readily. Li2CO3 decomposes at temperatures around 1300 °C.
+Lithium carbonate, and other carbonates of group 1, do not decarboxylate readily.  Li<sub>2</sub>CO<sub>3</sub> decomposes at temperatures around 1300 °C.
 ==Pharmacology==