Lithium carbonate is an inorganic compound, the lithium salt of carbonic acid with the formula Li2CO3. Lithium carbonate is an important industrial chemical. It is a precursor to compounds used in lithium-ion batteries. Glasses derived from lithium carbonate are useful in ovenware. Lithium carbonate is a common ingredient in both low-fire and high-fire ceramic glaze. It forms low-melting fluxes with silica and other materials. Its alkaline properties are conducive to changing the state of metal oxide colorants in glaze, particularly red iron oxide (Fe2O3). Cement sets more rapidly when prepared with lithium carbonate, and is useful for tile adhesives. When added to aluminium trifluoride, it forms LiF which yields a superior electrolyte for the processing of aluminium.
Rechargeable batteries Lithium carbonate-derived compounds are crucial to lithium-ion batteries. Lithium carbonate may be converted into lithium hydroxide as an intermediate. In practice, two components of the battery are made with lithium compounds: the cathode and the electrolyte. The electrolyte is a solution of lithium hexafluorophosphate, while the cathode uses one of several lithiated structures, the most popular of which are lithium cobalt oxide and lithium iron phosphate.
Medical uses
In 1843, lithium carbonate was used to treat bladder and kidney stones. In 1859, some doctors recommended the compound for a number of ailments, including gout, urinary calculi, rheumatism, mania, depression, and headache. In 1948, John Cade discovered the anti-manic effects of lithium ions. This finding led to lithium carbonate's use as a psychiatric medication to treat mania, the elevated phase of bipolar disorder. Mogens Schou and others continued Cade's research. They found that lithium is effective against both mania and depression, and has preventative effects. Lithium is also unique among medications in that it has anti-suicide properties in people with bipolar disorder or recurrent depression. It has been shown to dramatically reduce the risk of suicide by 87% in clinical trials. In addition to its effects on suicide, lithium also reduces the risk of death from all causes in people with mood disorders. Prescription lithium carbonate from a pharmacy is suitable for use as medicine in humans but industrial lithium carbonate is not since it may contain unsafe levels of toxic heavy metals or other toxicants. After ingestion, lithium carbonate is dissociated into pharmacologically active lithium ions (Li+) and (non-therapeutic) carbonate, with 300 mg of lithium carbonate containing approximately 8 mEq (8 mmol) of lithium ion. The usual dosage of lithium is 600-900 mg/day for the maintenance treatment of bipolar disorder. The exact dose of lithium given varies depending on factors such as the patient's serum lithium concentrations, which must be closely monitored by a physician to avoid lithium toxicity and potential kidney damage (or even kidney failure) from lithium-induced nephrogenic diabetes insipidus. Dehydration and certain drugs, including NSAIDs such as ibuprofen, can increase serum lithium concentrations to unsafe levels whereas other drugs, such as caffeine, may decrease concentrations.
In contrast to the elemental ions sodium, potassium, and calcium, there is no known cellular mechanism specifically dedicated to regulating intracellular lithium. Lithium can enter cells through epithelial sodium channels. Lithium ions interfere with ion transport processes (see "Sodium pump") that relay and amplify messages carried to the cells of the brain. Mania is associated with irregular increases in protein kinase C (PKC) activity within the brain. Lithium carbonate and sodium valproate, another drug conventionally used to treat the disorder, act in the brain by inhibiting PKC's activity and help to produce other compounds that also inhibit the PKC. Lithium carbonate's mood-controlling properties are not fully understood.
Health risks Taking lithium salts has risks and side effects. Extended use of lithium to treat mental disorders has been known to lead to acquired nephrogenic diabetes insipidus. Lithium toxicity can affect the central nervous system and renal system and can be lethal at levels above 2.0 mmol/L. Over a prolonged period, lithium can accumulate in the principal cells of the collecting duct and interfere with antidiuretic hormone (ADH), which regulates the water permeability of principal cells in the collecting tubule. The medullary interstitium of the collecting duct system naturally has a high sodium concentration and attempts to maintain it. There is no known mechanism for cells to distinguish lithium ions from sodium ions, so damage to the kidney's nephrons may occur if lithium concentrations become too high as a result of dehydration, hyponatremia, an unusually low sodium diet, or certain drugs.
Red pyrotechnic colorant Lithium carbonate is used to impart a red color to fireworks.
Properties and reactions Unlike sodium carbonate, which forms at least three 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 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 lithium bicarbonate, which is more soluble:
Li2CO3 + CO2 + H2O ⇌ 2 LiHCO3 The extraction of lithium carbonate at high pressures of CO2 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 Li2CO3. Lithium carbonate, and other carbonates of group 1, do not decarboxylate readily. Li2CO3 decomposes at temperatures around 1300 °C.
Production Lithium carbonate is made from primarily two sources: spodumene and petalite ores, and underground brine pools. About 82,000 tons were produced in 2020, showing significant and consistent growth.
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