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| Names | |
|---|---|
| IUPAC name Lithium carbonate | |
| Other names Dilithium carbonate, Carbolith, Cibalith-S, Duralith, Eskalith, Lithane, Lithizine, Lithobid, Lithonate, Lithotabs Priadel,Zabuyelite | |
| Identifiers | |
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3D model (JSmol) | |
| ChEBI | |
| ChEMBL | |
| ChemSpider |
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| ECHA InfoCard | 100.008.239 |
| KEGG |
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| RTECS number |
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| UNII | |
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| Properties | |
| Li 2CO 3 | |
| Molar mass | 73.89 g/mol |
| Appearance | Odorless white powder |
| Density | 2.11 g/cm3 |
| Melting point | 723 °C (1,333 °F; 996 K) |
| Boiling point | 1,310 °C (2,390 °F; 1,580 K) Decomposes from ~1300 °C |
| |
Solubility product (Ksp) | 8.15×10−4[2] |
| Solubility | Insoluble inacetone,ammonia,alcohol[3] |
| −27.0·10−6 cm3/mol | |
Refractive index (nD) | 1.428[4] |
| Viscosity |
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| Thermochemistry | |
| 97.4 J/mol·K[3] | |
Std molar entropy(S⦵298) | 90.37 J/mol·K[3] |
Std enthalpy of formation(ΔfH⦵298) | −1215.6 kJ/mol[3] |
Gibbs free energy(ΔfG⦵) | −1132.4 kJ/mol[3] |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | Irritant |
| GHS labelling: | |
 [5] | |
| Warning | |
| H302,H319[5] | |
| P305+P351+P338[5] | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 525 mg/kg (oral, rat)[6] |
| Safety data sheet (SDS) | ICSC 1109 |
| Related compounds | |
Othercations | Sodium carbonate Potassium carbonate Rubidium carbonate Caesium carbonate |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Lithium carbonate is aninorganic compound, thelithium salt ofcarbonic acid with theformulaLi
2CO
3. This whitesalt is widely used in processing metal oxides. It is on theWorld Health Organization's List of Essential Medicines[7] for its efficacy in thetreatment ofmood disorders such asbipolar disorder.[8][7]
Lithium carbonate is an importantindustrialchemical. Its main use is as aprecursor to compounds used inlithium-ion batteries.
Glasses derived from lithium carbonate are useful in ovenware. Lithium carbonate is a common ingredient in both low-fire and high-fireceramic glaze. It forms low-meltingfluxes withsilica and other materials. Itsalkaline properties are conducive to changing the state ofmetal oxide colorants inglaze, particularlyred iron oxide (Fe
2O
3).Cement sets more rapidly when prepared with lithium carbonate, and is useful for tileadhesives. When added toaluminium trifluoride, it formsLiF which yields a superiorelectrolyte for the processing ofaluminium.[9]
Lithium carbonate-derived compounds are crucial tolithium-ion batteries. Lithium carbonate may be converted intolithium hydroxide as an intermediate. In practice, two components of the battery are made with lithium compounds: thecathode and theelectrolyte. The electrolyte is a solution oflithium hexafluorophosphate, while the cathode uses one of severallithiated structures, the most popular of which arelithium cobalt oxide andlithium iron phosphate.
In 1843, lithium carbonate was used to treat stones in thebladder. In 1859, some doctors recommended a therapy with lithiumsalts for a number ofailments, includinggout,urinary calculi,rheumatism,mania,depression, andheadache.
In 1948,John Cade discovered the anti-manic effects of lithium ions.[10] This finding led to lithium carbonate's use as apsychiatric medication to treat mania, the elevated phase ofbipolar disorder.Mogens Schou and others continued Cade's research.[11] They found that lithium is effective against both mania and depression, and has preventative effects.[12]
Lithium is also unique among medications in that it has anti-suicide properties in people with bipolar disorder or recurrentdepression. It has been shown to dramatically reduce the risk of suicide by 87% inclinical trials.[13][14] In addition to its effects on suicide, lithium also reduces the risk of death from all causes in people withmood disorders.[15]
Prescription lithium carbonate from apharmacy is suitable for use as medicine in humans but industrial lithium carbonate is not since it may contain unsafe levels oftoxic heavy metals or othertoxicants. After ingestion, lithium carbonate isdissociated intopharmacologically activelithium ions (Li+) and (non-therapeutic)carbonate, with 300 mg of lithium carbonate containing approximately 8 mEq (8 mmol) of lithium ion.[8] The usual dosage of lithium is 600-900 mg/day for the maintenance treatment of bipolar disorder.[16]
The exact dose of lithium given varies depending on factors such as the patient'sserum lithium concentrations, which must be closely monitored by aphysician to avoidlithium toxicity and potentialkidney damage (or evenkidney failure) fromlithium-inducednephrogenic diabetes insipidus.[17][8]Dehydration and certain drugs, includingNSAIDs such asibuprofen, can increase serum lithium concentrations to unsafe levels whereas other drugs, such ascaffeine, may decrease concentrations.
In contrast to the elemental ionssodium,potassium, andcalcium, there is no known cellular mechanism specifically dedicated to regulatingintracellular lithium. Lithium can enter cells throughepithelial sodium channels.[18] Lithium ions interfere with ion transport processes(see "Sodium pump") that relay and amplify messages carried to the cells of the brain.[19] Mania is associated with irregular increases inprotein kinase C (PKC) activity within the brain. Lithium carbonate andsodium 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.[20] Lithium carbonate's mood-controlling properties are not fully understood.[21]
Takinglithium salts has risks and side effects. Extended use of lithium to treat mental disorders has been known to lead to acquirednephrogenic diabetes insipidus.[22]Lithium toxicity can affect thecentral nervous system andrenal system and can be lethal at levels above 2.0 mmol/L.[23][24] Over a prolonged period, lithium can accumulate in theprincipal cells of the collecting duct and interfere withantidiuretic hormone (ADH), which regulates the water permeability of principal cells in the collecting tubule.[18] Themedullary interstitium of thecollecting 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 thekidney'snephrons may occur if lithium concentrations become too high as a result ofdehydration,hyponatremia, an unusuallylow sodium diet, or certain drugs.
Lithium carbonate is used toimpart a red color to fireworks.[25]
Unlikesodium carbonate, which forms at least threehydrates, lithium carbonate exists only in theanhydrous form. Its solubility in water is low relative to other lithium salts. The isolation of lithium from aqueous extracts of lithiumores capitalizes on this poor solubility. Its apparent solubility increases 10-fold under a mild pressure ofcarbon dioxide; this effect is due to the formation of themetastablelithium bicarbonate, which is more soluble:[9][26]
The extraction of lithium carbonate at high pressures ofCO
2 and itsprecipitation upon depressurizing is the basis of the Quebec process.
Lithium carbonate can also be purified by exploiting its diminishedsolubility in hot water. Thus, heating a saturated aqueous solution causescrystallization ofLi
2CO
3.[27]
Lithium carbonate, and other carbonates ofgroup 1, do notdecarboxylate readily.Li
2CO
3 decomposes at temperatures around 1300 °C.
Lithium is extracted from primarily two sources:spodumene inpegmatite deposits, and lithium salts in undergroundbrine pools. About 82,000 tons were produced in 2020, showing significant and consistent growth.[28]
In theSalar de Atacama in theAtacama Desert of Northern Chile, lithium carbonate and lithium hydroxide are produced frombrine.[29][30]
The process pumps lithium rich brine from below ground intoshallow pans for evaporation. The brine contains many different dissolved ions, and as their concentration increases, salts precipitate out of solution and sink. The remainingsupernatant liquid is used for the next step. The sequence of pans may vary depending on the concentration of ions in a particular source of brine.
In the first pan,halite (sodium chloride or common salt) crystallizes. This has little economic value and is discarded. The supernatant, with ever increasing concentration of dissolved solids, is transferred successively to thesylvinite (sodium potassium chloride) pan, thecarnallite (potassium magnesium chloride) pan and finally a pan designed to maximize the concentration of lithium chloride. The process takes about 15 months. The concentrate (30-35% lithium chloride solution) is trucked to Salar del Carmen. There,boron and magnesium are removed (typically residual boron is removed by solvent extraction and/orion exchange and magnesium by raising thepH above 10 withsodium hydroxide)[31] then in the final step, by addition ofsodium carbonate, the desired lithium carbonate is precipitated out, separated, and processed.
Some of theby-products from the evaporation process may also have economic value.
There is considerable attention to the use of water in this water poor region.SQM commissioned alife-cycle analysis (LCA) which concluded that water consumption for SQM's lithium hydroxide and carbonate is significantly lower than the average consumption by production from the main ore-based process, usingspodumene. A more general LCA suggests the opposite for extraction from reservoirs.[32]
The majority of brine based production is in the "lithium triangle" in South America.
A potential source of lithium is theleachates ofgeothermal wells, carried to the surface.[33] Recovery of lithium has been demonstrated in the field; the lithium is separated by simpleprecipitation andfiltration.[34] The process andenvironmental costs are primarily those of the already-operating well; net environmental impacts may thus be positive.[35]
The brine ofUnited Downs Deep Geothermal Power project nearRedruth is claimed byCornish Lithium to be valuable due to its high lithium concentration (220 mg/L) with low magnesium (<5 mg/L) and total dissolved solids content of <29g/L,[36] and a flow rate of 40-60l/s.[32]
α-spodumene is roasted at 1100 °C for 1h to make β-spodumene, then roasted at 250 °C for 10 minutes withsulfuric acid.[37][29]
As of 2020, Australia was the world's largest producer of lithium intermediates,[38] all based on spodumene.
In recent years mining companies have begun exploration oflithium projects throughoutNorth America,South America andAustralia to identify economic deposits that can potentially bring new supplies of lithium carbonate online to meet the growingdemand for the product.[39]
In 2020Tesla Motors announced a revolutionary process to extract lithium fromclay in Nevada using only salt and no acid. This was met with skepticism.[40]
A few small companies arerecycling spent batteries, focusing on recoveringcopper andcobalt. Some recover lithium carbonate alongside the compound Li2Al4(CO3)(OH)12⋅3H2Oalso.[41][42][43][44]
In April 2017 MGX Minerals reported it had received independent confirmation of its rapidlithium extraction process to recover lithium and other valuable minerals fromoil and gas wastewaterbrine.[45]
Electrodialysis has been proposed to extract lithium from seawater, but it is not commercially viable.[46]
Natural lithium carbonate is known aszabuyelite.[47] This mineral is connected with deposits of somesalt lakes and somepegmatites.[48]
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