| Revision as of 12:15, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 476578369 of page Lithium_carbonate for the Chem/Drugbox validation project (updated: 'ChEMBL'). |
Latest revision as of 01:21, 30 October 2024 edit Randy Kryn (talk | contribs)Extended confirmed users286,121 edits →From underground brine reservoirs: uppercasing per direct link (Atacama Desert) |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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| verifiedrevid = 462092421 |
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| verifiedrevid = 476992822 |
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| Name = Lithium carbonate |
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| ImageFile = Lithium carbonate.jpg |
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| Name = Lithium carbonate |
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| ImageSize = 225px |
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| ImageSize = 150 |
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| ImageName = Lithium carbonate |
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| ImageFile1 = Lithium-carbonate-xtal-1979-Mercury-3D-sf.png |
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| ImageSize1 = 200 |
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| IUPACName = Lithium carbonate |
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| ImageFile2 = ] ] ] |
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| OtherNames = Dilithium carbonate, Carbolith, Cibalith-S, Duralith, Eskalith, Lithane, Lithizine, Lithobid, Lithonate, Lithotabs Priadel, ] |
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| ImageFile3 = Lithium carbonate A.jpg |
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| Section1 = {{Chembox Identifiers |
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| ImageName = Lithium carbonate |
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| IUPACName = Lithium carbonate |
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| OtherNames = Dilithium carbonate, Carbolith, Cibalith-S, Duralith, Eskalith, Lithane, Lithizine, Lithobid, Lithonate, Lithotabs Priadel, ] |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 10654 |
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| ChemSpiderID = 10654 |
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| UNII = 2BMD2GNA4V |
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| UNII = 2BMD2GNA4V |
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| ChEMBL_Ref = {{ebicite|changed|EBI}} |
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| ChEMBL_Ref = {{ebicite|changed|EBI}} |
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| ChEMBL = <!-- blanked - oldvalue: 1200826 --> |
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| ChEMBL = 1200826 |
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| InChI = 1/CH2O3.2Li/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 |
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| InChI = 1/CH2O3.2Li/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 |
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| InChIKey = XGZVUEUWXADBQD-NUQVWONBAY |
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| InChIKey = XGZVUEUWXADBQD-NUQVWONBAY |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 11125 |
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| PubChem = 11125 |
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| RTECS = OJ5800000 |
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| RTECS = OJ5800000 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG = D00801 |
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| KEGG = D00801 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = Li<sub>2</sub>CO<sub>3</sub> |
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| Formula = {{chem|Li|2|CO|3}} |
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| MolarMass = 73.891 g/mol |
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| MolarMass = 73.89 g/mol |
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| Appearance = Odorless white powder |
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| Appearance = Odorless white powder |
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| Density = 2.11 g/cm<sup>3</sup> |
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| Density = 2.11{{nbsp}}g/cm<sup>3</sup> |
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| MeltingPtC = 723 |
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| MeltingPtC = 723 |
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| BoilingPtC = 1310 |
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| BoilingPtC = 1310 |
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| BoilingPt_notes = <br />Decomposes from ~1300 °C |
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| Boiling_notes = decomp. |
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| Solubility = {{ubl |
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| Solubility = 15.4 g/L (0 °C) <br /> 13.2 g/L (20 °C) <br /> 7.2 g/L (100 °C) |
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| 1.54{{nbsp}}g/100{{nnbsp}}mL (0{{nbsp}}°C) |
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| SolubleOther = insoluble in ] and ] |
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| 1.43{{nbsp}}g/100{{nnbsp}}mL (10{{nbsp}}°C) |
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| RefractIndex = 1.428 <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> |
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| 1.29{{nbsp}}g/100{{nnbsp}}mL (25{{nbsp}}°C) |
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| 1.08{{nbsp}}g/100{{nnbsp}}mL (40{{nbsp}}°C) |
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| 0.69{{nbsp}}g/100{{nnbsp}}mL (100{{nbsp}}°C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand}}</ref> |
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}} |
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| SolubleOther = Insoluble in ], ], ]<ref name=chemister /> |
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| Section4 = {{Chembox Thermochemistry |
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| SolubilityProduct = 8.15{{e|−4}}<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1-138-56163-2 |pages=5–188|edition=99 |language=English}}</ref> |
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| DeltaHf = −16.46 kJ/g |
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| RefractIndex = 1.428<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> |
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| DeltaHc = |
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| Entropy = |
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| Viscosity = {{ubl |
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| 4.64{{nbsp}}cP (777{{nbsp}}°C) |
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| HeatCapacity = 1.341 J/(g·K) |
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| 3.36{{nbsp}}cP (817{{nbsp}}°C)<ref name=chemister /> |
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}} |
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| MagSus = −27.0·10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol |
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| Section7 = {{Chembox Hazards |
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}} |
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| ExternalMSDS = |
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| Section4 = {{Chembox Thermochemistry |
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| EUIndex = Not listed |
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| DeltaGf = −1132.4{{nbsp}}kJ/mol<ref name=chemister>{{cite web |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=608 |title=lithium carbonate |website=Chemister.ru |date=2007-03-19 |access-date=2017-01-02 |archive-date=2017-08-31 |archive-url=https://web.archive.org/web/20170831090748/http://chemister.ru/Database/properties-en.php?dbid=1&id=608 |url-status=dead }}</ref> |
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| MainHazards = irritant |
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| DeltaHf = −1215.6{{nbsp}}kJ/mol<ref name=chemister /> |
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| RPhrases = |
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| SPhrases = |
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| DeltaHc = |
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| Entropy = 90.37{{nbsp}}J/mol·K<ref name=chemister /> |
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| HeatCapacity = 97.4{{nbsp}}J/mol·K<ref name=chemister /> |
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}} |
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| Section7 = {{Chembox Hazards |
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| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=752843|name=Lithium carbonate|accessdate=2014-06-03}}</ref> |
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| GHSSignalWord = Warning |
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| HPhrases = {{H-phrases|302|319}}<ref name="sigma" /> |
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| PPhrases = {{P-phrases|305+351+338}}<ref name="sigma" /> |
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| ExternalSDS = |
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| MainHazards = Irritant |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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| LD50 = 525 mg/kg (oral, rat)<ref>{{cite web |author=Michael Chambers |url=https://chem.nlm.nih.gov/chemidplus/rn/554-13-2 |title=ChemIDplus - 554-13-2 - XGZVUEUWXADBQD-UHFFFAOYSA-L - Lithium carbonate [USAN:USP:JAN] - Similar structures search, synonyms, formulas, resource links, and other chemical information |website=Chem.sis.nlm.nih.gov |access-date=2017-01-02 |archive-date=2017-01-17 |archive-url=https://web.archive.org/web/20170117192414/https://chem.nlm.nih.gov/chemidplus/rn/554-13-2 |url-status=live }}</ref> |
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| LD50 = 525 mg/kg |
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| Section8 = {{Chembox Related |
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| Section8 = {{Chembox Related |
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| OtherCations = ]<br/>]<br/>]<br/>] |
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| OtherCations = ]<br /> ]<br /> ]<br /> ] |
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'''Lithium carbonate''' is an ], the ] of ] with the ] {{chem|Li|2|CO|3}}. This white ] is widely used in processing metal oxides. It is on the ]<ref name="WHO23rd">{{cite book | vauthors = ((World Health Organization)) | title = The selection and use of essential medicines 2023: web annex A: World Health Organization model list of essential medicines: 23rd list (2023) | year = 2023 | hdl = 10665/371090 | author-link = World Health Organization | publisher = World Health Organization | location = Geneva | id = WHO/MHP/HPS/EML/2023.02 | hdl-access=free }}</ref> for its efficacy in the ] of ]s such as ].<ref name=FDALithiumCarbonateHighlights /><ref name=WHO23rd /> |
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==Uses== |
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Lithium carbonate is an important ] ]. Its main use is as a precursor to compounds used in lithium-ion batteries. |
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Glasses derived from lithium carbonate are useful in ovenware. Lithium carbonate is a common ingredient in both low-fire and high-fire ]. It forms low-melting ]es with ] and other materials. Its ] properties are conducive to changing the state of metal oxide colorants in ], particularly red iron oxide ({{chem|Fe|2|O|3}}). Cement sets more rapidly when prepared with lithium carbonate, and is useful for tile ]s. When added to ], it forms ] which yields a superior ] for the processing of ].<ref name=Ullmann>{{cite encyclopedia|author=Ulrich Wietelmann |author2=Richard J. Bauer |title=Lithium and Lithium Compounds|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|year=2005|publisher=Wiley-VCH|location=Weinheim|doi=10.1002/14356007.a15_393|isbn=3-527-30673-0}}</ref> |
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===Rechargeable batteries=== |
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Lithium carbonate-derived compounds are crucial to ]. Lithium carbonate may be converted into ] as an intermediate. In practice, two components of the battery are made with lithium compounds: the ] and the ]. The electrolyte is a solution of ], while the cathode uses one of several lithiated structures, the most popular of which are ] and ]. |
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] |
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===Medical uses=== |
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{{main|Lithium (medication)}} |
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In 1843, lithium carbonate was used to treat stones in the ]. In 1859, some doctors recommended a therapy with lithium ] for a number of ], including ], ], ], ], ], and ]. |
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In 1948, ] discovered the anti-manic effects of lithium ions.<ref name="who-cade-treat-mania">{{Cite journal |last=Cade|first=J. F. |date=2000 |title=Lithium salts in the treatment of psychotic excitement. 1949. |journal=Bulletin of the World Health Organization |volume=78 |issue=4 |pages=518–520 |issn=0042-9686 |pmc=2560740 |pmid=10885180 }}</ref> This finding led to lithium carbonate's use as a ] to treat mania, the elevated phase of ]. Prescription lithium carbonate from a ] is suitable for use as medicine in humans but industrial lithium carbonate is not since it may contain unsafe levels of ]s or other ]s. After ingestion, lithium carbonate is ] into ] ] ions (Li<sup>+</sup>) and (non-therapeutic) ], with 300 ] of lithium carbonate containing approximately 8 ] (8 ]) of lithium ion.<ref name=FDALithiumCarbonateHighlights>{{Cite web|title=Lithium Carbonate Medication Guide|url=https://www.accessdata.fda.gov/drugsatfda_docs/label/2018/017812s031,018421s031,018558s026lbl.pdf|url-status=live|archive-url=https://archive.today/20220127181022/https://www.accessdata.fda.gov/drugsatfda_docs/label/2020/017812s034,018421s033,018558s028lbl.pdf|archive-date=27 January 2022|access-date=27 January 2022|website=U.S. FDA}}</ref> According to the ] (FDA), 300–600 mg of lithium carbonate taken two to three times daily is typical for maintenance of bipolar I disorder in adults,<ref name=FDALithiumCarbonateHighlights /> where the exact dose given varies depending on factors such as the patient's serum lithium concentrations, which must be closely monitored by a ] to avoid ] and potential ] (or even ]) from ] ].<ref name=Amdisen1978>{{cite journal|author=Amdisen A.|title=Clinical and serum level monitoring in lithium therapy and lithium intoxication|journal=J. Anal. Toxicol.|volume=2|issue=5|pages=193–202|year=1978|doi=10.1093/jat/2.5.193}}</ref><ref name=FDALithiumCarbonateHighlights /> ] and certain drugs, including ] such as ], can increase serum lithium concentrations to unsafe levels whereas other drugs, such as ], may decrease concentrations. In contrast to the elemental ions ], ], and ], there is no known cellular mechanism specifically dedicated to regulating ] lithium. |
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Lithium can enter cells through ]s.<ref name=UpToDateRenalToxicity /> Lithium ions interfere with ion transport processes {{crossreference|(see "]")}} that relay and amplify messages carried to the cells of the brain.<ref>{{cite web |url=http://www.medicinenet.com/lithium/article.htm |title=lithium, Lithobid: Drug Facts, Side Effects and Dosing |website=Medicinenet.com |date=2016-06-17 |access-date=2017-01-02 |archive-date=2016-12-31 |archive-url=https://web.archive.org/web/20161231153214/http://www.medicinenet.com/lithium/article.htm |url-status=live }}</ref> Mania is associated with irregular increases in ] (PKC) activity within the brain. Lithium carbonate and ], another drug traditionally 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.<ref>{{cite journal |last1=Yildiz |first1=A |last2=Guleryuz |first2=S |last3=Ankerst |first3=DP |last4=Ongür |first4=D |last5=Renshaw |first5=PF |title=Protein kinase C inhibition in the treatment of mania: a double-blind, placebo-controlled trial of tamoxifen |journal=Archives of General Psychiatry |volume=65 |issue=3 |pages=255–63 |year=2008 |pmid=18316672 |doi=10.1001/archgenpsychiatry.2007.43 |url=http://mediatum.ub.tum.de/doc/1185490/document.pdf |doi-access=free }}{{Dead link|date=October 2022 |bot=InternetArchiveBot |fix-attempted=yes }}</ref> Lithium carbonate's mood-controlling properties are not fully understood.<ref> {{Webarchive|url=https://web.archive.org/web/20181219001229/https://pubchem.ncbi.nlm.nih.gov/compound/lithium_carbonate |date=2018-12-19 }} at PubChem</ref> |
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====Health risks==== |
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Taking ] has risks and side effects. Extended use of lithium to treat mental disorders has been known to lead to acquired ].<ref>{{cite journal |author1=Richard T. Timmer |author2=Jeff M. Sands |url=http://jasn.asnjournals.org/content/10/3/666.short |title=Lithium Intoxication |journal=Journal of the American Society of Nephrology |date=1999-03-01 |volume=10 |issue=3 |pages=666–674 |doi=10.1681/ASN.V103666 |pmid=10073618 |access-date=2017-01-02 |doi-access=free |archive-date=2017-01-08 |archive-url=https://web.archive.org/web/20170108195724/http://jasn.asnjournals.org/content/10/3/666.short |url-status=live }}</ref> Lithium ] can affect the ] and ] and can be lethal.<ref>{{cite journal|doi=10.1001/archinte.149.1.36|last1=Simard|pmid=2492186|first1=M|year=1989|pages=36–46|issue=1|last2=Gumbiner|volume=149|journal=Archives of Internal Medicine|first2=B|last3=Lee|first3=A|last4=Lewis|first4=H|last5=Norman|first5=D|title=Lithium carbonate intoxication. A case report and review of the literature|url=http://archinte.highwire.org/cgi/reprint/149/1/36.pdf|access-date=2010-09-11|archive-url=https://web.archive.org/web/20110726151128/http://archinte.highwire.org/cgi/reprint/149/1/36.pdf|archive-date=2011-07-26}}</ref> Over a prolonged period, lithium can accumulate in the ] of the collecting duct and interfere with ] (ADH), which regulates the water permeability of principal cells in the collecting tubule.<ref name=UpToDateRenalToxicity>{{cite web|last=Lerma|first=Edgar V.|title=Renal toxicity of lithium|work=]|access-date=8 March 2022|url=https://www.uptodate.com/contents/renal-toxicity-of-lithium|archive-date=8 March 2022|archive-url=https://web.archive.org/web/20220308205106/https://www.uptodate.com/contents/renal-toxicity-of-lithium|url-status=live}}</ref> The medullary interstitium of the ] 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 ]'s ]s may occur if lithium concentrations become too high as a result of ], ], an unusually ], or certain drugs. |
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===Red pyrotechnic colorant=== |
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Lithium carbonate is used to ].<ref>{{cite web | title=Chemistry of Fireworks | url=https://fireworks.com/education-and-safety/chemistry-compounds | access-date=2020-07-05 | archive-date=2020-07-05 | archive-url=https://web.archive.org/web/20200705173238/https://fireworks.com/education-and-safety/chemistry-compounds | url-status=live }}</ref> |
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==Properties and reactions == |
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Unlike ], which forms at least three ], 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 ]s capitalizes on this poor solubility. Its apparent solubility increases 10-fold under a mild pressure of ]; this effect is due to the formation of the ] ], which is more soluble:<ref name=Ullmann/><ref>Spellman, F. R. (2023). ''The Science of Lithium''. CRC Press.</ref> |
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:{{chem|Li|2|CO|3}} + {{chem|CO|2}} + {{chem|H|2|O}} {{eqm}} 2 {{chem|LiHCO|3}} |
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The extraction of lithium carbonate at high pressures of {{chem|CO|2}} and its precipitation upon depressurizing is the basis of the Quebec process. |
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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> |
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Lithium carbonate, and other carbonates of ], do not ] readily. {{chem|Li|2|CO|3}} decomposes at temperatures around 1300 °C. |
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==Production== |
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Lithium is extracted from primarily two sources: ] in ] deposits, and lithium salts in underground ]s. About 82,000 tons were produced in 2020, showing significant and consistent growth.<ref>{{Cite web|url=https://www.statista.com/statistics/606684/world-production-of-lithium/|title=Global lithium production 2020|access-date=2021-06-03|archive-date=2021-06-03|archive-url=https://web.archive.org/web/20210603140725/https://www.statista.com/statistics/606684/world-production-of-lithium/|url-status=live}}</ref> |
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===From underground brine reservoirs=== |
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In the ] in the ] of Northern Chile, lithium carbonate and hydroxide are produced from brine.<ref name="SQM-SUS">{{cite web |title=Sustainability of lithium production in Chile |url=https://www.sqm.com/wp-content/uploads/2020/09/SQM_-_Sustainable_Lithium_-_English.pdf |website=SQM |access-date=1 December 2020 |archive-date=5 November 2020 |archive-url=https://web.archive.org/web/20201105191714/https://www.sqm.com/wp-content/uploads/2020/09/SQM_-_Sustainable_Lithium_-_English.pdf |url-status=live }}</ref><ref>{{cite conference |last1=Telsnig |first1=Thomas |last2=Potz |first2=Christian |last3=Haas |first3=Jannik |last4=Eltrop |first4=Ludger |last5=Palma-Behnke |first5=Rodrigo |title=Opportunities to integrate solar technologies into the Chilean lithium mining industry – reducing process related GHG emissions of a strategic storage resource |conference=Solarpaces 2016: International Conference on Concentrating Solar Power and Chemical Energy Systems |series=AIP Conference Proceedings |date=2017 |volume=1850 |issue=1 |page=110017 |doi=10.1063/1.4984491|bibcode=2017AIPC.1850k0017T |doi-access=free }}</ref> |
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The process pumps lithium rich brine from below ground into shallow pans for evaporation. The brine contains many different dissolved ions, and as their concentration increases, salts precipitate out of solution and sink. The remaining ] 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. |
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In the first pan, ] (sodium chloride or common salt) crystallises. This has little economic value and is discarded. The supernatant, with ever increasing concentration of dissolved solids, is transferred successively to the ] (sodium potassium chloride) pan, the ] (potassium magnesium chloride) pan and finally a pan designed to maximise 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, ] and magnesium are removed (typically residual boron is removed by solvent extraction and/or ] and magnesium by raising the ] above 10 with ])<ref>{{cite web |
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|last1=Dry |
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|first1=Mike |
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|title=Extraction of Lithium from Brine – Old and New Chemistry |
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|url=http://downloads.aqsim.com/Extraction%20of%20Lithium%20from%20Brine%20%2013%20Old%20and%20New%20Chemistry.pdf |
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|website=Critical Materials Symposium, EXTRACTION 2018, Ottawa, August 26–29 |
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|access-date=1 December 2020 |
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|archive-date=6 October 2021 |
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|archive-url=https://web.archive.org/web/20211006135312/http://downloads.aqsim.com/Extraction%20of%20Lithium%20from%20Brine%20%2013%20Old%20and%20New%20Chemistry.pdf |
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|url-status=dead |
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}}</ref> then in the final step, by addition of ], the desired lithium carbonate is precipitated out, separated, and processed. |
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Some of the by-products from the evaporation process may also have economic value. |
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There is considerable attention to the use of water in this water poor region. ] commissioned a ] (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, using ]. A more general LCA suggests the opposite for extraction from reservoirs.<ref name="BBC" >{{cite web |last1=Early |first1=Catherine |title=The new 'gold rush' for green lithium |url=https://www.bbc.com/future/article/20201124-how-geothermal-lithium-could-revolutionise-green-energy |website=Future Planet |publisher=BBC |access-date=2 December 2020 |date=25 Nov 2020 |archive-date=13 February 2024 |archive-url=https://web.archive.org/web/20240213053623/https://www.bbc.com/future/article/20201124-how-geothermal-lithium-could-revolutionise-green-energy |url-status=live }}</ref> |
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The majority of brine based production is in the "]" in South America. |
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=== From "geothermal" brine === |
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A potential source of lithium is the leachates of ], carried to the surface.<ref name="bourcier">Parker, Ann. {{webarchive|url=https://web.archive.org/web/20120917035952/https://www.llnl.gov/str/JanFeb05/Bourcier.html |date=17 September 2012 }}. Lawrence Livermore National Laboratory</ref> Recovery of lithium has been demonstrated in the field; the lithium is separated by simple precipitation and filtration.<ref name="Simbol">Patel, P. (16 November 2011) {{Webarchive|url=https://archive.today/20130203195827/http://www.technologyreview.com/news/426131/startup-to-capture-lithium-from-geothermal-plants/ |date=2013-02-03 }}. technologyreview.com</ref> The process and environmental costs are primarily those of the already-operating well; net environmental impacts may thus be positive.<ref name="NYT">Wald, M. (28 September 2011) {{webarchive|url=https://web.archive.org/web/20170408033249/http://www.nytimes.com/2011/09/28/business/energy-environment/simbol-materials-plans-to-extract-lithium-from-geothermal-plants.html |date=8 April 2017 }}. The New York Times</ref> |
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The brine of ] project near ] is claimed by ] 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,<ref>{{cite web |title=Cornish Lithium Releases Globally Significant Lithium Grades |url=https://cornishlithium.com/company-announcements/cornish-lithium-releases-globally-significant-lithium-grades/ |website=Cornish Lithium |date=17 September 2020 |access-date=17 July 2021 |archive-date=17 July 2021 |archive-url=https://web.archive.org/web/20210717144259/https://cornishlithium.com/company-announcements/cornish-lithium-releases-globally-significant-lithium-grades/ |url-status=live }}</ref> and a flow rate of 40-60l/s.<ref name="BBC"/> |
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===From ore=== |
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α-spodumene is roasted at 1100 °C for 1h to make β-spodumene, then roasted at 250 °C for 10 minutes with sulphuric acid.<ref>{{cite journal |last1=Meshram |first1=Pratima |last2=Pandey |first2=B. D. |last3=Mankhand |first3=T. R. |title=Extraction of lithium from primary and secondary sources by pre-treatment, leaching and separation: A comprehensive review |journal=Hydrometallurgy |date=1 December 2014 |volume=150 |pages=192–208 |doi=10.1016/j.hydromet.2014.10.012 |bibcode=2014HydMe.150..192M |url=https://www.sciencedirect.com/science/article/abs/pii/S0304386X14002278 |access-date=2 Dec 2020 |archive-date=13 June 2021 |archive-url=https://web.archive.org/web/20210613182331/https://www.sciencedirect.com/science/article/abs/pii/S0304386X14002278 |url-status=live }}</ref><ref name="SQM-SUS"/> |
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As of 2020, Australia was the world's largest producer of lithium intermediates,<ref>{{Cite web|url=https://pubs.usgs.gov/periodicals/mcs2020/mcs2020-lithium.pdf|title=Mineral Commodity Summaries 2020|last=Jaskula|first=Brian W.|date=January 2020|website=U.S. Geological Survey|access-date=29 June 2020|archive-date=1 November 2020|archive-url=https://web.archive.org/web/20201101085310/https://pubs.usgs.gov/periodicals/mcs2020/mcs2020-lithium.pdf|url-status=live}}</ref> all based on spodumene. |
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In recent years mining companies have begun exploration of ] projects throughout ], ] and ] to identify economic deposits that can potentially bring new supplies of lithium carbonate online to meet the growing demand for the product.<ref>{{cite web |
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| url= https://www.juniorminingnetwork.com/news-topics/topic/lithium.html |
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| title= Junior mining companies exploring for lithium |
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| agency= www.juniorminingnetwork.com |
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| access-date= 2017-03-30 |
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| archive-date= 2017-03-31 |
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| archive-url= https://web.archive.org/web/20170331034435/https://www.juniorminingnetwork.com/news-topics/topic/lithium.html |
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}}</ref> |
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===From clay=== |
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In 2020 ] announced a revolutionary process to extract lithium from clay in Nevada using only salt and no acid. This was met with scepticism.<ref>{{cite news |last1=Scheyder |first1=Ernest |title=Tesla's Nevada lithium plan faces stark obstacles on path to production |url=https://www.reuters.com/article/tesla-batteryday-lithium/teslas-nevada-lithium-plan-faces-stark-obstacles-on-path-to-production-idINL2N2GK2E1 |access-date=2 December 2020 |work=Reuters |date=24 Sep 2020 |archive-date=18 January 2021 |archive-url=https://web.archive.org/web/20210118124848/https://www.reuters.com/article/tesla-batteryday-lithium/teslas-nevada-lithium-plan-faces-stark-obstacles-on-path-to-production-idINL2N2GK2E1 |url-status=live }}</ref> |
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===From end-of-life batteries=== |
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A few small companies are ], focusing on recovering copper and cobalt. Some recover lithium carbonate alongside the compound Li<sub>2</sub>Al<sub>4</sub>(CO<sub>3</sub>)(OH)<sub>12</sub>⋅3H<sub>2</sub>O |
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also.<ref>{{cite journal |last1=Serna-Guerrero |first1=Rodrigo |title=A Critical Review of Lithium-Ion Battery Recycling Processes from a Circular Economy Perspective |journal=Batteries |page=68 |doi=10.3390/batteries5040068 |date=5 November 2019 |volume=5 |issue=4 |doi-access=free }}</ref><ref name="Dolotko Gehrke Malliaridou Sieweck 2023 p. ">{{cite journal | last1=Dolotko | first1=Oleksandr | last2=Gehrke | first2=Niclas | last3=Malliaridou | first3=Triantafillia | last4=Sieweck | first4=Raphael | last5=Herrmann | first5=Laura | last6=Hunzinger | first6=Bettina | last7=Knapp | first7=Michael | last8=Ehrenberg | first8=Helmut | title=Universal and efficient extraction of lithium for lithium-ion battery recycling using mechanochemistry | journal=Communications Chemistry | publisher=Springer Science and Business Media LLC | volume=6 | issue=1 | date=March 28, 2023 | page=49 | issn=2399-3669 | doi=10.1038/s42004-023-00844-2 | pmid=36977798 | pmc=10049983 }}</ref><ref name="Kropachev Kalabskiy 2020 p=106470">{{cite journal | last1=Kropachev | first1=Andrey | last2=Kalabskiy | first2=Igor | title=Hydrometallurgical preparation of lithium aluminum carbonate hydroxide hydrate, Li2Al4(CO3)(OH)12·3H2O from aluminate solution | journal=Minerals Engineering | publisher=Elsevier BV | volume=155 | year=2020 | issn=0892-6875 | doi=10.1016/j.mineng.2020.106470 | page=106470}}</ref><ref name="Dave Borlace 2023">{{cite AV media|title=Battery recycling just got a whole lot better.|type=YouTube video|publisher=Just Have a Think|location=London|date=15 May 2023|people=Dave Borlace|url=https://www.youtube.com/watch?v=XFmBX0Uq0wY|access-date=15 May 2023|archive-date=14 May 2023|archive-url=https://web.archive.org/web/20230514212801/https://www.youtube.com/watch?v=XFmBX0Uq0wY|url-status=live}}</ref> |
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===Other=== |
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In April 2017 MGX Minerals reported it had received independent confirmation of its rapid ] extraction process to recover lithium and other valuable minerals from ] wastewater ]. |
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<ref>{{cite web |
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|url = https://www.juniorminingnetwork.com/junior-miner-news/press-releases/28-cse/xmg/31459-mgx-minerals-receives-independent-confirmation-of-rapid-lithium-extraction-process.html |
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|title = MGX Minerals Receives Independent Confirmation of Rapid Lithium Extraction Process |
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|date = 20 April 2017 |
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|agency = www.juniorminingnetwork.com |
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|access-date = 2017-04-20 |
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|archive-date = 2017-04-20 |
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|archive-url = https://web.archive.org/web/20170420132515/https://www.juniorminingnetwork.com/junior-miner-news/press-releases/28-cse/xmg/31459-mgx-minerals-receives-independent-confirmation-of-rapid-lithium-extraction-process.html |
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|url-status = live |
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}}</ref> |
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] has been proposed to extract lithium from seawater, but it is not commercially viable.<ref name=":0">{{Cite web|url=https://www.technologyreview.com/s/538036/quest-to-mine-seawater-for-lithium-advances/|title=Quest to Mine Seawater for Lithium Advances|last=Martin|first=Richard|date=2015-06-08|website=MIT Technology Review|access-date=2016-02-10|archive-date=2020-03-08|archive-url=https://web.archive.org/web/20200308210028/https://www.technologyreview.com/s/538036/quest-to-mine-seawater-for-lithium-advances/|url-status=live}}</ref> |
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==Natural occurrence== |
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Natural lithium carbonate is known as ].<ref name="webmineral.com">{{cite web |
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| url=http://webmineral.com/data/Zabuyelite.shtml |
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| title=Zabuyelite Mineral Data |
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| author=David Barthelmy |
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| work=Mineralogy Database |
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| access-date=2010-02-07 |
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| archive-date=2023-05-30 |
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| archive-url=https://web.archive.org/web/20230530011138/http://webmineral.com/data/Zabuyelite.shtml |
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| url-status=live |
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}}</ref> This mineral is connected with deposits of some ]s and some ]s.<ref>{{Cite web |url=https://www.mindat.org/min-4380.html |title=mindat.org |access-date=2018-05-24 |archive-date=2018-06-27 |archive-url=https://web.archive.org/web/20180627005924/https://www.mindat.org/min-4380.html |url-status=live }}</ref> |
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==References== |
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{{Reflist}} |
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==External links== |
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{{Commons category|Lithium carbonate}} |
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{{Mood stabilizers}} |
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{{Lithium compounds}} |
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{{Carbonates}} |
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{{Oxytocin and vasopressin receptor modulators}} |
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{{Authority control}} |
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] |
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] |
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] |
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] |
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] |