Editing Lithium hydroxide

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 450704627
| ImageFile = Lithiumhydroxide t.png
| ImageSize = 150px
| ImageFile1 = Lithium-hydroxide-xtal-3D-SF.png
| ImageSize1 = 
| ImageName1 = Lithium hydroxide
| ImageFile2 = File:Kristallstruktur Lithiumhydroxid.png
| ImageSize2 = 
| ImageCaption2 = {{colorbox|#C0C0C0}}{{nbsp}}{{chem2|[[Lithium|Li]]+}}&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;{{colorbox|#EE0000}}{{nbsp}}{{chem2|[[Oxygen|O]](2−)}}&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;{{colorbox|#FFFFFF}}{{nbsp}}{{chem2|[[Hydrogen|H]]+}}
| ImageFile3 = Lithium hydroxide.jpg
| ImageSize3 = 
| ImageName3 = Lithium-hydroxide.jpg
| IUPACName = Lithium hydroxide
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 3802
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 903YL31JAS
| UNII1_Ref = {{fdacite|correct|FDA}}
| UNII1 = G51XLP968G
| UNII1_Comment = (monohydrate)
| InChI = 1/Li.H2O/h;1H2/q+1;/p-1
| InChIKey = WMFOQBRAJBCJND-REWHXWO
| ChEBI = 33979
| SMILES = [Li+].[OH-]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Li.H2O/h;1H2/q+1;/p-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = WMFOQBRAJBCJND-UHFFFAOYSA-M
| CASNo = 1310-65-2
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo2 = 1310-66-3
| CASNo2_Ref = {{cascite|correct|CAS}}
| CASNo2_Comment = (monohydrate)
| PubChem = 3939
| RTECS = OJ6307070
| UNNumber = 2680
| Gmelin = 68415
}}
|Section2={{Chembox Properties
| Odor = none
| Formula = LiOH
| MolarMass = {{ubl|23.95&nbsp;g/mol (anhydrous)|41.96&nbsp;g/mol (monohydrate)}}
| Appearance = white solid
| Density = {{ubl|1.46 g/cm<sup>3</sup> (anhydrous)|1.51 g/cm<sup>3</sup> (monohydrate)}}
| MeltingPtC = 462
| BoilingPtC = 924
| BoilingPt_notes = (decomposes)
| Solubility = {{ubl|anhydrous:|12.7&nbsp;g/(100 mL) (0&nbsp;°C)|12.8&nbsp;g/(100 mL) (20&nbsp;°C)|17.5&nbsp;g/(100 mL) (100&nbsp;°C)|<hr/>|monohydrate:|22.3&nbsp;g/(100 mL) (10&nbsp;°C)|26.8&nbsp;g/(100 mL) (80&nbsp;°C)<ref>{{RubberBible87th}}</ref>}}
| Solvent1 = methanol
| Solubility1 = {{ubl|9.76&nbsp;g/(100 g) (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)|13.69&nbsp;g/(100 g) (monohydrate; 20&nbsp;°C, 48&nbsp;hours mixing)<ref name=Khosravi>{{cite book|last1=Khosravi|first1=Javad|name-list-style = vanc|year=2007|at=Chapter&nbsp;9: Results|title=Production of Lithium Peroxide and Lithium Oxide in an Alcohol Medium|isbn=978-0-494-38597-5}}</ref>}}
| Solvent2 = ethanol
| Solubility2 = {{ubl|2.36&nbsp;g/(100 g) (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)|2.18&nbsp;g/(100 g) (monohydrate; 20&nbsp;°C, 48&nbsp;hours mixing)<ref name="Khosravi"/>}}
| Solvent3 = isopropanol
| Solubility3 = {{ubl|0&nbsp;g/(100 g) (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)|0.11&nbsp;g/(100 g) (monohydrate; 20&nbsp;°C, 48&nbsp;hours mixing)<ref name="Khosravi"/>}}
| RefractIndex = {{ubl|1.464 (anhydrous)|1.460 (monohydrate)}}
| pKa = 14.4<ref>{{cite journal|vauthors = Popov K, Lajunen LH, Popov A, Rönkkömäki H, Hannu-Kuure H, Vendilo A|year=2002|title=<sup>7</sup>Li, <sup>23</sup>Na, <sup>39</sup>K and <sup>133</sup>Cs NMR comparative equilibrium study of alkali metal cation hydroxide complexes in aqueous solutions. First numerical value for CsOH formation|url=https://www.infona.pl/resource/bwmeta1.element.elsevier-40fb73c1-ba37-32e0-914e-b264c7c0539b|journal=Inorganic Chemistry Communications|volume=5|issue=3|pages=223–225|doi=10.1016/S1387-7003(02)00335-0|access-date=2017-01-21|df=dmy-all|url-access=subscription}}</ref>
| ConjugateBase = [[Lithium monoxide anion]]
| MagSus = −12.3·10<sup>−6</sup> cm<sup>3</sup>/mol
| Dipole = 4.754&nbsp;[[Debye|D]]<ref>{{Cite book |url=https://www.worldcat.org/oclc/930681942 |title=CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. |date=2016 |others=William M. Haynes, David R. Lide, Thomas J. Bruno |isbn=978-1-4987-5428-6 |edition=2016-2017, 97th |location=Boca Raton, Florida |oclc=930681942}}</ref>
}}
|Section4 = {{Chembox Thermochemistry
| Thermochemistry_ref = <ref>{{Cite book|url=https://www.worldcat.org/oclc/930681942|title=CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data.|date=2016|others=William M. Haynes, David R. Lide, Thomas J. Bruno|isbn=978-1-4987-5428-6|edition=2016-2017, 97th|location=Boca Raton, Florida|oclc=930681942}}</ref>
| HeatCapacity = 49.6&nbsp;J/(mol·K)
| Entropy = 42.8&nbsp;J/(mol·K)
| DeltaHform = −487.5&nbsp;kJ/mol
| DeltaGfree = −441.5&nbsp;kJ/mol
| DeltaHcombust =
| DeltaHfus = 20.9&nbsp;kJ/mol (at melting point)
}}
|Section5 = {{Chembox Hazards
| ExternalSDS = {{cite web|url=http://www.inchem.org/documents/icsc/icsc/eics0913.htm|title=ICSC 0913}}<br/>{{cite web|url = http://www.inchem.org/documents/icsc/icsc/eics0914.htm|title=ICSC 0914}} (monohydrate)
| MainHazards = Corrosive
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S =
| FlashPt = Non-flammable
| LD50 = 210 mg/kg (oral, rat)<ref>{{cite web|url=https://chem.nlm.nih.gov/chemidplus/rn/1310-65-2|title=ChemIDplus – 1310-65-2 – WMFOQBRAJBCJND-UHFFFAOYSA-M – Lithium hydroxide anhydrous – Similar structures search, synonyms, formulas, resource links, and other chemical information|first=Michael|last=Chambers|name-list-style = vanc|website=chem.sis.nlm.nih.gov|access-date=12 April 2018}}</ref>
}}
|Section8 = {{Chembox Related
| OtherAnions = [[Lithium amide]]
| OtherCations = {{ubl|[[Sodium hydroxide]]|[[Potassium hydroxide]]|[[Rubidium hydroxide]]|[[Caesium hydroxide]]}}
| OtherCompounds = [[Lithium oxide]]
}}
}}

'''Lithium hydroxide''' is an [[inorganic compound]] with the [[chemical formula|formula]] LiOH. It can exist as anhydrous or hydrated, and both forms are white [[hygroscopic]] solids. They are soluble in water and slightly soluble in [[ethanol]]. Both are available commercially. While classified as a [[strong base]], lithium hydroxide is the weakest known alkali metal hydroxide.

==Production==
The preferred feedstock is hard-rock [[spodumene]], where the lithium content is expressed as % [[lithium oxide]].

===Lithium carbonate route===
Lithium hydroxide is often produced industrially from [[lithium carbonate]] in a [[Salt metathesis reaction|metathesis reaction]] with [[calcium hydroxide]]:<ref name="Ullmann">{{Ullmann|vauthors = Wietelmann U, Bauer RJ|year=2000|chapter=Lithium and Lithium Compounds|isbn=3-527-30673-0|doi=10.1002/14356007.a15_393}}</ref> 
:{{chem2|Li2CO3 + Ca(OH)2 → 2 LiOH + CaCO3}}
The initially produced hydrate is dehydrated by heating under vacuum up to 180&nbsp;°C.

===Lithium sulfate route===
An alternative route involves the intermediacy of [[lithium sulfate]]:<ref>{{cite web|title=Proposed Albemarle Plant Site|url=https://www.albemarle.com/storage/wysiwyg/alb_kemerton_literature_051618_a4_fnl.pdf|website=Albemarle|access-date=4 December 2020}}</ref><ref>{{cite web|title=Corporate presentation|url=https://www.nemaskalithium.com/assets/documents/docs/NMX_CorporatePresentation_May.pdf|website=Nemaska Lithium|access-date=5 December 2020|date=May 2018|archive-date=23 October 2021|archive-url=https://web.archive.org/web/20211023105539/https://www.nemaskalithium.com/assets/documents/docs/NMX_CorporatePresentation_May.pdf|url-status=dead}}</ref>
:α-[[spodumene]] → β-spodumene
:β-spodumene + CaO → {{chem2|Li2O}} + ...
:{{chem2|Li2O + H2SO4 → Li2SO4 + H2O}}
:{{chem2|Li2SO4 + 2 NaOH → Na2SO4 + 2 LiOH}}

The main by-products are [[gypsum]] and [[sodium sulphate]], which have some market value.

==Commercial setting==
According to Bloomberg, [[Ganfeng Lithium Co. Ltd.]]<ref name=":0" /> (GFL or Ganfeng)<ref>{{Cite web|title=Ganfeng Lithium Group|url=http://www.ganfenglithium.com/about1_en.html|access-date=25 March 2021|website=[[Ganfeng Lithium]]}}</ref> and [[Albemarle Corporation|Albemarle]] were the largest producers in 2020 with around 25kt/y, followed by Livent Corporation (FMC) and [[Sociedad Química y Minera|SQM]].<ref name=":0">{{cite web|title=China's Ganfeng to Be Largest Lithium Hydroxide Producer|url=https://about.bnef.com/blog/chinas-ganfeng-to-be-largest-lithium-hydroxide-producer/|website=BloombergNEF|access-date=4 December 2020|date=10 September 2020}}</ref> Significant new capacity is planned, to keep pace with demand driven by vehicle electrification. Ganfeng are to expand lithium chemical capacity to 85,000 tons, adding the capacity leased from Jiangte, Ganfeng will become the largest lithium hydroxide producer globally in 2021.<ref name=":0" />

Albemarle's [[Kemerton, Western Australia]] plant, originally planned to deliver 100kt/y has been scaled back to 50kt/y.<ref>{{cite news |last1=Stephens |first1=Kate |last2=Lynch |first2=Jacqueline |title=Slowing demand for lithium sees WA's largest refinery scaled back |url=https://www.abc.net.au/news/2020-08-27/wa-lithium-refinery-hiring-fewer-workers-than-expected/12599184 |work=ABC.net.au |date=27 August 2020 }}</ref>

In 2020 [[Tianqi Lithium|Tianqi Lithium's]], plant in [[City of Kwinana|Kwinana, Western Australia]] was the largest producer, with a capacity of 48kt/y.<ref>{{cite web |title=Largest of its kind lithium hydroxide plant launched in Kwinana |url=https://www.mediastatements.wa.gov.au/Pages/McGowan/2019/09/Largest-of-its-kind-lithium-hydroxide-plant-launched-in-Kwinana.aspx |website=Government of Western Australia |date=10 September 2019 |archive-date=17 February 2023 |archive-url=https://web.archive.org/web/20230217040250/https://www.mediastatements.wa.gov.au/Pages/McGowan/2019/09/Largest-of-its-kind-lithium-hydroxide-plant-launched-in-Kwinana.aspx }}</ref>

==Applications==
===Lithium-ion batteries===
Lithium hydroxide is mainly consumed in the production of [[cathode]] materials for [[lithium-ion batteries]] such as [[lithium cobalt oxide]] ({{chem2|LiCoO2}}) and [[lithium iron phosphate]]. It is preferred over [[lithium carbonate]] as a precursor for [[lithium nickel manganese cobalt oxides]].<ref>{{cite web|last1=Barrera|first1=Priscilla|title=Will Lithium Hydroxide Really Overtake Lithium Carbonate? {{!}} INN|url=https://investingnews.com/daily/resource-investing/battery-metals-investing/lithium-investing/will-lithium-hydroxide-overtake-lithium-carbonate/|website=Investing News Network|access-date=5 December 2020|date=27 June 2019}}</ref>

===Grease===
A popular lithium grease thickener is [[lithium 12-hydroxystearate]], which produces a general-purpose lubricating [[Grease (lubricant)|grease]] due to its high resistance to water and usefulness at a range of temperatures.

===Carbon dioxide scrubbing===
{{Main|Carbon dioxide scrubber}}
Lithium hydroxide is used in [[breathing gas]] purification systems for [[spacecraft]], [[submarine]]s, and [[rebreather]]s to remove [[carbon dioxide]] from exhaled gas by producing [[lithium carbonate]] and water:<ref>{{cite journal|vauthors=Jaunsen JR|year=1989|title=The Behavior and Capabilities of Lithium Hydroxide Carbon Dioxide Scrubbers in a Deep Sea Environment|url=http://archive.rubicon-foundation.org/4998|journal=US Naval Academy Technical Report|id=USNA-TSPR-157|access-date=2008-06-17|archive-url=https://web.archive.org/web/20090824104846/http://archive.rubicon-foundation.org/4998|archive-date=2009-08-24|url-status=usurped}}</ref>
:{{chem2|2 LiOH*H2O + CO2 → Li2CO3 + 3 H2O}}
or
:{{chem2|2 LiOH + CO2 → Li2CO3 + H2O}}
The latter, anhydrous hydroxide, is preferred for its lower mass and lesser water production for respirator systems in spacecraft. One gram of anhydrous lithium hydroxide can remove 450&nbsp;cm<sup>3</sup> of carbon dioxide gas. The monohydrate loses its water at 100–110&nbsp;°C.

===Precursor===
Lithium hydroxide, together with [[lithium carbonate]], is a key intermediates used for the production of other lithium compounds, illustrated by its use in the production of [[lithium fluoride]]:<ref name="Ullmann"/>
:{{chem2|LiOH + HF → LiF + H2O}}

===Other uses===
It is also used in [[ceramic]]s and some [[Portland cement]] formulations, where it is also used to suppress ASR ([[alkali–silica reaction|concrete cancer]]).<ref>{{cite journal|vauthors= Kawamura M, Fuwa H|year=2003|title=Effects of lithium salts on ASR gel composition and expansion of mortars|url=https://www.osti.gov/biblio/20658311|journal=Cement and Concrete Research|volume=33 |issue=6 |pages=913–919 |doi=10.1016/S0008-8846(02)01092-X |osti=20658311 |access-date=2022-10-17|url-access=subscription}}</ref> 

Lithium hydroxide ([[isotope separation|isotopically enriched]] in [[isotopes of lithium|lithium-7]]) is used to alkalize the reactor coolant in [[pressurized water reactor]]s for corrosion control.<ref>[http://www.gao.gov/products/GAO-13-716 Managing Critical Isotopes: Stewardship of Lithium-7 Is Needed to Ensure a Stable Supply, GAO-13-716] // [[Government Accountability Office|U.S. Government Accountability Office]], 19 September 2013; [http://www.gao.gov/assets/660/657964.pdf pdf]</ref>
It is good radiation protection against free neutrons.

==Price==
In 2012, the price of lithium hydroxide was about US$5–6/kg.<ref>{{cite web|url=http://investingnews.com/daily/resource-investing/energy-investing/lithium-investing/lithium-prices-2012/|title=Lithium Prices 2012|publisher=Investing News Network|website=investingnews.com|date=14 June 2012|access-date=12 April 2018|archive-date=11 March 2018|archive-url=https://web.archive.org/web/20180311082731/https://investingnews.com/daily/resource-investing/energy-investing/lithium-investing/lithium-prices-2012/|url-status=dead}}</ref>

In December 2020, it had risen to $9/kg.<ref>{{cite web|title=London Metal Exchange: Lithium prices|url=https://www.lme.com/Metals/Minor-metals/Lithium-prices#tabIndex=0|website=London metal exchange|access-date=4 December 2020}}</ref>

On 18 March 2021, the price had risen to $11.50/kg.<ref>{{Cite web|date=18 March 2021|title=LITHIUM AT THE LME|url=https://www.lme.com/Metals/Minor-metals/Lithium-prices#tabIndex=0|access-date=22 March 2021|website=[[LME The London Metal Exchange]]}}</ref>

==See also==
* [[Soda lime]]

==References==
{{Reflist}}

==External links==
{{Commons category}}
*{{ICSC|0913}} (anhydrous)
*{{ICSC|0914}} (monohydrate)

{{Lithium compounds}}
{{Hydroxides}}
{{Authority control}}

[[Category:Lithium compounds]]
[[Category:Hydroxides]]
[[Category:Rebreather components|*]]