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{{chembox {{chembox
| Verifiedfields = changed
| verifiedrevid = 443924852
| Watchedfields = changed
| ImageFile = Lithium-hydroxide-xtal-3D-vdW.png
| verifiedrevid = 450704627
| ImageSize = 200px
| ImageFile = Lithiumhydroxide t.png
| ImageName = Lithium hydroxide
| ImageSize = 150px
| ImageName2 = Lithium-hydroxide.jpg
| ImageFile1 = Lithium-hydroxide-xtal-3D-SF.png
| ImageSize1 =
| ImageName1 = Lithium hydroxide
| ImageFile2 = File:Kristallstruktur Lithiumhydroxid.png
| ImageSize2 =
| ImageCaption2 = {{colorbox|#C0C0C0}}{{nbsp}}{{chem2|]+}}     {{colorbox|#EE0000}}{{nbsp}}{{chem2|](2−)}}     {{colorbox|#FFFFFF}}{{nbsp}}{{chem2|]+}}
| ImageFile3 = Lithium hydroxide.jpg
| ImageSize3 =
| ImageName3 = Lithium-hydroxide.jpg
| IUPACName = Lithium hydroxide | IUPACName = Lithium hydroxide
|Section1={{Chembox Identifiers
| OtherNames = Lithine
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| Section1 =
| ChemSpiderID = 3802
{{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 903YL31JAS
| ChemSpiderID = 3802
| UNII_Ref = {{fdacite|correct|FDA}} | UNII1_Ref = {{fdacite|correct|FDA}}
| UNII = 903YL31JAS | UNII1 = G51XLP968G
| UNII1_Comment = (monohydrate)
| InChI = 1/Li.H2O/h;1H2/q+1;/p-1
| InChI = 1/Li.H2O/h;1H2/q+1;/p-1
| InChIKey = WMFOQBRAJBCJND-REWHXWOFAT
| InChIKey = WMFOQBRAJBCJND-REWHXWO
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 33979 | ChEBI = 33979
| SMILES = . | SMILES = .
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Li.H2O/h;1H2/q+1;/p-1 | StdInChI = 1S/Li.H2O/h;1H2/q+1;/p-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = WMFOQBRAJBCJND-UHFFFAOYSA-M | StdInChIKey = WMFOQBRAJBCJND-UHFFFAOYSA-M
| CASNo = 1310-65-2 | CASNo = 1310-65-2
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| CASOther = <br/>1310-66-3 (monohydrate) | CASNo2 = 1310-66-3
| CASNo2_Ref = {{cascite|correct|CAS}}
| PubChem = 3939
| CASNo2_Comment = (monohydrate)
| RTECS = OJ6307070
| UNNumber = 2680 | PubChem = 3939
| RTECS = OJ6307070
| UNNumber = 2680
| Gmelin = 68415
}} }}
| Section2 = |Section2={{Chembox Properties
| Odor = none
{{Chembox Properties
| Formula = LiOH | Formula = LiOH
| MolarMass = 23.95 g/mol | MolarMass = {{ubl|23.95&nbsp;g/mol (anhydrous)|41.96&nbsp;g/mol (monohydrate)}}
| Appearance = ] white solid <br> odorless | Appearance = white solid
| Density = 1.46 g/cm<sup>3</sup> (anhydrous) <br> 1.51 g/cm<sup>3</sup> (monohydrate) | Density = {{ubl|1.46 g/cm<sup>3</sup> (anhydrous)|1.51 g/cm<sup>3</sup> (monohydrate)}}
| MeltingPt = 462 °C | MeltingPtC = 462
| BoilingPt = 924 °C decomp. | BoilingPtC = 924
| BoilingPt_notes = (decomposes)
| Solubility = ''anhydrous:'' <hr> 12.8 g/100 mL (20 °C) <br> 12.5 g/100 mL (25 °C) <br> 17.5 g/100 mL (100 °C) <br> ''monohydrate:'' <hr> 22.3 g/100 mL (10 °C) <br> 26.8 g/100 mL (100 °C)<ref>{{RubberBible87th}}</ref>
| 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>}}
| RefractIndex = 1.464 (anhydrous) <br> 1.460 (monohydrate)
| 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}}</ref>
| ConjugateBase = ]
| MagSus = −12.3·10<sup>−6</sup> cm<sup>3</sup>/mol
| Dipole = 4.754&nbsp;]<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 = |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>
{{Chembox Thermochemistry
| HeatCapacity = 49.6&nbsp;J/(mol·K)
| DeltaHf = -20.36 kJ/g
| Entropy = 42.8&nbsp;J/(mol·K)
| DeltaHc =
| DeltaHform = −487.5&nbsp;kJ/mol
| Entropy =
| DeltaGfree = −441.5&nbsp;kJ/mol
| HeatCapacity = 2.071 J/g K
| DeltaHcombust =
| DeltaHfus = 20.9&nbsp;kJ/mol (at melting point)
}} }}
| Section5 = |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)
{{Chembox Hazards
| MainHazards = Corrosive
| ExternalMSDS = <br/> (monohydrate)
| EUIndex = Not listed | NFPA-H = 3
| NFPA-F = 0
| MainHazards = Corrosive
| NFPA-H = 3 | NFPA-R = 0
| NFPA-F = 0 | NFPA-S =
| FlashPt = Non-flammable
| NFPA-R = 0
| 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>
| NFPA-O =
| FlashPt = Non-flammable
}} }}
| Section8 = |Section8 = {{Chembox Related
| OtherAnions = ]
{{Chembox Related
| OtherCations = {{ubl|]|]|]|]}}
| OtherAnions = ]
| OtherCompounds = ]
| OtherCations = ]<br/>]<br/>]<br/>]
| OtherCpds = ]
}} }}
}} }}


'''Lithium hydroxide''' is an ] with the ] LiOH. It is a white ] ]line material. It is soluble in water, and slightly soluble in ]. It is available commercially in ] form and as the monohydrate (LiOH<sup>.</sup>H<sub>2</sub>O), both of which are strong bases. '''Lithium hydroxide''' is an ] with the ] LiOH. It can exist as anhydrous or hydrated, and both forms are white ] solids. They are soluble in water and slightly soluble in ]. Both are available commercially. While classified as a ], lithium hydroxide is the weakest known alkali metal hydroxide.


==Production and reactions== ==Production==
The preferred feedstock is hard-rock ], where the lithium content is expressed as % ].
Lithium hydroxide is produced in a ] between ] and ]:<ref name=Ullmann>{{cite book
|last1=Wietelmann |first1=U
|last2= Bauer |first2= RJ
|year=2000
|chapter= Lithium and Lithium Compounds
|title=]
|volume= |issue= |pages=
|isbn= 3527306730
|doi=10.1002/14356007.a15_393


===Lithium carbonate route===
}}</ref>
Lithium hydroxide is often produced industrially from ] in a ] with ]:<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>
:Li<sub>2</sub>CO<sub>3</sub> + Ca(OH)<sub>2</sub> &rarr; 2 LiOH + CaCO<sub>3</sub>
:{{chem2|Li2CO3 + Ca(OH)2 → 2 LiOH + CaCO3}}
The initially produced hydrate is dehydrated by heating under vacuum up to 180 °C.
The initially produced hydrate is dehydrated by heating under vacuum up to 180&nbsp;°C.


===Lithium sulfate route===
In the laboratory, lithium hydroxide arises by the action of water on ] or ]. The equations for these processes follow:
An alternative route involves the intermediacy of ]:<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>
:2 Li + 2 H<sub>2</sub>O → 2 LiOH + H<sub>2</sub>
:α-] → β-spodumene
: Li<sub>2</sub>O + H<sub>2</sub>O &rarr; 2 LiOH
:β-spodumene + CaO → {{chem2|Li2O}} + ...
Typically, these reactions are avoided.
:{{chem2|Li2O + H2SO4 → Li2SO4 + H2O}}
:{{chem2|Li2SO4 + 2 NaOH → Na2SO4 + 2 LiOH}}


The main by-products are ] and ], which have some market value.
Although ] is more widely used, the hydroxide is an effective precursor to lithium salts, e.g.

:LiOH<sub></sub> + HF → LiF + H<sub>2</sub>O.
==Commercial setting==
According to Bloomberg, ]<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=]}}</ref> and ] were the largest producers in 2020 with around 25kt/y, followed by Livent Corporation (FMC) and ].<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 ] WA 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=www.abc.net.au|date=27 August 2020|language=en-AU}}</ref>

In 2020 ], plant in ] is 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|access-date=4 December 2020|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|url-status=dead}}</ref>


==Applications== ==Applications==
===Lithium-ion batteries===
Lithium hydroxide is mainly consumed for the production of ]s. A popular lithium grease is ], which is a general purpose lubricating ] due to its high resistance to water and being useful at both high and low temperatures.
Lithium hydroxide is mainly consumed in the production of ] materials for ] such as ] ({{chem2|LiCoO2}}) and ]. It is preferred over ] as a precursor for ].<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 ], which produces a general-purpose lubricating ] due to its high resistance to water and usefulness at a range of temperatures.


===Carbon dioxide scrubbing=== ===Carbon dioxide scrubbing===
{{See|carbon dioxide scrubber}} {{Main|Carbon dioxide scrubber}}
Lithium hydroxide is used in ] purification systems for ], ]s, and ]s to remove ] from exhaled gas by producing ] 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 is used in ] purification systems for ] (Lithium hydroxide canisters in the ] and ] (after modification) were lifelines for the ] astronauts), ]s, and ]s to remove ] from exhaled gas by producing ] and water:<ref>
Lithium hydroxide, together with ], is a key intermediates used for the production of other lithium compounds, illustrated by its use in the production of ]:<ref name="Ullmann"/>
{{cite journal
:{{chem2|LiOH + HF → LiF + H2O}}
|last=Jaunsen |first=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
|accessdate=2008-06-17
}}</ref>
:2 LiOH&middot;H<sub>2</sub>O + CO<sub>2</sub> &rarr; Li<sub>2</sub>CO<sub>3</sub> + 3 H<sub>2</sub>O
Or,
:2LiOH + CO<sub>2</sub> &rarr; Li<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
The latter, anhydrous hydroxide is preferred for its lower mass and lesser water production for respirator systems in spacecraft. 1&nbsp;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 °C.


===Other uses=== ===Other uses===
It is also used in ]s and some ] formulations, where it is also used to suppress ASR (]).<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}}</ref>
It is used as a heat transfer medium, as a storage-] ]. It is also used in ]s and some ] formulations. Lithium hydroxide (] enriched in ]) is used to alkalize the reactor coolant in ]s for corrosion control.

Lithium hydroxide (] in ]) is used to alkalize the reactor coolant in ]s for corrosion control.<ref> // ], 19 September 2013; </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=]}}</ref>


==See also== ==See also==
* ] * ]


== References == ==References==
{{Reflist}} {{Reflist}}


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


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


{{DEFAULTSORT:Lithium Hydroxide}}
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