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| ImageFile2 = File:Kristallstruktur Lithiumhydroxid.png
| ImageFile2 = File:Kristallstruktur Lithiumhydroxid.png
| ImageSize2 =
| ImageSize2 =
| ImageCaption2 = {{colorbox|#C0C0C0}}{{nbsp}}[[Lithium|Li]]<sup>+</sup> &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;{{colorbox|#EE0000}}{{nbsp}}[[Oxygen|O]]<sup>2−</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;{{colorbox|#FFFFFF}}{{nbsp}}[[Hydrogen|H]]<sup>+</sup>
| 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
| ImageFile3 = Lithium hydroxide.jpg
| ImageSize3 =
| ImageSize3 =
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| UNII1_Comment = (monohydrate)
| 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 = [Li+].[OH-]
| SMILES = [Li+].[OH-]
Line 45: Line 44:
| Odor = none
| Odor = none
| Formula = LiOH
| Formula = LiOH
| MolarMass = {{ubl
| MolarMass = {{ubl|23.95&nbsp;g/mol (anhydrous)|41.96&nbsp;g/mol (monohydrate)}}
⚫
| Appearance = white solid
| 23.95&nbsp;g/mol (anhydrous)
| Density = {{ubl|1.46 g/cm<sup>3</sup> (anhydrous)|1.51 g/cm<sup>3</sup> (monohydrate)}}
| 41.96&nbsp;g/mol (monohydrate)
}}
⚫
| Appearance = {{ubl
| [[Hygroscopic]] white solid
}}
| Density = {{ubl
| 1.46{{nbsp}}g/cm<sup>3</sup> (anhydrous)
| 1.51{{nbsp}}g/cm<sup>3</sup> (monohydrate)
}}
| MeltingPtC = 462
| MeltingPtC = 462
| BoilingPtC = 924
| BoilingPtC = 924
| BoilingPt_notes = decomposes
| 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>}}
| Solubility = {{ubl
| (anhydrous:)
| 12.7&nbsp;g/100{{nnbsp}}mL (0&nbsp;°C)
| 12.8&nbsp;g/100{{nnbsp}}mL (20&nbsp;°C)
| 17.5&nbsp;g/100{{nnbsp}}mL (100&nbsp;°C)
| <hr/>
| (monohydrate:)
| 22.3&nbsp;g/100{{nnbsp}}mL (10&nbsp;°C)
| 26.8&nbsp;g/100{{nnbsp}}mL (80&nbsp;°C)<ref>{{RubberBible87th}}</ref>
}}
| Solvent1 = methanol
| 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>}}
| Solubility1 = {{ubl
| 9.76&nbsp;g/100{{nnbsp}}g (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)
| <hr/>
⚫
| 13.69&nbsp;g/100{{nnbsp}}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
| 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"/>}}
| Solubility2 = {{ubl
| 2.36&nbsp;g/100{{nnbsp}}g (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)
| <hr/>
⚫
| 2.18&nbsp;g/100{{nnbsp}}g (monohydrate; 20&nbsp;°C, 48&nbsp;hours mixing)<ref name="Khosravi"/>
}}
| Solvent3 = isopropanol
| 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"/>}}
| Solubility3 = {{ubl
| 0&nbsp;g/100{{nnbsp}}g (anhydrous; 20&nbsp;°C, 48&nbsp;hours mixing)
| 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>
| <hr/>
| 0.11&nbsp;g/100{{nnbsp}}g (monohydrate; 20&nbsp;°C, 48&nbsp;hours mixing)<ref name="Khosravi"/>
}}
| RefractIndex = {{ubl
| 1.464 (anhydrous)
| <hr/>
| 1.460 (monohydrate)
}}
| pKb = −0.04<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
| access-date=2017-01-21
| df=dmy-all
}}</ref>
| ConjugateBase = [[Lithium monoxide anion]]
| ConjugateBase = [[Lithium monoxide anion]]
| MagSus = −12.3·10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol
| 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
|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>
⚫
| DeltaHf = −20.36&nbsp;kJ/g
| HeatCapacity = 49.6&nbsp;J/(mol·K)
| DeltaHc =
| Entropy =
| Entropy = 42.8&nbsp;J/(mol·K)
| HeatCapacity = 2.071&nbsp;J/g⋅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
|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)
| 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
| MainHazards = Corrosive
| NFPA-H = 3
| NFPA-H = 3
Line 130: Line 80:
| NFPA-S =
| NFPA-S =
| FlashPt = Non-flammable
| FlashPt = Non-flammable
| LD50 = 210{{nbsp}}mg/kg (oral, rat)<ref>{{cite web |url=http://chem.sis.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>
| 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
|Section8 = {{Chembox Related
| OtherAnions = [[Lithium amide]]
| OtherAnions = [[Lithium amide]]
| OtherCations = [[Sodium hydroxide]]<br/>[[Potassium hydroxide]]<br/>[[Rubidium hydroxide]]<br/>[[Caesium hydroxide]]
| OtherCations = {{ubl|[[Sodium hydroxide]]|[[Potassium hydroxide]]|[[Rubidium hydroxide]]|[[Caesium hydroxide]]}}
| OtherCompounds = [[Lithium oxide]]
| OtherCompounds = [[Lithium oxide]]
}}
}}
}}
}}


'''Lithium hydroxide''' is an [[inorganic compound]] with the [[chemical formula|formula]] LiOH<sup>.</sup>(H<sub>2</sub>O)<sub>n</sub>. Both the anhydrous and hydrated 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.
'''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==
==Production==
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===Lithium carbonate route===
===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>
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>
:Li<sub>2</sub>CO<sub>3</sub> + Ca(OH)<sub>2</sub> → 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&nbsp;°C.
The initially produced hydrate is dehydrated by heating under vacuum up to 180&nbsp;°C.

===Lithium sulfate route===
===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}}</ref>
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
:α-[[spodumene]] → β-spodumene
:β-spodumene + CaO → Li<sub>2</sub>O + ...
:β-spodumene + CaO → {{chem2|Li2O}} + ...
:{{chem2|Li2O + H2SO4 → Li2SO4 + H2O}}
:Li<sub>2</sub>O + H<sub>2</sub>SO<sub>4</sub> → Li<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O
:Li<sub>2</sub>SO<sub>4</sub> + 2 NaOH → Na<sub>2</sub>SO<sub>4</sub> + 2 LiOH.
:{{chem2|Li2SO4 + 2 NaOH → Na2SO4 + 2 LiOH}}


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


==Commercial setting==
==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|url-status=live|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" />
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|Kemerton]] WA plant, originally planned to deliver 100kt/y has been scaled back to 50kt/yy.<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>
Albemarle's [[Kemerton, Western Australia|Kemerton]] 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 [[Tianqi Lithium|Tianqi Lithium's]], plant in [[City of Kwinana|Kwinana, Western Australia]] 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>
in 2023 AVZ Minerals,<ref>{{Cite web|title=AVZ Minerals Limited|url=https://avzminerals.com.au/|url-status=live|access-date=25 March 2021|website=[[AVZ Minerals Limited ]]}}</ref> an Australian company, are planning to produce the battery-grade high-purity Primary Lithium Sulphate (PLS) containing over 80% Lithium.<ref>{{Cite web|author-link=https://avzminerals.com.au/asx-announcements|date=13 January 2021|title=Metallurgical test work confirms Manono Primary Lithium Sulphate suitable for battery production Feedstock|url=https://avzminerals.com.au/investor-centre/2021/1/13/metallurgical-test-work-confirms-manono-primary-lithium-sulphate-suitable-for-battery-production-feedstock|url-status=live|access-date=25 March 2021|website=[[www.avzminerals.com.au]]}}</ref> PLS is a lithium chemical new to the market in the production of lithium hydroxide (a precursor to lithium-ion battery).

⚫
In 2020 [[Tianqi Lithium|Tianqi Lithium's]], plant in [[City of Kwinana|Kwinana, Western Australia]] 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}}</ref>


==Applications==
==Applications==
===Lithium ion batteries===
===Lithium-ion batteries===
Lithium hydroxide is mainly consumed in the production of cathode materials for [[lithium ion batteries]] such as [[lithium cobalt oxide]] (LiCoO<sub>2</sub>) 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>
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 ===
===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.
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===
===Carbon dioxide scrubbing===
{{Further|carbon dioxide scrubber}}
{{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=dead }}</ref>
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}}
:2 LiOH•H<sub>2</sub>O + CO<sub>2</sub> → Li<sub>2</sub>CO<sub>3</sub> + 3 H<sub>2</sub>O
or
or
:2 LiOH + CO<sub>2</sub> → Li<sub>2</sub>CO<sub>3</sub> + H<sub>2</sub>O
:{{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.
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===
===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"/>
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"/>
:LiOH + HF → LiF + H<sub>2</sub>O.
:{{chem2|LiOH + HF → LiF + H2O}}


=== Other uses ===
===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}}</ref>
⚫
It is also used in [[ceramic]]s and some [[Portland cement]] formulations. 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>

⚫
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.
It is good radiation protection against free neutrons.


==Price==
==Price==
In 2012, the price of lithium hydroxide was about $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 |access-date=12 April 2018}}</ref>
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>
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 has risen to US$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|url-status=live|access-date=22 March 2021|website=[[LME The London Metal Exchange]]}}</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 ==
==See also==
* [[Soda lime]]
* [[Soda lime]]


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


== External links ==
==External links==
{{Commons category}}
{{Commons category}}
*{{ICSC|0913}} (anhydrous)
*{{ICSC|0913}} (anhydrous)
Line 208: Line 159:


{{Lithium compounds}}
{{Lithium compounds}}
{{Hydroxides}}

{{Authority control}}
{{Authority control}}


{{DEFAULTSORT:Lithium Hydroxide}}
[[Category:Lithium compounds]]
[[Category:Lithium compounds]]
[[Category:Hydroxides]]
[[Category:Hydroxides]]
[[Category:Rebreathers|*]]
[[Category:Rebreather components|*]]

Latest revision as of 12:21, 25 August 2024

Lithium hydroxide
Lithium hydroxide

  Li+       O2−       H+
Lithium-hydroxide.jpg
Names
IUPAC name
Lithium hydroxide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.013.804 Edit this at Wikidata
68415
RTECS number
  • OJ6307070
UNII
UN number 2680
  • InChI=1S/Li.H2O/h;1H2/q+1;/p-1 checkY
    Key: WMFOQBRAJBCJND-UHFFFAOYSA-M checkY
  • InChI=1/Li.H2O/h;1H2/q+1;/p-1
    Key: WMFOQBRAJBCJND-REWHXWO
  • [Li+].[OH-]
Properties
LiOH
Molar mass
  • 23.95 g/mol (anhydrous)
  • 41.96 g/mol (monohydrate)
Appearance white solid
Odor none
Density
  • 1.46 g/cm3 (anhydrous)
  • 1.51 g/cm3 (monohydrate)
Melting point 462 °C (864 °F; 735 K)
Boiling point 924 °C (1,695 °F; 1,197 K) (decomposes)
  • anhydrous:
  • 12.7 g/(100 mL) (0 °C)
  • 12.8 g/(100 mL) (20 °C)
  • 17.5 g/(100 mL) (100 °C)
  • monohydrate:
  • 22.3 g/(100 mL) (10 °C)
  • 26.8 g/(100 mL) (80 °C)[1]
Solubility in methanol
  • 9.76 g/(100 g) (anhydrous; 20 °C, 48 hours mixing)
  • 13.69 g/(100 g) (monohydrate; 20 °C, 48 hours mixing)[2]
Solubility in ethanol
  • 2.36 g/(100 g) (anhydrous; 20 °C, 48 hours mixing)
  • 2.18 g/(100 g) (monohydrate; 20 °C, 48 hours mixing)[2]
Solubility in isopropanol
  • 0 g/(100 g) (anhydrous; 20 °C, 48 hours mixing)
  • 0.11 g/(100 g) (monohydrate; 20 °C, 48 hours mixing)[2]
Acidity (pKa) 14.4[3]
Conjugate base Lithium monoxide anion
−12.3·10−6 cm3/mol
  • 1.464 (anhydrous)
  • 1.460 (monohydrate)
4.754 D[4]
Thermochemistry[5]
49.6 J/(mol·K)
42.8 J/(mol·K)
−487.5 kJ/mol
−441.5 kJ/mol
Enthalpy of fusion (ΔfH⦵fus)
 20.9 kJ/mol (at melting point)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Corrosive
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
210 mg/kg (oral, rat)[6]
Safety data sheet (SDS) "ICSC 0913".
"ICSC 0914". (monohydrate)
Related compounds
Other anions
 Lithium amide
Other cations
Related compounds
 Lithium oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Lithium hydroxide is an inorganic compound with the 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

[edit]

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

Lithium carbonate route

[edit]

Lithium hydroxide is often produced industrially from lithium carbonate in a metathesis reaction with calcium hydroxide:[7]

Li2CO3 + Ca(OH)2 → 2 LiOH + CaCO3

The initially produced hydrate is dehydrated by heating under vacuum up to 180 °C.

Lithium sulfate route

[edit]

An alternative route involves the intermediacy of lithium sulfate:[8][9]

α-spodumene → β-spodumene
β-spodumene + CaO → Li2O + ...
Li2O + H2SO4 → Li2SO4 + H2O
Li2SO4 + 2 NaOH → Na2SO4 + 2 LiOH

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

Commercial setting

[edit]

According to Bloomberg, Ganfeng Lithium Co. Ltd.[10] (GFL or Ganfeng)[11] and Albemarle were the largest producers in 2020 with around 25kt/y, followed by Livent Corporation (FMC) and SQM.[10] 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.[10]

Albemarle's Kemerton WA plant, originally planned to deliver 100kt/y has been scaled back to 50kt/y.[12]

In 2020 Tianqi Lithium's, plant in Kwinana, Western Australia is the largest producer, with a capacity of 48kt/y.[13]

Applications

[edit]

Lithium-ion batteries

[edit]

Lithium hydroxide is mainly consumed in the production of cathode materials for lithium-ion batteries such as lithium cobalt oxide (LiCoO2) and lithium iron phosphate. It is preferred over lithium carbonate as a precursor for lithium nickel manganese cobalt oxides.[14]

Grease

[edit]

A popular lithium grease thickener is lithium 12-hydroxystearate, which produces a general-purpose lubricating grease due to its high resistance to water and usefulness at a range of temperatures.

Carbon dioxide scrubbing

[edit]
Main article: Carbon dioxide scrubber

Lithium hydroxide is used in breathing gas purification systems for spacecraft, submarines, and rebreathers to remove carbon dioxide from exhaled gas by producing lithium carbonate and water:[15]

2 LiOH·H2O + CO2 → Li2CO3 + 3 H2O

or

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 cm3 of carbon dioxide gas. The monohydrate loses its water at 100–110 °C.

Precursor

[edit]

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:[7]

LiOH + HF → LiF + H2O

Other uses

[edit]

It is also used in ceramics and some Portland cement formulations, where it is also used to suppress ASR (concrete cancer).[16]

Lithium hydroxide (isotopically enriched in lithium-7) is used to alkalize the reactor coolant in pressurized water reactors for corrosion control.[17] It is good radiation protection against free neutrons.

Price

[edit]

In 2012, the price of lithium hydroxide was about US$5–6/kg.[18]

In December 2020, it had risen to $9/kg[19]

On 18 March 2021, the price had risen to $11.50/kg[20]

See also

[edit]

References

[edit]
  1. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. ^ a b c Khosravi J (2007). Production of Lithium Peroxide and Lithium Oxide in an Alcohol Medium. Chapter 9: Results. ISBN 978-0-494-38597-5.
  3. ^ Popov K, Lajunen LH, Popov A, Rönkkömäki H, Hannu-Kuure H, Vendilo A (2002). "7Li, 23Na, 39K and 133Cs NMR comparative equilibrium study of alkali metal cation hydroxide complexes in aqueous solutions. First numerical value for CsOH formation". Inorganic Chemistry Communications. 5 (3): 223–225. doi:10.1016/S1387-7003(02)00335-0. Retrieved 21 January 2017.
  4. ^ CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  5. ^ CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  6. ^ Chambers M. "ChemIDplus – 1310-65-2 – WMFOQBRAJBCJND-UHFFFAOYSA-M – Lithium hydroxide anhydrous – Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Retrieved 12 April 2018.
  7. ^ a b Wietelmann U, Bauer RJ (2000). "Lithium and Lithium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_393. ISBN 3-527-30673-0.
  8. ^ "Proposed Albemarle Plant Site" (PDF). Albemarle. Retrieved 4 December 2020.
  9. ^ "Corporate presentation" (PDF). Nemaska Lithium. May 2018. Archived from the original (PDF) on 23 October 2021. Retrieved 5 December 2020.
  10. ^ a b c "China's Ganfeng to Be Largest Lithium Hydroxide Producer". BloombergNEF. 10 September 2020. Retrieved 4 December 2020.
  11. ^ "Ganfeng Lithium Group". Ganfeng Lithium. Retrieved 25 March 2021.
  12. ^ Stephens, Kate; Lynch, Jacqueline (27 August 2020). "Slowing demand for lithium sees WA's largest refinery scaled back". www.abc.net.au.
  13. ^ "Largest of its kind lithium hydroxide plant launched in Kwinana". Government of Western Australia. 10 September 2019. Archived from the original on 17 February 2023. Retrieved 4 December 2020.
  14. ^ Barrera, Priscilla (27 June 2019). "Will Lithium Hydroxide Really Overtake Lithium Carbonate? | INN". Investing News Network. Retrieved 5 December 2020.
  15. ^ Jaunsen JR (1989). "The Behavior and Capabilities of Lithium Hydroxide Carbon Dioxide Scrubbers in a Deep Sea Environment". US Naval Academy Technical Report. USNA-TSPR-157. Archived from the original on 2009-08-24. Retrieved 2008-06-17.{{cite journal}}: CS1 maint: unfit URL (link)
  16. ^ Kawamura M, Fuwa H (2003). "Effects of lithium salts on ASR gel composition and expansion of mortars". Cement and Concrete Research. 33 (6): 913–919. doi:10.1016/S0008-8846(02)01092-X. OSTI 20658311. Retrieved 2022-10-17.
  17. ^ Managing Critical Isotopes: Stewardship of Lithium-7 Is Needed to Ensure a Stable Supply, GAO-13-716 // U.S. Government Accountability Office, 19 September 2013; pdf
  18. ^ "Lithium Prices 2012". investingnews.com. Investing News Network. 14 June 2012. Archived from the original on 11 March 2018. Retrieved 12 April 2018.
  19. ^ "London Metal Exchange: Lithium prices". London metal exchange. Retrieved 4 December 2020.
  20. ^ "LITHIUM AT THE LME". LME The London Metal Exchange. 18 March 2021. Retrieved 22 March 2021.
[edit]
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