Editing Lithium hydroxide (section)

{{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.