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Lithium hydroxide

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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-REWHXWOFAT
  • [Li+].[OH-]
Properties
LiOH
Molar mass
  • 23.95 g/mol (anhydrous)
  • 41.96 g/mol (monohydrate)
Appearance
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]
Basicity (pKb) −0.04[3]
Conjugate base Lithium monoxide anion
−12.3·10−6 cm3/mol
  • 1.464 (anhydrous)
  • 1.460 (monohydrate)
Thermochemistry
2.071 J/g⋅K
−20.36 kJ/g
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)[4]
Safety data sheet (SDS) "ICSC 0913".
"ICSC 0914". (monohydrate)
Related compounds
Other anions
 Lithium amide
Other cations
 Sodium hydroxide
Potassium hydroxide
Rubidium hydroxide
Caesium hydroxide
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 is a white hygroscopic crystalline material. It is soluble in water and slightly soluble in ethanol, and is available commercially in anhydrous form and as the monohydrate (LiOH.H2O). While lithium hydroxide is a strong base, it is the weakest known alkali metal hydroxide.

Production

According to Bloomberg, Ganfeng Lithium Co. Ltd.[5] (GFL or Ganfeng) and Albemarle were the largest producers in 2020 with around 25kt/y, followed by Livent (FMC) and SQM.[5] 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.[5]

Albemarle's Kemerton WA plant, originally planned to deliver 100kt/y has been scaled back to 50kt[6]

Lithium hydroxide was mainly produced industrially from lithium carbonate in a metathesis reaction between lithium carbonate and calcium hydroxide:[7]

Li2CO3 + Ca(OH)2 → 2 LiOH + CaCO3

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

In 2020 the volume of direct production from spodumene had become significant.

In 2020 the largest lithium hydroxide plant in the world was reported to be Tianqi Lithium's, plant in Kwinana, Western Australia, with a capacity of 48kt/y.[8]

Typical process flows follow this route:[9][10]

α-Spodumene → β-spodumene (+CaO) → Li2O (+H2SO4) → Li2SO4 (+NaOH) → Na2SO4 + LiOH.

The main by-products, gypsum and sodium sulphate are sold if possible.

Chemistry and reactions

Lithium carbonate and hydroxide are the principal intermediates used for the production of other lithium compounds, e.g.

LiOH + HF → LiF + H2O.

Gas phase chemistry

The acidity of LiOH has been measured in the gas phase. The oxidolithium anion, LiO–, was produced by successive decarboxylation and decarbonylation of monolithium oxalate anion, LiO(C=O)(C=O)O–, by collision-induced dissociation and was identified by its exact mass. The gas-phase acidity of LiOH was inferred from the experimentally determined electron affinity of LiO• and previously known heats of formation to give a value of 426 ± 2 kcal/mol. This is considerably higher than the gas-phase acidity of water (390 kcal/mol) and even exceeds that of methane (417 kcal/mol). Thus, LiOH is a very weak acid and is in fact the weakest acid yet measured in the gas phase.[11]

Applications

Lithium ion batteries

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.[12]

Grease

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

Further information: 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:[13]

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.

Other uses

It is also used in ceramics and some Portland cement formulations. Lithium hydroxide (isotopically enriched in lithium-7) is used to alkalize the reactor coolant in pressurized water reactors for corrosion control.[14]

Price

on 18 March 2021 the price has risen to US$11.50/kg[15]

In 2012, the price of lithium hydroxide was about $5-6/kg.[16]

In December 2020 it had risen to $9/kg[17]

See also

References

  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. Retrieved 21 January 2017.
  4. ^ 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.
  5. ^ a b c "China's Ganfeng to Be Largest Lithium Hydroxide Producer". BloombergNEF. 10 September 2020. Retrieved 4 December 2020.
  6. ^ Stephens, Kate; Lynch, Jacqueline (27 August 2020). "Slowing demand for lithium sees WA's largest refinery scaled back". www.abc.net.au.
  7. ^ Wietelmann U, Bauer RJ (2000). "Lithium and Lithium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a15_393. ISBN 3-527-30673-0.
  8. ^ "Largest of its kind lithium hydroxide plant launched in Kwinana". Government of Western Australia. 10 September 2019. Retrieved 4 December 2020.
  9. ^ "Proposed Albemarle Plant Site" (PDF). Albemarle. Retrieved 4 December 2020.
  10. ^ "Corporate presentation" (PDF). Nemaska Lithium. May 2018. Retrieved 5 December 2020.
  11. ^ Tian Z, Chan B, Sullivan MB, Radom L, Kass SR (June 2008). "Lithium monoxide anion: a ground-state triplet with the strongest base to date". Proceedings of the National Academy of Sciences of the United States of America. 105 (22): 7647–51. doi:10.1073/pnas.0801393105. PMC 2409378. PMID 18511563.
  12. ^ Barrera, Priscilla (27 June 2019). "Will Lithium Hydroxide Really Overtake Lithium Carbonate? | INN". Investing News Network. Retrieved 5 December 2020.
  13. ^ 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.
  14. ^ 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
  15. ^ "LITHIUM AT THE LME". LME The London Metal Exchange. 18 March 2021. Retrieved 22 March 2021.{{cite web}}: CS1 maint: url-status (link)
  16. ^ "Lithium Prices 2012". investingnews.com. Investing News Network. Retrieved 12 April 2018.
  17. ^ "London Metal Exchange: Lithium prices". London metal exchange. Retrieved 4 December 2020.
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