| 词条 | Lithium hydroxide |
| 释义 |
| 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}}Li+ {{colorbox|#EE0000}}{{nbsp}}O2− {{colorbox|#FFFFFF}}{{nbsp}}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 | InChI = 1/Li.H2O/h;1H2/q+1;/p-1 | InChIKey = WMFOQBRAJBCJND-REWHXWOFAT | ChEBI_Ref = {{ebicite|correct|EBI}} | 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|changed|??}} | CASNo2_Comment = (monohydrate) | PubChem = 3939 | RTECS = OJ6307070 | UNNumber = 2680 | Gmelin = 68415 }} |Section2={{Chembox Properties | Odor = none | Formula = LiOH | MolarMass = {{ubl | 23.95 g/mol (anhydrous) | 41.96 g/mol (monohydrate) | Appearance = {{ubl | Hygroscopic white solid | Density = {{ubl | 1.46{{nbsp}}g/cm3 (anhydrous) | 1.51{{nbsp}}g/cm3 (monohydrate) | MeltingPtC = 462 | BoilingPtC = 924 | BoilingPt_notes = decomposes | Solubility = {{ubl | (anhydrous:) | 12.7 g/100{{nnbsp}}mL (0 °C) | 12.8 g/100{{nnbsp}}mL (20 °C) | 17.5 g/100{{nnbsp}}mL (100 °C) | | (monohydrate:) | 22.3 g/100{{nnbsp}}mL (10 °C) | 26.8 g/100{{nnbsp}}mL (80 °C)[1] | Solvent1 = methanol | Solubility1 = {{ubl | 9.76 g/100{{nnbsp}}g (anhydrous; 20 °C, 48 hours mixing) | | 13.69 g/100{{nnbsp}}g (monohydrate; 20 °C, 48 hours mixing)[2] | Solvent2 = ethanol | Solubility2 = {{ubl | 2.36 g/100{{nnbsp}}g (anhydrous; 20 °C, 48 hours mixing) | | 2.18 g/100{{nnbsp}}g (monohydrate; 20 °C, 48 hours mixing)[2] | Solvent3 = isopropanol | Solubility3 = {{ubl | 0 g/100{{nnbsp}}g (anhydrous; 20 °C, 48 hours mixing) | | 0.11 g/100{{nnbsp}}g (monohydrate; 20 °C, 48 hours mixing)[2] | RefractIndex = {{ubl | 1.464 (anhydrous) | | 1.460 (monohydrate) | pKb = −0.04[3] (LiOH(aq) = Li+ + OH–) | ConjugateBase = Lithium monoxide anion | MagSus = −12.3·10−6{{nbsp}}cm3/mol }} |Section4={{Chembox Thermochemistry | DeltaHf = −20.36 kJ/g | DeltaHc = | Entropy = | HeatCapacity = 2.071 J/g⋅K }} |Section5={{Chembox Hazards | ExternalSDS = {{cite web |url=http://www.inchem.org/documents/icsc/icsc/eics0913.htm |title=ICSC 0913}} {{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{{nbsp}}mg/kg (oral, rat)[4] }} |Section8={{Chembox Related | OtherAnions = Lithium amide | OtherCations = Sodium hydroxide Potassium hydroxide Rubidium hydroxide Caesium hydroxide | OtherCompounds = Lithium oxide }} }} 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), both of which are strong bases. It is the weakest base among the alkali metal hydroxides. Production and reactionsLithium hydroxide is produced in a metathesis reaction between lithium carbonate and calcium hydroxide:[5] Li2CO3 + Ca(OH)2 → 2 LiOH + CaCO3 The initially produced hydrate is dehydrated by heating under vacuum up to 180 °C. In the laboratory, lithium hydroxide arises by the action of water on lithium or lithium oxide. The equations for these processes follow: 2 Li + 2 H2O → 2 LiOH + H2 Li2O + H2O → 2 LiOH Typically, these reactions are avoided. Although lithium carbonate is more widely used, the hydroxide is an effective precursor to lithium salts, e.g. LiOH + HF → LiF + H2O. Gas phase chemistryThe 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.[6] ApplicationsLithium hydroxide is mainly consumed in the production of lithium greases. 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|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:[7] 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 usesIt is used as a heat transfer medium and as a storage-battery electrolyte. 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. MarketIn 2012, the price of lithium hydroxide was about $5,000 to $6,000 per tonne.[8] See also
References1. ^{{RubberBible87th}} 2. ^1 2 {{cite book | last1=Khosravi | first1=Javad | name-list-format = vanc | year=2007 | at=Chapter 9: Results | title=Production of Lithium Peroxide and Lithium Oxide in an Alcohol Medium | isbn=978-0-494-38597-5 }} 3. ^ {{cite journal | vauthors = Popov K, Lajunen LH, Popov A, Rönkkömäki H, Hannu-Kuure H, Vendilo A | year=2002 | title=7Li, 23Na, 39K and 133Cs 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 }} 4. ^{{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-format = vanc |website=chem.sis.nlm.nih.gov |access-date=12 April 2018}} 5. ^{{cite book | vauthors = Wietelmann U, Bauer RJ |year=2000 |chapter=Lithium and Lithium Compounds |title =Ullmann's Encyclopedia of Industrial Chemistry |isbn=3-527-30673-0 |doi=10.1002/14356007.a15_393}} 6. ^{{cite journal | vauthors = Tian Z, Chan B, Sullivan MB, Radom L, Kass SR | title = Lithium monoxide anion: a ground-state triplet with the strongest base to date | journal = Proceedings of the National Academy of Sciences of the United States of America | volume = 105 | issue = 22 | pages = 7647–51 | date = June 2008 | pmid = 18511563 | pmc = 2409378 | doi = 10.1073/pnas.0801393105 | url = http://www.pnas.org/content/105/22/7647 }} 7. ^{{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}} 8. ^{{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}} External links{{Commons category}}
4 : Bases (chemistry)|Lithium compounds|Hydroxides|Rebreathers |
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