| 外観 | 白色の結晶 |
| 種類 | 塩化リチウムは、数種類の水和物が存在します。他のアルカリ金属とは異なり、一水和物、三水和物、五水和物の水和物を形成します。
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| 性質 | 化学式はLiClで表され、分子量は42.39です。CAS番号は7447-41-8で登録されています。塩化リチウムは融点614°C、沸点は1357°Cで、常温で無色の結晶、密度2.07g/mlの固体です。
吸湿性で、無臭、塩味を持ちます。アルコーやエーテル、、に可溶です。塩化ナトリウムや塩化カリウムと比べて、などの極性の有機溶媒によく溶けます。水へは非常に溶けやすく、25 °Cで100gの水には84.5 g溶けます。水溶液はpH5.0〜7.0と、中性～弱アルカリ性です (50g/L、25℃) 。
塩化リチウムは、塩化物イオンの発生源として、金属塩と混合すると、不溶性の塩化物塩を沈殿させます。
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| 定義 | 本品は、リチウムの塩化物であり、次の化学式で表される。 |
| 溶解性 | 水に易溶。エタノールやピリジンなどの塩基性有機溶媒に可溶。水に溶けやすく、エタノールにやや溶けやすい。 |
| 解説 | 塩化リチウム．炭酸リチウムまたは水酸化リチウムを塩酸に溶かし，蒸発乾固して得られる．白色の岩塩型結晶．融点614 ℃，沸点1357 ℃．密度2.07 g cm－3．潮解性があり，水に易溶，エタノール，メタノール，エーテル，ピリジンに可溶．融解塩電解によるリチウム金属精錬の原料，アルミニウム精錬の際の融解塩電解浴の添加剤，空調装置の除湿剤，湿度センサー，熱交換用媒体，ろう付け用融剤，電池の電極製造，焔(えん)色剤(紅色)などに用いられる． |
| 用途 | 1) 電解して金属リチウムを製造する。2) 空気調節、熱交換用媒体に用いる。 |
| 製造法 | またはとを作用させることで、塩化リチウムが得られます。塩化リチウムを含む水溶液は強い腐食性を持つため、反応には特殊なスチール製、またはニッケル製の装置が必要です。
反応後の溶液を濃縮することで、塩化リチウムは結晶化します。その後母液から分離して乾燥させます。無水塩化リチウムは、塩化水素気流中で加熱することによって水和物から調製可能です。 |
| 用途 | ミネラルウォーターの製造、花火、アルミニウムのはんだ付け、冷凍機、気体の乾燥、吸収タイプの空調機、熔融した塩化リチュームは金属酸化物をよく溶解するので、溶接時のフラックス、アルミはんだのフラックス |
| 用途 | RNAの沈殿等。 |
| 用途 | 熱交換媒体、温度調整剤、医薬原料 |
| 使用上の注意 | 潮解性あり |
| 化学的特性 | Lithium chloride is a White cubic crystals; granules or powder; hygroscopic; sharp salt-like taste; melts at 605°C; vaporizes around 1360°C, It has an unusually high water solubility when compared to the other alkali metal chlorides; readily dissolves in water (64g/100mL at 0°C); also highly soluble in alcohol and pyridine; moderately soluble in acetone (4.1 g/100mL at 25°C).
The following hydrates are known: LiCl·H2O, LiCl-3H20 and LiCl- 5H2O. The higher hydrates are stable at progressively lower temperatures. Lithium chloride is deliquescent under normal atmospheric conditions.
Lithium chloride is soluble to a significant extent in many polar organic liquids. It is generally most soluble in alcohols in which the solubility decreases as the size of the organic radical increases.
It dehumidifies air for industrial drying and for air conditioning. Lithium chloride bums with a chrims on flame and is used in pyrotechnics. It is also used as a pyrotechnic in welding and brazing fluxes. |
| 物理的性質 | White cubic crystals; granules or powder; hygroscopic; sharp salt-like taste; refractive index 1.662; density 2.068 g/cm3; melts at 605°C; vaporizes around 1,360°C; readily dissolves in water (64g/100mL at 0°C); also highly soluble in alcohol and pyridine; moderately soluble in acetone (4.1 g/100mL at 25°C). |
| 使用 | Lithium chloride is useful for the production of lithium metal, and for the generation of Mn(0) species which can be used in free radical cyclizations. It can serve as a flame colorant to generate dark red flames, a brazing flux for aluminum in automobiles, a hygrometer, and a desiccant for drying air streams. On exposure to air, it becomes a solution with the concentration directly related to relative humidity of the atmosphere, and hence serves as a relative humidity standard in calibrating hygrometers. Apart from being a source of chloride, it serves as an additive in the Stille reaction in organic synthesis, and to precipitate RNA from cellular extracts. Being biologically significant, it finds applications in a wide variety of assays to study cell-fate and neurobiology. Lithium chloride has been found to inhibit virus infection. |
| 主な応用 | Lithium chloride solution can be used:
(1) obtaining dendritic cells in the form of LiClPAM3 DCs;
(2) LiCl buffer preparation for immunoprecipitation;
(3) in the preparation of washing buffers;
(4) in the preparation of washing buffers for radioimmunoprecipitation assays (RIPA);
(5) can be used for selective precipitation of RNA. |
| 定義 | ChEBI: Lithium chloride is a metal chloride salt with a Li(+) counterion. It has a role as an antimanic drug and a geroprotector. It is an inorganic chloride and a lithium salt. |
| 製造方法 | Lithium chloride may be prepared by reaction of lithium carbonate or lithium hydroxide with hydrochloric acid followed by crystallization:
(1) Li2CO3+ 2HCl →2LiCl + CO2+ H2O
(2) LiOH + HCl →LiCl + H2O
Crystallization above 95°C yields anhydrous salt. Hot solution upon cooling forms crystals of monohydrate, LiCl.H2O.
The solid and solution are separated and the supernatant solution is recycled for further evaporation. The crystals are dried to yield anhydrous lithium chloride.
Lithium chloride can be synthesized from its elements by heating lithium metal with chlorine gas.
It also may be obtained from natural brine. |
| 一般的な説明 | Colorless crystals or powder. Low toxicity. |
| 空気と水の反応 | Very hygroscopic. Very soluble in water. |
| 反応プロフィール | These materials have weak oxidizing or reducing powers. Redox reactions can however still occur. For example, CO2, which is often regarded as chemically inert, vigorously oxidizes the strong reducing agent Mg if the two are heated together. The majority of compounds in this class are slightly soluble or insoluble in water. If soluble in water, then the solutions are usually neither strongly acidic nor strongly basic. These compounds are not water-reactive. Some do react with acids: carbonates generate carbon dioxide and heat when treated with acids; fluorides, sulfites and sulfides generate toxic gases (hydrogen fluoride, sulfur dioxide and hydrogen sulfide, respectively) when treated with acids. |
| 火災危険 | Flash point data for Lithium chloride are not available. Lithium chloride is probably combustible. |
| 取り扱い及び保管上の注意 | 取り扱い時の対策
強酸化剤は、塩化リチウムの混触危険物質です。取り扱い時および保管時の接触を避けてください。塩化リチウム水溶液は、強い腐食性を持つため、目や皮膚に接触しないように、慎重に取り扱う必要があります。
取り扱う際は、保護手袋と側板付きの保護メガネ、袖の長い保護衣を着用し、ドラフトチャンバー内で使用してください。使用後は、手をよく洗います。
火災の場合
燃焼により、ハロゲン化物と金属酸化物など、刺激性で有毒なガスと蒸気を放出するおそれがあります。消火には、水噴霧や泡消火剤、粉末消火剤、炭酸ガス、乾燥砂などを用いてください。
保管する場合
ポリエチレン製の容器に密閉し、直射日光を避けた涼しい場所に保管してください。保管場所は施錠します。 |
| 化学性质 | 融点605℃，沸点1382℃，潮解性，種々の水和物LiCl?nHOが存在 |
| 使用用途 | 1. リチウム金属原料
塩化リチウムは、リチウム金属を製造するために使用されます。リチウム金属は、塩化リチウムとの混合物を450℃で融解させて電気分解することにより製造されます。
2. カップリング反応の添加剤
塩化リチウムは、右田・小杉・スティルカップリング (英: Migita-Kosugi-Stille coupling) の添加剤として用いられます。右田・小杉・スティルカップリングとは、存在下、有機スズ化合物とハロゲン化物をクロスカップリングさせ、炭素‐炭素結合を形成する反応です。
3. その他
溶融した塩化リチウムは、金属酸化物を溶解することから、アルミはんだの補助剤として、自動車部品の製造に利用されます。
吸湿性を持つことから、空調装置の除湿剤としても利用されています。塩化リチウムは、引火すると赤く燃えることから、花火などの炎色剤の1種です。
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| 工業用途 | Lithium chloride solutions are used in large dehumidification systems in the air-conditioning industry. This use depends on the low equilibrium pressure of water vapor above solutions of lithium chloride. After the solutions have absorbed water, they are regenerated by heating.
Lithium chloride is used in a number of salt mixtures. Such salt mixtures have low melting points allowing the material to be used in brazing fluxes and brazing baths. The molten lithium chloride-potassium chloride eutectic mixture can be used as an electrolyte. The mixture is electrolyzed for the production of lithium metal and is used as an electrolyte in voltaic cells.
Lithium chloride is also used in manufacture of mineral waters; in pyrotechnics; soldering aluminum; in refrigerating machines. |
| Biochem/physiol Actions | Lithium chloride has the ability to block glycogen synthase kinase (GSK). It may also possess anti-inflammatory effects at low and non-toxic concentrations. |
| 安全性プロファイル | Human poison by
ingestion. Experimental poison by
intravenous and intracerebral routes.
Moderately toxic by subcutaneous and
intraperitoneal routes. Experimental
teratogenic and reproductive effects. Human
systemic effects by ingestion: somnolence,
tremors, nausea or vomiting. An eye and
severe skin irritant. Human mutation data
reported. Questionable carcinogen with
experimental neoplastigenic data. This
material has been recommended and used as
a substitute for sodwm chloride in "saltfree" diets, but cases have been reported in
which the ingestion of lithium chloride has
produced dminess, ringing in the ears,
visual disturbances, tremors, and mental
confusion. In most cases, the symptoms
disappeared when use was discontinued.
Prolonged absorption may cause disturbed
electrolyte balance, impaired renal function.
Reaction is violent with BrF3. When heated
to decomposition it emits toxic fumes of
Cl-. Used for dehumidification in the air
conditioning industry. Also used to obtain
lithum metal. See also LITHIUM
COMPOUNDS. |
| 合成方法 | 炭酸リチウムに塩酸を加え，沈殿を200℃以上で加熱脱水する |
| 純化方法 | Crystallise it from water (1mL/g) or MeOH and dry it for several hours at 130o. Other metal ions can be removed by preliminary crystallisation from hot aqueous 0.01M disodium EDTA. It has also been crystallised from conc HCl, fused in an atmosphere of dry HCl gas, cooled under dry N2 and pulverised in a dry-box. Kolthoff and Bruckenstein [J Am Chem Soc 74 2529 1952] precipitated it with ammonium carbonate, washed it with Li2CO3 five times by decantation and finally with suction, then dissolved it in HCl. The LiCl solution is evaporated slowly with continuous stirring in a large evaporating dish, the dry powder being stored (while still hot) in a desiccator over CaCl2. |
| 参考文献 | G.I. Finch, S. Fordham, Proc. Phys. Soc., 48, 85 (1936), DOI: 10.1088/0959-5309/48/1/312. |