Lithium Hydroxide hydrate
Lithium hydroxide monohydrate
CAS: 1310-66-3
Molecular Formula: Li.HO.H2O
Lithium Hydroxide hydrate - Names and Identifiers
| Name | Lithium hydroxide monohydrate |
| Synonyms | lithium hydrate Lithium Hydroxide hydrate Lithium hydroxide hydrate LITHIUM HYDROXIDE-1-HYDRATE Lithium hydroxide monohydrate Monohydrate Lithium Hydroxide |
| CAS | 1310-66-3 |
| EINECS | 603-454-3 |
| InChI | InChI=1/Li.2H2O/h;2*1H2/q+1;;/p-1/i1+0; |
| InChIKey | WMFOQBRAJBCJND-UHFFFAOYSA-M |
Lithium Hydroxide hydrate - Physico-chemical Properties
| Molecular Formula | Li.HO.H2O |
| Molar Mass | 41.96 |
| Density | 1.51 |
| Melting Point | 462 °C |
| Boling Point | 920 °C |
| Water Solubility | 109 g/L (20 ºC) |
| Solubility | H2O: 1M at20°C, clear, colorless |
| Appearance | Solid |
| Specific Gravity | 1.51 |
| Color | White to cream or yellow |
| Odor | Odorless |
| Maximum wavelength(λmax) | ['λ: 260 nm Amax: 0.02', , 'λ: 280 nm Amax: 0.02'] |
| Merck | 14,5534 |
| PH | ~12 (25℃, 1M in H2O) |
| Storage Condition | Store at room temperature. |
| Stability | Stable. Incompatible with moisture. strong acids, carbon dioxide. Absorbs carbon dioxide from the air. |
| Sensitive | Air Sensitive & Hygroscopic |
| Physical and Chemical Properties | White crystalline powder. Density 1.46g/cm3. Melting point 462 C, boiling point 924 C (decomposition). Soluble in water, slightly soluble in alcohol. It can absorb carbon dioxide from the air and deteriorate. It is strongly alkaline. It will not burn, but it is highly corrosive. Usually in the form of a water. |
| Use | To be used as a raw material for the preparation of lithium compounds. Can also be used in metallurgy, petroleum, glass, ceramic and other industries |
Lithium Hydroxide hydrate - Risk and Safety
| Hazard Symbols | C - Corrosive |
| Risk Codes | R22 - Harmful if swallowed R35 - Causes severe burns R20/22 - Harmful by inhalation and if swallowed. R34 - Causes burns R52 - Harmful to aquatic organisms |
| Safety Description | S26 - In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. S36/37/39 - Wear suitable protective clothing, gloves and eye/face protection. S45 - In case of accident or if you feel unwell, seek medical advice immediately (show the label whenever possible.) S22 - Do not breathe dust. S27 - Take off immediately all contaminated clothing. |
| UN IDs | UN 2680 8/PG 2 |
| WGK Germany | 2 |
| RTECS | OJ6307080 |
| FLUKA BRAND F CODES | 3-9-34 |
| TSCA | Yes |
| HS Code | 28252000 |
| Hazard Class | 8 |
| Packing Group | II |
Lithium Hydroxide hydrate - Upstream Downstream Industry
| Raw Materials | Lithium atomic absorption standard solution |
Lithium Hydroxide hydrate - Reference Information
| pH indicator color change ph range | 14 |
| NIST chemical information | Information provided by: webbook.nist.gov (external link) |
| EPA chemical information | Information provided by: ofmpub.epa.gov (external link) |
| Introduction | Lithium hydroxide is a strong base, and its chemical properties are more similar to the group 2 hydroxide in the periodic table, but with the group 1 hydroxide There is a big difference. It is a white tetragonal crystal, which is strongly corrosive and irritating to the skin, with a melting point of 450 ℃ and a relative density of 1.46. The decomposition temperature is 924 ℃. Slightly soluble in ethanol, soluble in water, but less soluble than other alkali metal hydroxides. Monohydrate is obtained after moisture absorption in air or when crystallized in aqueous solution. Reacts with acid gases such as sulfur dioxide, hydrogen chloride, and hydrogen cyanide. It can also react completely with strong or weak acids in aqueous solution. Carbon dioxide is absorbed in the air to produce lithium carbonate. |
| application | lithium hydroxide is used as grease additive (thickener, anti-oxidant, extreme pressure agent), which can improve heat resistance, water resistance, stability and mechanical properties, and can be used for bearings of automobiles, airplanes, cranes, etc.; as electrolyte raw material for lithium batteries. The roasted solid lithium hydroxide can be used as a carbon dioxide absorber for spacecraft, submarines and other crew members. The early Mercury, Gemini and Apollo programs and space shuttles in the United States all used lithium hydroxide absorbers, which are reliable in performance. Carbon dioxide can be easily absorbed in the gas containing water vapor. Its chemical reaction formula is: 2LiOH + CO2 → Li2CO3 + H2O,1g of anhydrous lithium hydroxide can absorb 450ml of carbon dioxide, and only 750g per person a day is enough to absorb all exhaled carbon dioxide. In addition, lithium hydroxide is also widely used as raw materials for the preparation of other lithium compounds and lithium salts, as well as lithium soaps, lithium-based greases, alkyd resins, expansion agents for spectral analysis, additives in alkaline batteries, photographic developers and catalysts. As an additive for alkaline battery electrolyte, it can increase the capacitance by 12% ~ 15% and increase the service life by 2~3 times |
| Development history | In 1944, anhydrous lithium hydroxide was used as a carbon dioxide absorbent in submarines, and lithium hydride was used as an inflatable source for military balloons. In 1950, the isotope 6Li was used as a raw material for the production of thermonuclear weapons such as hydrogen bombs. The U.S. atomic energy industry began to use lithium hydroxide in large quantities, which made the lithium industry achieve amazing development. Lithium and lithiates are widely used in military and civil industries due to their unique chemical and physical properties. The electrolytic aluminum industry is the largest user of lithium. Adding lithium carbonate to aluminum electrolysis can reduce the melting point of the electrolyte and improve the current efficiency of the aluminum electrolysis cell, thereby increasing the aluminum output by about 10% and reducing the power consumption by 8-14%; in addition, it can also inhibit the discharge of 22%-38% harmful fluorine. In the United States and Europe, the amount of lithium carbonate consumed by the aluminum industry accounts for about 40% of the total amount of lithium. |
| Chemical reaction | 1. When lithium hydroxide is isolated from air and heated to 600 ℃, lithium oxide and water are generated. The chemical reaction equation: 2LiOH = Li2O H2O. 2. Under heating conditions, lithium hydroxide reacts with magnesium or calcium to generate metallic lithium and corresponding oxides. (1)2LiOH Mg = 2Li MgO H2O (2)2LiOH Ca = 2Li CaO H2O 3, lithium hydroxide reacts with chlorine or iodine to generate lithium halide and lithium hypohalide. (1)2LiOH Cl2 = LiCl LiOCl H2O (2)2LiOH I2 = LiI LiOI H2O 4, lithium hydroxide reacts with zinc to form lithium zincate and hydrogen, chemical reaction equation: 2LiOH Zn = LiZnO2 H2. 5. Lithium hydroxide reacts with acid to generate lithium salt (or lithium salt hydrate) and water of the corresponding acid. (1)LiOH HBO2 7H2O = LiBO2 8H2O(2)2LiOH H3PO4 = Li2HPO4 2H2O(3)2LiOH H2SO4 = Li2SO4 2H2O (4)LiOH (excess) HClO4 = LiClO4 H2O 6. Lithium chloride can be generated by the mixed solution of lithium hydroxide with ammonium chloride and lithium tetraiodionated mercury (II) acid, calcium chloride or barium chloride. (1)4LiOH 2Li2HgI4 NH4Cl=LiCl 7LiI Ohg2NH2I 3H2O(2)2LiOH CaCl2=2LiCl Ca(OH)2 (3)2LiOH BaCl2=2LiCl Ba(OH)2 |
| Preparation method | Using lithium carbonate as raw material and reacting with calcium hydroxide, lithium hydroxide monohydrate can be prepared. In this reaction, since the solubility of both raw materials is relatively small, it must be fully stirred. In the above reaction, only a solution containing the 3.5% concentration of this product can be obtained, and the solubility of lithium carbonate will be reduced due to the generation of lithium hydroxide, and it will remain in the precipitation of calcium carbonate and will not dissolve. Therefore, as the reaction progresses, the calcium carbonate precipitate must be removed at any time, and the lithium carbonate must be washed and recovered. The mother liquor after calcium carbonate precipitation is removed, and further concentrated under reduced pressure can precipitate monohydrate. After separation, it can be dried at 130~140 ℃ to obtain monohydrate. Anhydrous lithium hydroxide can be prepared by drying monohydrate at 150~180 ℃. |
| use | petroleum, chemical, light industry, nuclear industry, etc. When used in alkaline storage batteries, the aluminum content is not more than 0.06% and the lead content is not more than 0.01%. It is used as an analytical reagent, a photographic developer, and also used in the manufacture of lithium It is used as a raw material for the preparation of lithium compounds. It can also be used in metallurgy, petroleum, glass, ceramics and other industries Battery-grade lithium monohydrate is mainly used for the preparation of lithium ion battery cathode materials, and can also be used as an additive for alkaline battery electrolyte Photographic developer, Preparation of lithium salt, production of alcohol to resin, catalyst. Reagents for the decomposition of oxides and silicates Titration of organic acids. Photographic developer. Preparation of lithium salt. Manufacture alkyd resin. Catalyst. Alkaline batteries. |
| production method | lime sintering spodumene concentrate (generally containing 6% lithium oxide), mixed with limestone, ground, sintered at 1150~1250 ℃ to produce lithium aluminate and calcium silicate, crushed by wet grinding, leaching lithium hydroxide with washing liquid, sedimentation filtration, evaporation and concentration of leaching liquid, crystallization to produce lithium hydroxide monohydrate finished product, its Li2O?AI2O3?4SiO2_2 8CaO → Li2O?A12O3 4[2caO?SiO2]Li2O?AI2O3 Ca(OH)2 → 2LiOH CaO?AI2O3 |
Last Update：2024-04-10 22:29:15
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Lithium Hydroxide hydrate
2-OXOPENTANEDIOIC ACID MONOSODIUM SALT
HEPTYL CHLOROFORMATE
4-Iodobenzoic acid
4-溴-2-三甲基硅烷基噻唑
仲丁基溴化镁, 1.0 M 四氢呋喃溶液, J&KSEAL瓶
2-OXOPENTANEDIOIC ACID MONOSODIUM SALT
HEPTYL CHLOROFORMATE
4-Iodobenzoic acid
4-溴-2-三甲基硅烷基噻唑
仲丁基溴化镁, 1.0 M 四氢呋喃溶液, J&KSEAL瓶
Raw Materials for Lithium Hydroxide hydrate