1310-65-2 Usage
Physical Properties
Lithium hydroxide is a white tetragonal crystals; refractive index 1.464; density 1.46 g/cm3; melts at 450°C; decomposes at 924°C; dissolves in water (12.8g/100g at 20°C and 17.5 g/100g at 100°C); slightly soluble in alcohol.
Lithium hydroxide monohydrate is white monoclinic crystalline solid; refractive index 1.460; density 1.51 g/cm3; soluble in water, more soluble than the anhydrous salt (22.3g and 26.8g/100g at 10 and 100°C, respectively); slightly soluble in alcohol; insoluble in ether.
Uses
Different sources of media describe the Uses of 1310-65-2 differently. You can refer to the following data:
1. Lithium hydroxide is used as an electrolyte in certain alkaline storage batteries; and in the production of lithium soaps. Other uses of this compound include its catalytic applications in esterification reactions in the production of alkyd resins; in photographic developer solutions; and as a starting material to prepare other lithium salts.
2. The compound is soluble in water. The compound is used in the formulation of lithium soaps used in multipurpose greases; also in the manufacture of various lithium salts; and as an additive to the electrolyte of alkaline storage batteries. LiOH also is an efficient, light-weight absorbent for carbon dioxide.
3. Lithium hydroxide is used as a heat transfer medium, as a storage-battery electrolyte and also used for the production of lithium greases. It is also used in ceramics, in some portland cement formulations, in the absoption of carbondioxide from sealed enviornments such as submarines, spacecrafts and breathing apparatus. It is used in esterification reactions, as stabilizer in photographic developments and as a coolant in pressurized water reactors for corrosion control.
4. Lithium hydroxide is used in storage batteries and soaps and as CO2
absorber in spacecrafts.
Preparation
Lithium hydroxide is prepared by the reaction of lithium carbonate with calcium hydroxide:
Li2CO3 + Ca(OH)2 → 2LiOH + CaCO3
Calcium carbonate is filtered out and the solution is evaporated and crystallized.
The product obtained is the monohydrate, LiOH?H2O. The anhydrous compound is obtained by heating the hydrate above 100°C in vacuum or carbon dioxide-free air.
The hydroxide also may be prepared by treating lithium oxide with water.
Reaction
Lithium hydroxide is a base. However, it is less basic than sodium or potassium hydroxide.
The compound undergoes neutralization reactions with acids:
LiOH + HCl → LiCl + H2O
Heating the compound above 800°C in vacuum yields lithium oxide:
2LiOH Li2O + H2O
Lithium hydroxide readily absorbs carbon dioxide, forming lithium carbonate:
2LiOH + CO2 → Li2CO3 + H2O
Passing chlorine through a solution of lithium hydroxide yields lithium hypochlorite:
LiOH + Cl2 → LiOCl + HCl
Saponification of fatty acids with lithium hydroxide produces lithium soaps.
LiOH + CH3(CH2)16COOH → CH3(CH2)16COOLi + H2O
(stearic acid) ? ? ? ?(lithium stearate)
Chemical Properties
lithium hydroxide (LiOH) is a white solid made industrially as the monohydrate (LiOH.H2O) by reacting lime with a lithium ore or with a salt made from the ore. Lithium hydroxide has a closer resemblance to the group 2 hydroxides than to the group 1 hydroxides.
Physical properties
White tetragonal crystals; refractive index 1.464; density 1.46 g/cm3; melts at 450°C; decomposes at 924°C; dissolves in water (12.8g/100g at 20°C and 17.5 g/100g at 100°C); slightly soluble in alcohol. The monohydrate is white monoclinic crystalline solid; refractive index 1.460; density 1.51 g/cm3; soluble in water, more soluble than the anhydrous salt (22.3g and 26.8g/100g at 10 and 100°C, respectively); slightly soluble in alcohol; insoluble in ether.
Definition
A white crystallinesolid, LiOH, soluble in water,slightly soluble in ethanol and insolublein ether. It is known as the monohydrate(monoclinic; r.d. 1.51) and inthe anhydrous form (tetragonal, r.d.1.46; m.p. 450°C; decomposes at924°C). The compound is made by reacting lime with lithium salts orlithium ores. Lithium hydroxide isbasic but has a closer resemblance togroup 2 hydroxides than to the othergroup 1 hydroxides (an example ofthe first member of a periodic grouphaving atypical properties).
General Description
A clear to water-white liquid which may have a pungent odor. Contact may cause severe irritation to skin, eyes, and mucous membranes. Lithium hydroxide may be toxic by ingestion, inhalation and skin absorption. Lithium hydroxide is used to make other chemicals.
Air & Water Reactions
Dilution with water may generate enough heat to cause steaming or spattering.
Reactivity Profile
LITHIUM HYDROXIDE SOLUTION neutralizes acids exothermically to form salts plus water. Reacts with certain metals (such as aluminum and zinc) to form oxides or hydroxides of the metal and generate gaseous hydrogen. May initiate polymerization reactions in polymerizable organic compounds, especially epoxides. May generate flammable and/or toxic gases with ammonium salts, nitrides, halogenated organics, various metals, peroxides, and hydroperoxides. May serve as a catalyst. Reacts when heated above about 84°C with aqueous solutions of reducing sugars other than sucrose, to evolve toxic levels of carbon monoxide [Bretherick, 5th Ed., 1995].
Health Hazard
TOXIC; inhalation, ingestion or skin contact with material may cause severe injury or death. Contact with molten substance may cause severe burns to skin and eyes. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.
Fire Hazard
Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated.
Safety Profile
Poison by ingestion and
subcutaneous routes. Mtldly toxic by
inhalation. A corrosive. When heated to
decomposition it emits toxic fumes of Li.
Purification Methods
It crystallises from hot water (3mL/g) as the monohydrate. It is dehydrated at 150o in a stream of CO2-free air. It sublimes at 220o with partial decomposition [Cohen Inorg Synth V 3 1957, Bravo Inorg Synth VII 1 1963].
Check Digit Verification of cas no
The CAS Registry Mumber 1310-65-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 1,3,1 and 0 respectively; the second part has 2 digits, 6 and 5 respectively.
Calculate Digit Verification of CAS Registry Number 1310-65:
(6*1)+(5*3)+(4*1)+(3*0)+(2*6)+(1*5)=42
42 % 10 = 2
So 1310-65-2 is a valid CAS Registry Number.
1310-65-2Relevant articles and documents
Lithium-air and lithium-copper batteries based on a polymer stabilized interface between two immiscible electrolytic solutions (ITIES)
Wu, Borong,Chen, Xiaohui,Zhang, Cunzhong,Mu, Daobin,Wu, Feng
, p. 2140 - 2145 (2012)
We propose and demonstrate the direct application of immiscible aqueous/organic interfaces in lithium-air and lithium-copper batteries. Therefore, the two half-reactions are separated in their respectively favourable electrolytic environments without using any other membranes. In order to prevent water and oxygen from interrupting the reaction in organic phases, we add poly(methyl methacrylate) (PMMA) to propylene carbonate (PC) and investigate its concentration effects using Pt ultramicroelectrodes (UMEs). Pt UMEs provide us the sensitive measure of water contamination as well as the diffusion property of oxygen in the polymer electrolytes. By studying the discharge profiles under various electrolytic conditions, we demonstrate that these batteries are of longer discharge time and higher specific capacity when the polymer electrolyte contains about 10 to 20% of PMMA.
Plane, John M. C.,Rajasekhar, B.
, (1988)
Craggs, J. D.,Smee, J. F.
, p. 531 - 531 (1941)
Gucker, F. T.,Schminke, K. H.
, p. 1013 - 1019 (1933)
Fernelius,Watt
, p. 3482 (1933)
Thermal analysis of lithium peroxide prepared by various methods
Ferapontov,Kokoreva,Kozlova,Ul'Yanova
, p. 891 - 894 (2009)
Behavior of lithium peroxide samples at heating in air was studied by the methods of thermogravimetric analysis (TGA) and differential thermal analysis (DTA). In the temperature range from 32 to 82°C all the studied samples we found to react with water vapor forming lithium peroxide monohydrate as confirmed by the methods of chemical analysis and of qualitative X-ray phase analysis. It was found experimentally that in the temperature range from 340 to 348°C lithium peroxide began to decompose into lithium oxide and oxygen, the starting temperature depended on the method of preparation of lithium peroxide. For all the studied samples polymorphism in the temperature range from 25 to 340°C was not detected.
Ye, Zuo-Guang,Muehll, R. Von Der,Ravez, J.,Hagenmueller, P.
, p. 1153 - 1158 (1988)
Popescu, C.,Jianu, V.,Alexandrescu, Rodica,Mihailescu, I. N.,Morjan, I.,Pascu, M. L.
, p. 269 - 276 (1988)
The effect of 3D carbon nanoadditives on lithium hydroxide monohydrate based composite materials for highly efficient low temperature thermochemical heat storage
Li, Shijie,Huang, Hongyu,Li, Jun,Kobayashi, Noriyuki,Osaka, Yugo,He, Zhaohong,Yuan, Haoran
, p. 8199 - 8208 (2018)
Lithium hydroxide monohydrate based thermochemical heat storage materials were modified with in situ formed 3D-nickel-carbon nanotubes (Ni-CNTs). The nanoscale (5-15 nm) LiOH·H2O particles were well dispersed in the composite formed with Ni-CNTs. These composite materials exhibited improved heat storage capacity, thermal conductivity, and hydration rate owing to hydrogen bonding between H2O and hydrophilic groups on the surface of Ni-CNTs, as concluded from combined results of in situ DRIFT spectroscopy and heat storage performance test. The introduction of 3D-carbon nanomaterials leads to a considerable decrease in the activation energy for the thermochemical reaction process. This phenomenon is probably due to Ni-CNTs providing an efficient hydrophilic reaction interface and exhibiting a surface effect on the hydration reaction. Among the thermochemical materials, Ni-CNTs-LiOH·H2O-1 showed the lowest activation energy (23.3 kJ mol-1), the highest thermal conductivity (3.78 W m-1 K-1) and the highest heat storage density (3935 kJ kg-1), which is 5.9 times higher than that of pure lithium hydroxide after the same hydration time. The heat storage density and the thermal conductivity of Ni-CNTs-LiOH·H2O are much higher than 1D MWCNTs and 2D graphene oxide modified LiOH·H2O. The selection of 3D carbon nanoadditives that formed part of the chemical heat storage materials is a very efficient way to enhance comprehensive performance of heat storage activity components.
Determination of the role of Li2O on the corrosion of lithium hydride
Sifuentes, Adalis,Stowe, Ashley C.,Smyrl, Norm
, p. S271-S273 (2013)
Lithium hydride (LiH) will efficiently react with moisture, forming lithium hydroxide (LiOH) on the surface. Typically, diffuse reflectance infrared Fourier transform (DRIFT) spectroscopy is used for studying the surface corrosion reaction. The presence of a surface lithium oxide (Li2O) layer will enhance hydroxide formation kinetics; however, interference in the DRIFT spectrum prevents the role of Li2O on the reaction kinetics from being fully understood. In the current study, Raman spectroscopy has been used to follow the reaction of LiH with moisture, with particular focus on the Li2O vibrational signature. Three vibrations were observed for Li2O after thermal decomposition of LiOH on the LiH surface in contrast to the single vibration at 515 cm-1 for pure Li2O powder. The multiple peaks are indicative on multiple Li2O chemical domains and are likely the substrate through which unstable LiOH domains are formed during subsequent hydrolysis of the LiH/Li2O system.
Beutler, H.,Brauer, G.,Juenger, H. O.
, p. 347 - 347 (1936)
Extended Chemical Flexibility of Cubic Anti-Perovskite Lithium Battery Cathode Materials
Lai, Kwing To,Antonyshyn, Iryna,Prots, Yurii,Valldor, Martin
supporting information, p. 13296 - 13299 (2018/10/31)
Novel bichalcogenides with the general composition (Li2TM)ChO (TM = Mn, Co; Ch = S, Se) were synthesized by single-step solid-state reactions. These compounds possess cubic anti-perovskite crystal structure with Pm3m symmetry; TM and Li are disordered on the crystallographic site 3c. According to Goldschmidt tolerance factor calculations, the available space at the 3c site is too large for Li+ and TM2+ ions. As cathode materials, all title compounds perform less prominent in lithium-ion battery setups in comparison to the already known TM = Fe homologue; e.g., (Li2Co)SO has a charge density of about 70 mAh g-1 at a low charge rate. Nevertheless, the title compounds extend the chemical flexibility of the anti-perovskites, revealing their outstanding chemical optimization potential as lithium battery cathode material.
