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Lithium sulfate is an inorganic chemical compound with the formula Li₂SO₄, composed of two lithium ions (Li⁺) and one sulfate ion (SO₄²⁻), typically appearing as a white, crystalline solid that is highly soluble in water.
Lithium sulfate is produced industrially by neutralizing lithium hydroxide or lithium carbonate with sulfuric acid, and plays an important role in ceramics, glass manufacturing, battery research, and chemical synthesis.
Due to Lithium sulfate's high ionic conductivity, thermal stability, and chemical resilience, lithium sulfate is increasingly valued in electrochemical applications, particularly in emerging energy storage technologies.
CAS Number: 10377-48-7
EC Number: 233-820-4
Molecular Formula: Li2SO4
Molecular Mass: 109.94 g/mol
Synonyms: Lithium sulfate, 10377-48-7, dilithium sulfate, Sulfuric acid, dilithium salt, Dilthium sulfate, Lithiophor, Li2SO4, Lithium sulfate (2:1), EINECS 233-820-4, UNII-919XA137JK, DTXSID3049201, CHEBI:53474, AI3-04469, 919XA137JK, DILITHIUM SULPHATE, ANHYDROUS LITHIUM SULFATE, DTXCID8028472, EC 233-820-4, LITHIUM SULPHATE, ANHYDROUS, Lithionit, Lithium Sulphuratum, 233-820-4, Lithium sulphate, LITHIUM SULFATE, ANHYDROUS, dilithium;sulfate, Lithium sulfate(VI), 15147-42-9, LITHIUM SULFATE, ANHYDROUS/ 98+per cent/, MFCD00011086, Sulfuric acid, lithium salt (1:2), Li2O4S, Lithionit (TN), LITHIUM SULFATE, ANHYDROUS/ 98+%", Epitope ID:158531, LITHIUM SULFATE [MI], LITHIUM SULFATE [WHO-DD], Lithium sulfate; dilithium;sulfate, Tox21_202799, AKOS025243176, FL54590, NCGC00260345-01, BS-14198, CAS-10377-48-7, L0371, NS00087003, D08137, Q421106, 10377-48-7, 233-820-4, Dilithium sulfate, Dilithiumsulfat, Lithium sulfate, Lithium sulfate (2:1), LITHIUM SULPHATE, Lithium-7Li2 sulfate, MFCD00011086, Sulfate de dilithium, Sulfuric acid dilithium salt, Sulfuric acid, lithium salt (1:2), 1210273-37-2, 14104-06-4, 15147-42-9, dilithium and sulfate, dilithium(1+) sulfate, EINECS 233-820-4, Lithionit, Lithiophor, Lithium Sulfate Anhydrous, Lithium sulfate(vi), lithium sulfate, anhydrous, reagent, LITHIUM SULFATE, ANHYDROUS/ 98+per cent/, lithiumsulfate, Sulfuric acid, dilithium salt
Lithium sulfate is an inorganic chemical compound with the formula Li₂SO₄, composed of two lithium ions (Li⁺) and one sulfate ion (SO₄²⁻).
Lithium sulfate typically appears as a white, crystalline solid that is highly soluble in water and exhibits moderate solubility in alcohols.
Lithium sulfate can exist in two primary forms: anhydrous and monohydrate (Li₂SO₄·H₂O), with the monohydrate form being more common at standard temperature and pressure.
Lithium sulfate is known for its high ionic conductivity, particularly when dissolved in aqueous solutions, making it valuable in electrochemical applications.
Lithium sulfate is produced industrially by neutralizing lithium hydroxide or lithium carbonate with sulfuric acid.
Lithium sulfate finds broad usage in ceramics and glass manufacturing, where it acts as a flux to lower melting points, improving the properties of special glasses and glazes.
In battery technology, particularly in lithium-ion battery research, lithium sulfate has been investigated as an electrolyte additive due to its stability and ion transport characteristics.
Lithium sulfate is also used in pharmaceuticals, chemical synthesis, air treatment systems, and sometimes as an additive in cement and concrete to modify setting properties.
Lithium sulfate has a high melting point (approximately 860°C for the anhydrous form) and exhibits interesting thermal behavior; upon heating, it undergoes a solid–solid phase transition around 575°C.
Environmentally, lithium sulfate is relatively safe in low concentrations but can be hazardous if ingested or inhaled in large quantities, requiring proper handling and storage in cool, dry, and well-ventilated conditions.
Lithium sulfate's combination of chemical stability, thermal resilience, and electrochemical properties makes lithium sulfate a valuable material across industrial, technological, and scientific fields.
Lithium sulfate is a white inorganic salt with the formula Li2SO4.
Lithium sulfate is the lithium salt of sulfuric acid.
Lithium Sulfate is a moderately water and acid soluble Lithium source for uses compatible with sulfates.
Sulfate compounds are salts or esters of sulfuric acid formed by replacing one or both of the hydrogens with a metal.
Most metal sulfate compounds are readily soluble in water for uses such as water treatment, unlike fluorides and oxides which tend to be insoluble.
Organometallic forms are soluble in organic solutions and sometimes in both aqueous and organic solutions.
Metallic ions can also be dispersed utilizing suspended or coated nanoparticles and deposited utilizing sputtering targets and evaporation materials for uses such as solar cells and fuel cells.
Lithium Sulfate is generally immediately available in most volumes.
Lithium sulfate is an important inorganic salt formed by two lithium cations (Li⁺) and one sulfate anion (SO₄²⁻).
Lithium sulfate is typically encountered as a white, odorless crystalline solid that is highly soluble in water and slightly soluble in organic solvents such as ethanol.
Lithium sulfate exists in two major forms: the anhydrous form and the monohydrate form (Li₂SO₄·H₂O), with the monohydrate being more stable at room temperature and atmospheric pressure.
Lithium sulfate is distinguished by its high ionic mobility in aqueous solution, making it particularly interesting for electrochemical and battery research.
Lithium sulfate's crystals are hygroscopic, meaning they can absorb moisture from the air, and the monohydrate form loses water at around 130°C.
Lithium sulfate has a high melting point (about 860°C for the anhydrous form) and undergoes a notable solid–solid phase transition from a monoclinic to a hexagonal crystal structure at approximately 575°C.
Lithium sulfate is commonly produced industrially through the reaction of lithium carbonate (Li₂CO₃) or lithium hydroxide (LiOH) with sulfuric acid (H₂SO₄), resulting in a straightforward neutralization reaction that yields lithium sulfate and carbon dioxide or water.
Another method involves the treatment of spodumene or lithium brine sources, where lithium is first extracted and then processed into sulfate form.
Its purity is crucial for many specialized uses, and high-purity lithium sulfate is often produced for the electronics, battery, and pharmaceutical sectors.
In terms of applications, lithium sulfate plays a diverse role.
In the ceramics and glass industries, Lithium sulfate acts as a fluxing agent, helping to lower the melting temperature of silica-based materials and enhancing the properties of specialty glasses, optical materials, and glazes.
Lithium sulfate is also being explored as an electrolyte component or additive in lithium-ion battery technology, where it can improve ionic conductivity and thermal stability, although it is not yet as common as lithium salts like LiPF₆ in commercial cells.
In chemical manufacturing, lithium sulfate serves as a precursor or reagent in the synthesis of other lithium compounds.
Lithium sulfate has historical and limited current uses in pharmaceuticals, such as in the treatment of certain mood disorders, although lithium carbonate and lithium citrate are more common for these applications.
Furthermore, lithium sulfate can be used in air purification systems and desiccant applications due to its hygroscopic nature.
Lithium sulfate has also been investigated as an additive in concrete and cement, where it can influence setting times and material durability.
Although generally considered to be of low toxicity, high doses of lithium salts can be harmful, affecting the nervous and renal systems.
Therefore, when handling lithium sulfate, it is advised to avoid inhalation of dust, ingestion, and prolonged skin contact, and to store the material in tightly sealed containers under dry, cool conditions.
Because of Lithium sulfate's thermal stability, ionic conductivity, chemical inertness, and versatility, lithium sulfate is regarded as a highly valuable material not only for traditional industrial applications but also for advanced technologies in the fields of energy storage, electronics, and materials science.
Market Overview of Lithium Sulfate:
The global lithium sulfate market is experiencing significant growth, driven by the increasing demand for lithium-ion batteries in electric vehicles (EVs), energy storage systems, and electronic devices.
Market Size & Growth:
As of 2025, the global lithium sulfate market is valued at approximately USD 120.4 billion and is projected to reach USD 180.6 billion by 2033, growing at a CAGR of 5.2% during the forecast period.
Cognitive Market Research
Regional Insights:
Asia-Pacific:
Leading the market with a 38.87% share in 2025, driven by robust demand from countries like China (42.31% of APAC market), India (19.87%), and Japan (11.11%).
Cognitive Market Research:
Europe:
Holding a 27.33% market share in 2025, with significant contributions from Germany (22.80%), France (13.98%), and the UK (13.07%).
Cognitive Market Research:
North America:
Accounting for 25.83% of the global market in 2025, with the United States leading at 79.10% of the North American market.
Cognitive Market Research:
Key Applications:
Battery Materials:
Utilized in the production of lithium-ion batteries for EVs and energy storage systems.
Glass Industry:
Employed in manufacturing specialty glasses and ceramics.
Pharmaceutical Intermediates:
Lithium sulfate is used in the synthesis of various pharmaceutical compounds.
Uses of Lithium Sulfate:
Lithium sulfate is a highly versatile inorganic compound with applications across a broad range of industries.
In energy storage and electrochemistry, Lithium sulfate is used as an electrolyte additive in lithium-ion and aqueous batteries due to its high ionic conductivity and chemical stability.
The glass and ceramics industry utilizes lithium sulfate as a fluxing agent, lowering melting points and improving thermal and mechanical properties in specialty glasses and glazes.
In construction, Lithium sulfate serves as a concrete additive to accelerate setting time and reduce alkali-silica reactivity, which helps prevent cracking in concrete structures.
Lithium sulfate also plays a role in chemical synthesis, both as a lithium source and as an intermediate in the production of other lithium salts.
Owing to its hygroscopic nature, lithium sulfate is used in air treatment systems and as a desiccant in moisture-sensitive applications.
Although its direct pharmaceutical use is limited, Lithium sulfate has been studied for its neurological effects, and historically, it contributed to early research into lithium-based treatments.
Additionally, lithium sulfate is being explored in heat storage materials and as a mordant in specialized textile dyeing processes.
This wide range of applications reflects Lithium sulfate's unique combination of thermal stability, ion exchange capacity, and chemical compatibility with industrial processes.
Lithium sulfate is used to treat bipolar disorder.
Lithium sulfate is researched as a potential component of ion conducting glasses.
Transparent conducting film is a highly investigated topic as they are used in applications such as solar panels and the potential for a new class of battery.
In these applications, Lithium sulfate is important to have a high lithium content; the more commonly known binary lithium borate (Li2O.B2O3) is difficult to obtain with high lithium concentrations and difficult to keep as it is hygroscopic.
With the addition of lithium sulfate into the system, an easily produced, stable, high lithium concentration glass is able to be formed.
Most of the current transparent ionic conducting films are made of organic plastics, and Lithium sulfate would be ideal if an inexpensive stable inorganic glass could be developed.
Lithium sulfate has been tested as an additive for Portland cement to accelerate curing with positive results.
Lithium sulfate serves to speed up the hydration reaction (see Cement) which decreases the curing time.
A concern with decreased curing time is the strength of the final product, but when tested, lithium sulfate doped Portland cement had no observable decrease in strength.
Lithium-ion batteries:
Lithium sulfate monohydrate (Li2SO4.H2O) containing around 10% lithium is a useful chemical for the production of lithium hydroxide for the lithium-ion battery materials supply chain.
Lithium sulfate is a less reactive material than LiOH, and hence can be more easily stored and transported.
Feedstock of hard-rock spodumene concentrate is processed by acid roasting, followed by water leaching, achieving a lithium recovery of 84-88%.
Evaporation is then applied to the purified leach solution resulting in a primary lithium sulphate solid product made up mostly of lithium sulphate monohydrate (Li2SO4.H2O).
Battery and Electrochemical Applications:
Lithium sulfate is being investigated as an electrolyte additive or alternative lithium source in lithium-ion batteries and other electrochemical cells.
Thanks to its high ionic conductivity in aqueous media and its relative chemical stability, Lithium sulfate can enhance ion transport, particularly in solid-state battery research, aqueous lithium batteries, and supercapacitors.
Glass and Ceramics Industry:
In the manufacture of ceramics and specialty glasses, lithium sulfate is used as a fluxing agent.
Lithium sulfate lowers the melting point of silica-based materials, improves thermal expansion properties, and enhances mechanical strength, especially in optical and high-performance glass products.
Concrete and Construction:
Lithium sulfate can be added to cement and concrete formulations as a set accelerator and to help mitigate alkali–silica reaction (ASR), a problem that causes cracking in concrete.
Lithium sulfate may be used in conjunction with other lithium compounds (like lithium nitrate) in concrete durability treatments.
Chemical Synthesis and Industrial Processing:
Lithium sulfate serves as a reagent or intermediate in the preparation of other lithium compounds, such as lithium carbonate, lithium hydroxide, and organolithium reagents used in advanced chemical synthesis.
Lithium sulfate is also used in laboratory settings for precipitation reactions or as a source of lithium ions.
Air Treatment and Humidity Control:
Owing to its hygroscopic properties, lithium sulfate has applications in air purification systems and as a desiccant for removing moisture from air in controlled environments such as instrument housings or electronics enclosures.
Pharmaceutical Research:
Lithium sulfate has been used historically in psychiatric research, primarily in the study of lithium’s effects on mood stabilization.
While lithium carbonate is more commonly used in current medical practice, lithium sulfate has occasionally been studied for similar effects.
Textiles and Dyeing:
In specialized applications, lithium sulfate has been used as a mordant or chemical agent to fix dyes to fabrics, especially in research or non-standard textile production processes.
Heat Storage Materials:
Due to its thermal stability and high heat of dissolution, lithium sulfate is being evaluated as a component in phase change materials (PCMs) for thermal energy storage systems.
Medication:
Lithium ion (Li+) is used in psychiatry for the treatment of mania, endogenous depression, and psychosis, and also for treatment of schizophrenia.
Usually lithium carbonate (Li2CO3) is applied, but sometimes lithium citrate (Li3C6H5O7), lithium sulfate or lithium oxy-butyrate are used as alternatives.
Li+ is not metabolized.
Because of Li+ chemical similarity to sodium (Na+) and potassium (K+) cations, Lithium sulfate may interact or interfere with the biochemical pathways of these substances and displace these cations from intra- or extracellular compartments of the body.
Li+ seems to be transported out of nerve and muscle cells by the active sodium pump, although less efficiently.
Lithium sulfate has a rapid gastrointestinal absorption rate (within a few minutes), and complete following oral administration of tablets or the liquid form.
Lithium sulfate quickly diffuses into the liver and kidneys but requires 8–10 days to reach a body equilibrium.
Li+ produces many metabolic and neuroendocrine changes, but no conclusive evidence favors one particular mode of action.
For example, Li+ interacts with neurohormones, particularly the biogenic amines, serotonin (5-hydroxy tryptamine) and norepinephrine, which provides a probable mechanism for the beneficial effects in psychiatric disorders, e.g. manias.
In the central nervous system (CNS), Li+ affects nerve excitation, synaptic transmission, and neuronalmetabolism.
Li+ stabilizes serotoninergic neurotransmission.
Properties of Lithium Sulfate:
Physical properties:
Lithium sulfate is soluble in water, though it does not follow the usual trend of increasing solubility of most salts with temperature.
To the contrary, Lithium sulfate's solubility in water decreases with increasing temperature, as its dissolution is an exothermic process.
This relatively unusual property, also called retrograde solubility, is shared with few inorganic compounds, such as calcium hydroxide (portlandite, an important mineral phase of hydrated cement paste), the calcium sulfates (gypsum, bassanite, and anhydrite) and lanthanoid sulfates whose dissolution reactions are also exothermic.
The retrograde solubility is common for gases dissolution in water, but less frequently encountered for the dissolution of solids.
Calcium carbonate also exhibits a retrograde solubility, but Lithium sulfate also depends on the behavior of CO2 dissolution in the calco-carbonate equilibria.
Lithium sulfate crystals, being piezoelectric, are also used in ultrasound-type non-destructive testing because they are very efficient sound receivers.
However, they do suffer in this application because of their water solubility.
Since it has hygroscopic properties, the most common form of lithium sulfate is lithium sulfate monohydrate.
Anhydrous lithium sulfate has a density of 2.22 g/cm3 but, weighing lithium sulfate anhydrous can become cumbersome as it must be done in a water lacking atmosphere.
Lithium sulfate has pyroelectric properties.
When aqueous lithium sulfate is heated, the electrical conductivity also increases.
The molarity of lithium sulfate also plays a role in the electrical conductivity; optimal conductivity is achieved at 2 M and then decreases.
When solid lithium sulfate is dissolved in water it has an endothermic disassociation.
This is different from sodium sulfate which has an exothermic disassociation.
However, the exact energy of disassociation is difficult to quantify as Lithium sulfate seems also to depend on the quantity (number of mols) of the salt added to water.
Small amounts of dissolved lithium sulfate induce a much greater temperature change per mol than large amounts.
Crystal properties:
Lithium sulfate has two different crystal phases.
In common phase II form, Lithium sulfate has a sphenoidal monoclinic crystal system that has edge lengths of a = 8.23Å b = 4.95Å c = 8.47Å β = 107.98°.
When lithium sulfate is heated passed 130 °C it changes to a water free state but retains its crystal structure.
Lithium sulfate is not until 575 °C when there is a transformation from phase II to phase I.
The crystal structure changes to a face centered cubic crystal system, with an edge length of 7.07Å.
During this phase change, the density of lithium sulfate changes from 2.22 to 2.07 g/cm3.
Production of Lithium Sulfate:
Lithium sulfate is primarily produced through chemical reactions involving lithium-containing minerals or brines, with the most common sources being spodumene (a lithium-rich pyroxene mineral) and natural lithium-rich brine deposits.
In mineral-based production, spodumene ore is first subjected to calcination at high temperatures (around 1000–1100°C) to convert Lithium sulfate's crystal structure into a form more amenable to chemical treatment.
The calcined material is then reacted with sulfuric acid (H₂SO₄) in a process called acid leaching, producing soluble lithium sulfate (Li₂SO₄) and insoluble impurities.
The mixture is then filtered to remove the solids, and the lithium sulfate is crystallized from the purified solution.
In brine-based production, lithium-rich brines (commonly found in salt flats in countries like Chile, Argentina, and Bolivia) are pumped into large evaporation ponds, where solar energy concentrates the brine.
Once enough water has evaporated, the concentrated lithium chloride is treated with sodium sulfate or sulfuric acid to precipitate lithium sulfate, which can then be purified and dried.
A third route involves the neutralization of lithium carbonate or lithium hydroxide with sulfuric acid, commonly used in laboratory or specialty chemical production.
The final product can be obtained either as the anhydrous form or as lithium sulfate monohydrate (Li₂SO₄·H₂O) depending on the drying and crystallization conditions.
Each production route must be carefully controlled to ensure high purity, especially for applications in electronics, batteries, and pharmaceuticals.
Synthesis of Lithium Sulfate:
Organic chemistry synthesis:
Lithium sulfate is being used as a catalyst for the elimination reaction for transforming n-butyl bromide to 1-butene at close to 100% yields at a range of 320 °C to 370 °C.
The yields of this reaction change dramatically if heated beyond this range as higher yields of 2-butene is formed.
History of Lithium Sulfate:
The history of lithium sulfate is closely tied to the broader discovery and development of lithium chemistry, which began in the early 19th century.
Lithium itself was first identified in 1817 by the Swedish chemist Johan August Arfwedson while analyzing the mineral petalite.
Shortly thereafter, lithium salts—including lithium carbonate and lithium sulfate—began to attract scientific interest due to their unique chemical and physical properties.
Lithium sulfate, in particular, gained attention as one of the first water-soluble lithium compounds with notable thermal and electrochemical characteristics.
By the late 19th and early 20th centuries, lithium sulfate was studied for its medicinal effects, especially in treating gout and mood disorders, though lithium carbonate later became the more common pharmaceutical form.
During the 20th century, lithium sulfate’s use shifted more toward industrial and materials science applications, especially with the rise of ceramic engineering and electrolyte chemistry.
With the advent of battery technology and energy storage research in the latter half of the 20th century, lithium sulfate emerged as a compound of interest due to its high ionic mobility in aqueous media.
Today, Lithium sulfate is recognized not only as a valuable intermediate in lithium compound production but also as a functional additive in advanced technologies like concrete durability enhancement, specialty glass production, and potential solid-state batteries.
Lithium sulfate's evolution from a simple laboratory salt to a compound of industrial significance reflects the growing role of lithium materials in modern chemistry and technology.
Handling and Storage of Lithium Sulfate:
Lithium sulfate should be handled in well-ventilated areas to minimize dust exposure.
Avoid contact with skin, eyes, and clothing.
Do not inhale dust or vapors.
Containers should be tightly closed and stored in a cool, dry, and well-ventilated place away from moisture and incompatible materials such as strong acids and strong oxidizing agents.
Store separately from food and drink.
Hygroscopic materials should be protected from atmospheric moisture.
Reactivity and Stability of Lithium Sulfate:
Lithium sulfate is chemically stable under normal temperatures and pressures.
Lithium sulfate is not prone to hazardous polymerization.
However, Lithium sulfate is incompatible with strong acids (may release toxic sulfur oxides) and strong oxidizers.
When heated above 860°C, Lithium sulfate decomposes, releasing sulfur dioxide (SO₂) and lithium oxide (Li₂O).
Lithium sulfate is stable under dry conditions but may absorb moisture from the air if exposed for prolonged periods.
First Aid Measures of Lithium Sulfate:
Inhalation:
Move the person to fresh air.
If breathing difficulties occur, administer oxygen and seek immediate medical attention.
Skin Contact:
Remove contaminated clothing and rinse skin immediately with plenty of water.
Wash thoroughly with soap and water.
Seek medical attention if irritation persists.
Eye Contact:
Rinse cautiously with water for at least 15 minutes, lifting the upper and lower eyelids occasionally.
Seek immediate medical attention if irritation develops.
Ingestion:
Rinse mouth thoroughly with water.
Do not induce vomiting.
Seek immediate medical advice.
If the person is conscious, offer water to dilute the material.
Firefighting Measures of Lithium Sulfate:
Suitable Extinguishing Media:
Use water spray, dry chemical powder, carbon dioxide (CO₂), or foam.
Hazardous Combustion Products:
Heating to decomposition may release toxic gases such as sulfur oxides (SOₓ) and lithium oxide (Li₂O).
Special Protective Equipment for Firefighters:
Firefighters should wear self-contained breathing apparatus (SCBA) and full protective clothing to prevent contact with skin and eyes.
Special Firefighting Instructions:
Move containers away from the fire area if Lithium sulfate can be done safely.
Cool fire-exposed containers with water spray.
Accidental Release Measures of Lithium Sulfate:
Personal Precautions:
Evacuate personnel to safe areas.
Avoid breathing dust.
Use appropriate personal protective equipment (PPE).
Environmental Precautions:
Prevent further leakage or spillage if safe to do so.
Avoid release into the environment, especially waterways.
Methods for Cleaning Up:
Sweep up and shovel spilled material carefully.
Avoid generating dust.
Collect in properly labeled, dry containers for disposal according to local regulations.
Ventilate the affected area.
Exposure Controls / Personal Protective Equipment of Lithium Sulfate:
Engineering Controls:
Ensure adequate ventilation, particularly in confined areas.
Use local exhaust ventilation if dust formation is likely.
Personal Protective Equipment:
Respiratory Protection:
Dust mask or NIOSH-approved respirator if dust levels exceed exposure limits.
Eye Protection:
Safety glasses with side shields or chemical splash goggles.
Skin Protection:
Wear protective gloves (nitrile, PVC) and suitable protective clothing to minimize skin contact.
Hygiene Measures:
Wash hands thoroughly after handling.
Remove contaminated clothing and wash before reuse.
Do not eat, drink, or smoke when handling this product.
Identifiers of Lithium Sulfate:
CAS Number:
10377-48-7
10102-25-7 (monohydrate)
ChemSpider: 59698
ECHA InfoCard: 100.030.734
PubChem CID: 66320
RTECS number: OJ6419000
UNII:
919XA137JK
KHZ7781670 (monohydrate)
CompTox Dashboard (EPA): DTXSID3049201
InChI: InChI=1S/2Li.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
Key: INHCSSUBVCNVSK-UHFFFAOYSA-L
InChI=1/2Li.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
Key: INHCSSUBVCNVSK-NUQVWONBAF
SMILES: [Li+].[Li+].[O-]S(=O)(=O)[O-]
Linear Formula: Li2SO4
Pubchem CID: 66320
MDL Number: MFCD00011086
EC No.: 233-820-4
IUPAC Name: dilithium sulfate
Beilstein/Reaxys No.: N/A
SMILES: [Li+].[Li+].[O-]S([O-])(=O)=O
InchI Identifier: InChI=1S/2Li.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
InchI Key: INHCSSUBVCNVSK-UHFFFAOYSA-L
Linear Formula: Li2SO4
CAS Number: 10377-48-7
Molecular Weight: 109.94
EC Number: 233-820-4
Chemical Name: Lithium sulfate
IUPAC Name: Dilithium sulfate
Chemical Formula:
Anhydrous: Li₂SO₄
Monohydrate: Li₂SO₄·H₂O
CAS Numbers:
Anhydrous lithium sulfate: 10377-48-7
Lithium sulfate monohydrate: 10102-25-7
EC Number:
Anhydrous: 233-820-4
Monohydrate: 600-147-7
Molar Mass:
Anhydrous: 109.94 g/mol
Monohydrate: 127.96 g/mol
PubChem CID: 24582
HS Code (Customs): 2833.39
InChI: InChI=1S/2Li.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
InChI Key: RYFZHTQNOFWBCW-UHFFFAOYSA-L
SMILES: [Li+].[Li+].[O-]S(=O)(=O)[O-]
Appearance: White crystalline solid (powder or granules)
Solubility: Highly soluble in water; slightly soluble in alcohol
Properties of Lithium Sulfate:
Chemical formula: Li2SO4
Molar mass: 109.94 g/mol
Appearance: White crystalline solid, hygroscopic
Density:
2.221 g/cm3 (anhydrous)
2.06 g/cm3 (monohydrate)
Melting point: 859 °C (1,578 °F; 1,132 K)
Boiling point: 1,377 °C (2,511 °F; 1,650 K)
Solubility in water
monohydrate:
34.9 g/100 mL (25 °C)
29.2 g/100 mL (100 °C)
Solubility: insoluble in absolute ethanol, acetone and pyridine
Magnetic susceptibility (χ): −40.0·10−6 cm3/mol
Refractive index (nD): 1.465 (β-form)
Compound Formula: Li2O4S
Molecular Weight: 109.945
Appearance: White
Melting Point: 859° C (1,578° F)
Boiling Point: 1,377° C (2,511° F)
Density: 2-C.22 g/cm3
Solubility in H2O: N/A
Exact Mass: 109.984
Monoisotopic Mass: 109.984
Molecular Weight: 110.0 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 4
Rotatable Bond Count: 0
Exact Mass: 109.98373652 Da
Monoisotopic Mass: 109.98373652 Da
Topological Polar Surface Area: 88.6 Ų
Heavy Atom Count: 7
Complexity: 62.2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 3
Compound Is Canonicalized: Yes
Specifications of Lithium Sulfate:
Potassium (K): =<0.02 %
Iron (Fe): =<0.005 %
Magnesium (Mg): =<0.02 %
Appearance (Form): Crystalline powder
Water: =<1 %
Titration after Ion exchange: >=98.5 %
Solubility: (10 % in water) Clear colorless to slightly hazy
Heavy metals (as Pb): =<0.002 %
Calcium (Ca): =<0.02 %
Appearance (Color): White
Structure of Lithium Sulfate:
Crystal structure: Primitive monoclinic
Space group: P 21/a, No. 14
Lattice constant
a = 8.239 Å, b = 4.954 Å, c = 8.474 Å
α = 90°, β = 107.98°, γ = 90°
Lattice volume (V): 328.9 Å3
Formula units (Z): 4
Coordination geometry: Tetrahedral at sulfur
Thermochemistry of Lithium Sulfate:
Heat capacity (C): 1.07 J/g K
Std molar entropy (S⦵298): 113 J/mol K
Std enthalpy of formation (ΔfH⦵298): −1436.37 kJ/mol
Gibbs free energy (ΔfG⦵): −1324.7 kJ/mo
Related compounds of Lithium Sulfate:
Other anions:
Lithium chloride
Other cations:
Sodium sulfate
Potassium sulfate
Rubidium sulfate
Caesium sulfate
Names of Lithium Sulfate:
IUPAC name:
Lithium sulfate
Other names:
Lithium sulphate
