SULFURIC ACID
SULFURIC ACID
Sulfuric acid 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.
Sulfuric acid is produced industrially by neutralizing lithium hydroxide or lithium carbonate with sulfur, and plays an important role in ceramics, glass manufacturing, battery research, and chemical synthesis.
Due to Sulfuric acid’s high ionic conductivity, thermal stability, and chemical resilience, Sulfuric acid 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
Sulfuric acid is an inorganic chemical compound with the formula Li₂SO₄, composed of two lithium ions (Li⁺) and one sulfate ion (SO₄²⁻).
Sulfuric acid typically appears as a white, crystalline solid that is highly soluble in water and exhibits moderate solubility in alcohols.
Sulfuric acid can exist in two primary forms: anhydrous and monohydrate (Li₂SO₄·H₂O), with the monohydrate form being more common at standard temperature and pressure.
Sulfuric acid is known for its high ionic conductivity, particularly when dissolved in aqueous solutions, making it valuable in electrochemical applications.
Sulfuric acid is produced industrially by neutralizing lithium hydroxide or lithium carbonate with sulfur.
Sulfuric acid 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, Sulfuric acid has been investigated as an electrolyte additive due to its stability and ion transport characteristics.
Sulfuric acid is also used in pharmaceuticals, chemical synthesis, air treatment systems, and sometimes as an additive in cement and concrete to modify setting properties.
Sulfuric acid 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, Sulfuric acid 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.
Its combination of chemical stability, thermal resilience, and electrochemical properties makes Sulfuric acid a valuable material across industrial, technological, and scientific fields.
Sulfuric acid is a white inorganic salt with the formula Li2SO4.
Sulfuric acid is the lithium salt of sulfur.
Sulfuric acid is a moderately water and acid soluble Lithium source for uses compatible with sulfates.
Sulfate compounds are salts or esters of sulfur 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.
Sulfuric acid is generally immediately available in most volumes.
Sulfuric acid is an important inorganic salt formed by two lithium cations (Li⁺) and one sulfate anion (SO₄²⁻).
Sulfuric acid is typically encountered as a white, odorless crystalline solid that is highly soluble in water and slightly soluble in organic solvents such as ethanol.
Sulfuric acid 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.
Sulfuric acid is distinguished by its high ionic mobility in aqueous solution, making it particularly interesting for electrochemical and battery research.
Sulfuric acid’s crystals are hygroscopic, meaning they can absorb moisture from the air, and the monohydrate form loses water at around 130°C.
Sulfuric acid 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.
Sulfuric acid is commonly produced industrially through the reaction of lithium carbonate (Li₂CO₃) or lithium hydroxide (LiOH) with sulfur, resulting in a straightforward neutralization reaction that yields Sulfuric acid 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 Sulfuric acid is often produced for the electronics, battery, and pharmaceutical sectors.
In terms of applications, Sulfuric acid plays a diverse role.
In the ceramics and glass industries, Sulfuric acid 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.
Sulfuric acid 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, Sulfuric acid serves as a precursor or reagent in the synthesis of other lithium compounds.
Sulfuric acid 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, Sulfuric acid can be used in air purification systems and desiccant applications due to its hygroscopic nature.
Sulfuric acid 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 Sulfuric acid, 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 Sulfuric acid’s thermal stability, ionic conductivity, chemical inertness, and versatility, Sulfuric acid 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 Sulfuric Acid:
The global Sulfuric acid 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 Sulfuric acid 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:
Sulfuric acid is used in the synthesis of various pharmaceutical compounds.
Uses of Sulfuric Acid:
Sulfuric acid is a highly versatile inorganic compound with applications across a broad range of industries.
In energy storage and electrochemistry, Sulfuric acid 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 Sulfuric acid as a fluxing agent, lowering melting points and improving thermal and mechanical properties in specialty glasses and glazes.
In construction, Sulfuric acid serves as a concrete additive to accelerate setting time and reduce alkali-silica reactivity, which helps prevent cracking in concrete structures.
Sulfuric acid 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, Sulfuric acid is used in air treatment systems and as a desiccant in moisture-sensitive applications.
Although its direct pharmaceutical use is limited, Sulfuric acid has been studied for its neurological effects, and historically, it contributed to early research into lithium-based treatments.
Additionally, Sulfuric acid is being explored in heat storage materials and as a mordant in specialized textile dyeing processes.
This wide range of applications reflects Sulfuric acid’s unique combination of thermal stability, ion exchange capacity, and chemical compatibility with industrial processes.
Sulfuric acid is used to treat bipolar disorder.
Sulfuric acid 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, Sulfuric acid 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 Sulfuric acid 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 Sulfuric acid would be ideal if an inexpensive stable inorganic glass could be developed.
Sulfuric acid has been tested as an additive for Portland cement to accelerate curing with positive results.
Sulfuric acid 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, Sulfuric acid doped Portland cement had no observable decrease in strength.
Lithium-ion batteries:
Sulfuric acid 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.
Sulfuric acid 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:
Sulfuric acid 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, Sulfuric acid 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, Sulfuric acid is used as a fluxing agent.
Sulfuric acid 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:
Sulfuric acid 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.
Sulfuric acid may be used in conjunction with other lithium compounds (like lithium nitrate) in concrete durability treatments.
Chemical Synthesis and Industrial Processing:
Sulfuric acid 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.
Sulfuric acid 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, Sulfuric acid 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:
Sulfuric acid 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, Sulfuric acid has occasionally been studied for similar effects.
Textiles and Dyeing:
In specialized applications, Sulfuric acid 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, Sulfuric acid 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), Sulfuric acid or lithium oxy-butyrate are used as alternatives.
Li+ is not metabolized.
Because of Li+ chemical similarity to sodium (Na+) and potassium (K+) cations, Sulfuric acid 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.
Sulfuric acid has a rapid gastrointestinal absorption rate (within a few minutes), and complete following oral administration of tablets or the liquid form.
Sulfuric acid 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 Sulfuric Acid:
Physical properties:
Sulfuric acid is soluble in water, though it does not follow the usual trend of increasing solubility of most salts with temperature.
To the contrary, Sulfuric acid’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 Sulfuric acid also depends on the behavior of CO2 dissolution in the calco-carbonate equilibria.
Sulfuric acid 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 Sulfuric acid is Sulfuric acid monohydrate.
Anhydrous Sulfuric acid has a density of 2.22 g/cm3 but, weighing Sulfuric acid anhydrous can become cumbersome as it must be done in a water lacking atmosphere.
Sulfuric acid has pyroelectric properties.
When aqueous Sulfuric acid is heated, the electrical conductivity also increases.
The molarity of Sulfuric acid also plays a role in the electrical conductivity; optimal conductivity is achieved at 2 M and then decreases.
When solid Sulfuric acid 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 Sulfuric acid seems also to depend on the quantity (number of mols) of the salt added to water.
Small amounts of dissolved Sulfuric acid induce a much greater temperature change per mol than large amounts.
Crystal properties:
Sulfuric acid has two different crystal phases.
In common phase II form, Sulfuric acid has a sphenoidal monoclinic crystal system that has edge lengths of a = 8.23Å b = 4.95Å c = 8.47Å β = 107.98°.
When Sulfuric acid is heated passed 130 °C it changes to a water free state but retains its crystal structure.
Sulfuric acid 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 Sulfuric acid changes from 2.22 to 2.07 g/cm3.
Production of Sulfuric Acid:
Sulfuric acid 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 Sulfuric acid’s crystal structure into a form more amenable to chemical treatment.
The calcined material is then reacted with sulfur in a process called acid leaching, producing soluble Sulfuric acid (Li₂SO₄) and insoluble impurities.
The mixture is then filtered to remove the solids, and the Sulfuric acid 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 sulfur to precipitate Sulfuric acid, which can then be purified and dried.
A third route involves the neutralization of lithium carbonate or lithium hydroxide with sulfur, commonly used in laboratory or specialty chemical production.
The final product can be obtained either as the anhydrous form or as Sulfuric acid 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 Sulfuric Acid:
Organic chemistry synthesis:
Sulfuric acid 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 Sulfuric Acid:
The history of Sulfuric acid 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 Sulfuric acid—began to attract scientific interest due to their unique chemical and physical properties.
Sulfuric acid, 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, Sulfuric acid 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, Sulfuric acid’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, Sulfuric acid emerged as a compound of interest due to its high ionic mobility in aqueous media.
Today, Sulfuric acid 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.
Sulfuric acid’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 Sulfuric Acid:
Sulfuric acid 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 Sulfuric Acid:
Sulfuric acid is chemically stable under normal temperatures and pressures.
Sulfuric acid is not prone to hazardous polymerization.
However, Sulfuric acid is incompatible with strong acids (may release toxic sulfur oxides) and strong oxidizers.
When heated above 860°C, Sulfuric acid decomposes, releasing sulfur dioxide (SO₂) and lithium oxide (Li₂O).
Sulfuric acid is stable under dry conditions but may absorb moisture from the air if exposed for prolonged periods.
First Aid Measures of Sulfuric Acid:
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 Sulfuric Acid:
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 Sulfuric acid can be done safely.
Cool fire-exposed containers with water spray.
Accidental Release Measures of Sulfuric Acid:
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 Sulfuric Acid:
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 Sulfuric Acid:
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: diSulfuric acid
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: Sulfuric acid
IUPAC Name: DiSulfuric acid
Chemical Formula:
Anhydrous: Li₂SO₄
Monohydrate: Li₂SO₄·H₂O
CAS Numbers:
Anhydrous Sulfuric acid: 10377-48-7
Sulfuric acid 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 Sulfuric Acid:
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 Sulfuric Acid:
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 Sulfuric Acid: 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 Sulfuric Acid: 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 Sulfuric Acid: Other anions: Lithium chloride Other cations: Sodium sulfate Potassium sulfate Rubidium sulfate Caesium sulfate Names of Sulfuric Acid: IUPAC name: Lithium sulfate Other names: Lithium sulphate