Lithium sulfate
Names | |
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IUPAC name
Lithium sulfate
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Other names
Lithium sulphate
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Identifiers | |
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3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.030.734 |
PubChem CID
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RTECS number
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UNII |
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CompTox Dashboard (EPA)
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Properties[1] | |
Li2SO4 | |
Molar mass | 109.94 g/mol |
Appearance | White crystalline solid, hygroscopic
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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) |
monohydrate: 34.9 g/100 mL (25 °C) 29.2 g/100 mL (100 °C) | |
Solubility | insoluble in absolute ethanol, acetone and pyridine |
−-40.0·10−6 cm3/mol | |
Refractive index (nD)
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1.465 (β-form) |
Structure[2] | |
Primitive monoclinic | |
P 21/a, No. 14 | |
a = 8.239 Å, b = 4.954 Å, c = 8.474 Å α = 90°, β = 107.98°, γ = 90°[2]
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Lattice volume (V)
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328.9 Å3 |
Formula units (Z)
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4 |
Tetrahedral at sulfur
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Thermochemistry | |
Heat capacity (C)
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1.07 J/g K |
Std molar
entropy (S⦵298) |
113 J/mol K |
Std enthalpy of (ΔfH⦵298)formation |
−1436.37 kJ/mol |
Gibbs free energy (ΔfG⦵)
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-1324.7 kJ/mol |
Hazards | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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613 mg/kg (rat, oral)[3] |
Related compounds | |
Other anions
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Lithium chloride |
Other cations
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Sodium sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium sulfate is a white inorganic salt with the formula Li2SO4. It is the lithium salt of sulfuric acid.
Properties
Physical properties
Lithium sulfate is
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.[4]
When solid lithium sulfate is dissolved in water it has an
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. It 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.[6] During this phase change, the density of lithium sulfate changes from 2.22 to 2.07 g/cm3.[7]
Uses
Lithium sulfate is used to treat
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, it 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 it would be ideal if an inexpensive stable inorganic glass could be developed.[8]
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.[9]
Lithium-ion batteries
Lithium sulphate monohydrate (Li
2SO
4 · H
2O) containing around 10% lithium is a useful chemical for the production of lithium hydroxide for the lithium-ion battery materials supply chain. It is a less reactive material than LiOH, and hence can be more easily stored and transported.[10][11]
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 (Li
2SO
4 · H
2O).
Medication
Lithium ion (Li+) is used in psychiatry for the treatment of
Lithium sulfate has a rapid
.Organic chemistry synthesis
Lithium sulfate is being used as a
References
- ^
Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. ISBN 0-07-049439-8.
- ^ .
- ^ Chambers, Michael. "ChemIDplus - 10377-48-7 - INHCSSUBVCNVSK-UHFFFAOYSA-L - Lithium sulfate - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Retrieved 12 October 2018.
- ^ Angel C.; Sobron F.; Jose I. (1995). Density, viscosity, and electrical conductivity of aqueous solutions of lithium sulfate. J. Chem. Eng., 40, 987–991.
- ^ Thomson T. P.; Smith D. E.; Wood R. H. (1974). Enthalpy of dilution of aqueous Na2SO4 and Li2SO4. J. Chem. Eng., 19, 386–388.
- ^ Rao C. N. R.; Prakash B. Crystal Structure Transformations in Inorganic sulfates, Phosphates, Perchlorates, and Chromates. NSRDS. 1975, 56, 2-12
- ^ Fordland, T.; Keogh, M. J. The structure of the High temperature Modification of lithium Sulfate. 1957, 565-567
- ^ E. I. Chemists; M. A. Karakassides; G. D. Chryssikos. A Vibrational Study of Lithium Sulfate Based Fast Ionic Conducting Borate Glasses. J. Phys. Chem. 1986, 90 4528-4533
- ^ Yuhai D.; Changing Z.; Xiaosheng W. Influence of lithium sulfate addition on the properties of Portland cement paste. Construction and Building 2014, 50, 457-462
- ^ "Metallurgical test work confirms Manono Primary Lithium Sulphate suitable for battery production feedstock" (PDF). AVZ Minerals Limited. 13 January 2021. Retrieved 25 March 2021.
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- ^ "AVZ Minerals Limited". AVZ Minerals. Retrieved 25 March 2021.
- ^ a b c Haddad, L.M., Winchester, J.F. Clinical Management of Poisoning and Drug Overdose. 1990 2nd ed, 656-665
- ^ Poisindex, Thomson Micromedex 2005
- ^ Noller, H., Rosa-Brusin, M. and Andréu, P. (1967), Stereoselective Synthesis of 1-Butene with Lithium Sulfate as Elimination Catalyst. Angew. Chem. Int. Ed. Engl., 6: 170–171. doi:10.1002/anie.196701702