Lithium sulfate

Lithium sulfate
Names
IUPAC name
Lithium sulfate
Other names
Lithium sulphate
Identifiers
10377-48-7 YesY
10102-25-7 (monohydrate) N
ChemSpider 59698 N
Jmol 3D model Interactive image
PubChem 66320
RTECS number OJ6419000
Properties[1]
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)
monohydrate:
34.9 g/100 mL (25 °C)
29.2 g/100 mL (100 °C)
Solubility insoluble in absolute ethanol, acetone and pyridine
1.465 (β-form)
Thermochemistry
1.07 J/g K
113 J/mol K
−1436.37 kJ/mol
-1324.7 kJ/mol
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
1
0
Lethal dose or concentration (LD, LC):
613 mg/kg (rat, oral)[2]
Related compounds
Other cations
 Sodium sulfate
Potassium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

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 soluble in water, though it does not follow the usual trend of solubility versus temperature — its solubility in water decreases with increasing temperature, as its dissolution is an exothermic process. This property is shared with few inorganic compounds, such as the lanthanoid sulfates.

Lithium sulfate crystals, being piezoelectric, are also used in ultrasound-type non-destructive testing because they are very efficient sound generators. 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 sulfated 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 2M and then decreases.[3]

When solid lithium sulfate is dissolved in water it has an endothermic disassociation. This is different than sodium sulfate which is has an exothermic disassociation. The exact energy of disassociation is difficult to quantify as it seems relative to the mols of the salt added. Small amounts of dissolved lithium sulfate have a much greater temperature change ≠then≠ THAN large amounts.[4]

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 ℃ it changes to a water free state but retains its crystal structure. It is not until 575 ℃ 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.[5] During this phase change, the density of Lithium Sulfate changes from 2.22 to 2.07 g/cm3.[6]

Uses

Lithium sulfate is used to treat bipolar disorder (see lithium pharmacology).

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.[7]

Lithium Sulfate has being 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.[8]

Medication

Lithium (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 oxybutyrate are used as alternatives.[9] Li is not metabolized. Because of Li chemical similarity to sodium (Na+) and potassium (K+), it may interact or interfere with biochemical pathways for 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 inefficiently.

Lithium sulfate has a rapid gastrointestinal absorption rate (within a few minutes), and complete following oral administration of tables or the liquid form.[10] It diffuses quickly into the liver and kidneys but requires 8–10 days to reach bodily equilibrium. Li produces many metabolic and neuroendocrine changes, but no conclusive evidence favors one particular mode of action.[11] 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 CNS, Li affects nerve excitation, synaptic transmission, and neuronal metabolism.[12] Li stabilizes serotoninergic neurotransmission.

Reactions

Lithium sulfate has been used in organic chemistry synthesis. Lithium sulfate is being used as a catalyst for the elimination reaction in changing n-butyl bromide to 1-butene at close to 100% yields at a range of 320℃ to 370℃. The yields of this reaction change dramatically if heated beyond this range as higher yields of 2-butene is formed.[13]

References

  1. ↑ Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
  2. ↑ http://chem.sis.nlm.nih.gov/chemidplus/rn/10377-48-7
  3. ↑ Angel C.; Sobron F.; Jose I. Density, Viscosity, and Electrical Conductivity of Aqueous Solutions of Lithium Sulfate. J. Chem. Eng. 1995, 40, 987-991
  4. ↑ Thomson T. P.; Smith D. E.; Wood R. H. Enthalpy of dilution of aqueous Na2SO4 and Si2SO4 J Chem. Eng. 1974, 19, 386-388
  5. ↑ Rao C. N. R.; Prakash B. Crystal Structure Transformations in Inorganic sulfates, Phosphates, Perchlorates, and Chromates. NSRDS. 1975, 56, 2-12
  6. ↑ Fordland, T.; Keogh, M. J. The structure of the High temperature Modification of lithium Sulfate. 1957, 565-567
  7. ↑ 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
  8. ↑ 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
  9. ↑ Haddad, L.M., Winchester, J.F. Clinical Management of Poisoning and Drug Overdose. 1990 2nd ed, 656-665
  10. ↑ Haddad, L.M., Winchester, J.F. Clinical Management of Poisoning and Drug Overdose. 1990 2nd ed, 656-665
  11. ↑ Haddad, L.M., Winchester, J.F. Clinical Management of Poisoning and Drug Overdose. 1990 2nd ed, 656-665
  12. ↑ Poisindex, Thomson Micromedex 2005
  13. ↑ 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
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