Lithium chlorate

In this article, we will explore the fascinating world of Lithium chlorate, a topic that has captured the attention of many people over time. From its origins to its impact on modern society, Lithium chlorate has left an indelible mark on different aspects of our daily lives. Through detailed and insightful analysis, we will discover the many facets of Lithium chlorate and its influence in different contexts. From its relevance in history to its role in contemporary culture, we will be addressing a wide range of perspectives that will allow us to better understand the importance and relevance of Lithium chlorate in today's world. Get ready to embark on an exciting journey through the depths of Lithium chlorate!

Lithium chlorate

Names
Other names Chloric acid, lithium salt
Identifiers
CAS Number	13453-71-9 Y
3D model (JSmol)	Interactive image
ChemSpider	55520
ECHA InfoCard	100.033.288
PubChem CID	23682463
CompTox Dashboard (EPA)	DTXSID1074258
InChI InChI=1S/ClHO3.Li/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1
SMILES .Cl(=O)=O
Properties
Chemical formula	LiClO3
Molar mass	90.39 g/mol
Melting point	127.6 to 129 °C (261.7 to 264.2 °F; 400.8 to 402.1 K)[2][3][4]
Solubility in water	241 g/100 mL (0 °C) 459 g/100 mL (25 °C) 777 g/100 mL (60 °C) 2226 g/100 mL (100 °C)[1]
Magnetic susceptibility (χ)	−28.8·10−6 cm3/mol
Related compounds
Other anions	Lithium chloride Lithium hypochlorite Lithium perchlorate
Other cations	Sodium chlorate Potassium chlorate Caesium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references

Chemical compound

Lithium chlorate is the inorganic chemical compound with the formula LiClO₃. Like all chlorates, it is an oxidizer and may become unstable and possibly explosive if mixed with organic materials, reactive metal powders, or sulfur.

It can be manufactured by the reaction of hot, concentrated lithium hydroxide with chlorine:

3 Cl₂ + 6 LiOH → 5 LiCl + LiClO₃ + 3 H₂O

Lithium chlorate has one of the highest solubilities in water for a chemical compound. It is also a six-electron oxidant. Its electrochemical reduction is facilitated by acid, electrocatalysts and redox mediators. These properties make lithium chlorate a useful oxidant for high energy density flow batteries.^[5] Lithium chlorate has a very low melting point for an inorganic ionic salt.

References

1. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 4–47. ISBN 978-1138561632.
2. ^ Wang, Su-Chee Simon (1983). "The Electrochemistry of Molten Lithium Chlorate and its Possible Use with Lithium in a Battery". Journal of the Electrochemical Society. 130 (4): 741–747. Bibcode:1983JElS..130..741W. doi:10.1149/1.2119796.
3. ^ A. N. Campbell, E. M. Kartzmark, W. B. Maryk (1966). "The Systems Sodium Chlorate - Water - Dioxane and Lithium Chlorate - Water - Dioxane, at 25°". Can. J. Chem. 44 (8): 935–937. doi:10.1139/v66-136. S2CID 97413079.{{cite journal}}: CS1 maint: multiple names: authors list (link)
4. ^ http://scitation.aip.org/getabs/servlet/GetabsServlet?prog=normal&id=JESOAN000130000004000741000001&idtype=cvips&gifs=yes&ref=no ^{[dead link‍]}
5. ^ US 20140170511