:Lithium chlorate

{{Chembox

| verifiedrevid =

| Name = Lithium chlorate

| ImageFile = Lithium ion   File:Chlorate-2D.png

| ImageSize =

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| IUPACName =

| OtherNames = Chloric acid, lithium salt

|Section1={{Chembox Identifiers

| SMILES = [Li+].[O-]Cl(=O)=O

| CASNo = 13453-71-9

| CASNo_Ref = {{cascite|correct|CAS}}

| PubChem = 23682463

| ChemSpiderID = 55520

| InChI = 1S/ClHO3.Li/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1

}}

|Section2={{Chembox Properties

| Formula = LiClO₃

| MolarMass = 90.39 g/mol

| Appearance =

| Odor =

| Density =

| Solubility = 241 g/100 mL (0 °C)
459 g/100 mL (25 °C)
777 g/100 mL (60 °C)
2226 g/100 mL (100 °C){{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=4–47|edition=99 |language=English}}

| SolubleOther =

| Solvent =

| MeltingPtC = 127.6 to 129

| MeltingPt_ref = {{cite journal | doi = 10.1149/1.2119796 | title = The Electrochemistry of Molten Lithium Chlorate and its Possible Use with Lithium in a Battery | journal = Journal of the Electrochemical Society | volume = 130 | issue = 4 | pages = 741–747 | year = 1983 | last1 = Wang | first1 = Su-Chee Simon | bibcode = 1983JElS..130..741W }}{{cite journal | author = A. N. Campbell, E. M. Kartzmark, W. B. Maryk | title = The Systems Sodium Chlorate - Water - Dioxane and Lithium Chlorate - Water - Dioxane, at 25° | journal = Can. J. Chem. | date = 1966 | volume = 44 | issue = 8 | pages = 935–937 | doi = 10.1139/v66-136 | s2cid = 97413079 }}http://scitation.aip.org/getabs/servlet/GetabsServlet?prog=normal&id=JESOAN000130000004000741000001&idtype=cvips&gifs=yes&ref=no {{dead link|date=January 2019}}

| BoilingPt =

| MagSus = −28.8·10⁻⁶ cm³/mol

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|Section3={{Chembox Structure

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|Section4={{Chembox Thermochemistry

| DeltaHf =

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|Section7={{Chembox Hazards

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| NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S =

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|Section8={{Chembox Related

| OtherAnions = Lithium chloride
Lithium hypochlorite
Lithium perchlorate

| OtherCations = Sodium chlorate
Potassium chlorate
Caesium chlorate

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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.{{cite patent|country=US|number=20140170511}} Lithium chlorate has a very low melting point for an inorganic ionic salt.