Calcium chlorate: Difference between revisions

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|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|??}}

| CASNo = -74-3

| UNII_Ref = {{fdacite|changed|FDA}}

| UNII = 2R958OYG8P

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

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SMILES = [Ca+2].[O-]Cl(=O)=O.[O-]Cl(=O)=O

| InChI = 1/Ca.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2

| InChIKey = YALMXYPQBUJUME-NUQVWONBAM

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChI = 1S/Ca.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = YALMXYPQBUJUME-UHFFFAOYSA-L

|Section2={{Chembox Properties

| Appearance = white solid

| Odor = odorless

| Solubility = 209 g/100mL (20 °C)

| MeltingPt = °C

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|Section3={{Chembox Structure

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|Section7={{Chembox Hazards

| NFPA- = OX

|Section8={{Chembox Related

| OtherCations = [[potassium chlorate]]<br/>[[sodium chlorate]]<br/>[[barium chlorate]]

'''Calcium chlorate''' is the [[calcium]] [[Salt (chemistry)|salt]] of [[chloric acid]] with the [[chemical formula]] Ca(ClO₃)₂. Like [[chlorate]], it is a strong [[oxidizer]].

==Production==

Calcium chlorate is produced by passing [[chlorine]] gas through a hot suspension of [[calcium hydroxide]] in water, producing [[calcium hypochlorite]], which [[Disproportionation|disproportionates]] when heated with excess chlorine to give calcium chlorate and [[calcium chloride]]:<ref name=text>{{cite book|last1=Samuel P. Sadtler, Virgil Coblentz and Jeannot Hostmann|title=A textbook of chemistry, intended for the use of pharmaceutical and medical students|date=1918|page=329|url=https://books.google.com/books?id=cWhZAAAAYAAJ}}</ref>

: 6 Ca(OH)₂ + 6 Cl₂ → Ca(ClO₃)₂ + 5 CaCl₂ + 6 H₂O

This is also the first step of the [[Liebig process]] for the manufacture of [[potassium chlorate]].{{cn|date=September 2023}}

In theory, [[electrolysis]] of hot calcium chloride solution will produce the chlorate salt,{{cn|date=September 2023}} analogous to the process used for the manufacture of [[sodium chlorate]]. In practice, electrolysis is complicated by calcium hydroxide depositing on the [[cathode]], preventing the flow of current.

==Reactions==

When concentrated solutions of calcium chlorate and [[potassium chloride]] are combined, potassium chlorate precipitates:{{r|text}}<ref name=Mellor>{{cite book|last1=Mellor|first1=Joseph William|title=Modern Inorganic Chemistry|date=1917|page=287|url=https://books.google.com/books?id=1iQ7AQAAMAAJ}}</ref>

: Ca(ClO₃)₂ + 2 KCl → 2 KClO₃ + CaCl₂

This is the second step of the Liebig process for the manufacture of potassium chlorate.{{r|Mellor}}

Solutions of calcium chlorate react with solutions of alkali carbonates to give a precipitate of [[calcium carbonate]] and the alkali chlorate in solution:

: Ca(ClO₃)₂ + Na₂CO₃ → 2 NaClO₃ + CaCO₃

On strong heating, calcium chlorate decomposes to give oxygen and calcium chloride:

: Ca(ClO₃)₂ → CaCl₂ + 3 O₂

Cold, dilute solutions of calcium chlorate and [[sulfuric acid]] react to give a precipitate of [[calcium sulfate]] and [[chloric acid]] in solution:<ref name="ACJ">{{cite journal|title=American Chemical Journal|last1=Ira Remsen, Charles August Rouillu|date=1883|volume=4|page=309|url=https://books.google.com/books?id=vBhLAAAAYAAJ|quote=Solution of pure calcium chlorate, treated by sulphuric acid, would of course give a solution of chloric acid}}</ref>

: Ca(ClO₃)₂ + H₂SO₄ → 2 HClO₃ + CaSO₄

Contact with strong sulfuric acid can result in explosions<ref name=pubchem>[https://pubchem.ncbi.nlm.nih.gov/compound/calcium_chlorate#section=Experimental-Properties PubChem - Calcium Chlorate: Experimental Properties]</ref> due to the instability of concentrated chloric acid. Contact with ammonium compounds can also cause violent decomposition due to the formation of unstable [[ammonium chlorate]].{{r|pubchem}}

==Uses==

Calcium chlorate has been used as an [[herbicide]],{{cn|date=September 2023}} like [[sodium chlorate]].

Calcium chlorate is occasionally used in [[pyrotechnics]],{{cn|date=September 2023}} as an oxidizer and pink flame colorant. Its hygroscopic nature and incompatibility with other common pyrotechnic materials (such as [[sulfur]]) limit its utility in these applications.

{{reflist}}

{{Chlorates}}