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| ImageFile = Sodium-chlorate-component-ions-2D.png
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|Section2=((Chembox Properties
| Formula = NaClO<sub>3</sub>
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| Appearance = Colorless or white solid, [[hygroscopic]]
| Odor = Odorless
| Density = 2.49 g/cm<sup>3</sup> (15&nbsp;°C)<ref name=chemister>((cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=786|title=Sodium chlorate))</ref><br> 2.54 g/cm<sup>3</sup> (20.2&nbsp;°C)<ref name=arkema>((cite web|url=http://www.arkema.com/export/shared/.content/media/downloads/socialresponsability/safety-summuries/safety-summaries-hydrogen-peroxide-sodium-chlorate-2012-06-30.pdf|title=GPS Safety Summary of Sodium Chlorate|website=arkema.com|publisher=Arkema|access-date=2014-05-25|archive-date=2014-05-25|archive-url=https://web.archive.org/web/20140525232738/http://www.arkema.com/export/shared/.content/media/downloads/socialresponsability/safety-summuries/safety-summaries-hydrogen-peroxide-sodium-chlorate-2012-06-30.pdf|url-status=dead))</ref>
| Solubility = 79 g/100 mL (0&nbsp;°C)<br> 89 g/100 mL (10&nbsp;°C)<br> 105.7 g/100 mL (25&nbsp;°C)<br>125 g/100 mL (40&nbsp;°C)<br> 220.4 g/100 mL (100&nbsp;°C)<ref name=sioc>((cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand))</ref>
| Solubility1 = Sparingly soluble<ref name=chemister />
| Solvent1 = acetone
| Solubility2 = 20 g/100 g (15.5&nbsp;°C)<ref name=chemister />
| Solvent2 = glycerol
| Solubility3 = 14.7 g/100 g<ref name=chemister />
| Solvent3 = ethanol
| MeltingPtC = 248-261
| BoilingPtC = 300-400
| BoilingPt_notes = <br> decomposes<ref name=chemister />
| RefractIndex = 1.515 (20&nbsp;°C)<ref name=pubchem />
| SolubleOther = Soluble in [[glycerol]], [[hydrazine]], [[methanol]]<br> Slightly soluble in [[ethanol]], [[ammonia]]<ref name=chemister />
| VaporPressure = <0.35 mPa<ref name=arkema />
| MagSus = &minus;34.7·10<sup>−6</sup> cm<sup>3</sup>/mol
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| Structure_ref = <ref>((cite journal|title=Remeasurement of Optically Active NaClO<sub>3</sub> and NaBrO<sub>3</sub>|author=S. C. Abrahams, J. L. Bernstein|date=1977|doi=10.1107/S0567740877011637|doi-access=free|journal=Acta Crystallographica|volume=B33|issue=11|pages=3601–3604|bibcode=1977AcCrB..33.3601A ))</ref>
| CrystalStruct = cubic
| SpaceGroup = 
| PointGroup = P2<sub>1</sub>3
| LattConst_a = 6.57584 Å
| LattConst_b = 
| LattConst_c = 
| LattConst_alpha = 
| LattConst_beta = 
| LattConst_gamma = 
| LattConst_ref =
| LattConst_Comment = 
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| UnitCellFormulas = 4
| Coordination = 
| MolShape = 
| OrbitalHybridisation = 
| Dipole = 
  ))
|Section5=((Chembox Thermochemistry
| DeltaHf = -365.4 kJ/mol<ref name=chemister />
| DeltaGf = -275 kJ/mol<ref name=chemister />
| Entropy = 129.7 J/mol·K<ref name=chemister />
| HeatCapacity = 104.6 J/mol·K<ref name=chemister />
  ))
|Section7=((Chembox Hazards
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1117.htm ICSC 1117]
| GHSPictograms = ((GHS03))((GHS07))((GHS09))<ref name="sigma">[[Sigma-Aldrich|Sigma-Aldrich Co.]], [https://www.sigmaaldrich.com/US/en/product/sigald/403016 Sodium chlorate]. Retrieved on 2022-02-21.</ref>
| GHSSignalWord = Danger
| HPhrases = ((H-phrases|271|302|411))<ref name="sigma" />
| PPhrases = ((P-phrases|220|273))<ref name="sigma" />
| NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 3 
| NFPA-S = OX
| FlashPt = Non-flammable
| LD50 = 600 mg/kg (rats, oral)<br> 700 mg/kg (dogs, oral)<ref name=chemister />
  ))
|Section8=((Chembox Related
| OtherAnions = [[Sodium chloride]]<br> [[Sodium hypochlorite]]<br> [[Sodium chlorite]]<br> [[Sodium perchlorate]]<br> [[Sodium bromate]]<br> [[Sodium iodate]]
| OtherCations = [[Ammonium chlorate]]<br> [[Potassium chlorate]]<br> [[Barium chlorate]]
| OtherCompounds = [[Chloric acid]]
  ))
))

'''Sodium chlorate''' is an [[inorganic compound]] with the [[chemical formula]] [[Sodium|Na]][[Chlorate|ClO<sub>3</sub>]]. It is a white [[crystalline]] powder that is readily soluble in water. It is [[hygroscopic]]. It decomposes above 300&nbsp;°C to release [[oxygen]]<ref name=pubchem>((PubChemLink|516902))</ref> and leaves [[sodium chloride]]. Several hundred million tons are produced annually, mainly for applications in [[bleach]]ing [[Pulp (paper)|pulp]] to produce high brightness [[paper]].<ref name=Ullmann/>

==Synthesis==
((More citations needed section|date=May 2022))
Industrially, sodium chlorate is produced by the [[electrolysis]] of concentrated sodium chloride solutions. All other processes are obsolete. The sodium chlorate process is not to be confused with the [[chloralkali process]], which is an industrial process for the electrolytic production of sodium hydroxide and chlorine gas.

The overall reaction can be simplified to the equation:
((block indent|NaCl + 3 H<sub>2</sub>O  → NaClO<sub>3</sub> + 3 H<sub>2</sub>))

First, [[chloride]] is oxidised to form intermediate [[hypochlorite]], ClO<sup>−</sup>, which undergoes further oxidation to chlorate along two competing reaction paths: (1) Anodic chlorate formation at the boundary layer between the electrolyte and the anode, and (2) Autoxidation of hypochlorite in the bulk electrolyte.

Under electrolysis hydrogen and sodium hydroxide are formed at the cathode and chloride ions are discharged at the anode ([[mixed metal oxide]] electrode is often used). The evolved chlorine does not escape as a gas but undergoes hydrolysis:
((block indent|Cl<sub>2</sub> + H<sub>2</sub>O ⇋ HClO + H<sup>+</sup> + Cl<sup>−</sup>))

The hydrolysis of chlorine is considered to be fast. The formation of H<sup>+</sup> ions should make the boundary layer at the anode strongly acidic and this is observed at low chloride concentrations. However, large concentrations of chloride, as they occur in industrial chlorate cells, shift the hydrolysis equilibrium to the left. At the boundary layer the concentration of H<sup>+</sup> is not high enough to permit diffusion into the bulk electrolyte. Therefore hydrogen is transported away from the anode mostly as hypochlorous acid rather than H<sup>+</sup>. The hypochlorous acid dissociates in the bulk electrolyte where the pH is high and the hypochlorite ion diffuses back to the anode. More than two thirds of the hypochlorite is consumed by buffering before reaching the anode. The remainder is discharged at the anode to form chlorate and oxygen:

((block indent|3 ClO<sup>−</sup> + 1.5 H<sub>2</sub>O → ClO<sub>3</sub><sup>−</sup> + 3 H<sup>+</sup> + 2 Cl<sup>−</sup> + 0.75 O<sub>2</sub>))

The autoxidation of hypochlorous acid in the bulk electrolyte proceeds according to the simplified overall equation:
((block indent|3 HClO → ClO<sub>3</sub><sup>−</sup> + 2 Cl<sup>−</sup> + 3 H<sup>+</sup>))
It is preceded by the dissociation of a part of the hypochlorous acid involved:
((block indent|HClO → ClO<sup>−</sup> + H<sup>+</sup>))
The reaction requires a certain distance from the anode to occur to a significant degree, where the electrolyte is sufficiently buffered by the hydroxyl formed at the cathode. The hypochlorite  then reacts with the rest of the acid:
((block indent|2 HClO + ClO<sup>−</sup> → ClO<sub>3</sub><sup>−</sup> + 2 Cl<sup>−</sup> + 2 H<sup>+</sup>))
In addition to anode distance the autoxidation also depends on temperature and pH. A typical cell operates at temperatures between 80&nbsp;°C and 90&nbsp;°C and at a pH of 6.1–6.4.

Independent of the reaction route the discharge of 6&nbsp;mol of chloride is required to yield 1&nbsp;mol of chlorate. However, the anodic oxidation route requires 50% additional electric energy. Therefore, industrial cells are optimised to favour autoxidation. Chlorate formation at the anode is treated as a loss reaction and is minimised by design.

Other loss reactions also decrease the current efficiency and must be suppressed in industrial systems. The main loss occurs by the back reduction of hypochlorite at the cathode. The reaction is suppressed by the addition of a small amount of [[dichromate]] (1–5&nbsp;g/L) to the electrolyte. A porous film of chromium hydroxide is formed by cathodic deposition. The film impedes the diffusion of anions to the cathode, whereas the access of cations and their reduction is facilitated. The film stops growing on its own after it reaches a certain thickness.<ref name=Ullmann>((Ullmann|doi=10.1002/14356007.a06_483|title=Chlorine Oxides and Chlorine Oxygen Acids|year=2000|last1=Vogt|first1=Helmut|last2=Balej|first2=Jan|last3=Bennett|first3=John E.|last4=Wintzer|first4=Peter|last5=Sheikh|first5=Saeed Akbar|last6=Gallone|first6=Patrizio|isbn=3527306730))</ref>

==Uses==
The main commercial use for sodium chlorate is for making [[chlorine dioxide]] (ClO<sub>2</sub>). The largest application of ClO<sub>2</sub>, which accounts for about 95% of the use of chlorate, is in bleaching of pulp. All other, less important [[chlorate]]s are derived from sodium chlorate, usually by [[salt metathesis]] with the corresponding chloride. All [[perchlorate]] compounds are produced industrially by the oxidation of solutions of sodium chlorate by electrolysis.<ref name=Ullmann/>

===Herbicides===
Sodium chlorate is used as a non-selective [[herbicide]]. It is considered [[phytotoxicity|phytotoxic]] to all green plant parts. It can also kill through root absorption.

Sodium chlorate may be used to control a variety of plants including [[morning glory]], [[canada thistle]], [[johnson grass]], [[bamboo]], [[senecio|Ragwort]], and [[Hypericum perforatum|St John's wort]]. The herbicide is mainly used on non-crop land for spot treatment and for total vegetation control on areas including roadsides, fenceways, and ditches. Sodium chlorate is also used as a [[defoliant]] and [[desiccant]] for:

((div col|colwidth=12em))
*[[maize|Corn]]
*[[Cotton]]
*Dry beans
*[[Flax]]
*Grain [[sorghum]]
*[[capsicum|Peppers]]
*[[Rice]]
*[[Safflower]]
*Southern peas
*[[Soybean]]s
*[[Sunflower]]s
((div col end))

If used in combination with [[atrazine]], it increases the persistence of the effect. If used in combination with [[2,4-D]], performance is improved. Sodium chlorate has a [[soil sterilant]] effect. Mixing with other herbicides in aqueous solution is possible to some extent, so long as they are not susceptible to oxidation.

The sale of sodium chlorate as a weedkiller was banned in the European Union in 2009 citing health dangers, with existing stocks to be used within the following year.<ref>((cite web |url=https://www.hortweek.com/sodium-chlorate-banned-ec/fresh-produce/article/841864 |title=Sodium chlorate banned by EC |website=Horticulture Week|date=28 August 2008  ))</ref>

===Chemical oxygen generation===
[[Chemical oxygen generator]]s, such as those in commercial aircraft, provide emergency oxygen to passengers to protect them from drops in cabin pressure.  Oxygen is generated by high-temperature decomposition of sodium chlorate:<ref>((Greenwood&Earnshaw2nd))</ref>
((block indent|2 NaClO<sub>3</sub>  →  2 NaCl  +  3 O<sub>2</sub>))

Heat required to initiate this reaction is generated by [[Redox|oxidation]] of a small amount of iron powder mixed with the sodium chlorate, and the reaction consumes less oxygen than is produced. [[Barium peroxide]] ([[barium|Ba]][[Oxygen|O<sub>2</sub>]]) is used to absorb the [[chlorine]] that is a minor product in the decomposition.<ref>((cite journal|journal = Ind. Eng. Chem. Res. 
| title = Functions of Barium Peroxide in Sodium Chlorate Chemical Oxygen 
|author1=Yunchang Zhang |author2=Girish Kshirsagar |author3=James C. Cannon  |name-list-style=amp | volume = 32 
| issue = 5
| pages = 966–969 
| year = 1993 
| doi = 10.1021/ie00017a028  ))</ref>
An ignitor charge is activated by pulling on the emergency mask. Similarly, the [[SolidOx (welding)|Solidox]] welding system used pellets of sodium chlorate mixed with combustible fibers to generate oxygen.

===Oxygenless combustion===

Sodium chlorate can be mixed with sucrose sugar to make a highly energetic fuel, similar to that of [[gunpowder]], that burns in airtight spaces. This is the reaction:

((block indent|8 NaClO<sub>3</sub> + C<sub>12</sub>H<sub>22</sub>O<sub>11</sub> → 8 NaCl + 12 CO<sub>2</sub> + 11 H<sub>2</sub>O))

However this sodium chlorate is mostly replaced by [[potassium chlorate]].((citation needed|date=March 2020))

===Organic synthesis===

Sodium chlorate can be used with [[hydrochloric acid]] (or also [[sulfuric acid]] and [[sodium chloride]], the reaction of which generates HCl) to chlorinate aromatic compounds without the use of organic solvents. In this case its function is to oxidize the HCl to obtain either HOCl or Cl<sub>2</sub> (depending upon the pH) in-situ which are the active chlorinating agents.<ref>((cite journal |last1=Sharma |first1=Sushil Kumar |last2=Agarwal |first2=D. D. |date=July 2014 |title=Oxidative Chlorination of Aromatic Compounds in Aqueous Media  |url=https://www.ijsrp.org/research-paper-0714/ijsrp-p3182.pdf |journal=International Journal of Scientific and Research Publications |volume=4 |issue=7 |pages= |doi= |access-date=August 23, 2021))</ref>

==Toxicity in humans==
Sodium chlorate is toxic: "doses of a few grams of chlorate are lethal".<ref name=Ullmann/> (ld50 oral in rats [https://fscimage.fishersci.com/msds/21100.htm 1200mg]/kg) The oxidative effect on [[hemoglobin]] leads to [[methaemoglobin]] formation, which is followed by [[denaturation (biochemistry)|denaturation]] of the [[globin]] protein and a [[cross-link]]ing of [[erythrocyte]] membrane proteins with resultant damage to the membrane enzymes. This leads to increased permeability of the membrane, and severe [[hemolysis]]. The denaturation of hemoglobin overwhelms the capacity of the [[Glucose-6-phosphate dehydrogenase|G6PD]] [[metabolic pathway]]. In addition, this enzyme is directly denatured by chlorate.

Acute severe hemolysis results, with [[organ failure|multi-organ failure]], including [[disseminated intravascular coagulation|DIC]] and [[kidney failure]]. In addition there is a direct toxicity to the [[Proximal tubule|proximal renal tubule]].<ref>((cite journal |author1=Oliver J. |author2=MacDowell M., Tracy A |title=The Pathogenesis of Acute Renal Failure Associated with Traumatic and Toxic Injury. Renal Ischemia, Nephrotoxic Damage and the Ischemuric Episode 1 | journal = [[J Clin Invest]] | year = 1951 | issue = 12 | pages = 1307–439 | pmid = 14897900 | volume = 30 | doi = 10.1172/JCI102550 | pmc = 441312))</ref> The treatment will consist of [[exchange transfusion]], [[peritoneal dialysis]] or [[hemodialysis]].<ref>Goldfrank's Toxicologic Emergencies, McGraw-Hill Professional; 8th edition (March 28, 2006), ((ISBN|978-0-07-143763-9))</ref>

== Formulations ==
Sodium chlorate comes in [[dust]], [[spray (liquid drop)|spray]] and [[:wikt:granule|granule]] formulations. Mixtures of chlorates and organic compounds pose a severe risk of explosions<ref>((cite book |last=Beveridge |first=Alexander |title=Forensic Investigation of Explosions |publisher=[[Taylor & Francis Ltd]] |year=1998 |isbn=0-7484-0565-8))</ref>

Marketed formulations contain a [[fire retardant]]. Most commercially available chlorate weedkillers contain approximately 53% sodium chlorate with the balance being a fire depressant such as [[sodium metaborate]] or [[ammonium phosphate]]s.

==Trade names==
Sodium chlorate is the active ingredient in a variety of commercial herbicides. Some trade names for products containing sodium chlorate include Atlacide, Defol, De-Fol-Ate, Drop-Leaf, Fall, Harvest-Aid, Kusatol, Leafex, and Tumbleaf. The compound may be used in combination with other herbicides such as atrazine, 2,4-D, [[bromacil]], [[diuron]], and sodium metaborate.

Sodium chlorate was an extensively used weed killer within the EU, until 2009 when it was withdrawn after a decision made under terms of EU Regulations. Its use as a herbicide outside the EU remains unaffected, as does its use in other non-herbicidal applications, such as in the production of chlorine dioxide biocides and for pulp and paper bleaching.

==Cultural references==
Historian James Watson of [[Massey University]] in New Zealand wrote a widely reported article, "The Significance of Mr. Richard Buckley's [[exploding trousers|Exploding Trousers]]"<ref>[http://aghist.metapress.com/content/q3224660874x8q51/ "The Significance of Mr. Richard Buckley's Exploding Trousers: Reflections on an Aspect of Technological Change in New Zealand Dairy Farming between the World Wars"] ((webarchive|url=https://web.archive.org/web/20131023043832/http://aghist.metapress.com/content/q3224660874x8q51/ |date=2013-10-23 )), Agricultural History magazine</ref><ref>[https://www.newscientist.com/article/mg18424771.800-histories-farmer-buckleys-exploding-trousers-.html "Histories: Farmer Buckley's exploding trousers"], New Scientist</ref> about accidents with sodium chlorate when used as a herbicide to control [[Jacobaea vulgaris|ragwort]] in the 1930s.<ref>[http://paperspast.natlib.govt.nz/cgi-bin/paperspast?a=d&d=EP19330421.2.104&e=-------10--1----0--"Trousers Explode], Evening Post, 21 April 1933</ref> This later won him an [[Ig Nobel Prize]] in 2005,<ref>[http://improbable.com/ig/ig-pastwinners.html#ig2005 James Watson for "The Significance of Mr. Richard Buckley’s Exploding Trousers."], improbable.com</ref> and was the basis for the May 2006 [[MythBusters (2006 season)#Episode 53 – "Exploding Pants"|"Exploding Pants" episode]] of [[MythBusters]].

==See also==
*[[Sodium chloride]]

==References==
((reflist))

==Further reading==
*"Chlorate de potassium. Chlorate de sodium", ''Fiche toxicol. n° 217'', Paris:Institut national de recherche et de sécurité, 2000. 4pp.

==External links==
((stack|float=right|((Commons category|Sodium chlorate))))
*[https://www.cdc.gov/niosh/ipcsneng/neng1117.html International Chemical Safety Card 1117]

((Sodium compounds))
((Chlorates))

((DEFAULTSORT:Sodium Chlorate))
[[Category:Chlorates]]
[[Category:Sodium compounds]]
[[Category:Desiccants]]
[[Category:Pyrotechnic oxidizers]]
[[Category:Oxidizing agents]]

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