View source for Borax

{{short description|Boron compound, a salt of boric acid}}
{{Other uses}}
{{distinguish|Borex|Borox|Borat}}
{{Use mdy dates|date=October 2019}}
{{chembox
| Name = Borax
| OtherNames = {{ubl|Borax decahydrate|Sodium borate decahydrate|Sodium tetraborate decahydrate|Sodium tetrahydroxy tetraborate hexahydrate}}
| ImageFile = Borax crystals.jpg
| ImageName = Borax crystals
| ImageSize = 260px
| ImageFile1 = BoraxChem.png{{!}}class=skin-invert-image
| ImageName1 = Ball-and-stick model of the unit cell of borax decahydrate
| ImageSize1 = 244px
| IUPACName = disodium;3,7-dioxido-2,4,6,8,9-pentaoxa-1,3,5,7-tetraborabicyclo[3.3.1]nonane;decahydrate<ref name="NIMH.borax"/>
| Section1 = {{chembox Identifiers
| CASNo = 1303-96-4
| CASNo_Ref = {{cascite|correct|CAS}}
| ChEMBL = 3833375
| ChEBI = 86222
| ChemSpiderID = 17339255
| EINECS = [https://echa.europa.eu/substance-information/-/substanceinfo/100.129.152 603-411-9]<ref name="NIMH.borax"/>
| KEGG = D03243
| PubChem = 16211214
| RTECS = VZ2275000
| UNII = 91MBZ8H3QO
| InChI = 1/B4O7.2Na.10H2O/c5-1-7-3-9-2(6)10-4(8-1)11-3;;;;;;;;;;;;/h;;;10*1H2/q-2;2*+1;;;;;;;;;;
| SMILES = [Na+].[Na+].O0B(O)O[B-]1(O)OB(O)O[B-]0(O)O1.O.O.O.O.O.O.O.O
| InChIKey = CDMADVZSLOHIFP-UHFFFAOYAP
| StdInChI = 1S/B4O7.2Na.10H2O/c5-1-7-3-9-2(6)10-4(8-1)11-3;;;;;;;;;;;;/h;;;10*1H2/q-2;2*+1;;;;;;;;;;
| StdInChIKey = CDMADVZSLOHIFP-UHFFFAOYSA-N
 }}
| Section2 = {{Chembox Properties
| Formula = {{chem2|Na2B4O5(OH)4*8H2O}}
| Na=2|B=4|O=17|H=20
| Appearance = White or colorless crystalline solid
| Density = 1.73 g/cm<sup>3</sup> (decahydrate, solid)<ref name=haynes2011/>
| Solubility = 31.7 g/L <ref name=haynes2011/>
| MeltingPtC = 743
| MeltingPt_notes = (anhydrous)<ref name=haynes2011/><br />75&nbsp;°C (decahydrate, decomposes)<ref name=haynes2011/>
| BoilingPtC = 1575
| BoilingPt_notes = (anhydrous)<ref name=haynes2011/>
| pKb =
| MagSus = −85.0·10<sup>−6</sup> cm<sup>3</sup>/mol (anhydrous)<ref name=haynes2011/>{{rp|p.4.135}}
| RefractIndex = ''n''<sub>1</sub>=1.447, ''n''<sub>2</sub>=1.469, ''n''<sub>3</sub>=1.472 (decahydrate)<ref name=haynes2011/>{{rp|p.4.139}}
  }}
| Section3 = {{Chembox Structure
| Structure_ref =<ref name=levy1978/>
| CrystalStruct = [[Monoclinic]], [[Pearson symbol|mS92]], No. 15
| SpaceGroup = C2/c
| PointGroup = 2/m
| LattConst_a = 1.1885 nm
| LattConst_b = 1.0654 nm
| LattConst_c = 1.2206 nm
| UnitCellFormulas = 4
| UnitCellVolume = 1.4810 nm<sup>3</sup>
| LattConst_alpha =
| LattConst_beta = 106.623°
| LattConst_gamma =
| Coordination =
| MolShape =
| OrbitalHybridisation =
| Dipole =
  }}
| Section6 = {{Chembox Pharmacology
| ATCCode_prefix = S01
| ATCCode_suffix = AX07
}}
| Section7 = {{Chembox Hazards
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| NFPA_ref = <ref name=NFPA2016/>
| IDLH = N.D.<ref name=PGCH57/>
| REL = TWA 1 mg/m<sup>3</sup> (anhydrous and pentahydrate)<ref name=PGCH57/><ref name=PGCH59/><br /> TWA 5 mg/m<sup>3</sup> (decahydrate)<ref name=PGCH58/>
| PEL = none<ref name=PGCH57/>
| GHSPictograms = {{GHS08}}
| HPhrases = {{H-phrases|360}}
| PPhrases = {{P-phrases|201|308+313}}
 }}
<!--{{Chembox/DeltaHf298|-3276.75}}
{{Chembox/S298|189.53}}
-->| Section8 = {{Chembox Related
| OtherAnions = [[Sodium aluminate]]
| OtherCations = [[Lithium tetraborate]]
| OtherCompounds = [[Boric acid]], [[sodium perborate]]
 }}
}}

'''Borax''' (also referred to as '''sodium borate''', '''tincal''' <span class="noexcerpt">({{IPAc-en|ˈ|t|ɪ|ŋ|k|əl}})</span> and '''tincar''' <span class="noexcerpt">({{IPAc-en|ˈ|t|ɪ|ŋ|k|ər}})</span>) is a [[salt (chemistry)|salt]] ([[ion]]ic compound) normally encountered as a [[hydration (chemistry)|hydrated]] [[borate]] of [[sodium]], with the [[chemical formula]] {{chem2|Na2H20B4O17|auto=1}}.<ref name="NIMH.borax"/>{{efn|It is also written as {{chem2|Na2B4O7|auto=1}}·{{chem2|10H2O|auto=1}}, which shows that it is a decahydrated tetraborate.}} [[Borax (mineral)|Borax mineral]] is a crystalline [[borate mineral]] that occurs in only a few places worldwide in quantities that enable it to be mined economically.

Borax can be dehydrated by heating into other forms with less [[water of hydration]]. The anhydrous form of borax can also be obtained from the decahydrate or other hydrates by heating and then grinding the resulting glasslike solid into a powder. It is a white crystalline solid that dissolves in water to make a [[base (chemistry)|basic]] [[aqueous solution|solution]] due to the [[tetraborate]] [[anion]].

Borax is commonly available in powder or granular form and has many industrial and household uses, including as a [[pesticide]], as a metal soldering [[flux (metallurgy)|flux]], as a component of [[glass]], [[Enamelled glass|enamel]], and [[glaze (pottery)|pottery glaze]]s, for [[tanning (leather)|tanning]] of skins and [[hide (skin)|hide]]s, for artificial aging of wood, as a [[Wood preservation|preservative against]] [[Wood-decay fungus|wood fungus]], as a [[food additive]], and as a pharmaceutic [[alkalizer]]. In chemical laboratories it is used as a [[buffer solution|buffering]] agent.<ref name="NIMH.borax"/><ref name=CompTox/>

The terms ''tincal'' and ''tincar'' refer to the naturally occurring borax historically mined from dry lake beds in various parts of Asia.<ref name=amoz2004/>

== History ==
Borax was first discovered in dry lake beds in [[Tibet]]. Native tincal from Tibet, [[Persia]], and other parts of Asia was traded via the [[Silk Road]] to the [[Arabian Peninsula]] in the 8th century AD.<ref name=amoz2004/>

Borax first came into common use in the late 19th century when [[Francis Marion Smith]]'s [[Pacific Coast Borax Company]] began to market and popularize a large variety of applications under the [[20 Mule Team Borax]] [[trademark]], named for [[Twenty-mule team|the method]] by which borax was originally hauled out of the [[Death Valley National Park|California and Nevada deserts]].<ref name=SciAm1877/><ref name=hild1982/>

== Etymology ==
The English word ''borax'' and its previous [[Middle English|Middle]] form {{Lang|enm|boras}} is a Latinate loan from [[Old French]] {{Lang|fro|boras}} ~ {{Lang|fro|bourras}}<ref name="OED.borax">{{Cite OED|borax|16485735}}</ref> which may have been from [[Medieval Latin]] {{lang|la|baurach}} (another English spelling), {{lang|la|borac(-/um/em), borax}}, along with [[Spanish language|Spanish]] {{lang|es|borrax}} (> {{lang|es|borraj}}) and [[Italian language|Italian]] {{Lang|it|borrace}}, in the 9th century, and from [[Arabic]] {{lang|ar|بورق}} {{Transliteration|ar|bawraq}} ~ {{Transliteration|ar|būraq}} ~ {{Transliteration|ar|bōraq}} which is attested in [[Ibn Sayyar al-Warraq]]'s ''Kitāb al-Ṭabīkh'' among many examples,<ref name="OED.borax"/><ref>{{cite dictionary|last=Wehr |first=Hans |authorlink=Hans Wehr |editor-first=J. Milton |editor-last=Cowan |dictionary=A Dictionary of Modern Written Arabic |title={{lang|ar|بورق|cat=no}} |url=https://ejtaal.net/aa/#hw4=113,ll=312,ls=5,la=386,sg=169,ha=68,br=145,pr=28,vi=86,mgf=124,mr=93,mn=119,aan=86,kz=188,uqq=39,ulq=419,uqa=62,uqw=189,umr=148,ums=108,umj=86,bdw=129,amr=84,asb=81,auh=239,dhq=69,mht=65,msb=33,tla=33,amj=75,ens=89,mis=1801
|location=Ithaca, NY |publisher=Spoken Language Services |year=1979 |page=100 |edition=4th |isbn=0-87950-003-4}}</ref><ref>{{cite book |last1=Ibn Sayyār al-Warrāq |first1=al-Muẓaffar ibn Naṣr |editor1-last=Nasrallah |editor1-first=Nawal |editor1-link=Nawal  Nasrallah |title=Annals of the caliphs' kitchens: Ibn Sayyār al-Warrāq's tenth-century Baghdadi cookbook |date=2007 |publisher=Brill |isbn=978-90-04-15867-2 |page=1}}</ref> from Middle Persian bwlk' (bōrag), which yielded Persian {{lang|fa|بوره}} ''bure''. 

The words ''tincal'' and ''tincar'' were adopted into [[English language|English]] in the 17th century from [[Malay language|Malay]] {{Lang|ms|tingkal}} and from [[Urdu language|Urdu]]/[[Persian language|Persian]]/[[Arabic language|Arabic]] {{script|Arab|تنکار}} {{Transliteration|ur|tinkār/tankār}}; thus the two forms in English. These all appear to be related to the [[Sanskrit language|Sanskrit]] {{Lang|sa|टांकण}} {{Transliteration|sa|ṭānkaṇa}}.<ref name=OED.tinkal/><ref name=ChemIn1976/>

== Chemistry ==
[[File:Borax-unit-cell-3D-balls.png|thumb|upright|left|The structure of borax according to [[X-ray crystallography]].]]

From a chemical perspective, borax contains the {{chem2|[B4O5(OH)4](2-)}} ion. In this structure, there are two four-coordinate boron centers and two three-coordinate boron centers.

It is a [[proton conductor]] at temperatures above {{convert|21|C|F}}. Conductivity is maximum along the ''b-''axis.<ref name=mari1962/>

Borax is also easily converted to [[boric acid]] and other [[borate]]s, which have many applications. Its reaction with hydrochloric acid to form boric acid is:

:{{chem2|Na2B4O7*10H2O + 2 HCl → 4 H3BO3 + 2 NaCl + 5 H2O}}
Borax is sufficiently stable to find use as a [[primary standard]] for acid-base [[titrimetry]].<ref name=vogel/>{{rp|p.316}}

Molten borax dissolves many metal oxides to form glasses. This property is important for its uses in metallurgy and for the [[borax bead test]] of qualitative chemical analysis.

Borax is soluble in a variety of solvents; however, it is notably insoluble in ethanol.<ref name="NIMH.borax"/>

{| class="wikitable sortable mw-collapsible"
|+ Solubility of borax in some solvents<ref name=BorCom.borax/>
! Organic solvent
! Temperature<br>°C (°F)
! Borax % by weight<br>in saturated solution
|-
|Glycerol 98.5%
|20 (68)
|52.60
|-
|Glycerol 86.5%
|20 (68)
|47.19
|-
|Ethylene glycol
|25 (77)
|41.60
|-
|Diethylene glycol
|25 (77)
|18.60
|-
|Methanol
|25 (77)
|19.90
|-
|Aqueous ethanol 46.5%
|15.5 (60)
|2.48
|-
|Acetone
|25 (77)
|0.60
|-
|Ethyl acetate
|25 (77)
|0.14
|}

{| class="wikitable"
|+ Solubility of borax in water<ref name=BorCom.borax/>
! Temperature<br>°C (°F)
! Borax % by weight in saturated solution
|-
|0 (32)
|1.99
|-
|5 (41)
|2.46
|-
|10 (50)
|3.09
|-
|15 (59)
|3.79
|-
|20 (68)
|4.70
|-
|25 (77)
|5.80
|-
|30 (86)
|7.20
|-
|35 (95)
|9.02
|-
|40 (104)
|11.22
|-
|45 (113)
|14.21
|-
|50 (122)
|17.91
|-
|55 (131)
|23.22
|-
|60 (140)
|30.32
|-
|65 (149)
|33.89
|-
|70 (158)
|36.94
|-
|75 (167)
|40.18
|-
|80 (176)
|44.31
|-
|85 (185)
|48.52
|-
|90 (194)
|53.18
|-
|95 (203)
|58.94
|-
|100 (212)
|65.63
|}

The term ''borax'' properly refers to the so-called "decahydrate" {{chem2|Na2B4O7*10H2O}}, but that name is not consistent with its structure. It is actually octahydrate. The [[anion]] is not [[tetraborate]] {{chem2|[B4O7](2-)}} but [[tetraborate|tetrahydroxy tetraborate]] {{chem2|[B4O5(OH)4](2-)}},<ref name=mari1962/> so the more correct formula should be {{chem2|Na2B4O5(OH)4*8H2O}}. However, the term may be applied also to the related compounds. Borax "pentahydrate" has the formula {{chem2|Na2B4O7*5H2O}}, which is actually a trihydrate {{chem2|Na2B4O5(OH)4*3H2O}}. It is a colorless solid with a density of {{val|1.880|u=kg/m3}} that crystallizes from water solutions above {{convert|60.8|C|F}} in the [[rhombohedral crystal system]]. It occurs naturally as the mineral [[tinkhanite]].<ref name=akgu2021/> It can be obtained by heating the "decahydrate" above {{convert|61|C|F}}.<ref name=sahin2002/> Borax "dihydrate" has the formula {{chem2|Na2B4O7*2H2O}}, which is actually anhydrous, with the correct formula {{chem2|Na2B4O5(OH)4}}. It can be obtained by heating the "decahydrate" or "pentahydrate" to above {{convert|116-120|C|F}}.<ref name=sahin2002/> Anhydrous borax is sodium tetraborate proper, with formula {{chem2|Na2B4O7}}. It can be obtained by heating any hydrate to {{convert|300|C|F}}.<ref name=sahin2002/> It has one amorphous (glassy) form and three crystalline forms – α, β, and γ, with melting points of {{convert|1015|K}}, {{convert|993|K}} and {{convert|936|K}} respectively. {{chem2|α\-Na2B4O7}} is the stable form.<ref name=sahin2002/>

== Natural sources ==
{{main|Borax (mineral)}}
[[File:Borax ball.jpg|thumb|Borax "cottonball" {{explain|reason=This term isn't mentioned anywhere and it's unclear whether this is even a natural source from the caption, or how this isn't just a rock from the 1980s digital camera quality picture.|date=July 2025}}]]

Borax occurs naturally in [[evaporite]] deposits produced by the repeated evaporation of [[seasonal lake]]s. The most commercially important deposits are found in:  [[Boron, California]]; and [[Searles Lake]], [[California]]. Also, borax has been found at many other locations in the [[Southwestern United States]], the [[Atacama Desert]] in [[Chile]], newly discovered deposits in [[Bolivia]], and in [[Tibet]] and [[Romania]]. Borax can also be produced synthetically from other boron compounds.<ref>{{Cite web |title=Borax - The Chemical Company |url=https://thechemco.com/chemical/borax/ |access-date=2024-04-08 |website=thechemco.com |language=en-US}}</ref>

Naturally occurring borax (known by the trade name Rasorite–46 in the United States and many other countries) is refined by a process of [[Recrystallization (chemistry)|recrystallization]].<ref name=wizn2005/>
[[File:Hauling Borax, Death Valley, 1904.jpg|thumb|[[traction engine|Traction]] steam engine hauling borax, [[Death Valley National Park]], California, 1904]]

== Uses ==
[[File:Borax.jpg|thumb|left|upright|Borax-based [[laundry detergent]]]]

Borax is used in pest control solutions because it is toxic to ants and rats. Because it is slow-acting, worker ants will carry the borax to their nests and poison the rest of the colony.<ref name=klotz2000/> Borax is more effective than zinc borate for termite control but a 1997 paper concluded that exposing at least 10% of the total colony population was needed for effective treatment. In Japan the practice of laying newspapers treated with o-boric acid and borax under buildings has been effective in controlling [[Coptotermes formosanus]] and [[Reticulitermes speratus]] populations. Decaying wood treated with 0.25 to 0.5 percent DOT was also found to be effective for baiting [[Heterotermes aureus]] populations. The paper concluded: "Borate baits would undoubtably be helpful in the long-term, but do not appear sufficient as a sole method of structural protection."<ref>{{cite journal  | title = Review of recent research on the use of borates for termite prevention | journal = In Proceedings of the 2nd International Conference on Wood Protection with Diffusible Preservatives and Pesticides |date=1997 | url = http://manoa.hawaii.edu/ctahr/termite/aboutcontact/grace/pdfs/123.pdf  | pages = 85–92  }}</ref>

Borax is used in various household laundry and cleaning products,<ref name=HPD136/><ref name=USBor2022/> including the [[20 Mule Team Borax]] laundry booster, [[Boraxo]] powdered hand soap, and some [[tooth bleaching]] formulas.<ref name=hamm2004/><ref name=oneil2013/>

Borate ions (commonly supplied as boric acid) are used in biochemical and chemical laboratories to make [[buffer solution|buffers]], e.g. for [[polyacrylamide gel electrophoresis]] of DNA and RNA, such as [[TBE buffer]] (borate buffered tris-hydroxymethylaminomethonium)<ref name=peac1967/><ref name=ande1981/> or the newer SB buffer or [[BBS buffer]] (borate buffered saline) in coating procedures. Borate buffers (usually at pH 8) are also used as preferential equilibration solutions in [[dimethyl pimelimidate]] (DMP) based crosslinking reactions.<ref>{{cite book |last1=Harvey |first1=Dexter |last2=Rutledge |first2=Nicky |title=Industrial Chemistry |date=1 April 2019 |publisher=EdTech Press |location=Waltham Abbey |isbn=978-1-83947-197-1 |page=255 |url=https://books.google.com/books?id=feLEDwAAQBAJ&dq=dimethyl+pimelimidate+borax&pg=PA255 |language=en}}</ref>

Borax as a source of borate has been used to take advantage of the co-complexing ability of borate with other agents in water to form complex ions with various substances. Borate and a suitable [[polymer]] bed are used to [[chromatograph]] non-glycated [[hemoglobin]] differentially from [[glycated hemoglobin]] (chiefly [[HbA1c]]), which is an indicator of long-term [[hyperglycemia]] in [[diabetes mellitus]]{{citation needed|date=July 2025}}

Borax alone does not have a high affinity for [[Hard water#Types|hardness cations]], although it has been used for water softening. A general chemical equation for [[water softening]] is (R is the dissolved cation, usually calcium or magnesium):

:{{chem2|R(2+)(aq) + Na2B4O7(aq) → RB4O7(s)↓ + 2 Na+(aq)}}

The sodium ions introduced do not make water "hard". This method is suitable for removing both temporary and permanent types of hardness.{{citation needed|date=July 2025}}

A mixture of borax and [[ammonium chloride]] is used as a [[Flux (metallurgy)|flux]] when [[welding]] [[iron]] and [[steel]]. It lowers the melting point of the unwanted [[iron oxide]] ([[Mill scale|scale]]), allowing it to run off. Borax is also mixed with water as a flux when [[soldering]] [[jewelry]] [[metal]]s such as [[gold]] or [[silver]], where it allows the molten [[solder]] to [[Wetting|wet]] the metal and flow evenly into the joint.<ref>{{cite book |last1=Hasluck |first1=Paul Nooncree |author1-link=Paul N. Hasluck |title=The Mechanic's Workshop Handybook |date=1895 |publisher=Crosby Lockwood |location=London |page=62 |url=https://books.google.com/books?id=R1xRAAAAYAAJ&dq=borax+gold+jewellery&pg=PA62}}</ref> Borax is also a flux for "pre-tinning" [[tungsten]] with [[zinc]], making the tungsten soft-solderable.<ref name=dodd1966/> Borax is often used as a flux for [[forge welding]].<ref name="Moehring-2016" />

[[File:Borax wagons.jpg|thumb|Old [[steam tractor]] with borax wagons, [[Death Valley National Park]] ]]

In [[Artisanal mining|artisanal gold mining]], borax is sometimes used as part of a process known as the [[borax method]] (as a flux) meant to eliminate the need for toxic mercury in the [[gold extraction]] process, although it cannot directly replace mercury. Borax was reportedly used by gold miners in parts of the Philippines in the 1900s.<ref name=BSmith2012/><ref name=GEUS2008/> There is evidence that, in addition to reducing the environmental impact, this method achieves better gold recovery for suitable ores and is less expensive. This borax method is used in northern [[Luzon]] in the Philippines, but miners have been reluctant to adopt it elsewhere for reasons that are not well understood.<ref name=appel2012/> The method has also been promoted in Bolivia<ref name=ande2015/> and Tanzania.<ref name=appel1969/>

A rubbery polymer sometimes called [[Slime (toy)|Slime]], [[Flubber (material)|Flubber]], "gluep" or "glurch" (or erroneously called [[Silly Putty]], which is based on silicone polymers), can be made by [[cross-link]]ing [[polyvinyl alcohol]] with borax.<ref>{{cite web |title=How to Make Homemade Slime {{!}} Crafts for Kids |url=https://www.pbs.org/parents/crafts-and-experiments/homemade-gak |website=PBS KIDS for Parents |publisher=[[PBS]] |access-date=8 July 2025 |language=en}}</ref> Making flubber from [[polyvinyl acetate]]-based glues, such as Elmer's Glue, and borax is a common elementary science demonstration.<ref name=parr1998/><ref name=ChemAboutXXXX/>

Borax, given the [[E number]] ''E285'', is used as a [[food additive]] but this use is banned in some countries, such as Australia, China, Thailand and the United States.<ref name=reil2019/> As a consequence, certain foods, such as [[caviar]], produced for sale in the United States contain higher levels of salt to assist preservation.<ref name=HansonLtd2008/> In addition to its use as a preservative, borax imparts a firm, rubbery texture to food. In China, borax ({{lang-zh|c=硼砂|p=péng shā}} or {{lang-zh|c=月石|p=yuè shí|link=no}}) has been found in foods including wheat and rice noodles named ''[[lamian]]'' ({{lang-zh|s=拉面|p=lāmiàn|link=no}}), ''[[shahe fen]]'' ({{lang-zh|s=沙河粉|p=shāhéfěn|link=no}}), ''[[char kway teow]]'' ({{lang-zh|c=粿條|p=guǒ tiáo|link=no}}), and ''[[chee cheong fun]]'' ({{lang-zh|s=肠粉|p=chángfěn|link=no}}){{clarify|Most of these are dishes, not wheat and rice noodles, and at least one is just a dish made from another listed noodle.|date=March 2023}}<ref name="Chow2005" /> In Indonesia, it is a common, but forbidden,<ref name="PomGo2021" /> additive to such foods as noodles, [[bakso]] (meatballs), and steamed rice.

[[File:Boron mine pit.jpg|thumbnail|Rio Tinto borax mine pit, [[Boron, California]]]]

=== Other ===
Other uses include:

* Ingredient in [[vitreous enamel|enamel glazes]].<ref name=Sheff2019/>
* Component of [[glass]], [[pottery]], and [[ceramic]]s.<ref name="Schubert-2003"/>
* Used as an additive in ceramic slips and [[ceramic glaze]]s to improve fit on wet, greenware, and [[bisque (pottery)|bisque]].{{citation needed|date=September 2019}}
* [[Flame retardant]] treatment for fabric.<ref name=shen1998/><ref>{{cite web | url=https://www.arkansasairandmilitary.com/post/artifact-friday-k2b-flight-suit | title=Artifact Friday: K2B Flight Suit | date=August 11, 2023 }}</ref><ref>{{cite web | url=http://www.vietnamgear.com/kit.aspx?kit=61 | title=K-2B Flying Coveralls }}</ref>
* [[Fungicide|Anti-fungal]] compound for [[cellulose insulation]].<ref name="Schubert-2003" />
* Mothproofing 10% solution for wool.<ref name=CAltTech2016/>
* Pulverized for the prevention of stubborn pests (e.g. [[German cockroach]]es) in closets, pipe and cable inlets, wall panelling gaps, and inaccessible locations where ordinary [[pesticide]]s are undesirable.<ref>{{cite book |last1=Rierson |first1=Donald A. |title=Understanding and controlling the German cockroach |date=1995 |publisher=Oxford University Press |isbn=9780195345087 |page=232|url=https://books.google.com/books?id=4j8n8hIBEa0C&dq=cockroach+borax&pg=PA232}}</ref>
* [[Tackifier]] ingredient in [[casein]], [[starch]] and [[dextrin]]-based adhesives.<ref name=suar2011/>
* To make indelible ink for [[dip pen]]s by dissolving [[shellac]] into heated borax.{{citation needed|date=September 2019}}
* [[Curing agent]] for [[snake]] skins.{{citation needed|date=September 2019}}
* Curing agent for [[salmon]] eggs, for use in sport fishing for salmon.<ref name=rams2021/>
* Swimming pool [[buffering agent]] to control [[pH]].<ref name=Pools2008/>
* In [[boiling water reactor|nuclear reactor]]s and spent fuel pools as a [[neutron absorber]] to control reactivity and to shut down a nuclear chain reaction.<ref name=BARC2010/>
* As a [[micronutrient]] fertilizer to correct [[Boron deficiency (plant disorder)|boron-deficient soils]].<ref name=NatBer2016/><ref name=SpeAnal2016/>
* [[Preservative]] in [[taxidermy]].<ref name=Taxid2021/>
* To color fires with a green tint.<ref name=marie2016/>
* Traditionally used to coat dry-cured meats such as hams to improve the appearance and discourage flies.<ref name=nich1991/><ref name=NHSBH1906/><ref name=IndonesiaDCP/>
* Used as a flux for melting metals and alloys in [[Casting (metalworking)|casting]] to draw out impurities and prevent [[Redox|oxidation]].{{citation needed|date=September 2019}}
* Used as a [[woodworm]] treatment (diluted in water).{{citation needed|date=September 2019}}
* In [[particle physics]] as an additive to [[nuclear emulsion]], to extend the latent image lifetime of charged particle tracks. The first observation of the [[pion]], which was awarded the 1950 [[Nobel Prize]], used this type of emulsion.<ref name=latt1947/><ref name=latt1947b/>

== Toxicity ==
According to one study, borax is not acutely toxic. Its {{LD50}} (median lethal dose) score is tested at 2.66 g/kg in rats, meaning that a significant dose of the chemical is needed to cause severe symptoms or death.{{citation needed|date=July 2025}}

The lethal dose is not necessarily the same for humans; human studies in three borate exposure-rich comparison groups (U.S. Borax mine and production facility workers, Chinese boron workers, Turkish residents living near boron rich regions) produced no indicators of developmental toxicity in blood and semen tests. The highest estimated exposure was 5&nbsp;mg B/kg/day, likely due to eating in contaminated workplaces, more than 100 times the average daily exposure.<ref name="CLH2018">{{cite web |title= CLH report for boric acid – Proposal for Harmonised Classification and Labelling |publisher= Bureau for Chemical Substances |url= https://echa.europa.eu/documents/10162/23665416/clh_rep_boric_acid_5521_en.pdf/ee39f026-9d2d-28f7-5d90-63a424112162 |date= 23 April 2018 |access-date= 18 October 2018 |place= Lodz, Poland }}</ref>

Borax is absorbed poorly through intact skin, although fatalities have been recorded in persistent treatment of rashes and open wounds with boric acid-containing ointments and bath solutions. Borax is readily absorbed orally, well above 90%, and mostly excreted through the urine. Fatal cases attributed to ingestion include small children mistakenly drinking pesticides or suicide attempts with large volumes of crystals. No genotoxicity or carcinogenicity has been recorded in studies.<ref>{{cite journal  | title = Toxicity of boric acid, borax and other boron containing compounds: A review| journal = Regul Toxicol Pharmacol |date=2021 | doi = 10.1016/j.yrtph.2021.104873| pmid = 33485927  | last1 = Hadrup | first1 = Niels | last2 = Frederiksen | first2 = Marie | last3 = Sharma | first3 = Anoop K. | volume = 121 | article-number = 104873 }}</ref>

Borax has been in use as an insecticide in the United States with various restrictions since 1946. All restrictions were removed in February 1986 due to the low toxicity of borax, as reported in two EPA documents relating to boric acid and borax.<ref name=EPA.Pest/><ref name=EPA.BoraxOK/>

{{blockquote|EPA has determined that, because they are of low toxicity and occur naturally, boric acid and its sodium salts should be exempted from the requirement of a tolerance (maximum residue limit) for all raw agricultural commodities.<ref name=EPA.Pest />}}

Although it cited inconclusive data, a re-evaluation in 2006 by the EPA still found that "There were no signs of toxicity observed during the study and no evidence of [[cytotoxicity]] to the target organ."<ref name=EPA.Reg62.4/> In the reevaluation, a study of toxicity due to overexposure was checked and the findings were that "The residential handler inhalation risks due to boric acid and its sodium salts as active ingredients are not a risk concern and do not exceed the level of concern", but that there could be some risk of irritation to children inhaling it if used as a powder for cleaning rugs.

Overexposure to borax dust can cause respiratory irritation, while no skin irritation is known to exist due to external borax exposure. Ingestion may cause gastrointestinal distress including [[nausea]], persistent vomiting, abdominal pain, and [[diarrhea]]. Effects on the vascular system and [[human brain]] include headaches and lethargy but are less frequent. In severe cases, a "beefy" red rash affecting the palms, soles, buttocks and scrotum has occurred.<ref name=reig2009/>

Borax was added to the [[Substance of very high concern|Substance of Very High Concern (SVHC)]] candidate list on December 16, 2010. The SVHC candidate list is part of the [[European Union|EU]] Regulations on the [[Registration, Evaluation, Authorisation and Restriction of Chemicals]] 2006 (REACH), and the addition was based on the revised classification of borax as ''toxic for reproduction'' category 1B under the [[CLP Regulation]]s. Substances and mixtures imported into the EU which contain borax are now required to be labelled with the warnings "May damage fertility" and "May damage the unborn child".<ref name=ECHA2010/> It was proposed for addition to REACH Annex XIV by the [[European Chemicals Agency|ECHA]] on July 1, 2015.<ref name=ECHA2015/> If this recommendation is approved, all imports and uses of borax in the EU will have to be authorized by the ECHA.{{update after|2016|8|17}}

A review of the boron toxicity (as boric acid and borates) published in 2012 in the ''[[Journal of Toxicology and Environmental Health]]'' concluded: "It clearly appears that human B [boron] exposures, even in the highest exposed cohorts, are too low to reach the blood (and target tissue) concentrations that would be required to exert adverse effects on reproductive functions."<ref name=bolt2012/> A draft risk assessment released by [[Health Canada]] in July 2016 has found that overexposure to boric acid has the potential to cause developmental and reproductive health effects. Since people are already exposed to boric acid naturally through their diets and water, Health Canada advised that exposure from other sources should be reduced as much as possible, especially for children and pregnant women.

The concern is not with any one product, but rather multiple exposures from a variety of sources. With this in mind, the department also announced that certain pesticides that contain boric acid, which are commonly used in homes, will have their registrations cancelled and be phased out of the marketplace. As well, new, more protective label directions are being introduced for other boric acid pesticides that continue to be registered in Canada (for example, enclosed bait stations and spot treatments using gel formulations).<ref name=CanHealth2016/>

== See also ==
* [[Borax bead test]]
* [[John Veatch]]
* [[List of cleaning agents]]
* [[Sodium borohydride]]
* [[Ulexite]]

== Explanatory footnotes ==
{{Notelist|1}}

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<ref name="CanHealth2016">{{Cite web |date=July 22, 2016 |title=Information Update&nbsp;– Health Canada advises Canadians to avoid homemade craft and pesticide recipes using boric acid&nbsp;– Recalls & alerts |url=http://healthycanadians.gc.ca/recall-alert-rappel-avis/hc-sc/2016/59514a-eng.php |access-date=August 7, 2016 |website=Healthycanadians.gc.ca}}</ref>
<ref name="oneil2013">{{Cite encyclopedia |year=2013 |encyclopedia=The Merck Index&nbsp;— An Encyclopedia of Chemicals, Drugs, and Biologicals |publisher=Royal Society of Chemistry |location=Cambridge, UK |editor-last=O'Neil |editor-first=M.J. |page=1595}}</ref>
<ref name="akgu2021">{{Cite journal |last1=Akgül |first1=Mehmet |last2=Çamlıbel |first2=Osman |date=March 2021 |title=The use of borax pentahydrate of inorganic filler in medium density fiberboard production |url=http://www.scielo.cl/scielo.php?script=sci_arttext&pid=S0718-221X2021000100422&lng=es&nrm=iso&tlng=es |journal=Maderas. Ciencia y tecnología |language=en |volume=23 |doi=10.4067/S0718-221X2021000100422 |issn=0718-221X}}</ref>
<ref name="sahin2002">{{Cite journal |last1=Şahin |first1=Ömer |last2=Bulutcu |first2=A. Nusret |year=2002 |title=Dehydration Behaviour of Borax Pentahydrate to Anhydrous Borax by Multi-Stage Heating in a Fluidized |url=https://journals.tubitak.gov.tr/chem/vol26/iss1/10 |journal=Turkish Journal of Chemistry |volume=26 |pages=89–96 |article-number=10}}</ref>
</references>

== External links ==
{{Commons category|Borax}}
{{wiktionary}}
{{AmCyc Poster|Borax}}
* {{ICSC|0567}}
* {{ICSC|1229}} (fused borax)
* [https://web.archive.org/web/20060209040519/http://www.npi.gov.au/database/substance-info/profiles/15.html National Pollutant Inventory&nbsp;– Boron and compounds]
* [https://www.cdc.gov/niosh/npg/npgd0058.html NIOSH Pocket Guide to Chemical Hazards]
* [https://web.archive.org/web/20020821230321/http://www.sefsc.noaa.gov/HTMLdocs/SodiumBorate.htm Sodium Borate in sefsc.noaa.gov]

{{Borates}}
{{Sodium compounds}}
{{Authority control}}

[[Category:Borates]]
[[Category:E-number additives]]
[[Category:Evaporite]]
[[Category:Cleaning product components]]
[[Category:Cleaning products]]
[[Category:Food additives]]
[[Category:Household chemicals]]
[[Category:Neutron poisons]]
[[Category:Photographic chemicals]]
[[Category:Sodium compounds]]