{{short description|Weak acid of boron}} {{Redirect|Boric||Boric (disambiguation)}} {{Use dmy dates|date=June 2013}} {{Chembox | Watchedfields = changed | verifiedrevid = 476995365 | ImageFileL1_Ref = {{chemboximage|correct|??}} | Name = Orthoboric acid | ImageFile = | ImageFileL1 = Boric-acid-2D.png | ImageNameL1 = Structural formula | ImageFileR1 = Boric-acid-3D-vdW.png | ImageNameR1 = Space-filling model | ImageFile2 = Boric acid.jpg | ImageName2 = Boric acid crystals | IUPACName = Boric acid | SystematicName = Trihydroxidoboron (not validated) | OtherNames = Orthoboric acid, Boracic acid, Sassolite, Borofax, Trihydroxyborane, Boranetriol, Hydrogen borate | Section1 = {{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 7346 | PubChem = 7628 | SMILES1 = [OH+]=[B-](O)O | ChEMBL_Ref = {{ebicite|correct|EBI}} | ChEMBL = 42403 | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/BH3O3/c2-1(3)4/h2-4H | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = KGBXLFKZBHKPEV-UHFFFAOYSA-N | CASNo = 10043-35-3 | CASNo_Ref = {{cascite|correct|CAS}} | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 33118 | SMILES = OB(O)O | UNII_Ref = {{fdacite|correct|FDA}} | UNII = R57ZHV85D4 | KEGG_Ref = {{keggcite|correct|kegg}} | KEGG = D01089 | InChI=1/BH3O3/c2-1(3)4/h2-4H | InChIKey = KGBXLFKZBHKPEV-UHFFFAOYAI | EINECS = 233-139-2 }} | Section2 = {{Chembox Properties | H=3 | B=1 | O=3 | Appearance = White crystalline solid | Density = 1.435 g/cm3 | Solubility = 2.52 g/100 mL (0 °C)
4.72 g/100 mL (20 °C)
5.7 g/100 mL (25 °C)
19.10 g/100 mL (80 °C)
27.53 g/100 mL (100 °C) | SolubleOther = Soluble in lower [[Alcohol (chemistry)|alcohol]]s
moderately soluble in [[pyridine]]
very slightly soluble in [[acetone]] | Solvent = other solvents | MeltingPtC = 170.9 | BoilingPtC = 300 | ConjugateBase = [[Borate]] | pKa = 9.24, 12.4, 13.3 | MagSus = -34.1·10−6 cm3/mol | LogP = -0.29 }} | Section3 = {{Chembox Structure | MolShape = Trigonal planar | Dipole = Zero }} | Section4 = | Section5 = | Section6 = {{Chembox Pharmacology | ATCCode_prefix = S02 | ATCCode_suffix = AA03 | ATC_Supplemental = {{ATC|D08|AD}} }} | Section7 = {{Chembox Hazards | GHSPictograms = {{GHS08}} | NFPA-H = 1 | NFPA-F = 0 | NFPA-R = 0 | FlashPt = Non-flammable | LD50 = 2660 mg/kg, oral (rat) }} | Section8 = {{Chembox Related | OtherCompounds = [[Boron trioxide]]
[[Borax]]}} }} '''Boric acid''', more specifically '''orthoboric acid''', is a compound of [[boron]], [[oxygen]], and [[hydrogen]] with formula {{chem2|BO3H3}} or {{chem2|B(OH)3}}. It may also be called '''hydrogen borate''' or '''boracic acid'''. It is usually encountered as colorless crystals or a white powder, that dissolves in [[water]], and occurs in nature as the [[mineral]] [[sassolite]]. It is a weak a weak [[acid]] that yields various [[borate]] [[anion]]s and [[salt (chemistry)|salts]], and can react with [[alcohol]]s to form borate [[ester]]s. Boric acid is often used as an [[antiseptic]], [[insecticide]], [[flame retardant]], [[neutron absorber]], or precursor to other boron compounds. The term "boric acid" is also used generically for any [[oxoacid]] of boron, such as [[metaboric acid]] {{chem2|HBO2}} and [[tetraboric acid]] {{chem2|H2B4O7}}. ==History== Orthoboric acid was first prepared by [[Wilhelm Homberg]] (1652–1715) from borax, by the action of mineral acids, and was given the name {{lang|la|sal sedativum Hombergi}} ("sedative salt of Homberg"). However boric acid and [[borate]]s have been used since the time of the [[ancient Greece|ancient Greek]]s for cleaning, preserving food, and other activities. ==Preparation== Boric acid may be prepared by reacting [[borax]] (sodium tetraborate decahydrate) with a [[mineral acid]], such as [[hydrochloric acid]]: : {{chem2|Na2B4O7}}·10{{H2O}} + 2 HCl → 4 {{chem2|B(OH)3}} + 2 NaCl + 5 {{H2O}} It is also formed as a by product of hydrolysis of boron trihalides and [[diborane]]: : {{chem2|B2H6}} + 6 {{H2O}} → 2 {{chem2|B(OH)3}} + 6 {{chem2|H2}} : {{chem2|BX3}} + 3 {{H2O}} → {{chem2|B(OH)3}} + 3 HX (X = Cl, Br, I) ==Reactions== ===Pyrolysis=== When heated above 170 °C, it dehydrates, forming [[metaboric acid]] ({{chem2|HBO2}}): : {{chem2|B(OH)3}} → {{chem2|HBO2}} + {{H2O}} Heating metaboric acid above about 300 °C eliminates another water molecule forming [[tetraboric acid]], also called pyroboric acid ({{chem2|H2B4O7}}): : 4 {{chem2|HBO2}} → {{chem2|H2B4O7}} + {{H2O}} Further heating (to about 330 °C) leads to [[boron trioxide]]. : {{chem2|H2B4O7}} → 2 {{chem2|B2O3}} + {{H2O}} ===Aqueous solution=== When orthoboric acid is dissolved in water, it partially dissociates to give [[metaboric acid]]: : {{chem2|B(OH)3}} {{Eqm}} {{chem2|HBO2}} + {{H2O}} The solutions is mildly mildly acidic due to ionization of the acids: : {{chem2|B(OH)3}} + {{H2O}} {{Eqm}} {{chem2|[BO(OH)2]-}} + {{H3O+}} : {{chem2|HBO2}} + {{H2O}} {{Eqm}} {{chem2|[BO2]-}} + {{H3O+}} However, [[Raman spectroscopy]] of strongly alkaline solutions has shown the presence of {{chem2|[B(OH)4]−}} ion, leading some to conclude that the acidity is exclusively due to the abstraction of {{chem2|OH-}} from water: :{{chem2|B(OH)3}} + {{H2O}} {{Eqm}} {{chem2|B(OH)4-}} + {{H+}} (''K'' = 7.3×10−10; p''K'' = 9.14) or more properly: :{{chem2|B(OH)3}} + 2 {{H2O}} {{Eqm}} {{chem2|B(OH)4-}} + {{H3O+}} This may be characterized as [[Lewis acid]]ity of boron toward {{chem2|[HO]-}}, rather than as [[Brønsted acid]]ity. However, some of its behaviour towards some chemical reactions suggest it to be tribasic acid in the Brønsted sense as well. Boric acid, mixed with [[borax]] ([[sodium tetraborate decahydrate]]) at the weight ratio of 4:5, is highly soluble in water, though they are not so soluble separately. ===Sulfuric acid solution=== Boric acid also dissolves in anhydrous sulfuric acid according to the equation :{{chem2|B(OH)3}} + 6 {{chem2|H2SO4}} → {{chem2|[B(SO4H)4]-}} + 2 {{chem2|[HSO4]-}} + 3 {{H3O+}} ===With vicinal diols=== The acidity of boric acid solutions is greatly increased in the presence of [[cis–trans isomerism|cis]]-[[diol#Vicinal diols|vicinal diols]] ([[organic compound]]s containing similarly-oriented [[hydroxyl]] groups in adjacent [[carbon]] atoms, {{chem2|(R1,R2)\dC(OH)\sC(OH)\d(R3,R4)}}) such as [[glycerol]] and [[mannitol]]. With the latter, for example, the ionization of {{chem2|B(OH)3}} may increase from pK = 9 to pK = 5.5 or even 3.8, depending on concentration. The resulting solution may be called "mannitoboric acid".This is due to the formation of stable complexes between the diol and the {{chem2|[B(OH)4]-}} anions, that shift the ionization equilibrium towards the latter. ===Esterification=== Boric acid reacts with alcohols to form [[borate ester]]s, {{chem2|B(OR)3}} where R is [[alkyl]] or [[aryl]]. The reaction is typically driven by a dehydrating agent, such as concentrated [[sulfuric acid]]: :{{chem2|B(OH)3}} + 3 ROH → {{chem2|B(OR)3}} + 3 {{H2O}} ==Molecular and crystal structure== The three oxygen atoms form a [[Trigonal planar molecular geometry|trigonal planar geometry]] around the boron. The B-O bond length is 136 pm and the O-H is 97 pm. The [[molecular symmetry|molecular point group]] is ''C''3h. Crystalline boric acid consists of layers of {{chem2|B(OH)3}} molecules held together by hydrogen bonds of length 272 pm. The distance between two adjacent layers is 318 pm. {| style="margin:auto;" class="wikitable" |
[[File:Boric-acid-unit-cell-3D-balls.png|200px]]
||
[[File:Boric-acid-layer-3D-balls.png|250px]]
|- |
The [[unit cell]] of boric acid
||
[[hydrogen bond]]ing (dashed lines)
allows boric acid molecules to form
parallel layers in the solid state
|} ==Toxicology== Based on mammalian [[median lethal dose]] (LD50) rating of 2,660 mg/kg body mass, boric acid is only poisonous if taken internally or inhaled in large quantities. The Fourteenth Edition of the ''[[Merck Index]]'' indicates that the LD50 of boric acid is 5.14 g/kg for oral dosages given to rats, and that 5 to 20 g/kg has produced death in adult humans. For a 70 kg adult, at the lower 5g limit, 350g could produce death in humans. For comparison's sake, the LD50 of [[sodium chloride|salt]] is reported to be 3.75 g/kg in rats according to the ''Merck Index''. According to the [[Agency for Toxic Substances and Disease Registry]], "The minimal lethal dose of ingested boron (as boric acid) was reported to be 2–3 g in infants, 5–6 g in children, and 15–20 g in adults. [...] However, a review of 784 human poisonings with boric acid (10–88 g) reported no fatalities, with 88% of cases being asymptomatic." Long-term exposure to boric acid may be of more concern, causing kidney damage and eventually kidney failure (see links below). Although it does not appear to be [[carcinogenic]], studies in dogs have reported [[testicular atrophy]] after exposure to 32 mg/kg bw/day for 90 days. This level, were it applicable to humans at like dose, would equate to a cumulative dose of 202g over 90 days for a 70 kg adult, not far lower than the above LD50. According to the CLH report for boric acid published by the Bureau for Chemical Substances Lodz, Poland, boric acid in high doses shows significant developmental toxicity and [[teratogenicity]] in rabbit, rat, and mouse fetuses as well as cardiovascular defects, skeletal variations, and mild kidney lesions. As a consequence in the 30th ATP to EU directive 67/548/EEC of August 2008, the European Commission decided to amend its classification as [[reprotoxic]] category 2, and to apply the [[risk phrase]]s R60 (may impair fertility) and R61 (may cause harm to the unborn child). At a 2010 European Diagnostics Manufacturing Association (EDMA) Meeting, several new additions to the Substance of Very High Concern (SVHC) candidate list in relation to the [[Registration, Evaluation, Authorisation and Restriction of Chemicals]] Regulations 2007 (REACH) were discussed. Following the registration and review completed as part of REACH, the classification of Boric Acid CAS 10043-35-3 / 11113-50-1 is listed from 1 December 2010 is ''H360FD (May damage fertility. May damage the unborn child.)'' ==Uses== ===Industrial=== The primary industrial use of boric acid is in the manufacture of monofilament [[fiberglass]] usually referred to as textile fiberglass. Textile fiberglass is used to reinforce plastics in applications that range from boats, to industrial piping to computer circuit boards. In the jewelry industry, boric acid is often used in combination with [[denatured alcohol]] to reduce surface [[oxidation]] and [[firescale]] from forming on metals during [[annealing (metallurgy)|annealing]] and [[soldering]] operations. Boric acid is used in the production of the glass in [[liquid crystal display|LCD]] [[flat panel display]]s. In [[electroplating]], boric acid is used as part of some proprietary formulas. One such known formula calls for about a 1 to 10 ratio of {{chem|H|3|BO|3}} to [[nickel(II) sulfate|{{chem|NiSO|4}}]], a very small portion of [[sodium lauryl sulfate]] and a small portion of [[sulfuric acid|{{chem|H|2|SO|4}}]]. The solution of orthoboric acid and borax in 4:5 ratio is used as a [[Fire retardant|fire retarding agent]] of wood by impregnation. It is also used in the manufacturing of [[ramming mass]], a fine [[silica]]-containing powder used for producing [[induction furnace]] linings and [[ceramic]]s. Boric acid is added to [[borax]] for use as [[welding]] [[flux (metallurgy)|flux]] by [[blacksmith]]s. Boric acid, in combination with [[polyvinyl alcohol]] (PVA) or [[silicone oil]], is used to manufacture [[Silly Putty]]. Boric acid is also present in the list of chemical additives used for [[hydraulic fracturing]] (fracking) in the [[Marcellus Shale]] in Pennsylvania. Indeed, it is often used in conjonction with [[guar gum]] as [[cross-link]]ing and gelling agent for controlling the [[viscosity]] and the rheology of the fracking fluid injected at high pressure in the well. Indeed, it is important to control the fluid viscosity for keeping in suspension on long transport distances the grains of the [[Hydraulic fracturing proppants|propping agents]] aimed at maintaining the cracks in the [[shale]]s sufficiently open to facilitate the gas extraction after the hydraulic pressure is relieved. The rheological properties of borate cross-linked guar gum [[hydrogel]] mainly depend on the [[pH]] value. ===Medical=== Boric acid can be used as an [[antiseptic]] for minor burns or cuts and is sometimes used in salves and [[medical dressing|dressings]], such as [[boracic lint]]. Boric acid is applied in a very dilute solution as an eye wash. Dilute boric acid can be used as a vaginal douche to treat [[bacterial vaginosis]] due to excessive alkalinity, as well as [[candidiasis]] due to non-albicans candida. Boric acid largely spares [[lactobacilli]] within the vagina. As [[TOL-463]], it is under development as an [[vaginal administration|intravaginal]] medication for the treatment of bacterial vaginosis and [[vulvovaginal candidiasis]]. As an [[antibacterial]] compound, boric acid can also be used as an [[acne]] treatment. It is also used as prevention of [[athlete's foot]], by inserting powder in the socks or stockings. Various preparations can be used to treat some kinds of {{lang|la|[[otitis externa]]}} (ear infection) in both humans and animals. The preservative in [[urine]] sample bottles in the UK is boric acid. Boric acid solutions used as an eye wash or on abraded skin are known to be toxic, particularly to infants, especially after repeated use; this is because of its slow elimination rate. Boric acid is one of the most commonly used substances that can counteract the harmful effects of reactive [[hydrofluoric acid]] (HF) after an accidental contact with the skin. It works by forcing the free {{chem2|F-}} anions into the inert [[tetrafluoroborate]] anion. This process defeats the extreme toxicity of hydrofluoric acid, particularly its ability to [[chelation|sequester]] [[Calcium in biology|ionic calcium]] from [[Serum (blood)|blood serum]] which can lead to [[cardiac arrest]] and bone decomposition; such an event can occur from just minor skin contact with HF. ===Insecticidal=== Boric acid was first registered in the US as an insecticide in 1948 for control of [[cockroach]]es, [[termite]]s, [[fire ant]]s, [[flea]]s, [[silverfish]], and many other [[insect]]s. The product is generally considered to be safe to use in household kitchens to control cockroaches and ants. It acts as a stomach poison affecting the insects' [[metabolism]], and the dry powder is [[abrasive]] to the insects' [[exoskeleton]]s. Boric acid also has the reputation as "the gift that keeps on killing" in that cockroaches that cross over lightly dusted areas do not die immediately, but that the effect is like shards of glass cutting them apart. This often allows a roach to go back to the nest where it soon dies. Cockroaches, being [[Cannibalism (zoology)|cannibalistic]], eat others killed by contact or consumption of boric acid, consuming the powder trapped in the dead roach and killing them, too.{{citation needed|date=July 2020}} ===Preservation=== In combination with its use as an insecticide, boric acid also prevents and destroys existing wet and dry rot in timbers. It can be used in combination with an [[ethylene glycol]] carrier to treat external wood against fungal and insect attack. It is possible to buy borate-impregnated rods for insertion into wood via drill holes where dampness and moisture is known to collect and sit. It is available in a gel form and injectable paste form for treating rot affected wood without the need to replace the timber. Concentrates of borate-based treatments can be used to prevent slime, mycelium, and algae growth, even in marine environments.{{cn|date=June 2022}} Boric acid is added to salt in the curing of cattle hides, [[calfskin]]s, and [[sheepskin]]s. This helps to control bacterial development, and helps to control insects.{{cn|date=June 2022}} ===pH buffer=== [[File:Borate pH.gif|thumb|alt=Distribution between boric acid and borate ion versus pH assuming p''K''{{sub|a}} = 9.0 (e.g. salt-water swimming pool)|Boric acid predominates in solution below pH 9]] [[File:Borate buffer.gif|thumb|alt=Buffer capacity of the boric acid - borate system versus pH assuming p''K''{{sub|a}} = 9.0 (e.g. salt-water swimming pool)|Boric acid buffers against rising pH in swimming pools]] Boric acid in equilibrium with its conjugate base the borate ion is widely used (in the concentration range 50 - 100 ppm boron equivalents) as a primary or adjunct pH buffer system in [[swimming pools]]. Boric acid is a weak acid, with p''K''{{sub|a}} (the pH at which buffering is strongest because the free acid and borate ion are in equal concentrations) of 9.24 in pure water at 25 °C. But apparent p''K''{{sub|a}} is substantially lower in swimming pool or ocean waters because of interactions with various other molecules in solution. It will be around 9.0 in a salt-water pool. No matter which form of soluble boron is added, within the acceptable range of pH and boron concentration for swimming pools, boric acid is the predominant form in aqueous solution, as shown in the accompanying figure. The boric acid - borate system can be useful as a primary buffer system (substituting for the [[bicarbonate]] system with p''K''{{sub|a{{sub|1}}}} = 6.0 and p''K''{{sub|a{{sub|2}}}} = 9.4 under typical salt-water pool conditions) in pools with salt-water chlorine generators that tend to show upward drift in pH from a working range of pH 7.5 - 8.2. [[Buffer capacity]] is greater against rising pH (towards the pKa around 9.0), as illustrated in the accompanying graph. The use of boric acid in this concentration range does not allow any reduction in free [[Hypochlorous acid|HOCl]] concentration needed for pool sanitation, but it may add marginally to the photo-protective effects of [[cyanuric acid]] and confer other benefits through anti-corrosive activity or perceived water softness, depending on overall pool solute composition. ===Lubrication=== Colloidal suspensions of nanoparticles of boric acid dissolved in petroleum or vegetable oil can form a remarkable lubricant on ceramic or metal surfaces with a coefficient of sliding friction that decreases with increasing pressure to a value ranging from 0.10 to 0.02. Self-lubricating {{chem2|B(OH)3}} films result from a spontaneous chemical reaction between water molecules and {{chem2|B2O3}} coatings in a humid environment. In bulk-scale, an inverse relationship exists between friction coefficient and Hertzian contact pressure induced by applied load.{{cn|date=June 2022}} Boric acid is used to lubricate [[carrom]] and [[novuss]] boards, allowing for faster play. ===Nuclear power=== Boric acid is used in some [[nuclear power plant]]s as a [[neutron poison]]. The boron in boric acid reduces the probability of [[nuclear fission|thermal fission]] by absorbing some [[thermal neutron]]s. [[Nuclear chain reaction|Fission chain reaction]]s are generally driven by the probability that free neutrons will result in fission and is determined by the material and geometric properties of the reactor. Natural boron consists of approximately 20% boron-10 and 80% boron-11 isotopes. Boron-10 has a high [[nuclear cross section|cross-section]] for absorption of low energy (thermal) neutrons. By increasing boric acid concentration in the reactor coolant, the probability that a neutron will cause fission is reduced. Changes in boric acid concentration can effectively regulate the rate of fission taking place in the reactor. Boric acid is used only in [[pressurized water reactor]]s (PWRs) whereas [[boiling water reactor]]s (BWRs) employ [[control rod]] pattern and coolant flow for power control. BWRs use an aqueous solution of boric acid and [[borax]] or sodium pentaborate for an emergency shut down system. Boric acid may be dissolved in [[spent fuel pool]]s used to store [[Spent nuclear fuel|spent fuel]] elements. The concentration is high enough to keep neutron multiplication at a minimum. Boric acid was dumped over Reactor 4 of the [[Chernobyl disaster|Chernobyl]] nuclear power plant after its [[nuclear meltdown|meltdown]] to prevent another reaction from occurring.{{citation needed|date=October 2013}} ===Pyrotechnics=== Boron is used in [[pyrotechnics]] to prevent the [[amide]]-forming reaction between [[aluminium]] and [[nitrate]]s. A small amount of boric acid is added to the composition to neutralize alkaline amides that can react with the aluminum. Boric acid can be used as a colorant to make fire green. For example, when dissolved in [[methanol]] it is popularly used by [[torch (juggling)|fire jugglers]] and fire spinners to create a deep green flame much stronger than copper sulfate. ===Agriculture=== Boric acid is used to treat or prevent [[Boron deficiency (plant disorder)|boron deficiencies]] in plants. It is also used in preservation of grains such as rice and wheat. ==References== [https://www.merriam-webster.com/dictionary/boracic%20acid Entry "boracic acid"] in the online ''Merriamm-Webster Dictionary''. Gives the first use as 1790. 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I. |last2= Adenin |first3= Y. M. |last3= Lubis }} {{cite book |last= Harvey |first= S. C. |editor1-last= Gilman |editor1-first= A. G. |editor1-link= Alfred G. Gilman |editor2-last= Goodman |editor2-first= L. S. |editor2-link= Louis S. Goodman |editor3-last= Gilman |editor3-first= A. |editor3-link= Alfred Gilman, Sr. |chapter= Antiseptics and Disinfectants; Fungicides; Ectoparasiticides |title= Goodman & Gillman's The Pharmacological Basis of Therapeutics |year= 1980 |edition= 6th |page= [https://archive.org/details/goodmangilmansphe6good/page/971 971] |isbn= 978-0-02-344720-4 |title-link= Goodman & Gillman's The Pharmacological Basis of Therapeutics }} {{cite web |url= http://www3.epa.gov/epawaste/hazard/testmethods/sw846/pdfs/3052.pdf |title= Method 3052 microwave assisted acid digestion of siliceous and organically based matrices |publisher= US EPA |date= 2015-06-22 }} {{Cite web | url=http://www.americanborate.com/all-about-borates/borate-applications/borates-in-pesticides/ | title=Borates in Pesticides | AMERICAN BORATE COMPANY}} {{Cite web |date=2012|authors=Boone, C.; Bond, C.; Stone, D.|title=Boric Acid General Fact Sheet|publisher=[[National Pesticide Information Center]], Oregon State University Extension Services|url=http://npic.orst.edu/factsheets/boricgen.html}} {{cite web |url=https://www3.epa.gov/pesticides/chem_search/reg_actions/reregistration/fs_PC-011001_1-Sep-93.pdf |title=R.E.D. Facts - Boric Acid |publisher=United States Environmental Protection Agency |access-date=2 April 2022 |archive-url=https://web.archive.org/web/20211223131332/https://www3.epa.gov/pesticides/chem_search/reg_actions/reregistration/fs_PC-011001_1-Sep-93.pdf |archive-date=23 December 2021 |url-status=live}} {{cite web |last= Birch |first= Robert G |title= Boric acid as a swimming pool buffer |publisher= The University of Queensland |date= 2013 |url= https://scithings.id.au/Boric_acid.pdf |access-date= 30 Nov 2013 }} {{cite journal |last1= Düzcükoğlu |first1=H. |last2=Acaroğlu |first2=M. |title= Lubrication Properties of Vegetable Oils Combined with Boric Acid and Determination of Their Effects on Wear |journal= Energy Sources, Part A: Recovery, Utilization, and Environmental Effects |volume= 32 |issue= 3 |year= 2009 |pages= 275–285 |doi= 10.1080/15567030802606053 |s2cid=97537085 }} {{cite web |url= http://pscamohali.googlepages.com/standardequipments |title= Standard equipments |publisher= Punjab State Carrom Association |access-date= 2009-09-24 |first= Harpreet |last=Singh}} {{Cite book|title=Pyrotechnics|last=Weingart|first=George|publisher=Chemical Publishing Company|year=1947|isbn=978-0820601120}} {{Cite web|url=https://www.cfs.gov.hk/english/programme/programme_rafs/programme_rafs_fa_02_06.html|title=Use of Boric Acid and Borax in Food|website=www.cfs.gov.hk|access-date=2019-05-22}} ==Further reading== * {{cite book | author = Jolly, W. L. | title = Modern Inorganic Chemistry | edition = 2nd | location = New York | publisher = McGraw-Hill | year = 1991 | isbn = 978-0-07-112651-9 }} * {{cite book |author1=Goodman, L. |author2=Gilman, A. |author3=Brunton, L. |author4=Lazo, J. |author5=Parker, K. | location = New York | publisher = McGraw Hill | year = 2006 | title = Goodman & Gilman's The Pharmacological Basis of Therapeutics }} * Cordia JA, Bal EA, Mak WA and Wils ERJ (2003), ''Determination of some physico-chemical properties of Optibor'' EP. Rijswijk, The Netherlands: TNO Prins Maurits Laboratory, report PML 2002-C42rr, GLP, Unpublished, confidential data provided by Bor ax Europe Limited ==External links== * {{commons category-inline|Boric acid}} * [http://npic.orst.edu/factsheets/borictech.pdf Boric Acid Technical Fact Sheet - National Pesticide Information Center] * [http://npic.orst.edu/factsheets/boricgen.pdf Boric Acid General Fact Sheet - National Pesticide Information Center] * [http://www.inchem.org/documents/icsc/icsc/eics0991.htm International Chemical Safety Card 0991] * [https://web.archive.org/web/20080406065032/http://www.epa.gov/oppsrrd1/REDs/factsheets/0024fact.pdf US EPA Pesticide Reregistration Eligibility Decision] * [https://web.archive.org/web/20060209040519/http://www.npi.gov.au/database/substance-info/profiles/15.html National Pollutant Inventory - Boron and compounds] * [https://web.archive.org/web/20021212234630/http://www.chemicalland21.com/arokorhi/industrialchem/inorganic/BORIC%20ACID.htm Boric acid at ChemicalLand21] * [https://web.archive.org/web/20100401084438/http://echa.europa.eu/doc/press/pr_10_03_svhc_consultation_20100308.pdf European Chemicals Agency (ECHA)"New Public Consultation on Eight Potential Substances of Very High Concern" - includes Boric Acid. Closes 22 April 2010] * [http://chemsub.online.fr/name/Boric_acid.html ChemSub Online: Boric acid] {{Boron compounds}} {{Hydrogen compounds}} {{Otologicals}} {{Insecticides}} {{Authority control}} {{DEFAULTSORT:Boric Acid}} [[Category:Antifungals]] [[Category:Antifungals for dermatologic use]] [[Category:Antiseptics]] [[Category:Ants]] [[Category:Borates]] [[Category:E-number additives]] [[Category:Inorganic compounds]] [[Category:Inorganic insecticides]] [[Category:Insecticides]] [[Category:Mineral acids]] [[Category:Neutron poisons]] [[Category:Otologicals]] [[Category:Photographic chemicals]] [[Category:Preservatives]] [[Category:Pyrotechnic chemicals]] [[Category:Rheology]] [[Category:Testicular toxicants]]