Boric acid

"Boric" redirects here. For other uses, see Boric (disambiguation).
Boric acid
Names
IUPAC names
Boric acid
Trihydrooxidoboron
Other names
Orthoboric acid,
Boracic acid,
Sassolite,
Optibor,
Borofax,
Trihydroxyborane
Identifiers
ATC code S02AA03
D08AD
10043-35-3 Yes
ChEBI CHEBI:33118 Yes
ChEMBL ChEMBL42403 Yes
ChemSpider 7346 Yes
EC number 233-139-2
Jmol-3D images Image
Image
KEGG D01089 Yes
PubChem 7628
UNII R57ZHV85D4 Yes
Properties
Molecular formula
 H3BO3
Molar mass 61.83 g·mol−1
Appearance White crystalline solid
Density 1.435 g/cm3
Melting point 170.9 °C (339.6 °F; 444.0 K)
Boiling point 300 °C (572 °F; 573 K)
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)
Solubility in other solvents Soluble in lower alcohols
moderately soluble in pyridine
very slightly soluble in acetone
Acidity (pKa) 9.24, 12.4, 13.3
Structure
Molecular shape Trigonal planar
Dipole moment Zero
Hazards
MSDS External MSDS
EU classification Harmful (Xn)
Repr. Cat. 2
R-phrases R60 R61
S-phrases S53 S45
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
2
0
Flash point Non-flammable
2660 mg/kg, oral (rat)
Related compounds
Related compounds
 Boron trioxide
Borax
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 Yes verify (what is: Yes/?)
Infobox references

Boric acid, also called hydrogen borate, boracic acid, orthoboric acid and acidum boricum, is a weak, monobasic Lewis acid of boron often used as an antiseptic, insecticide, flame retardant, neutron absorber, or precursor to other chemical compounds. It has the chemical formula H3BO3 (sometimes written B(OH)3), and exists in the form of colorless crystals or a white powder that dissolves in water. When occurring as a mineral, it is called sassolite.

Occurrence

Boric acid, or sassolite, is found natively in its free state in some volcanic districts, for example, in the Italian region of Tuscany, the Lipari Islands and the US state of Nevada. In these volcanic settings it issues, mixed with steam, from fissures in the ground. It is also found as a constituent of many naturally occurring minerals – borax, boracite, boronatrocaicite and colemanite. Boric acid and its salts are found in seawater. It is also found in plants, including almost all fruits.[1]

Boric acid was first prepared by Wilhelm Homberg (1652–1715) from borax, by the action of mineral acids, and was given the name sal sedativum Hombergi ("sedative salt of Homberg"). However borates, including boric acid, have been used since the time of the Greeks 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:

Na2B4O7·10H2O + 2 HCl → 4 B(OH)3 [or H3BO3] + 2 NaCl + 5 H2O

It is also formed as a by product of hydrolysis of boron trihalides and diborane:[2]

B2H6 + 6 H2O → 2 B(OH)3 + 6 H2
BX3 + 3 H2O → B(OH)3 + 3 HX (X = Cl, Br, I)

Properties

Boric acid is soluble in boiling water. When heated above 170 °C, it dehydrates, forming metaboric acid (HBO2):

H3BO3 → HBO2 + H2O

Metaboric acid is a white, cubic crystalline solid and is only slightly soluble in water. Metaboric acid melts at about 236 °C, and when heated above about 300 °C further dehydrates, forming tetraboric acid or pyroboric acid (H2B4O7):

4 HBO2 → H2B4O7 + H2O

The term boric acid may sometimes refer to any of these compounds. Further heating leads to boron trioxide.

H2B4O7 → 2 B2O3 + H2O

There are conflicting interpretations for the origin of the acidity of aqueous boric acid solutions. Raman spectroscopy of strongly alkaline solutions has shown the presence of B(OH)−
4 ion,[3] leading some to conclude that the acidity is exclusively due to the abstraction of OH− from water:[3][4][5][6]

B(OH)3 + H2O is in a disfavored equilibrium with B(OH)−
4 + H+ (K = 7.3x10−10; pK = 9.14)

or more properly expressed in the aqueous solution:

B(OH)3 + 2 H2O is in a disfavored equilibrium with B(OH)−
4 + H3O+

This may be characterized[4][5][6] as Lewis acidity of boron toward OH−, rather than as Brønsted acidity.

However other sources[7] say that boric acid is also a tribasic Brønsted acid, with successive ionization steps:

B(OH)3 is in a disfavored equilibrium with BO(OH)−
2 + H+ (Ka1 = 5.8x10−10; pKa1 = 9.24)
BO(OH)−
2 is in a disfavored equilibrium with BO2(OH)2− + H+ (Ka2 = 4x10−13; pKa2 = 12.4)
BO2(OH)2− is in a disfavored equilibrium with BO3−
3 + H+ (Ka3 = 4x10−14; pKa3 = 13.3)

Since the value of Ka1 is comparable to that of the reaction with OH−, the concentrations of BO(OH)−
2 and B(OH)−
4 are similar.[7]

Polyborate anions are formed at pH 7–10 if the boron concentration is higher than about 0.025 mol/L. The best known of these is the tetraborate ion, found in the mineral borax:

4[B(OH)4]− + 2H+ is in equilibrium with [B4O5(OH)4]2− + 7H2O

Boric acid makes an important contribution to the absorption of low frequency sound in seawater.[8]

Reactions

With polyhydric alcohols such as glycerol and mannitol the acidity of is increased. With mannitol for example the pK decreases to 5.15. This is due to the formation of a chelate, [((OH)4C6H8O2)2B]−, and this feature is used in analytical chemistry.[9]

Boric acid dissolves in anhydrous sulfuric acid and acts a strong acid:[9]

B(OH)3 + 6H2SO4 → 3H3O+ + 2HSO4− + B(HSO4)4−

Boric acid reacts with alcohols to form borate esters, B(OR)3 where R is alkyl or aryl. A dehydrating agent, such as concentrated sulfuric acid is typically added:[10]

B(OH)3 + 3 ROH → B(OR)3 +3 H2O

Crystal structure

Crystalline boric acid consists of layers of B(OH)3 molecules held together by hydrogen bonds. The B-O bond length is 136 pm and the O-H is 97 pm with a hydrogen bond of 272pm. The distance between two adjacent layers is 318 pm.[9]

The unit cell of boric acid
hydrogen bonding (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 poisonous if taken internally or inhaled in large quantities. The Thirteenth 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 comparison's sake, the LD50 of salt is reported to be 3.75 g/kg in rats according to the Merck Index. But this is highly misleading, as humans have been known to die from amounts only a small fraction of the LD50. "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", according to the Agency for Toxic Substances and Disease Registry.[11]

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 is far lower than the LD50.[12]

According to boric acid IUCLID Dataset published by the European Commission, boric acid in high doses shows significant developmental toxicity and teratogenicity in rabbit, rat, and mouse fetuses as well as cardiovascular defects, skeletal variations, mild kidney lesions.[13] As a consequence, in August 2008, in the 30th ATP to EU directive 67/548/EEC, the EC decided to amend its classification as reprotoxic category 2 and to apply the risk phrases R60 (may impair fertility) and R61 (may cause harm to the unborn child).[14][15][16][17][18]

At a recent 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. The registration and review completed as part of REACH has meant the current classification of Boric Acid CAS 10043-35-3 / 11113-50-1 as of 1 December 2010 will be listed as H360FD (May damage fertility. May damage the unborn child.)[19][20]

Uses

Medical

Boric acid can be used as an antiseptic for minor burns or cuts and is sometimes used in dressings or salves. 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,[21] as well as candidiasis due to non-albicans candida.[22] 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, and in alcohol solution can be used to treat some kinds of 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.[23]

Insecticidal

Boric acid was first registered in the US as an insecticide in 1948 for control of cockroaches, termites, fire ants, fleas, silverfish, and many other insects. The product is generally considered to be safe to use in household kitchens to control cockroaches and ants.[24] It acts as a stomach poison affecting the insects' metabolism, and the dry powder is abrasive to the insects' exoskeletons.

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.

Boric acid is added to salt in the curing of cattle hides, calfskins, and sheepskins. This helps to control bacteria development, and helps to control insects.

pH buffer

Distribution between boric acid and borate ion versus pH assuming pKa = 9.0 (e.g. salt-water swimming pool)
Boric acid predominates in solution below pH 9
Buffer capacity of the boric acid - borate system versus pH assuming pKa = 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 pKa (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 pKa 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 pKa1 = 6.0 and pKa2 = 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 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.[25]

Lubrication

Colloidal suspensions of nanoparticles of boric acid dissolved in petroleum or vegetable oil can form a remarkable lubricant on ceramic or metal surfaces[26] with a coefficient of sliding friction that decreases with increasing pressure to a value ranging from 0.10 to 0.02. Self-lubricating H3BO3 films result from a spontaneous chemical reaction between water molecules and B2O3 coatings in a humid environment. In bulk-scale, an inverse relationship exists between friction coefficient and Hertzian contact pressure induced by applied load.

Boric acid is used to lubricate carrom and novuss boards, allowing for faster play.[27]

Nuclear power

Boric acid is used in some nuclear power plants as a neutron poison. The boron in boric acid reduces the probability of thermal fission by absorbing some thermal neutrons. Fission chain reactions 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 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 reactors (PWRs) (boiling water reactors (BWRs) use Sodium Pentaborate for the same purpose). Boric acid may be dissolved in spent fuel pools used to store 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 Nuclear Power Plant after its meltdown to prevent another reaction from occurring.

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.[28]

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 and soldering operations.

Boric acid is used in the production of the glass in LCD flat panel displays.

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 H
3BO
3 to NiSO
4, a very small portion of sodium lauryl sulfate and a small portion of H
2SO
4.

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.[29] The solution is used for fire retarding agent of wood by impregnation.[30]

It is also used in the manufacturing of ramming mass, a fine silica-containing powder used for producing induction furnace linings and ceramics.

Boric acid is one of the most commonly used substances that can neutralize active hydrofluoric acid (HF). It works by forcing the free F− anions into complex salts. This process defeats the extreme toxicity of hydrofluoric acid, particularly its ability to sequester ionic calcium from blood serum which can lead to cardiac arrest and bone decomposition; such an event can occur from just minor skin contact with HF.[31]

Boric acid is added to borax for use as welding flux by blacksmiths.[32]

Boric acid, in combination with silicone oil, is used to manufacture Silly Putty.[33]

Boric acid, may be used in Marcellus Shale hydraulic fracturing, in the state of Pennsylvania.[34]

Pyrotechnics

Boron is used in pyrotechnics to prevent the amide-forming reaction between aluminum and nitrates. 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 fire jugglers and fire spinners to create a deep green flame.

References

  1. ↑ Allen, A. H.; Tankard, A. R. (1904). "The Determination of Boric Acid in Cider, Fruits, etc.". Analyst 29 (October): 301–304. doi:10.1039/an9042900301.
  2. ↑ Housecroft, C. E.; Sharpe, A. G. (2008). "Chapter 13: The Group 13 Elements". Inorganic Chemistry (3rd ed.). Pearson. p. 340. ISBN 978-0-13-175553-6.
  3. ↑ 3.0 3.1 Jolly, W. L. (1984). Modern Inorganic Chemistry. McGraw-Hill. p. 198.
  4. ↑ 4.0 4.1 Housecroft, C.E.; Sharpe, A.G. (2005). Inorganic Chemistry (2nd ed.). Pearson Prentice-Hall. pp. 314–5.
  5. ↑ 5.0 5.1 Comprehensive Chemistry for JEE Advanced 2014, p15.5
  6. ↑ 6.0 6.1 Competition Science Vision
  7. ↑ 7.0 7.1 Perelygin, Yu. P.; Chistyakov, D. Yu. (2006). "Boric acid" (PDF). Russian Journal of Applied Chemistry (Pleiades Publishing) 79 (12): 2041–2042. doi:10.1134/S1070427206120305. ISSN 1070-4272. Retrieved 29 August 2013.
  8. ↑ "Underlying Physics and Mechanisms for the Absorption of Sound in Seawater". National Physical Laboratory. Retrieved 2008-04-21.
  9. ↑ 9.0 9.1 9.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
  10. ↑ Brown, Herbert C.; Mead, Edward J.; Shoaf, Charles J. (1956). "Convenient Procedures for the Preparation of Alkyl Borate Esters". J. Am. Chem. Soc 78 (15): 3613–3614. doi:10.1021/ja01596a015.
  11. ↑ HHS, Public Health Service, Agency for Toxic Substances and Disease Registry (November 2010), Toxicological Profile for Boron (PDF), p. 11
  12. ↑ Office of Prevention, Pesticides and Toxic Substances (2006). "Report of the Food Quality Protection Act (FQPA) Tolerance Reassessment Eligibility Decision (TRED) for Boric Acid/Sodium Borate Salts" (PDF). United States Environmental Protection Agency. Retrieved 2008-04-21.
  13. ↑ ECB. "Boric Acid IUCLID Dataset" (PDF). European Commission.
  14. ↑ "Boric acid, ACC# 03260 MSDS" (PDF). 11 February 2008. Retrieved 2009-09-24.
  15. ↑ Ishii, Y.; Fujizuka, N.; Takahashi, T. et al. (1993). "A Fatal Case of Acute Boric Acid Poisoning". Clinical Toxicology 31 (2): 345–352. doi:10.3109/15563659309000402. PMID 8492348.
  16. ↑ = Restuccio, A.; Mortensen, M. E.; Kelley, M. T. (1992). "Fatal Ingestion of Boric Acid in an Adult". American Journal of Emergency Medicine 10 (6): 545–547. doi:10.1016/0735-6757(92)90180-6. PMID 1388380.
  17. ↑ Duldner, J. E. (30 January 2009). "Boric Acid Poisoning". A.D.A.M. Medical Encyclopedia. MedLine Plus.
  18. ↑ NSW Food Authority. "Borax and Boric Acid". Australia: New South Wales Government. Retrieved 2009-09-24.
  19. ↑ "Document library - ECHA" (PDF). Echa.europa.eu. Retrieved 2013-05-26.
  20. ↑ http://www.deti.ie/employment/chemicalspolicy/clpregulation1272.pdf
  21. ↑ Abercrombie, P. (2010). "Vaginitis". In Maizes, V.; Low Dog, T. Integrative Women's Health. New York, NY: Oxford University Press. p. 192. ISBN 978-0-19-537881-8.
  22. ↑ Iavazzo C, Gkegkes ID, Zarkada IM, Falagas ME (August 2011). "Boric acid for recurrent vulvovaginal candidiasis: the clinical evidence". J Womens Health (Larchmt) 20 (8): 1245–55. doi:10.1089/jwh.2010.2708. PMID 21774671.
  23. ↑ Harvey, S. C. (1980). "Antiseptics and Disinfectants; Fungicides; Ectoparasiticides". In Gilman, A. G.; Goodman, L. S.; Gilman, A. Goodman & Gillman's The Pharmacological Basis of Therapeutics (6th ed.). p. 971. ISBN 978-0-02-344720-4.
  24. ↑ Office of Prevention, Pesticides and Toxic Substances (1993). "R.E.D. Facts: Boric Acid" (PDF). United States Environmental Protection Agency. Retrieved 2008-04-21.
  25. ↑ Birch, Robert G (2013). "Boric acid as a swimming pool buffer" (PDF). The University of Queensland. Retrieved 30 Nov 2013.
  26. ↑ Düzcükoğlu, H.; Acaroğlu, M. (2009). "Lubrication Properties of Vegetable Oils Combined with Boric Acid and Determination of Their Effects on Wear". Energy Sources, Part A: Recovery, Utilization, and Environmental Effects 32 (3): 275–285. doi:10.1080/15567030802606053.
  27. ↑ Singh, Harpreet. "Standard equipments". Punjab State Carrom Association. Retrieved 2009-09-24.
  28. ↑ Kistler, R. B.; Helvaci, C. (1994). "Boron and Borates". In Carr, D. D. Industrial Minerals and Rocks (6th ed.). Littleton, CO: SME. pp. 171–186.
  29. ↑ Tsuyumoto, I.; Oshio, T.; Katayama, K. (2007). "Preparation of Highly Concentrated Aqueous Solution of Sodium Borate". Inorganic Chemistry Communications 10 (1): 20–22. doi:10.1016/j.inoche.2006.08.019.
  30. ↑ Tsuyumoto, I.; Oshio, T. (2009). "Development of Fire Resistant Laminated Wood Using Concentrated Sodium Polyborate Aqueous Solution". Journal of Wood Chemistry and Technology 29 (4): 277–285. doi:10.1080/02773810903033721.
  31. ↑ "Method 3052 microwave assisted acid digestion of siliceous and organically based matrices" (PDF). US EPA.
  32. ↑ Dempsey, Jock (2009) [1998]. "BORAX". Dempsey's Forge. Retrieved 2010-07-23.
  33. ↑ Prager, Felice. "Science Becomes a Toy - Silly Putty". Loti.com. Rewind the Fifites. Retrieved 2013-06-07.
  34. ↑ "Chemicals Used by Hydraulic Fracturing Companies in Pennsylvania for Surface and Hydraulic Fracturing Activities" (PDF). Pennsylvania Department of Environmental Protection, Bureau of Oil and Gas Management. 30 June 2010.

Further reading

External links