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Boric acid

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Boric acid

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Boric acid
Boric acid Boric acid
General
Other names Orthoboric acid,
Boracic acid,
Sassolite,
Optibor®,
Borofax®
Molecular formula H3BO3
Molar mass 61.832 g/mol
Appearance White crystalline liquid
CAS number [10043-35-3]
Properties
Density and phase 1.435 g/cm³, solid.
Solubility in water 5.7 g/100 ml (25°C)
Melting point 169°C decomp.
Acidity (pKa) 9.24 (see text)
Structure
Molecular shape Planar
Dipole moment Zero
Thermodynamic data
Standard enthalpy
of formation ΔfHosolid
−1093.99 kJ/mol
Standard molar entropy
Sosolid
88.7 J.K−1.mol−1
Hazards
MSDS External MSDS
EU classification N/A
NFPA 704
1
0
0
 
Flash point Non-flammable.
Related compounds
Related compounds Boron trioxide
Borax
Except where noted otherwise, data are given for
materials in their standard state (at 25°C, 100 kPa)

Boric acid, also called boracic acid or orthoboric acid, is a mild acid often used as an antiseptic, insecticide, flame retardant, in nuclear power plants to control the fission rate of uranium, and as a precursor of other chemical compounds. It exists in the form of colorless crystals or a white powder and dissolves in water. It has the chemical formula H3BO3, sometimes written B(OH)3. When occurring as a mineral, it is called sassolite.

Contents

Preparation

Boric acid is produced mainly from borate minerals by the reaction with sulfuric acid. The largest source of borates in the world is an open-pit mine in Death Valley, California, USA.

Properties

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. The presence of boric acid or its salts has been noted in sea-water, whilst it is also said to exist in plants and especially in almost all fruits (A. H. Allen, Analyst, 1904, 301). The free acid is found native in certain volcanic districts such as Tuscany, the Lipari Islands and Nevada, issuing mixed with steam from fissures in the ground; it is also found as a constituent of many minerals (borax, boracite, boronatrocaicite and colemanite).Boric acid is soluble in boiling water. When heated above 170°C it dehydrates, forming metaboric acid HBO2. Metaboric acid is a white, cubic crystalline solid and is only slightly soluble in water. It melts at about 236°C, and when heated above about 300°C further dehydrates, forming tetraboric acid or pyroboric acid, H2B4O7. Boric acid can refer to any of these compounds. Further heating leads to boron trioxide.

Boric acid does not dissociate in aqueous solution, but is acidic due to its interaction with water molecules:

B(OH)3 + H2O ⇌ B(OH)4 + H+
Ka = 5.8x10−10 L/mol; pKa = 9.24.

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:

4B(OH)4 + 2H+ ⇌ B4O72− + 9H2O

Uses

It can be used as an antiseptic for minor burns or cuts and is sometimes used in dressings or salves or is applied in a very dilute solution as an eye wash. It is poisonous if taken internally or inhaled, although it is generally not considered to be much more toxic than table salt (based on its mammal LD50 rating of 2660mg/kg body mass). (Toxicity ref: http://www.natbat.com/docs/boron.htm)

Boric acid can be used to treat yeast and fungal infections such as candidiasis (vaginal yeast infections) by filling gelcaps with boric acid powder and inserting two into the vaginal canal at bedtime for three to four nights in a row. It is also used as prevention of athlete's foot, by inserting powder in the socks or stockings, and in solution can be used to treat some kinds of otitis externa (ear infection) in both humans and animals. The preservative in urine sample bottles (red cap) in the UK is Boric acid.

It is often used as a relatively nontoxic insecticide, for killing cockroaches, termites, fire ants, fleas, and many other insects. It can be used directly in powdered form for fleas and cockroaches, or mixed with sugar or grape jelly for ants. It is also a component of many commercial insecticides. In this use, especially in the case of cockroaches, the boric acid in the form of a powder is applied to areas frequented by the insects. The lightweight particles cling to the legs of the insects and eventually cause fatal chemical burns. Boric acid for this use in residential apartments is sold commercially in urban areas afflicted with cockroaches. (Insect control ref: http://alsnetbiz.com/homeimprovement/boric_acid.html)

Boric acid is used in nuclear power plants to slow down the rate at which fission is occurring. Fission chain reactions are generally driven by the amount of neutrons present (as products from previous fissions). Boron has a high cross-section for absorption of neutrons and is therefore dissolved into the primary coolant which circulates through the reactor. By changing the concentration of boric acid in the water, fission can be regulated. Boron is also dissolved into the spent fuel pools containing used uranium rods. The concentration is high enough to keep fissions at a minimum.

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.

Borates including boric acid have been used since the time of the Greeks for cleaning, preserving food, and other activities.

Lithium boric acid is the lithium salt of boric acid and is used in the laboratory as buffer for gel. TBE buffer is widely used for the electrophoresis of nucleic acids and has a higher buffer capacity than a TAE Buffer. It can be used for DNA and RNA polyacrylamide and agarose gel electrophoresis.

It 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.

It is also used in India and across the world to dust down Carrom Boards to decrease friction and increase speed of play.

References

  • Jolly, W. L. (1991). Modern Inorganic Chemistry (2nd Edn.). New York: McGraw-Hill. ISBN 0-07-112651-1.

External links


Home | Up | Iodine | Alcohol | Boric acid | Calcium hypochlorite | Hydrogen peroxide | Listerine | Naphthalene | Natron | Phenol | Salicylic acid | Silver nitrate | Sodium chloride | Sodium hypochlorite

Drugs & Medication, made by MultiMedia | Free content and software

This guide is licensed under the GNU Free Documentation License. It uses material from the Wikipedia.


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