Boric acid: Difference between revisions
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'''Boric acid''' is a [[Chemical compounds|chemical compound]] of [[boron]], [[oxygen]], and [[hydrogen]] with formula B(OH)<sub>3</sub>. 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 acid that yields various borate anions and salts, and can react with alcohols to form borate esters. | '''Boric acid''' is a [[Chemical compounds|chemical compound]] of [[boron]], [[oxygen]], and [[hydrogen]] with formula B(OH)<sub>3</sub>. 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 acid that yields various borate anions and salts, and can react with alcohols to form borate esters. | ||
== Materials needed == | |||
* '''Borax''' (sodium tetraborate decahydrate) | |||
* '''Mineral acid''' such as [[hydrochloric acid]] | |||
== Crafting instructions == | |||
The reaction of Borax with HCl is as follows: | |||
Na<sub>2</sub>B<sub>4</sub>O<sub>7</sub>·10H<sub>2</sub>O + 2 HCl → 4 B(OH)<sub>3</sub> + 2 NaCl + 5 H<sub>2</sub>O | |||
It is also formed as a byproduct of hydrolysis of boron trihalides and diborane: | |||
: B<sub>2</sub>H<sub>6</sub> + 6 H<sub>2</sub>O → 2 B(OH)<sub>3</sub> + 6 H<sub>2</sub> | |||
: BX<sub>3</sub> + 3 H<sub>2</sub>O → B(OH)<sub>3</sub> + 3 HX (X = Cl, Br, I) | |||
== Uses == | == Uses == | ||
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* [[Oxygen]] | * [[Oxygen]] | ||
** [[Boric acid]] | ** [[Boric acid]] | ||
== See also == | |||
<div style="column-count:2"> | |||
* [[Ammonia]] | |||
* [[Carbon dioxide]] | |||
* [[Cyanide]] | |||
* [[Ethanol]] | |||
* [[Methane]] | |||
* [[Nitric acid]] | |||
* [[Nitroglycerin]] | |||
* [[Saltpeter]] | |||
* [[Sulfuric acid]] | |||
* [[Water]] | |||
* [[Chemical compounds]] | |||
</div> | |||
== References == | == References == | ||
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[[Category:Acids]] | [[Category:Acids]] | ||
[[Category:Stubs]] | |||
Latest revision as of 02:46, 6 May 2025
Boric acid is a chemical compound of boron, oxygen, and hydrogen with formula B(OH)3. 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 acid that yields various borate anions and salts, and can react with alcohols to form borate esters.
Materials needed
- Borax (sodium tetraborate decahydrate)
- Mineral acid such as hydrochloric acid
Crafting instructions
The reaction of Borax with HCl is as follows:
Na2B4O7·10H2O + 2 HCl → 4 B(OH)3 + 2 NaCl + 5 H2O
It is also formed as a byproduct of hydrolysis of boron trihalides and diborane:
- B2H6 + 6 H2O → 2 B(OH)3 + 6 H2
- BX3 + 3 H2O → B(OH)3 + 3 HX (X = Cl, Br, I)
Uses
Boric acid is often used as an antiseptic, insecticide, flame retardant, neutron absorber, or precursor to other boron compounds.
Dependencies
See also
References
| This article uses material from the Wikipedia article Boric_acid, which is released under the Creative Commons Attribution-ShareAlike 3.0 Unported License (view authors). | 
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