Boric acid: Difference between revisions
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Added sections: "Materials needed" and "Crafting instructions" |
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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 | 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: | It is also formed as a byproduct of hydrolysis of boron trihalides and diborane: | ||
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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