Boric Acid as a Weak Monobasic Acid - Is it Really?

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SUMMARY

Boric acid (H3BO3) is classified as a weak monobasic acid due to its behavior as a Lewis acid rather than a Brønsted acid. It does not dissociate in aqueous solution but interacts with water to form the tetrahydroxyborate ion (B(OH)4−) and releases a proton (H+). This interaction is supported by Raman spectroscopy evidence. Despite some sources listing three dissociation constants for boric acid, indicating potential reactions with additional water molecules, its primary classification remains as a weak monobasic acid.

PREREQUISITES
  • Understanding of Lewis and Brønsted acid-base theories
  • Familiarity with aqueous solution chemistry
  • Knowledge of dissociation constants and their significance
  • Basic principles of spectroscopy, particularly Raman spectroscopy
NEXT STEPS
  • Research the Lewis acid concept in greater detail
  • Explore the implications of dissociation constants in weak acids
  • Study the role of Raman spectroscopy in chemical analysis
  • Investigate the properties and applications of tetrahydroxyborate ions
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Chemistry students, researchers in acid-base chemistry, and professionals involved in chemical analysis and spectroscopy will benefit from this discussion.

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how can boric acid be a weak monobasic acid?i thought it was tribasic.
 
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According to Wikipedia:
Boric acid does not dissociate in aqueous solution as a Brønsted acid, but is a Lewis acid which interacts with water molecules to form the tetrahydroxyborate ion, as confirmed by Raman spectroscopy:

B(OH)3 + H2O <--> B(OH)4− + H+

https://en.wikipedia.org/wiki/Boric_acid
 
To make things more complicated many sources list three dissociation constants for H3BO3 (which can mean it is able to react with another two water molecules in the same manner).
 

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