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Classify each reactant and product in this reaction as an acid or base according to the Brønsted theory.
HF + H2O = F + H30+


Answer Bank
HF
H30+
F-
H2O

Respuesta :

jacob193

Answer:

Reaction: [tex]\rm HF + H_2O \rightleftharpoons F^{-} + H_3O^{+}[/tex].

  • [tex]\rm HF[/tex]: Bronsted-Lowry Acid.
  • [tex]\rm H_3O^{+}[/tex]: Bronsted-Lowry conjugate Acid of
  • [tex]\rm F^{-}[/tex]: Bronsted-Lowry conjugate Base of [tex]\rm HF[/tex].
  • [tex]\rm H_2O[/tex]: Bronsted-Lowry Base.

Explanation:

In the Bronsted-Lowry acid-base theory, the acid in a reaction is the species that loses a proton, [tex]\rm H^{+}[/tex]. The resultant species would be the conjugate base of that acid.

On the other hand, the Bronsted-Lowry base in a reaction is the species that accepts a proton [tex]\rm H^{+}[/tex]. The resultant species would be the conjugate acid of that base.

Identify the conjugate acid-base pairs in this reaction. Note that the two species in each pair are related by the gain or loss of a single proton. Therefore, their formula should look similar to each other.

For this reaction, [tex]\rm HF[/tex] and [tex]\rm F^{-}[/tex], as well as [tex]\rm H_2O[/tex] and [tex]\rm H_3O^{+}[/tex] form two similar-looking reactant-product pairs:

  • The reactant [tex]\rm HF[/tex] loses one proton to form the product [tex]\rm F^{-}[/tex]. Therefore, [tex]\rm HF\![/tex] would be the Bronsted-Lowry acid, while [tex]\rm F^{-}\![/tex] would be its conjugate base.
  • The reactant [tex]\rm H_2O[/tex] gains one proton to form the product [tex]\rm H_3O^{+}[/tex]. Therefore, [tex]\rm H_2O\![/tex] would be the Bronsted-Lowry base, while [tex]\rm H_3O^{+}\![/tex] would be the conjugate acid.