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When a aqueous solution of a certain acid is prepared, the acid is dissociated. Calculate the acid dissociation constant of the acid. Round your answer to significant digits.

Respuesta :

[tex]K_a[/tex] = [tex]\dfrac{[H^{+}] [A^{-}]}{[HA]}[/tex]

Explanation:

  • When an aqueous solution of a certain acid is prepared it is dissociated is as follows-

        [tex]{\displaystyle {\ce {HA[/tex]  ⇄  [tex]{H^+}+{A^{-}}} }}[/tex]

Here HA is a protonic acid such as acetic acid, [tex]CH_3COOH[/tex]

  • The double arrow signifies that it is an equilibrium process, which means the dissociation and recombination of the acid occur simultaneously.
  • The acid dissociation constant can be given by -

        [tex]K_a[/tex] = [tex]\dfrac{[H^{+}] [A^{-}]}{[HA]}[/tex]

  • The reaction is can also be represented by Bronsted and lowry -

         [tex]\\{\displaystyle {\ce {{HA}+ H_2O}[/tex] ⇄  [tex][H_3O^+] [A^-][/tex]

  • Then the dissociation constant will be

        [tex]K_a[/tex] = [tex]\dfrac{[H_3O^{+}] [A^{-}]}{[HA]}[/tex]

Here, [tex]K_a[/tex] is the dissociation constant of an acid.

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