Question

Write the formula for the conjugate acid of each of the following bases. 1. NH₃

Answer 1

Answer:

According to Bronsted-Lowry theory, an acid is any species that can donate H+ (proton), while a base is any species that can accept a H+ ion.

1. $NH_{3}$  

                          $NH_{3}$(aq) + $H_{2}O$(aq) → $NH_{4}^{+}$(aq)+ $OH^{-}$(aq)

$NH_{4}^{+}$ is the conjugate acid of $NH_{3}$

      2. $ClO_{3}^{-}$

                           $ClO_{3}^{-}$(aq) + $H_{2}O$(aq) → $HClO_{3}$(aq) + $OH^{-}$(aq)

$HClO_{3}$ is the conjugate acid of $ClO_{3}^{-}$

       3. $SO_{4}^{2-}$

                             $SO_{4}^{2-}$(aq) + $H_{2}O$(aq) → $HSO_{4}^{-}$(aq) + $OH^{-}$(aq)

$HSO_{4}^{-}$ is the conjugate acid of  $SO_{4}^{2-}$  

         4. $OH^{-}$

                              $OH^{-}$(aq) + $H^{+}$(aq) → $H_{2}O$(aq)

$H_{2}O$ is the conjugate acid of $OH^{-}$