Question

Calculate the pH of each of the following solutions. 0.40 M NH4ClO40.40\ M\ \mathrm { NH } _ { 4 } \mathrm { ClO } _ { 4 }

Solution

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NH4_4ClO4_4 solution has weak acidic\text{\textcolor{#c34632}{acidic}} properties since it is formed by a strong\textbf{strong} acid (HClO4_4) and and a weak\textbf{weak} base (NH3_3).

The major species\textbf{major species} present in the solution are NH4+_4^+, ClO4_4^-, H2_2O.

Since HClO4_4 is a strong\textbf{strong} acid, its conjugate base does not affect the pH of the solution.

Since NH3_3 is a weak\textbf{weak} base, its conjugate acid NH4+_4^+ will dissociate and contribute to the [H+^+].

Therefore, we must focus on the following reaction:

NH4  (aq)+NH3  (aq)+H(aq)+\text{NH}_{4\;(aq)}^+ \Leftrightarrow \text{NH}_{3\;(aq)} + \text{H}_{(aq)}^+

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