AP Chemistry
8.3 Weak Acid and Base Equilibria
A student prepares a \(0.20\text{ M}\) aqueous solution of a weak monoprotic acid, \(\text{HA}\), with an acid-dissociation constant \(K_a = 2.0 \times 10^{-5}\) at \(25\ ^\circ\text{C}\). The ionization reaction is represented by the equation below.
\[\text{HA(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{A}^-\text{(aq)}\]
What is the percent ionization of \(\text{HA}\) in this solution?
\[\text{HA(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{A}^-\text{(aq)}\]
What is the percent ionization of \(\text{HA}\) in this solution?
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