AP Chemistry
8.3 Weak Acid and Base Equilibria
A student prepares a \(0.020\text{ M}\) aqueous solution of acetic acid, \(\text{CH}_3\text{COOH(aq)}\), at \(25\ ^\circ\text{C}\). The acid ionization constant, \(K_a\), for \(\text{CH}_3\text{COOH}\) at this temperature is \(1.8 \times 10^{-5}\).
\[\text{CH}_3\text{COOH(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{CH}_3\text{COO}^-\text{(aq)}\]
Based on this information, what is the percent ionization of \(\text{CH}_3\text{COOH}\) in the solution?
\[\text{CH}_3\text{COOH(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{CH}_3\text{COO}^-\text{(aq)}\]
Based on this information, what is the percent ionization of \(\text{CH}_3\text{COOH}\) in the solution?
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