AP Chemistry
8.3 Weak Acid and Base Equilibria
A student prepares a solution of acetic acid, \(\text{CH}_3\text{COOH(aq)}\), by dissolving enough acid in water to create a \(0.18 \text{ M}\) solution at \(25^\circ\text{C}\). Given that the acid dissociation constant for acetic acid is \(K_a = 1.8 \times 10^{-5}\) at \(25^\circ\text{C}\), what is the percent ionization of acetic acid in this solution?
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