AP Chemistry
8.3 Weak Acid and Base Equilibria
A student prepares an aqueous solution of a weak monoprotic acid, \(\text{HA}\), by dissolving \(0.010 \text{ mol}\) of pure \(\text{HA(s)}\) in distilled water to give a total volume of \(250 \text{ mL}\). The acid dissociation constant, \(K_a\), for \(\text{HA}\) is \(6.4 \times 10^{-5}\) at \(25^\circ\text{C}\). What is the percent ionization of \(\text{HA}\) in this solution?
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