AP Chemistry
8.3 Weak Acid and Base Equilibria
Formic acid, \(\text{HCOOH}\), ionizes in water according to the equation below.
\[ \text{HCOOH(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{HCOO}^-\text{(aq)} + \text{H}_3\text{O}^+\text{(aq)} \]
A student prepares a \(0.20\text{ M}\) aqueous solution of \(\text{HCOOH}\) at \(25\ ^\circ\text{C}\). Given that \(K_a = 1.8 \times 10^{-4}\) for \(\text{HCOOH}\) at this temperature, what is the equilibrium concentration of \(\text{H}_3\text{O}^+\text{(aq)}\) in the solution?
\[ \text{HCOOH(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{HCOO}^-\text{(aq)} + \text{H}_3\text{O}^+\text{(aq)} \]
A student prepares a \(0.20\text{ M}\) aqueous solution of \(\text{HCOOH}\) at \(25\ ^\circ\text{C}\). Given that \(K_a = 1.8 \times 10^{-4}\) for \(\text{HCOOH}\) at this temperature, what is the equilibrium concentration of \(\text{H}_3\text{O}^+\text{(aq)}\) in the solution?
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