AP Chemistry
8.8 Properties of Buffers
8.3 Weak Acid and Base Equilibria
7.10 Reaction Quotient and Le Châtelier’s Principle
7.9 Introduction to Le Châtelier’s Principle
Multi-Unit
A student prepares a buffer solution by dissolving equimolar amounts of a weak acid, \(\text{HA}\), and its conjugate base, \(\text{NaA}\), in distilled water at \(25^\circ\text{C}\). The ionization of \(\text{HA(aq)}\) is represented by the equation below.
\[\text{HA(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{A}^-\text{(aq)} + \text{H}_3\text{O}^+\text{(aq)} \quad \Delta H^\circ > 0\]
The solution is subsequently heated from \(25^\circ\text{C}\) to \(50^\circ\text{C}\). Assuming the volume of the solution remains constant, which of the following correctly predicts the effect of this temperature increase on the acid-dissociation constant, \(K_a\), and the \(\text{pH}\) of the buffer solution?
\[\text{HA(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{A}^-\text{(aq)} + \text{H}_3\text{O}^+\text{(aq)} \quad \Delta H^\circ > 0\]
The solution is subsequently heated from \(25^\circ\text{C}\) to \(50^\circ\text{C}\). Assuming the volume of the solution remains constant, which of the following correctly predicts the effect of this temperature increase on the acid-dissociation constant, \(K_a\), and the \(\text{pH}\) of the buffer solution?
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