AP Chemistry
4.8 Introduction to Acid-Base Reactions
A student combines a phosphate-buffered water sample with a bicarbonate-containing water sample in a sealed flask. The following proton-transfer equilibrium is considered.
\[ \text{H}_2\text{PO}_4^-\text{(aq)}+\text{HCO}_3^-\text{(aq)}\rightleftharpoons \text{HPO}_4^{2-}\text{(aq)}+\text{H}_2\text{CO}_3\text{(aq)} \]
Independent measurements at the same temperature establish that \(\text{H}_2\text{CO}_3\) is a stronger Brønsted–Lowry acid than \(\text{H}_2\text{PO}_4^-\). Which choice correctly identifies the roles of the species in the reaction as written and the side favored at equilibrium?
\[ \text{H}_2\text{PO}_4^-\text{(aq)}+\text{HCO}_3^-\text{(aq)}\rightleftharpoons \text{HPO}_4^{2-}\text{(aq)}+\text{H}_2\text{CO}_3\text{(aq)} \]
Independent measurements at the same temperature establish that \(\text{H}_2\text{CO}_3\) is a stronger Brønsted–Lowry acid than \(\text{H}_2\text{PO}_4^-\). Which choice correctly identifies the roles of the species in the reaction as written and the side favored at equilibrium?
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