Answer
$C_7H_5{O_2}^-$ acts as a weak base in solution.
- $C_7H_5{O_2}^-(aq) + H_2O(l) \lt -- \gt C_7H_6{O_2}(aq) + OH^-(aq)$
Work Step by Step
1. Protonate this anion, to get its conjugate acid:
$C_7H_5{O_2}^- --\gt C_7H_6{O_2}$
2. Analyze the protonated compound.
- Weak acids have weak bases as conjugate pair.
- $C_7H_6{O_2}$ is a weak acid, therefore, $C_7H_5{O_2}^-$ acts as a weak base.
3. Now that we know that, write the equation where $C_7H_5{O_2}^-$ receives a proton from a water molecule, producing $OH^-$
- $C_7H_5{O_2}^-(aq) + H_2O(l) \lt -- \gt C_7H_6{O_2}(aq) + OH^-(aq)$
