A student prepares two aqueous solutions of ammonia, \(\text{NH}_3\text{(aq)}\), at \(25^\circ\text{C}\). Solution 1 has an initial concentration of \(0.010\text{ M}\), and Solution 2 has an initial concentration of \(0.10\text{ M}\). The equilibrium reaction is represented by the equation below.

\[ \text{NH}_3\text{(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{NH}_4^+\text{(aq)} + \text{OH}^-\text{(aq)} \]

The student determines that Solution 2 has a higher \(\text{pH}\) than Solution 1, even though the percent ionization of \(\text{NH}_3\) is lower in Solution 2. Which of the following statements correctly explains why Solution 2 has a higher \(\text{pH}\)?