A student prepares an aqueous mixture containing both \(0.10\text{ M }\text{HNO}_2\text{(aq)}\) and \(0.10\text{ M }\text{HClO(aq)}\) at \(25^\circ\text{C}\). The chemical equations and acid-ionization constants for the two weak acids are given below:

\[ \text{HNO}_2\text{(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{NO}_2^-\text{(aq)} \quad K_a = 4.0 \times 10^{-4} \]
\[ \text{HClO(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{H}_3\text{O}^+\text{(aq)} + \text{ClO}^-\text{(aq)} \quad K_a = 3.0 \times 10^{-8} \]

Which of the following correctly predicts how the percent ionization of \(\text{HClO}\) in this mixture compares to its percent ionization in a pure \(0.10\text{ M }\text{HClO(aq)}\) solution, and provides the correct justification?