Step 1: Apply the pOH formula
For a strong base like sodium hydroxide \( \text{NaOH} \), which dissociates completely in water, the \( \text{OH}^- \) ion concentration equals the base concentration. The pOH is calculated as:\[\text{pOH} = -\log[\text{OH}^-]\]Step 2: Compute pOH
Given:- \( \text{NaOH} \) concentration = \( 0.01 \, \text{M} \),- Thus, \( [\text{OH}^-] = 0.01 \, \text{M} \).Substitute into the formula:\[\text{pOH} = -\log(0.01) = 2\]Step 3: Utilize the pH-pOH relationship The relationship is:\[\text{pH} + \text{pOH} = 14\]Substitute the calculated pOH:\[\text{pH} = 14 - 2 = 12\]Result: The pH of a \( 0.01 \, \text{M} \) \( \text{NaOH} \) solution is \( 12 \). Therefore, option (1) is the correct answer.