A 100 mL solution has 0.01 moles of NaOH dissolved in it. What is the pH of the solution?
Correct Answer: 13
Subject: chemistry
Explanation: • <b>Key Fact</b>
First find Molarity (concentration of OH⁻ ions): Moles / Volume in Litres.
• <b>Supporting Detail</b>
100 mL = 0.1 L. Concentration [OH⁻] = 0.01 / 0.1 = 0.1 M (or 10⁻¹ M).
• <b>Related Concept</b>
Calculate pOH = -log[OH⁻] = -log(10⁻¹) = 1.
• <b>Why wrong options are wrong</b>
Use relation: pH + pOH = 14. Therefore, pH = 14 - 1 = 13.
• <b>Exam Trick</b>
If [OH⁻] is 10⁻ˣ, pOH is x. pH is 14-x.
• <b>Additional Info</b>
Since NaOH is a strong base, its pH will naturally be near the high end (13-14).