What is the pH value of N/1000 KOH solution — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

# Solution: pH of N/1000 KOH Solution **Step 1: Determine the molarity of KOH** N/1000 means normality = 1/1000 = $10^{-3}$ N Since KOH is a monoprotic base, Normality = Molarity $$[\text{KOH}] = 10^{-3} \text{ M}$$ **Step 2: Find [OH⁻] concentration** KOH is a strong base and completely dissociates: $$\text{KOH} \rightarrow K^+ + OH^-$$ $$[\text{OH}^-] = 10^{-3} \text{ M}$$ **Step 3: Calculate pOH** $$\text{pOH} = -\log[\text{OH}^-] = -\log(10^{-3}) = 3$$ **Step 4: Calculate pH** Using the relationship: $\text{pH} + \text{pOH} = 14$ $$\text{pH} = 14 - 3 = 11$$ **Answer: pH = 11** The solution is basic (pH > 7) because KOH is a strong base that produces hydroxide ions, making the solution alkaline.