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

💡 Solution & Explanation

# pH of N/1000 KOH Solution **Step 1: Determine the molarity of KOH** $$N/1000 = \frac{1}{1000} \text{ N}$$ Since $KOH$ is a monoprotic base, Normality = Molarity $$[KOH] = 10^{-3} \text{ M}$$ **Step 2: Find $[OH^-]$ concentration** $KOH$ is a strong base that completely ionizes: $$KOH \rightarrow K^+ + OH^-$$ Therefore: $$[OH^-] = 10^{-3} \text{ M}$$ **Step 3: Calculate pOH** $$pOH = -\log[OH^-] = -\log(10^{-3}) = 3$$ **Step 4: Calculate pH** Using the relationship $pH + pOH = 14$ (at 25°C): $$pH = 14 - pOH = 14 - 3 = 11$$ **Answer: pH = 11** The solution is basic because $KOH$ is a strong base producing $OH^-$ ions, resulting in $pH > 7$.