0.05 M solution is dissolved in 0.001 M solution. Calculate the of this solution if . — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

This is a basic buffer. $pOH = pK_b + \log([Salt]/[Base]) = pK_b + \log(0.001/0.05) = pK_b + \log(1/50)$. $[OH^-] = K_b \times ([Base]/[Salt]) = 1.8 \times 10^{-5} \times (0.05 / 0.001) = 1.8 \times 10^{-5} \times 50 = 90 \times 10^{-5} = 9.0 \times 10^{-4} \text{ M}$.