for at a certain temperature is . The pH of a basic buffer containing equimolar concentrations of an — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

For a basic buffer, $pOH = pK_b + \log\frac{[Salt]}{[Base]}$. Since the concentrations of salt and base are equimolar, the log term becomes $\log(1) = 0$. Thus, $pOH = pK_b = 4.74$. The pH of the solution is $14 - pOH = 14 - 4.74 = 9.26$.