What is the pH of a basic buffer solution containing equimolar concentrations of and if of is 4.74 a — Ionic Equilibrium Chemistry Question
Question
What is the pH of a basic buffer solution containing equimolar concentrations of $NH_4OH$ and $NH_4Cl$ if $pK_b$ of $NH_4OH$ is 4.74 at $25^\circ C$?
Answer: B
💡 Solution & Explanation
By Henderson's equation, $pOH = pK_b + \log([Salt]/[Base])$. Since concentrations are equimolar, $\log(1) = 0$, so $pOH = pK_b = 4.74$. $pH = 14 - 4.74 = 9.26$.
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