0.05 M solution is dissolved in 0.001 M solution. Calculate the of this solution if . — Ionic Equilibrium Chemistry Question
Question
0.05 M $NH_4OH$ solution is dissolved in 0.001 M $NH_4Cl$ solution. Calculate the $[OH^-]$ of this solution if $K_b(NH_4OH) = 1.8 \times 10^{-5}$.
Answer: A
💡 Solution & Explanation
This is a basic buffer. $pOH = pK_b + \log([Salt]/[Base]) = pK_b + \log(0.001/0.05) = pK_b + \log(1/50)$. $[OH^-] = K_b \times ([Base]/[Salt]) = 1.8 \times 10^{-5} \times (0.05 / 0.001) = 1.8 \times 10^{-5} \times 50 = 90 \times 10^{-5} = 9.0 \times 10^{-4} \text{ M}$.
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