What is the pH of 10 L of a buffer solution | vedclass

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(C) Given: Concentration of salt $[NH_4Cl] = 0.01 \ M$. Concentration of base $[NH_4OH] = 0.1 \ M$. $pK_b = 5$. $A$ mixture of $NH_4OH$ and $NH_4Cl$ f

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$10$

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(C) Given: Concentration of salt $[NH_4Cl] = 0.01 \ M$. Concentration of base $[NH_4OH] = 0.1 \ M$. $pK_b = 5$. $A$ mixture of $NH_4OH$ and $NH_4Cl$ forms a basic buffer solution. The Henderson-Hasselbalch equation for a basic buffer solution is: $pOH = pK_b + \log \frac{[Salt]}{[Base]}$. Substituting the values into the equation: $pOH = 5 + \log \frac{0.01}{0.1} = 5 + \log(0.1) = 5 - 1 = 4$. Since $pH + pOH = 14$ at $25^{\circ}C$: $pH = 14 - pOH = 14 - 4 = 10$.

What is the $pH$ of $10 \ L$ of a buffer solution containing $0.01 \ M \ NH_4Cl$ and $0.1 \ M \ NH_4OH$ having $pK_b$ of $5$?

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