A buffer solution has equal volumes of 0.2 M $NH_{4}OH\ and\ 0.02\ M\ NH_{4}Cl$. The $pK_{b}$ of the base is 5. The pH is

Question

Dr. Abubacker · Accepted Answer

(a)
$pOH = pK_{b} + \log\frac{\lbrack salt\rbrack}{\lbrack base\rbrack}$ (Henderson’s equation)
$= 5 + \log\frac{0.02}{0.2} = 5 + \log\frac{1}{10}$
$= 5 + ( - 1) = 4$
pH=$14 - pOH = 14 - 4 = 10$

Q. A buffer solution has equal volumes of 0.2 M $NH_{4}OH\ and\ 0.02\ M\ NH_{4}Cl$. The $pK_{b}$ of the base is 5. The pH is

Explanation

Reviewed by Dr. Abubacker

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