Calculate the amount of $N H_{3}$ and $N H_{4} C l$ required to prepare a buffer solution of $p H 9.0$ when total concentration of buffering reagents is $0.6 m o l L^{-}$ . $p K_{b}$ for $N H_{3} = 4.7, log 2 = 0.30$ .

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Solution

$p O H = p K_{b} + l o g \frac{S a l t}{b a s e}$
$S = 4.7 + l o g \frac{(a)}{(b)}$
$l o g \frac{(a)}{(b)} = l o g (2) ⟹ \frac{a}{b} = 2$
Also, $a + b = 0.6$ (given)
$2 b + b = 0.6$
$b = 0.2 ⟶ a = 0.4$
$[S a l t] = 0.4 M$ $[B a s e] = 0.2 M$
$[N H_{4} C l] = 0.4 M$ $[N H_{3}] = 0.2 M$
Amount of $N H_{4} C l = 0.4 \times 53.5 = 21.4 \frac{g}{L}$
Amount of $N H_{3} = 0.2 \times 17 = 3.4 \frac{g}{L}$

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Calculate the amount of NH3 and NH4Cl required to prepare a buffer solution of pH 9.0 when total concentration of buffering reagents is 0.6 mol L−. pKb for NH3=4.7,log2=0.30.

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