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A weak base is $1.42 \%$ dissociated in its $0.05 \mathrm{M}$ solution. Calculate its dissociation constant.
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Verified Answer
The correct answer is:
$1.0 \times 10^{-5}$
Percent dissociation $=1.42 \%$
$\therefore \quad \alpha=0.0142$
For a weak monoacidic base,
$\begin{aligned}
\mathrm{K}_{\mathrm{b}} & =\alpha^2 \mathrm{C} \\
& =(0.0142)^2 \times(0.05) \\
& =1.0082 \times 10^{-5}
\end{aligned}$
$\therefore \quad \alpha=0.0142$
For a weak monoacidic base,
$\begin{aligned}
\mathrm{K}_{\mathrm{b}} & =\alpha^2 \mathrm{C} \\
& =(0.0142)^2 \times(0.05) \\
& =1.0082 \times 10^{-5}
\end{aligned}$
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