Calculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.
- A$6 \times 10^{-5}$
- B$4 \times 10^{-5}$
- C$2 \times 10^{-5}$
- D$1 \times 10^{-5}$
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