Calculate $[H_3O^{+}]$ in $0.02 \ M$ solution of monobasic acid if dissociation constant is $1.8 \times 10^{-5}$.
- A$3.0 \times 10^{-4} \ M$
- B$6.0 \times 10^{-4} \ M$
- C$2.0 \times 10^{-4} \ M$
- D$4.0 \times 10^{-4} \ M$
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View SolutionThe $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)
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