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For a weak acid HA, the percentage of dissociation is nearly 1% at equilibrium. If the concentration of acid is 0.1 mol L$^{-1}$, then the correct option for its $K_a$ at the same temperature is:
A
$1\times10^{-4}$
B
$1\times10^{-6}$
C
$1\times10^{-5}$
D
$1\times10^{-3}$
Detailed Solution
$K_a=C\alpha^2=(0.1)\times(0.01)^2=1\times10^{-5}$.