For a weak acid $HA,$ Ostwald's dilution law is represented by the equation

  • A

    ${K_a} = \frac{{\alpha c}}{{1 - {\alpha ^2}}}$

  • B

    ${K_a} = \frac{{{\alpha ^2}c}}{{1 - \alpha }}$

  • C

    $\alpha = \frac{{{K_a}c}}{{1 - c}}$

  • D

    ${K_a} = \frac{{{\alpha ^2}c}}{{1 - {\alpha ^2}}}$

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$0.01$ moles of a weak acid $HA \left( K _{ a }=2.0 \times 10^{-6}\right)$ is dissolved in $1.0\, L$ of $0.1\, M\, HCl$ solution. The degree of dissociation of $HA$ is ............. $\times 10^{-5}$

(Round off to the Nearest Integer).

[Neglect volume change on adding $HA$. Assume degree of dissociation $<< 1]$

  • [JEE MAIN 2021]