For a concentrated solution of a weak electrolyte ( $K _{ eq }=$ equilibrium constant) $A _2 B _3$ of concentration ' $c$ ', the degree of dissociation " $\alpha$ ' is

  • [JEE MAIN 2023]
  • A

    $\left(\frac{ K _{ eq }}{108 c ^4}\right)^{\frac{1}{5}}$

  • B

    $\left(\frac{ K _{ eq }}{6 c ^5}\right)^{\frac{1}{5}}$

  • C

    $\left(\frac{K_{e q}}{5 c^4}\right)^{\frac{1}{5}}$

  • D

    $\left(\frac{ K _{ eq }}{25 c ^2}\right)^{\frac{1}{5}}$

Similar Questions

The ionization constant of propanoic acid is $1.32 \times 10^{-5}$. Calculate the degree of ionization of the acid in its $0.05\, M$ solution and also its $pH$. What will be its degree of ionization if the solution is $0.01$ $M$ in $HCl$ also?

The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

Which oxychloride has maximum $pH$

The $ pH$  of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be

$50\ ml$ of $0.02\ M$ $NaHSO_4$ is mixed with $50$ $ml$ of $0.02\ M\ Na_2SO_4$. Calculate $pH$ of the resulting solution.$[pKa_2 (H_2SO_4) = 2]$