Dissociation constant and degree of dissociation of a weak acid are $1.8 \times 10^{-5}$ and $0.03$ respectively. What will be the concentration of the solution of the weak acid (in $M$)?

Calculate the percentage dissociation of a $0.05 \ M$ solution of a weak electrolyte if its molar conductivity and molar conductivity at infinite dilution are respectively $3.3 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and $132 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. (in $\%$)

In aqueous solution,strong electrolytes

At infinite dilution,the percentage ionization for both strong and weak electrolytes is ...... $100 \%$

Electrolytes when dissolved in water dissociate into their constituent ions. The degree of dissociation of an electrolyte increases with

Given the two concentrations of $HCN$ $(K_a = 10^{-9})$ are $0.1 \ M$ and $0.001 \ M$ respectively. What will be the ratio of their degrees of dissociation?