The degree of dissociation in a weak electrolyte increases

If $\alpha$ is the degree of ionization,$C$ is the concentration of a weak electrolyte,and $K_a$ is the acid ionization constant,then the correct relationship between $\alpha$,$C$,and $K_a$ is:

Which of the following,when dissolved in water,forms a solution that is non-conducting?

The equivalent conductance of $M/32$ solution of a weak monobasic acid is $8.0 \, \text{mho} \, \text{cm}^2$ and at infinite dilution is $400 \, \text{mho} \, \text{cm}^2.$ The dissociation constant of this acid is

Which of the following will occur if a $0.1 \, M$ solution of a weak acid is diluted to $0.01 \, M$ at constant temperature?

What is the relationship between the degree of dissociation of a weak base and its concentration?