The degree of dissociation of $0.1 \, N \, CH_3COOH$ is (Dissociation constant $K_a = 1 \times 10^{-5}$)

The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

The $pH$ of a $0.01 \, M$ solution of acetic acid having a degree of dissociation of $12.5 \%$ is:

The $pH$ of a $0.1 \ M$ solution of a monobasic acid is $2.34$. Calculate the degree of dissociation of the acid.

The ionization constant of acetic acid is $1.74 \times 10^{-5}$. Calculate the degree of dissociation of acetic acid in its $0.05 \ M$ solution. Calculate the concentration of acetate ion in the solution and its $pH$.

$A$ weak base is $1.42 \%$ dissociated in its $0.05 \ M$ solution. Calculate its dissociation constant.