$A$ weak acid is $0.1\%$ ionised in $0.1 \ M$ solution. Its $pH$ is

For a $10 \ M \ CH_3COOH$ solution,if $K_a = 10^{-5}$,what will be the values of $[H^{+}]$ and $pH$ respectively?

Weak acid $HX$ has dissociation constant $1 \times 10^{-5}$. Calculate the percent dissociation in its $0.1 \ M$ solution. (in $\%$)

It has been found that the $pH$ of a $0.01 \ M$ solution of an organic acid is $4.15$. Calculate the concentration of the anion,the ionization constant of the acid and its $pK_a$.

The $K_b$ of ammonia $(NH_3)$ is $1.8 \times 10^{-5}$ at $298 \ K$. Calculate the $pH$ of a $0.1 \ M$ ammonia solution. (in $.13$)

The concentration of $[CN^{-}]$ in $0.1 \, M \, HCN$ solution is: $(K_a = 4 \times 10^{-10})$