$50 \ mL$ of $10^{-3} \ M \ HCl$ is mixed with $50 \ mL$ of $0.05 \ M \ CH_3COOH$ $(pK_a = 4.7)$. The degree of dissociation of water in the resulting solution is

One mole of ammonia was completely absorbed in one litre solution each of $(a)$ $1 \ M \ HCl$,$(b)$ $1 \ M \ CH_{3}COOH$,and $(c)$ $1 \ M \ H_{2}SO_{4}$ at $298 \ K$. The decreasing order for the $pH$ of the resulting solutions is (Given $pK_{b}(NH_{3}) = 4.74$)

$0.1 \ M$ solution of which of the following has almost unity degree of dissociation?

Calculate the ionic product of the solution formed by mixing equal volumes of $0.004 \, M \, CaSO_4$ and $0.002 \, M \, H_2SO_4$.

The ionization constant of $ClCH_{2}COOH$ is $1.35 \times 10^{-3}$. What will be the $pH$ of $0.1 \ M$ acid and its $0.1 \ M$ sodium salt solution?

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?