Which of the following statements are incorrect?

The dissociation constant of a certain weak acid is $1.0 \times 10^{-4}$. What is the equilibrium constant for its reaction with a strong base?

The $pH$ of $0.1 \ M$ solution of the following salts increases in the order:

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 $pK_{b}(NH_{3}) = 4.74$)

Given below are two statements :
Statement $I$ : Aqueous solution of ammonium carbonate is basic.
Statement $II$ : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on $K_a$ and $K_b$ value of acid and the base forming it.
In the light of the above statements,choose the most appropriate answer from the options given below :

What is the degree of dissociation of $CH_3COOH$ if $\wedge^{\circ}(CH_3COO^{-}) = 50 \ S \ cm^2 \ mol^{-1}$,$\wedge^{\circ}(H^{+}) = 350 \ S \ cm^2 \ mol^{-1}$ and the molar conductivity of $5 \times 10^{-2} \ M \ CH_3COOH$ is $20 \ S \ cm^2 \ mol^{-1}$?