Which of the following shows weak ionisation in water?

$A$ $Lewis$ acid is a .....

Match the following acids in List-$I$ with their respective acid dissociation constants $(K_a)$ in List-$II$:

List-$I$ (Acid)	List-$II$ $(K_a)$
$A$. Phenol	$I$. $1 \times 10^{-13}$
$B$. Benzoic acid	$II$. $3.0 \times 10^{-8}$
$C$. $HClO$	$III$. $1.0 \times 10^{-10}$
$D$. $CH_3COOH$	$IV$. $6.5 \times 10^{-5}$
	$V$. $1.75 \times 10^{-5}$

The correct match is:

Consider the following data for a series of hydrogen halide Bronsted acids:-

Acid	$HF$	$HCl$	$HBr$	$HI$
$K_a$	$7.2 \times 10^{-4}$	$1 \times 10^6$	$1 \times 10^9$	$3 \times 10^{11}$

Which of these Bronsted acids would have the weakest conjugate base?

What is meant by the conjugate acid-base pair? Find the conjugate acid/base for the following species:
$HNO_{2}$,$CN^{-}$,$HClO_{4}$,$F^{-}$,$OH^{-}$,$CO_{3}^{2-}$,and $S^{2-}$

Which of the following is not an example of the $Br\text{ø}nsted-Lowry$ theory?