Cis-butene dioic acid $\overset{K_{a_1}(-H^+)}{\longleftrightarrow} X_1^- \overset{K_{a_2}(-H^+)}{\longleftrightarrow} X_2^{2-}$
Trans-butene dioic acid $\overset{K'_{a_1}(-H^+)}{\longleftrightarrow} Y_1^- \overset{K'_{a_2}(-H^+)}{\longleftrightarrow} Y_2^{2-}$
The incorrect statement regarding the above information is:

The enthalpies of neutralization of $HCN$ and $H_2S$ with a strong base are $12.13 \ kJ \ equi^{-1}$ and $15.9 \ kJ \ equi^{-1}$ respectively. Then:

Identify the conjugate acid-base pairs in the reaction: $NH_{3(aq)} + H_2O_{(l)} \rightleftharpoons NH_{4(aq)}^+ + OH_{(aq)}^-$

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?

Consider the following reaction involving two acids shown below: formic acid and $HF$.
$K^+F^- + HCOOH \rightleftharpoons HCOO^-K^+ + HF$
Given: $pK_a$ of $HCOOH = 3.8$ and $pK_a$ of $HF = 3.2$.
Which of the following statements about this reaction are true?
$(A)$ Formic acid is the strongest Bronsted acid in the reaction
$(B)$ $HF$ is the strongest Bronsted acid in the reaction
$(C)$ $KF$ is the strongest Bronsted base in the reaction
$(D)$ $KO_2CH$ is the strongest Bronsted base in the reaction
$(E)$ The equilibrium favours the reactants
$(F)$ The equilibrium favours the products
$(G)$ Formic acid has a weaker conjugate base
$(H)$ $HF$ has a weaker conjugate base

Identify each species in the following equilibrium according to the code: $SA = \text{stronger acid}$; $SB = \text{stronger base}$; $WA = \text{weaker acid}$; $WB = \text{weaker base}$. The $pK_a$ of $(CH_3)_2NH_2^+$ is $10.7$ (conjugate acid of $(CH_3)_2NH$) and the $pK_a$ of $CH_3OH$ is $15.2$.
$CH_3OH$ $(1)$ + $(CH_3)_2NH$ $(2)$ $\rightleftarrows CH_3O^- + (CH_3)_2NH_2^+$