Ionization of Acids and Bases

When base dissolves in water, it should dissociate to form:

Two vessels $\mathrm{X}$ and $\mathrm{Y}$ contain aqueous solutions of a weak acid $\mathrm{HA}$  and its salt $\mathrm{NaA}$, respectively. The following two equilibria $\mathrm{HA}+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{A}}^{-}$and ${\mathrm{A}}^{-}+{\mathrm{H}}_2\mathrm{O}$ $\rightleftharpoons \mathrm{HA}+{\mathrm{OH}}^{-}$, exist in vessels $\mathrm{X}$ and $\mathrm{Y}$, respectively. At equilibrium (at a given temperature $\mathrm{T}$), the concentrations of $\mathrm{HA},{\mathrm{H}}_3{\mathrm{O}}^{+}$and ${\mathrm{A}}^{-}$in vessel $\mathrm{X}$ are ${\mathrm{C}}_1,{\mathrm{C}}_2$ and ${\mathrm{C}}_3$, respectively, while that of ${\mathrm{A}}^{-},\mathrm{HA}$ and ${\mathrm{OH}}^{-}$in vessel $\mathrm{Y}$, are ${\mathrm{C}}_4,{\mathrm{C}}_5$ and ${\mathrm{C}}_6$, respectively. Let the quantity $\left({\mathrm{C}}_2·{\mathrm{C}}_3·{\mathrm{C}}_5·{\mathrm{C}}_6\right)/\left({\mathrm{C}}_1·{\mathrm{C}}_4\right)$ be denoted by $\mathrm{Q}$. The correct plot $(\ln Q$ vs $1 / \mathrm{T})$ is

The ionization of base MOH can be represented by the equation:

$\mathrm{MOH}\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{M}}^{-}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{+}\left(\mathrm{aq}\right)$

Which of the following equation follows for base ionization constant is expressed in terms of concentration in molarity of various species in equilibrium.

Define base ionization constant.

The $\mathrm{pH}$ of an aqueous solution of ${10}^{-8}\mathrm{MHCl}$ is

The correct order of increasing $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ in the following aqueous solution is 

Which element has the lowest first ionisation energy?

Which of the following species has the ionization potential ?

An acid base indicator has ${\mathrm{K}}_{\mathrm{a}}=3\times 10^{-5}$ . The acid form of the indicator is red and the basic form is blue. By how much must the pH change in order to change the indicator from 75% red to 75% blue (log 3 $=$ 0.4770)

In an experiment, $0.04 \mathrm{F}$ was passed through $400 \mathrm{mL}$ of a $1 \mathrm{M}$ solution of $\mathrm{NaCl}$. What would be the $\mathrm{pH}$ of the solution after the electrolysis?

What is a true statement with regard to $\mathrm{0}.10\mathrm{M}\mathrm{\hspace{0.33em}}{\mathrm{H}}_{\mathrm{2}}{\mathrm{SO}}_{\mathrm{4}}$ solution?

The pH of a solution obtained by mixing equal volume of solutions having pH = 3 and pH = 4.

[log 5.5 = 0.7404]

The degree of ionization of 0.4 M acetic acid will be $({\mathrm{K}}_{\mathrm{a}}=1.8\times {10}^{-5})$ .

Adding a few drops of hydrochloric acid to a beaker containing water results in the formation of hydrated species. Identify which hydrated species can exist in solution.

(1) ${\mathrm{H}}_3{\mathrm{O}}^{+}$

(2) ${\mathrm{H}}_3{\mathrm{O}}_2^{-}$

(3) ${\mathrm{H}}_5{\mathrm{O}}_2^{+}$

(4) ${\mathrm{H}}_2{\mathrm{ClO}}^{-}$

What will be the $\mathrm{pH}$ of a $0.01 \mathrm{M}$ ammonia solution which is $5 \%$ ionised?

Select the correct statements out of the following.

In an aqueous solution, the ionization constants for carbonic acid are

${\text{K}}_1=\text{4.2}\times 10^{-7}$ and ${\text{ K}}_2=\text{4.8}\times 10^{-11}$

Select the correct statement for a saturated $\text{0.034 M}$ solution of the carbonic acid:

Which are correct for the dissociation of weak monobasic acid represented by the given case :
$\begin{array}{ccccc}& \text{BH}& \rightleftharpoons & {\text{B}}^{-}+& {\text{H}}^{+}\\ \text{Initial concentration}& c& & 0& 0\\ \text{Equilibrium concentration}& c-\mathit{\text{x}}& & \mathit{\text{x}}& \mathit{\text{x}}\end{array}$
                                   (dissociation constant of acid is K_a )

Given, $\text{HF}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{a}}}{⟶}{\text{H}}_3{\text{O}}^{+}+{\text{F}}^{-};$  ${\text{F}}^{-}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{b}}}{⟶}\text{H}\text{F}+{\text{OH}}^{-}$.  Which of the following relation is correct?