Ionic Equilibrium in Solution

${\mathrm{H}}_3{\mathrm{PO}}_4$ undergoes dissociation as ${\mathrm{H}}_3{\mathrm{PO}}_4⟶3{\mathrm{H}}^{+}+{\mathrm{PO}}_4^{3-}$ if $\frac{{\mathrm{n}}_{\text{cation }}+{\mathrm{n}}_{\text{anion }}}{{\left({\mathrm{n}}_{{\mathrm{H}}_3{\mathrm{PO}}_4}\right)}_{\text{undissoicated }}}=\frac{8}{3}$. $\%$ dissociation of ${\mathrm{H}}_3{\mathrm{PO}}_4$ is " $\mathrm{x}$ ", report your answer as $\left[\frac{\mathrm{x}}{10}\right]$

What is the concentration in $\mathrm{gm}/\mathrm{litre}$ of a solution of glucose which is isotonic with a deci-normal $\mathrm{NaCl}$ solution which is $50\%$ dissociated?

The electrochemical equivalent of a material depends on 

Sodium chloride conducts electric current in its solid state.

In which of the following solution should the other electrode be immersed to get maximum e.m.f , If galvanic cell is composed of two hydrogen electrodes, one of which is a standard one.

(${\mathrm{K}}_{\mathrm{a}}={10}^{-5}$ for acetic acid and $\mathrm{ }{\mathrm{K}}_{{\mathrm{a}}_1\mathrm{ }}={10}^{-3}$ for phosphoric acid $)$.

A certain weak acid has a dissociation constant of ${10}^{-5}$. What is the value of the equilibrium constant for its reaction with a strong base?

At equilibria, select the false statement, considering the given equation:
${\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{H}}_3{\mathrm{O}}^{+}+{\mathrm{CH}}_3{\mathrm{COO}}^{-}$
${\mathrm{H}}_2{\mathrm{SO}}_4+{\mathrm{CH}}_3\mathrm{COOH}\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COOH}}_2^{+}+{\mathrm{HSO}}_4^{-}$
${\mathrm{H}}_2{\mathrm{SO}}_4+{\mathrm{HNO}}_3\rightleftharpoons {\left[{\mathrm{H}}_2{\mathrm{NO}}_3\right]}^{+}+{\mathrm{HSO}}_4^{-}$
${\mathrm{NH}}_3+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{NH}}_4^{+}+{\mathrm{OH}}^{-}$

${\mathrm{C}\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H}$ and ${\mathrm{N}\mathrm{H}}_4\mathrm{O}\mathrm{H}$ have equal value of dissociation constants as $1.8\times {10}^{–5}$ at $25°\mathrm{C}$. The equilibrium constant for the reaction of ${\mathrm{C}\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H}$ and ${\mathrm{N}\mathrm{H}}_4\mathrm{O}\mathrm{H}$ will be:

The relation between the degree of dissociation $\left(\alpha \right)$ of a weak electrolyte ${\mathrm{A}}_{\mathrm{x}}{\mathrm{B}}_{\mathrm{y}}$ and van't Hoff factor $\left(\mathrm{i}\right)$ is expressed by the expression:

The ionisation constant of $\mathrm{NH}_{4}^{+}$ in water is $5.6 \times 10^{-10} \mathrm{at}$ $25^{\circ} \mathrm{C} .$ The rate constant for the reaction of $\mathrm{NH}_{4}^{+}$ and $\mathrm{OH}^{-}$ to form $\mathrm{NH}_{3}$ and $\mathrm{H}_{2} \mathrm{O}$ at $25^{\circ} \mathrm{C}$ is $3.4 \times 10^{10}$ litre
$\mathrm{mol}^{-1} \mathrm{sec}^{-1} .$ If equilibrium constant of water at $25^{\circ} \mathrm{C}$ is $1.8 \times 10^{-16},$ then

The degree of dissociation of $\mathrm{NH}_{4} \mathrm{OH}$ is :

At infinite dilution, the percentage ionisation of both strong and weak electrolytes is:

Acetic acid and propionic acid have ${\mathrm{K}}_{\mathrm{a}}$ values $1.75\times {10}^{-5}$ and $\mathrm{1}.3\times {10}^{-\mathrm{5}}$ respectively at a certain temperature. An equimolar solution of a mixture of the two acids is partially neutralized by $\mathrm{NaOH}$. How is the ratio of the contents of acetate and propionate ions related to the ${\mathrm{K}}_{\mathrm{a}}$ values and the molarity ?

The solubility product of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ is $32\times {10}^{-12}.$ What is the concentration of ${\mathrm{CrO}}_4^{2-}$ ions in that solution?

Which of the following salts will not undergo hydrolysis?

The solubility $\left(\mathrm{S}\right)$ of a solute in water varies with the temperature as follows: $\mathrm{S}=\mathrm{A}{\mathrm{e}}^{-\mathrm{\Delta }\mathrm{H}/\mathrm{R}\mathrm{T}}$.
For which of the following solute, $\ln \mathrm{S}\mathrm{ }\mathrm{v}\mathrm{s}\mathrm{ }1/\mathrm{T}$ plot is:





when $\mathrm{\Delta }\mathrm{H}$ represents the enthalpy of the solution?

Aniline behaves as a weak base.When 0.1M, 50ml solution of aniline was mixed with 0.1M, 25ml solution of HCl the pH of resulting solution was 8. Then the pH of 0.01 M solution of aniliniumchloride will be (Kw = 10^-14)

Electrolytes when dissolved in water dissociates into ions because

An acid solution of 0.005 M has a pH of 5. The degree of ionisation of acid is

Vapour density of ${\mathrm{N}}_2{\mathrm{O}}_4$ at $60°\mathrm{C}$ is found to be $30.6$. The degree of dissociation of ${\mathrm{N}}_2{\mathrm{O}}_4$ is: