Equilibrium — JEE Advanced PYQs

At 25°C, the concentration of ${\mathrm{H}}^{+}$ ions in $1.00\times 10^{-3}\mathrm{M}$ aqueous solution of a weak monobasic acid having acid dissociation constant $\left(K_a\right)=4.00\times 10^{-11}$ is $\mathbf{X}\times 10^{-7}\mathrm{M}$. The value of …

The solubility of barium iodate in an aqueous solution prepared by mixing 200 mL of 0.010 M barium nitrate with 100 mL of 0.10 M sodium iodate is $\mathbf{X}\times 10^{-6}\mathrm{mol}{\mathrm{dm}}^{-3}$. The value of $\mathbf{X}$ is ____.

Use: Solubility product consta …

On decreasing the $p\mathrm{H}$ from 7 to 2, the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from $10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}$ to $10^{-3}\mathrm{mol}{\mathrm{L}}^{-1}$. The $p{\mathrm{K}}_{\mathrm{a}}$ of HX is:

A solution is prepared by mixing 0.01 mol each of ${\mathrm{H}}_2{\mathrm{CO}}_3,{\mathrm{NaHCO}}_3,{\mathrm{Na}}_2{\mathrm{CO}}_3$, and NaOH in 100 mL of water. pH of the resulting solution is ____.
[Given : $p{\mathrm{K}}_{\mathrm{a}1}$ and …

Concentration of ${\mathrm{H}}_2{\mathrm{SO}}_4$ and ${\mathrm{Na}}_2{\mathrm{SO}}_4$ in a solution is 1 M and $1.8\times 10^{-2}\mathrm{M}$, respectively. Molar solubility of ${\mathrm{PbSO}}_4$ in the same solution is …

A solution of 0.1 M weak base (B) is titrated with 0.1 M of a strong acid (HA). The variation of pH of the solution with the volume of HA added is shown in the figure below. What is the $\mathrm{p}{K}_{\mathrm{b}}$ of the base? The neutralization reaction is given by …

An acidified solution of $0.05\mathrm{M}{\mathrm{Zn}}^{2+}$ is saturated with $0.1\mathrm{M}{\mathrm{H}}_2\mathrm{S}$. What is the minimum molar concentration (M) of ${\mathrm{H}}^{+}$required to prevent the precipitation of ZnS ?
Use …

For the following reaction, the equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ at 298 K is $1.6\times 10^{17}$.

When equal volumes of …

The solubility of a salt of weak acid (AB) at pH 3 is $\mathbf{Y}\times 10^{-3}\mathrm{mol}{\mathrm{L}}^{-1}$. The value of Y is ____. (Given that the value of solubility product of $\mathbf{AB}$ $(K_{sp})=2\times 10^{-10}$ and the value of ionization constant of HB …

Dilution processes of different aqueous solutions, with water, are given in LIST-I. The effects of dilution of the solutions on $\left[{\mathrm{H}}^{+}\right]$ are given in LIST-II.

(Note: Degree of dissociation $(\alpha )$ of weak acid and weak base is << 1; degree of hydrolysis o …

Thermal decomposition of gaseous ${\mathrm{X}}_2$ to gaseous X at 298 K takes place according to the following equation:

The standard reaction Gibbs energy, ${\Delta }_r{G}^{\circ }$, of this reaction is po …

Thermal decomposition of gaseous ${\mathrm{X}}_2$ to gaseous X at 298 K takes place according to the following equation:

The standard reaction Gibbs energy, ${\Delta }_r{G}^{\circ }$, of this reaction is po …

The %yield of ammonia as a function of time in the reaction
${\mathrm{N}}_2(g)+3{\mathrm{H}}_2(g)\rightleftharpoons 2{\mathrm{NH}}_3(g),\Delta \mathrm{H}<0$
at $\left(P,T_1\right)$ is given below.
If this reaction is conducted at $\left(P,T_2\right)$, with …

PARAGRAPH 2

When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7 °C was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong ba …

The initial rate of hydrolysis of methyl acetate $(1M)$ by a weak acid $(HA,1M)$ is $1/100^{\text{th}}$ of that of a strong acid $(HX,1M)$, at 25 °C. The $K_a$ of $HA$ is

The thermal dissociation equilibrium of ${\mathrm{CaCO}}_3(s)$ is studied under different conditions.
${\mathrm{CaCO}}_3(\mathrm{s})\rightleftharpoons \mathrm{CaO}(\mathrm{s})+{\mathrm{CO}}_2(\mathrm{g})$
For this equilibrium, the correct statement(s) is(are)

The $K_{sp}$ of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ is $1.1\times 10^{-12}$ at 298 K. The solubility (in $\mathrm{mol}/\mathrm{L}$) of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ in a $0.1\mathrm{M}{\mathrm{AgNO}}_3$ solution is

Aqueous solutions of ${\mathrm{HNO}}_3,\mathrm{KOH},{\mathrm{CH}}_3\mathrm{COOH}$, and ${\mathrm{CH}}_3\mathrm{COONa}$ of identical concentrations are provided. The pair(s) of solutions which form a buffer upon mixing is(are)

Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is
| KCN | ${\mathrm{K}}_2{\mathrm{SO}}_4$ | ${\left({\mathrm{NH}}_4\right)}_2{\mathrm{C}}_2{\mathrm{O}}_4$ | NaCl | $\mathrm{Zn}{\left({\mathrm{NO}}_3\right)}_2$ || …

The dissociation constant of a substituted benzoic acid at $25^{\circ }\mathrm{C}$ is $1.0\times 10^{-4}$. The pH of a 0.01 M solution of its sodium salt is

2.5 mL of $\frac{2}{5}\mathrm{M}$ weak monoacidic base $({\mathrm{K}}_{\mathrm{b}}=1\times 10^{-12}$ at $25^{\circ }\mathrm{C})$ is titrated with $\frac{2}{15}\mathrm{M}\mathrm{HCl}$ in water at $25^{\circ }\mathrm{C}$. The concentration of …

Solubility product constants (${\mathrm{K}}_{\text{sp}}$) of salts of types $\mathrm{MX}$, ${\mathrm{MX}}_2$ and ${\mathrm{M}}_3\mathrm{X}$ at temperature 'T' are $4.0\times 10^{-8}$, $3.2\times 10^{-14}$ and $2.7\times 10^{-15}$, respectively. Solubilities (mol dm …

${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$
Which is correct statement if ${\mathrm{N}}_2$ is added at equilibrium condition?