Equilibrium — JEE Main PYQs

At 600 K, 2 mol of NO are mixed with 1 mol of O₂.
2NO₍ₘ₎ + O₂₍ₘ₎ ⇌ 2NO₂₍ₘ₎
The reaction occurring as above comes to equilibrium under a total pressure of 1 atm. Analysis of the system shows that 0.6 mol of oxygen are present at equilibrium. The equilibrium constant for the reacti …

At 310 K , the solubility of ${\mathrm{CaF}}_2$ in water is
$2.34\times 10^{-3}\mathrm{g}/100\mathrm{mL}$. The solubility product of ${\mathrm{CaF}}_2$ is $\_\_\_\_$ $\times 10^{-8}(\mathrm{mol}/\mathrm{L}{)}^3$. (Given molar mass : …

20 mL of $0.1\mathrm{M}{\mathrm{NH}}_4\mathrm{OH}$ is mixed with 40 mL of 0.05 M HCl . The pH of the mixture is nearest to:
(Given: ${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=1\times 10^{-5},\log 2=0.30$, $\log 3=0.48,\log 5=0.69,\log 7=0.84$, …

Class XII students were asked to prepare one litre of buffer solution of pH 8.26 by their chemistry teacher. The amount of ammonium chloride to be dissolved by the student in 0.2 M ammonia solution to make one litre of the buffer is (Given …

Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A :Phenolphthalein is a pH dependent indicator, remains colourless in acidic solution and gives pink colour in basic medium
Reason R : Phenolphthalein is a weak acid. …

The Plot of pH-metric titration of weak base ${\mathrm{NH}}_4\mathrm{OH}$ vs strong acid HCl looks like:

${\mathrm{Ka}}_1,{\mathrm{Ka}}_2$ and ${\mathrm{Ka}}_3$ are the respective ionization constants for the following reactions (a),(b), and (c).
(a) ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{HC}}_2{\mathrm{O}}_4^{-}$
(b) …

In base vs. Acid titration, at the end point methyl orange is present as

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4 . The ratio of $\frac{\left[{\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{COO}}^{-}\right]}{\left[{\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{COOH}\right]}$ required to make buffer is ____

Gi …

pH value of 0.001 M NaOH solution is ______.

4.0 moles of argon and 5.0 moles of $\mathrm{PCl}{}_5$ are introduced into an evacuated flask of 100 litre capacity at 610 K. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be 6.0 atm. The $K_p$ for the reaction is [Given: …

The solubility of AgCl will be maximum in which of the following ?

50 mL of $0.1\mathrm{M}{\mathrm{CH}}_3\mathrm{COOH}$ is being titrated against 0.1 M NaOH . When 25 mL of NaOH has been added, the pH of the solution will be
____ $\times 10^{-2}$. (Nearest integer)
(Given : …

$2\mathrm{NOCl}(\mathrm{g})\rightleftharpoons 2\mathrm{NO}(\mathrm{g})+{\mathrm{Cl}}_2(\mathrm{g})$

In an experiment, 2.0 moles of NOCl was placed in a one-litre flask and the concentration of NO after equilibrium established, was found to be 0.4 $\mathrm{mol}/\mathrm{L}$. …

If the solubility product of PbS is $8\times 10^{-28}$, then the solubility of PbS in pure water at 298 K is $x\times 10^{-16}\mathrm{mol}{\mathrm{L}}^{-1}$. The value of $x$ is ______.
(Nearest Integer)
[Given $\sqrt{2}=1.41$]

For a reaction at equilibrium
$\mathrm{A}(\mathrm{g})\rightleftharpoons \mathrm{B}(\mathrm{g})+\frac{1}{2}\mathrm{C}(\mathrm{g})$
the relation between dissociation constant (K), degree of dissociation ($\alpha$) and equilibrium pressure (p) is given by :

${\mathrm{PCl}}_5$ dissociates as


5 moles of ${\mathrm{PCl}}_5$ are placed in a 200 litre vessel which contains 2 moles of ${\mathrm{N}}_2$ and is maintained a …

The ${\mathrm{K}}_{\mathrm{sp}}$ for bismuth sulphide $({\mathrm{Bi}}_2{\mathrm{S}}_3)$ is $1.08\times 10^{-73}$. The solubility of ${\mathrm{Bi}}_2{\mathrm{S}}_3$ in $\mathrm{mol}{\mathrm{L}}^{-1}$ at 298 K is

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R:

Assertion A : The amphoteric nature of water is explained by using Lewis acid/base concept.
Reason R: Water acts as an acid with ${\mathrm{NH}}_3$ and as a base with …

The neutralization occurs when 10 mL of 0.1 M acid 'A' is allowed to react with 30 mL of 0.05 M base $\mathrm{M}(\mathrm{OH}{)}_2$. The basicity of the acid 'A' is ______. [M is a metal]

At 1990 K and 1 atm pressure, there are equal number of ${\mathrm{Cl}}_2$ molecules and Cl atoms in the reaction mixture. The value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction ${\mathrm{Cl}}_{2(\mathrm{g})}\rightleftharpoons 2{\mathrm{Cl}}_{(\mathrm{g})}$ under the above c …

Given below are two statements.
Statement I: In the titration between strong acid and weak base methyl orange is suitable as an indicator.
Statement II: For titration of acetic acid with NaOH phenolphthalein is not a suitable indicator. In the light of the above statements, choos …

The ${\mathrm{OH}}^{-}$ concentration in a mixture of 5.0 mL of $0.0504\mathrm{M}{\mathrm{NH}}_4\mathrm{Cl}$ and 2 mL of $0.0210\mathrm{M}{\mathrm{NH}}_3$ solution is $x\times 10^{-6}\mathrm{M}$. The value of $x$ is ______. (Nearest integer)
[Given …

The equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ at 298 K for the reaction
A + B ⇌ C + D
is 100. Starting with an equimolar solution with concentrations of $\mathrm{A},\mathrm{B},\mathrm{C}$ and D all equal to 1 M, the equilibrium concentration of D is $\_\_\_\_$ …

$2{\mathrm{SO}}_2(\mathrm{g})+{\mathrm{O}}_2(\mathrm{g})\rightleftharpoons 2{\mathrm{SO}}_3(\mathrm{g})$

In an equilibrium mixture, the partial pressures are
${\mathrm{P}}_{{\mathrm{SO}}_3}=43\mathrm{kPa};{\mathrm{P}}_{{\mathrm{O}}_2}=530\mathrm{Pa}$ and …

The solubility product of ${\mathrm{PbI}}_2$ is $8.0\times 10^{-9}$. The solubility of lead iodide in 0.1 molar solution of lead nitrate is $x\times 10^{-6}\mathrm{mol}/\mathrm{L}$. The value of x is $\_\_\_\_$ (Rounded off to the nearest integer) [Given $\sqrt{2}=1.41$ ]

A solution is 0.1 M in ${\mathrm{Cl}}^{-}$ and $0.001\mathrm{M}$ in ${\mathrm{CrO}}_4^{2-}$. Solid ${\mathrm{AgNO}}_3$ is gradually added to it. Assuming that the addition does not change in volume and ${\mathrm{K}}_{\mathrm{sp}}(\mathrm{AgCl})=1.7\times 10^{-10}{\mathrm{M}}^2$ an …

When 5.1 g of solid ${\mathrm{NH}}_4\mathrm{HS}$ is introduced into a two litre evacuated flask at $27^{\circ }\mathrm{C}$, 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The ${\mathrm{K}}_{\mathrm{p}}$ for the reaction at $27^{\circ }\mathrm{C}$ is x …

The solubility of AgCN in a buffer solution of $\mathrm{pH}=3$ is x . The value of x is :
[Assume : No cyano complex is formed ; ${\mathrm{K}}_{\mathrm{sp}}(\mathrm{AgCN})=2.2\times 10^{-16}$ and ${\mathrm{K}}_{\mathrm{a}}(\mathrm{HCN})=6.2\times 10^{-10}$ ]

Value of $K_p$ for the equilibrium reaction $\mathrm{N}{}_2\mathrm{O}{}_4(\mathrm{g})\rightleftharpoons 2\mathrm{NO}{}_2(\mathrm{g})$ at 288 K is 47.9. The $K_c$ for this reaction at same temperature is ______. (Nearest integer)
($R=0.083{\text{ L bar K}}^{-1}{\text{ mol}}^{-1}$)

A homogeneous ideal gaseous reaction ${\mathrm{AB}}_{2(\mathrm{g})}\rightleftharpoons {\mathrm{A}}_{(\mathrm{g})}+2{\mathrm{B}}_{(\mathrm{g})}$ is carried out in a 25 litre flask at $27^{\circ }\mathrm{C}$. The initial amount of $A{B}_2$ was 1 mole and the equilibrium pressure was …

The pH of ammonium phosphate solution, if ${\mathrm{pk}}_{\mathrm{a}}$ of phosphoric acid and ${\mathrm{pk}}_{\mathrm{b}}$ of ammonium hydroxide are 5.23 and 4.75 respectively, is ____

The pH of a solution obtained by mixing 50 mL of 1 M HCl and 30 mL of 1 M NaOH is $x\times 10^{-4}$. The value of $x$ is ____. (Nearest integer)
[log $2.5=0.3979$ ]

${\mathrm{A}}_3{\mathrm{B}}_2$ is a sparingly soluble salt of molar mass $\mathrm{M}\left(\mathrm{g}{\mathrm{mol}}^{-1}\right)$ and solubility $x\mathrm{g}{\mathrm{L}}^{-1}$. The solubility product satisfies $K_{sp}=a{\left(\frac{x}{M}\right)}^5$. The value of $a$ is ______. (In …

$\mathrm{PCl}{}_5\rightleftharpoons \mathrm{PCl}{}_3+\mathrm{Cl}{}_2$ $K_C=1.844$
3.0 moles of $\mathrm{PCl}{}_5$ is introduced in a 1 L closed reaction vessel at 380 K. The number of moles of $\mathrm{PCl}{}_5$ at equilibrium is ______ $\times 10^{-3}$. (Round off to the Nearest integer)

Which of the following compound CANNOT act as a Lewis base?

0.01 moles of a weak acid $\mathrm{HA}\left(\mathrm{Ka}=2.0\times 10^{-6}\right)$ is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is ____ $\times 10^{-5}$.
(Round off to the nearest integer).
[ Neglect volume change on adding HA.
Assume degr …

For the reaction
A + B ⇌ C
The value of equilibrium constant is 100 at 298 K. If the initial concentration of all the three species is 1 M each, then the equilibrium concentration of C is $x\times 10^{-1}\mathrm{M}$. The value of x is ______. (Nearest integer)

The equilibrium constant for the reaction
$\mathrm{A}(\mathrm{s})\rightleftharpoons \mathrm{M}(\mathrm{s})+\frac{1}{2}{\mathrm{O}}_2(\mathrm{g})$
In ${\mathrm{K}}_{\mathrm{p}}=4$. At equilibrium, the partial pressure of ${\mathrm{O}}_2$ is $\_\_\_\_$ atm.
(Round off to the Neare …

The molar solubility of $\mathrm{Zn}(\mathrm{OH}{)}_2$ in 0.1 M NaOH solution is $x\times 10^{-18}\mathrm{M}$. The value of $x$ is ____. (Nearest integer)
(Given : The solubility product of $\mathrm{Zn}(\mathrm{OH}{)}_2$ is $2\times 10^{-20}$ )

Two salts A₂X and MX have the same value of solubility product of 4.0 × 10⁻¹². The ratio of their molar solubilities i.e S(A₂X)/S(MX) = ____.
(Round off to the Nearest Integer).

For the reaction $\mathrm{A}(\mathrm{g})\rightleftharpoons \mathrm{B}(\mathrm{g})$ at $495\mathrm{K},{\Delta }_{\mathrm{r}}{\mathrm{G}}^{\circ }=-9.478\mathrm{kJ}{\mathrm{mol}}^{-1}$. If we start the reaction in a closed container at 495 K with 22 millimoles of A , the amoun …

The exact volumes of 1 M NaOH solution required to neutralize 50 mL of $1\mathrm{M}{\mathrm{H}}_3{\mathrm{PO}}_3$ solution and 100 mL of $2\mathrm{M}{\mathrm{H}}_3{\mathrm{PO}}_2$ solution respectively, are:

Sulphurous acid $\left({\mathrm{H}}_2{\mathrm{SO}}_3\right)$ has ${\mathrm{Ka}}_1=1.7\times 10^{-2}$ and ${\mathrm{Ka}}_2=6.4\times 10^{-8}$. The pH of $0.588\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_3$ is ______. (Round off to the nearest integer).

The solubility of ${\mathrm{CdSO}}_4$ in water is $8.0\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}$. Its solubility in $0.01\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_4$ solution is
______ $\times 10^{-6}\mathrm{mol}{\mathrm{L}}^{-1}$.
(Round off to the nearest integer).
(Assum …

Consider the reaction ${\mathrm{N}}_2{\mathrm{O}}_4(\mathrm{g})\rightleftharpoons 2{\mathrm{NO}}_2(\mathrm{g})$. The temperature at which ${\mathrm{K}}_{\mathrm{C}}=20.4$ and ${\mathrm{K}}_{\mathrm{p}}=600.1$, is ______ K. (Round off to the nearest integer).
[Assume all gase …

In order to prepare a buffer solution of pH 5.74 , sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0 M , the concentration of sodium acetate in the buffer is ______ M. (Round off to the nearest integer).
[Given: pKa (acetic acid) = 4 …

Assuming that Ba(OH)₂ is completely ionized in aqueous solution under the given conditions, the concentration of H₃O⁺ ions in 0.005 M aqueous solution of Ba(OH)₂ at 298 K is ______ × 10⁻¹² mol L⁻¹. (nearest integer)

Two solutions A and B, each of 100 L was made by dissolution of 4 g of NaOH and 9.8 g of ${\mathrm{H}}_2{\mathrm{SO}}_4$ in water, respectively. The pH of the resultant solution obtained from mixing 40 L of solution A and 10 L of solution B is

3 g of acetic acid is added to 250 mL of 0.1 M HCl and the solution made up to 500 mL. To 20 mL of this solution $\frac{1}{2}$ mL of 5 M NaOH is added. The pH of the solution is ______
[Given: ${\mathrm{pK}}_{\mathrm{a}}$ of acetic acid $=4.75$, molar mass of acetic acid …