Equilibrium — JEE Main PYQs

The first and second ionization constants of ${\mathrm{H}}_2\mathrm{X}$ are $2.5\times 10^{-8}$ and $1.0\times 10^{-13}$ respectively. The concentration of ${\mathrm{X}}^{2-}$ in $0.1\mathrm{M}$ ${\mathrm{H}}_2\mathrm{X}$ solution is $\_\_\_\_$ $\times 10^{-15}\mathrm{M}$. (N …

Which of the following mixture gives a buffer solution with $\mathrm{pH}=9.25$ ?
Given : ${\mathrm{pK}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=4.75$

Consider the general reaction given below at 400 K

The values of $K_p$ and $K_c$ are studied under the same condition of temperature but variation in x and y.
(i) $K_p=85.87$ and $K_c=2.586$ appropriate units
(ii) $K_p=0.862$ and …

For the following gas phase equilibrium reaction at constant temperature,

If the total pressure is $\sqrt{3}$ atm and the pressure equilibrium constant ($K_p$) is 9 atm, then the degree of dissociation is given as …

${\mathrm{X}}_2(\mathrm{g})+{\mathrm{Y}}_2(\mathrm{g})\rightleftharpoons 2\mathrm{Z}(\mathrm{g})$
${\mathrm{X}}_2(\mathrm{g})$ and ${\mathrm{Y}}_2(\mathrm{g})$ are added to a 1 L flask and it is found that the system attains the above equilibrium at …

Consider three metal chlorides $\mathrm{x},\mathrm{y}$ and z , where x is water soluble at room temperature, $y$ is sparingly soluble in water at room temperature and z is soluble in hot water. $\mathrm{x},\mathrm{y}$ and z are respectively

Consider two Group IV metal ions ${\mathrm{X}}^{2+}$ and ${\mathrm{Y}}^{2+}$.

A solution containing $0.01{\mathrm{MX}}^{2+}$ and $0.01{\mathrm{MY}}^{2+}$ is saturated with ${\mathrm{H}}_2\mathrm{S}$. The pH at which the metal sulphide YS will form as a precipitate is ______
(Nearest …

Consider the following gaseous equilibrium in a closed container of volume "V" at T(K).
${\mathrm{P}}_2(\mathrm{g})+{\mathrm{Q}}_2(\mathrm{g})\rightleftharpoons 2\mathrm{PQ}(\mathrm{g})$
2 moles each of ${\mathrm{P}}_2(\mathrm{g}),{\mathrm{Q}}_2(\mathrm{g})$ and …

Consider a weak base ' B ' of ${\mathrm{pK}}_{\mathrm{b}}=5.699$. ' x ' mL of 0.02 M HCl and ' y ' mL of 0.02 M weak base ' B ' are mixed to make 100 mL of a buffer of pH 9 at $25^{\circ }\mathrm{C}$. The values of ' $x$ ' and ' $y$ ' respectively are:
[Given: …

Consider the dissociation equilibrium of the following weak acid $\mathrm{HA}\rightleftharpoons {\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{A}}^{-}(\mathrm{aq})$
If the pKa of the acid is 4, then the pH of 10 mM HA solution is ______. (Nearest integer)
[Given : The degree of dissociati …

Observe the following equilibrium in a 1 L flask.


At $\mathrm{T}(\mathrm{K})$, the equilibrium concentrations of A and B are 0.5 M and 0.375 M respectively. 0.1 moles of A is added into the flask and heated to $\mathrm{T}(\mathrm{K})$ to es …

The solubility product constants of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ and AgBr are 32 x and 4 y respectively at 298 K.

The value of $\left(\frac{\text{molarity of }{\mathrm{Ag}}_2{\mathrm{CrO}}_4}{\text{molarity of }\mathrm{AgBr}}\right)$ can be expressed as :

At $T(K)$, the equilibrium constant of $\mathrm{A}{}_2(\mathrm{g})+\mathrm{B}{}_2(\mathrm{g})\rightleftharpoons \mathrm{C}(\mathrm{g})$ is $2.7\times 10^{-5}$.

What is the equilibrium constant for
$\frac{1}{3}\mathrm{A}{}_2(\mathrm{g})+\frac{1}{3}\mathrm{B}{}_2(\mathrm{g})\rightleftharpoons \frac{1}{3}\mathrm{C}(\mathrm{g})$ at the same temperature?

The pH a solution obtained by mixing 5 mL of $0.1\mathrm{M}$ ${\mathrm{NH}}_4\mathrm{OH}$ solution with 250 mL of 0.1 M ${\mathrm{NH}}_4\mathrm{Cl}$ solution is ______ $\times 10^{-2}$. (Nearest integer)

Given : …

The first and second ionization constants of a weak dibasic acid $\mathrm{H}{}_2\mathrm{A}$ are $8.1\times 10^{-8}$ and $1.0\times 10^{-13}$ respectively. 0.1 mol of $\mathrm{H}{}_2\mathrm{A}$ was dissolved in 1L of 0.1 M HCl solution. The concentration of $\mathrm{HA}{}^{-}$ in the resultant solution is:

At $25^{\circ }\mathrm{C}$, 20.0 mL of 0.2 M weak monoprotic acid HX is titrated against 0.2 M NaOH. The pH of the solution (a) at the start of the titration (when NaOH has not been added) and (b) when 10 mL of NaOH is added respectively, are:

Given: $K_a=5\times 10^{-4}$, …

20 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M NaOH solution. What is the pH of the solution (X)? (pKₐ value of acetic acid is 4.75).

${\mathrm{M}}_3{\mathrm{A}}_2$ is a sparingly soluble salt of molar mass y $\mathrm{g}{\mathrm{mol}}^{-1}$ and solubility $\times \mathrm{g}{\mathrm{L}}^{-1}$. The ratio of the molar concentration of the anion ( ${\mathrm{A}}^{3-}$ ) to the solubility product of the salt i …

Arrange the following resultant mixtures in increasing order of their pH values
A. $10\mathrm{mL}0.2\mathrm{M}\mathrm{Ca}(\mathrm{OH}{)}_2+25\mathrm{mL}0.1\mathrm{M}\mathrm{HCl}$
B. …

The reaction $\mathrm{A}(\mathrm{g})\rightleftharpoons \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$ was initiated with the amount ' a ' of $\mathrm{A}(\mathrm{g})$. At equilibrium it is found that the amount of $\mathrm{A}(\mathrm{g})$ remaining is …

One mole each of He and $\mathrm{A}(\mathrm{g})$ are taken in a 10 L closed flask and heated to 400 K to establish the following equilibrium.
$\mathrm{A}(\mathrm{g})\rightleftharpoons \mathrm{B}(\mathrm{g})$
${\mathrm{K}}_{\mathrm{C}}$ for this reaction at 400 K is 4.0. The partia …

Given is a concentrated solution of a weak electrolyte ${\mathrm{A}}_{\mathrm{x}}{\mathrm{B}}_{\mathrm{y}}$ of concentration ' c ' and dissociation constant ' K '. the degree of dissociation is given by:

Consider the following reactions in which all the reactants and products are present in gaseous state
$2\mathrm{xy}\rightleftharpoons {\mathrm{x}}_2+{\mathrm{y}}_2$ ${\mathrm{K}}_1=2.5\times 10^5$
$\mathrm{xy}+\frac{1}{2}{\mathrm{z}}_2\rightleftharpoons \mathrm{xyz}$ …

Solid carbon, CaO and ${\mathrm{CaCO}}_3$ are mixed and allowed to attain equilibrium at T K.

${\mathrm{CaCO}}_3\rightleftharpoons \mathrm{CaO}(\mathrm{s})+{\mathrm{CO}}_2(\mathrm{g})$ $K_{p_1}=0.08$ atm …

A vessel at 1000 K contains ${\mathrm{CO}}_2$ with a pressure of 0.5 atm. Some of ${\mathrm{CO}}_2$ is converted into CO on addition of graphite. If total pressure at equilibrium is 0.8 atm, then ${\mathrm{K}}_{\mathrm{p}}$ is :

The molar solubility(s) of zirconium phosphate with molecular formula ${\left({\mathrm{Zr}}^{4+}\right)}_3{\left({\mathrm{PO}}_4^{3-}\right)}_4$ is given by relation :

Ksp for $\mathrm{Cr}(\mathrm{OH}{)}_3$ is $1.6\times 10^{-30}$. What is the molar solubility of this salt in water?

$37.8\mathrm{g}{\mathrm{N}}_2{\mathrm{O}}_5$ was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K $2{\mathrm{N}}_2{\mathrm{O}}_{5(\mathrm{g})}\to 2{\mathrm{N}}_2{\mathrm{O}}_{4(\mathrm{g})}+{\mathrm{O}}_{2(\mathrm{g})}$

T …

Which of the following happens when ${\mathrm{NH}}_4\mathrm{OH}$ is added gradually to the solution containing $1\mathrm{M}{\mathrm{A}}^{2+}$ and $1\mathrm{M}{\mathrm{B}}^{3+}$ ions?

Given : …

If 1 mM solution of ethylamine produces $\mathrm{pH}=9$, then the ionization constant $\left({\mathrm{K}}_{\mathrm{b}}\right)$ of ethylamine is $10^{-x}$. The value of $x$ is ____ (nearest integer). [The degree of ionization of ethylamine can be neglected with respect t …

A weak acid HA has degree of dissociation x. Which option gives the correct expression of $\mathrm{pH}={\mathrm{pK}}_{\mathrm{a}}$ ) ?

Ice and water are placed in a closed container at a pressure of 1 atm and temperature 273.15 K . If pressure of the system is increased 2 times, keeping temperature constant, then identify correct observation from following :

Consider the reaction

The equation representing correct relationship between the degree of dissociation (x) of ${\mathrm{X}}_2\mathrm{Y}(\mathrm{g})$ with …

pH of water is 7 at $25^{\circ }\mathrm{C}$. If water is heated to $80^{\circ }\mathrm{C}$, it's pH will :

Arrange the following in increasing order of solubility product :
$\mathrm{Ca}(\mathrm{OH}{)}_2,\mathrm{AgBr},\mathrm{PbS},\mathrm{HgS}$

At temperature T, compound ${\mathrm{AB}}_{2(\mathrm{g})}$ dissociates as ${\mathrm{AB}}_{2(\mathrm{g})}\rightleftharpoons {\mathrm{AB}}_{(\mathrm{g})}+\frac{1}{2}{\mathrm{B}}_{2(\mathrm{g})}$ having degree of dissociation x (small compared to unity). The correct expression for …

Consider the equilibrium
$\mathrm{CO}(\mathrm{g})+3{\mathrm{H}}_2(\mathrm{g})\rightleftharpoons {\mathrm{CH}}_4(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})$
If the pressure applied over the system increases by two fold at constant temperature then
(A) Concentration of …

If equal volumes of $\mathrm{AB}{}_2$ and XY (both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of $\mathrm{AY}{}_2$ at 300 K?
(Given $K_{sp}$ (at 300 K) for $\mathrm{AY}{}_2=5.2\times 10^{-7}$)

Consider the following equilibrium,
$\mathrm{CO}(\mathrm{g})+2{\mathrm{H}}_2(\mathrm{g})\rightleftharpoons {\mathrm{CH}}_3\mathrm{OH}(\mathrm{g})$
0.1 mol of CO along with a catalyst is present in a $2{\mathrm{dm}}^3$ flask maintained at 500 K . Hydrogen is introduced into t …

Consider the following chemical equilibrium of the gas phase reaction at a constant temperature : $\mathrm{A}(\mathrm{g})\rightleftharpoons \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$

If p being the total pressure, ${\mathrm{K}}_{\mathrm{p}}$ is the pressure equilibrium co …

Given below are two statements

Statement I : A catalyst cannot alter the equilibrium constant ( ${\mathrm{K}}_{\mathrm{c}}$ ) of the reaction, temperature remaining constant
Statement II : A homogenous catalyst can change the equilibrium composition of a system temperature remaini …

In the following system,
${\mathrm{PCl}}_5(\mathrm{g})\rightleftharpoons {\mathrm{PCl}}_3(\mathrm{g})+{\mathrm{Cl}}_2(\mathrm{g})$ at equilibrium, upon addition of xenon gas at constant $T\&p$, the concentration of

$x$ mg of $\mathrm{Mg}(\mathrm{OH}{)}_2$ (molar mass $=58$) is required to be dissolved in 1.0 L of water to produce a pH of 10.0 at 298 K. The value of x is ______ mg. (Nearest integer)
(Given: $\mathrm{Mg}(\mathrm{OH}{)}_2$ is assumed to dissociate completely in …

The pH of a 0.01 M weak acid HX (Kₐ = 4 × 10⁻¹⁰) is found to be 5. Now the acid solution is diluted with excess of water so that the pH of the solution changes to 6. The new concentration of the diluted weak acid is given as x × 10⁻⁴ M. The value of x is ____ (nearest integer)

Only litre buffer solution was prepared by adding 0.10 mol each of ${\mathrm{NH}}_3$ and ${\mathrm{NH}}_4\mathrm{Cl}$ in deionised water. The change in pH on addition of 0.05 mol of HCl to the above solution is $\_\_\_\_$ $\times 10^{-2}$,(Nearest integer)
(Given : …

An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would

(Given $\log 2=0.30$ )

The equilibrium constant for decomposition of ${\mathrm{H}}_2\mathrm{O}(\mathrm{g})$

${\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{H}}_2(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_2(\mathrm{g})$ ($\Delta G^{\circ }=92.34$ kJ mol⁻¹) is $8.0\times 10^{-3}$ at 2300 K and tot …

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), the attainment of equilibrium is predicted correctly by: [molar concentration vs time graph options in source]

What will be the decreasing order of basic strength of the following conjugate bases?
${}^{-}\mathrm{OH},\mathrm{R}\overline{\mathrm{O}},{\mathrm{CH}}_3\mathrm{CO}\overline{\mathrm{O}},\mathrm{C}\overline{\mathrm{l}}$

The equilibrium constant for the reaction
${\mathrm{SO}}_3(\mathrm{g})\rightleftharpoons {\mathrm{SO}}_2(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_2(\mathrm{g})$ is ${\mathrm{K}}_{\mathrm{C}}=4.9\times 10^{-2}$. The value of ${\mathrm{K}}_{\mathrm{C}}$ for the reaction given be …