Equilibrium — JEE Main PYQs

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively:

For the following Assertion and Reason, the correct option is :

Assertion : The pH of water increase with increase in temperature.
Reason : The dissociation of water into ${\mathrm{H}}^{+}$and ${\mathrm{OH}}^{-}$ is an exothermic reaction

The solubility product of $\mathrm{Cr}(\mathrm{OH}{)}_3$ at 298 K is $6.0\times 10^{-31}$. The concentration of hydroxide ions in a saturated solution of $\mathrm{Cr}(\mathrm{OH}{)}_3$ will be :

If the figure shown below reactant A (represented by square) is in equilibrium with product B (represented by circle). The equilibrium constant is:

The ${\mathrm{K}}_{\mathrm{sp}}$ for the following dissociation is $1.6\times 10^{-5}$


Which of the following choices is correct for a mixture of $300\mathrm{mL}$ …

For a reaction $X+Y=2Z$, $1.0\mathrm{mol}$ of $X$, $1.5\mathrm{mol}$ of $Y$ and $0.5\mathrm{mol}$ of $Z$ were taken in a $1\mathrm{L}$ vessel and allowed to react. At equilibrium, the concentration of $Z$ was $1.0\mathrm{mol}{\mathrm{L}}^{-1}$. The equilibrium constant of the re …

An acidic buffer is obtained on mixing:

The value of ${\mathrm{K}}_{\mathrm{C}}$ is 64 at 800 K for the reaction
${\mathrm{N}}_2(\mathrm{g})+3{\mathrm{H}}_2(\mathrm{g})\rightleftharpoons 2{\mathrm{NH}}_3(\mathrm{g})$
The value of ${\mathrm{K}}_{\mathrm{C}}$ for the following reaction is: …

If the solubility product of AB₂ is 3.20 × 10⁻¹¹ M³, then the solubility of AB₂ in pure water is _____ × 10⁻⁴ mol L⁻¹. [Assuming that neither kind of ion reacts with water]

Consider the following reaction:

For each of the following cases ( $\mathrm{a},\mathrm{b}$ ) the direction in which the equilibrium shifts is:
(a) Tem …

Arrange the following solutions in the decreasing order of pOH
(1) 0.01 M HCl
(2) 0.01 M NaOH
(3) $0.01\mathrm{M}{\mathrm{CH}}_3\mathrm{COONa}$
(4) 0.01 M NaCl

For the reaction
${\mathrm{Fe}}_2\mathrm{N}(\mathrm{s})+\frac{3}{2}{\mathrm{H}}_2(\mathrm{g})=2\mathrm{Fe}(\mathrm{s})+{\mathrm{NH}}_3(\mathrm{g})$

If the equilibrium constant for $\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$ is ${\mathrm{K}}_{(\mathrm{eq})}^{(1)}$ and that of $\mathrm{B}+\mathrm{C}\rightleftharpoons \mathrm{P}$ is ${\mathrm{K}}_{(\mathrm{eq})}^{(2)}$, the equilibrium constant for …

If solubility product of ${\mathrm{Zr}}_3({\mathrm{PO}}_4{)}_4$ is denoted by ${\mathrm{K}}_{\mathrm{SP}}$ and its molar solubility is denoted by S, then which of the following relation between S and ${\mathrm{K}}_{\mathrm{SP}}$ is correct?

For the following reactions, equilibrium constants are given:
$\mathrm{S}(\mathrm{s})+{\mathrm{O}}_2(\mathrm{g})\rightleftharpoons {\mathrm{SO}}_2(\mathrm{g});{\mathrm{K}}_1=10^{52}$ …

The values of ${\mathrm{K}}_{\mathrm{p}}/{\mathrm{K}}_{\mathrm{c}}$ for the following reactions at 300 K are respectively:
(At $300\mathrm{K},\mathrm{Rt}=24.62{\mathrm{dm}}^3\mathrm{atm}{\mathrm{mol}}^{-1}$ ) …

A mixture of 100 m mol of $\mathrm{Ca}(\mathrm{OH}{)}_2$ and 2 g of sodium sulphate was dissolved in water and the volume was made upto 100 mL . The mass of calcium sulphate formed and the concentration of ${\mathrm{OH}}^{-}$in resulting solution, respectively are
(Molar mass of …

What is the molar solubility of $\mathrm{Al}(\mathrm{OH}{)}_3$ in 0.2 M NaOH solution? Given that, solubility product of $\mathrm{Al}(\mathrm{OH}{)}_3=2.4\times 10^{-24}$ :

For the reaction,

${\Delta }_{\mathrm{H}}=-57.2\mathrm{kJ}{\mathrm{mol}}^{-1}$ and
${\mathrm{K}}_{\mathrm{C}}=1.7\times 10^{16}$
Which of the following statement is INCOR …

The pH of a $0.02\mathrm{M}{\mathrm{NH}}_4\mathrm{Cl}$ solution will be [given ${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=10^{-5}$ and $\log 2=0.301$ ]

Consider the reaction
${\mathrm{N}}_2(\mathrm{g})+3{\mathrm{H}}_2(\mathrm{g})\rightleftharpoons 2{\mathrm{NH}}_3(\mathrm{g})$
The equilibrium constant of the above reaction is ${\mathrm{K}}_3$. If pure ammonia is left to dissociate, the partial pressure of ammonia at equili …

In a chemical reaction $A+2B\rightleftharpoons 2C+D$, the initial concentration of $B$ was 1.5 times of A but the equilibrium concentrations of A and B were found to be equal. The equilibrium constant(K) for the aforesaid chemical reaction is

Two solids dissociate as follows
$\mathrm{A}(\mathrm{s})\rightleftharpoons \mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$; $K_{p_1}=x$ atm${}^2$
$\mathrm{D}(\mathrm{s})\rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{E}(\mathrm{g})$; $K_{p_2}=y$ atm${}^2$
The total pressure when both the solids dissociate simultaneously is

In which one of the following equilibria, ${\mathrm{K}}_{\mathrm{p}}\ne {\mathrm{K}}_{\mathrm{c}}$ ?

The molar solubility of $\mathrm{Cd}(\mathrm{OH}{)}_2$ is $1.84\times 10^{-5}\mathrm{M}$ in water. The expected solubility of $\mathrm{Cd}(\mathrm{OH}{)}_2$ in a buffer solution of $\mathrm{pH}=12$ is:

The decreasing order of electrical conductivity of the following aqueous solutions is:
0.1 M Formic acid (a)
0.1 M Acetic acid (b)
0.1 M Benzoic acid (c)

If ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{Ag}}_2{\mathrm{CO}}_3$ is $8\times 10^{-12}$, the molar solubility of ${\mathrm{Ag}}_2{\mathrm{CO}}_3$ in $0.1\mathrm{M}{\mathrm{AgNO}}_3$ is :

In an acid - base titration, 0.1 M HCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titration mixture in this experiment?

Consider the following reversible chemical reactions:


The relation between ${\mathrm{K}}_1$ and …

20 mL of $0.1\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_4$ is added to 30 mL of $0.2\mathrm{M}{\mathrm{NH}}_4\mathrm{OH}$ solution. The pH of the resultant mixture is [${\mathrm{pk}}_{\mathrm{b}}$ of ${\mathrm{NH}}_4\mathrm{OH}=4.7$]

Consider the following statements
(a) The pH of a mixture containing 400 mL of $0.1\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_4$ and 400 mL of 0.1 M NaOH will be approximately 1.3 .
(b) Ionic product of water is temperature dependent.
(c) A monobasic acid with …

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination ?
| (3) | Strong | S …

An aqueous solution contains an unknown concentration of ${\mathrm{Ba}}^{2+}$. When 50 mL of a 1 M solution of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is added, ${\mathrm{BaSO}}_4$ just begins to precipitate. The final volume is 500 mL . The solubility product of ${\mathrm{BaSO}}_4$ is …

An aqueous solution contains $0.10\mathrm{M}{\mathrm{H}}_2\mathrm{S}$ and 0.20 M HCl . If the equilibrium constants for the formation of ${\mathrm{HS}}^{-}$from ${\mathrm{H}}_2\mathrm{S}$ is $1.0\times 10^{-7}$ and that of ${\mathrm{S}}^{2-}$ from ${\mathrm{HS}}^{-}$ …

Which of the following salts is the most basic in aqueous solution?

$\mathrm{p}{K}_{\mathrm{a}}$ of a weak acid (HA) and $\mathrm{p}{K}_{\mathrm{b}}$ of a weak base $(\mathrm{BOH})$ are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

The equilibrium constant at 298 K for a reaction $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$ is 100 . If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in $\mathrm{mol}{\mathrm{L}}^{-1}$ ) will be:

The standard Gibbs energy change at 300 K for the reaction $2\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$ is 2494.2 J . At a given time, the composition of the reaction mixture is $[A]=\frac{1}{2},[B]=2$ and $[C]=\frac{1}{2}$. The reaction proceeds in the: [ …

For the reaction, ${\mathrm{SO}}_{2(\mathrm{g})}+\frac{1}{2}{\mathrm{O}}_{2(\mathrm{g})}\rightleftharpoons {\mathrm{SO}}_{3(\mathrm{g})}$, if ${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}(\mathrm{RT}{)}^{\mathrm{x}}$ where the symbols have usual meaning then the value of x is: (a …

How many litres of water must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2 ?

The equilibrium constant $({\mathrm{K}}_{\mathrm{C}})$ for the reaction ${\mathrm{N}}_2(\mathrm{g})+{\mathrm{O}}_2(\mathrm{g})\to 2\mathrm{NO}(\mathrm{g})$ at temperature T is $4\times 10^{-4}$. The value of ${\mathrm{K}}_{\mathrm{C}}$ for the reaction, …

The pH of a 0.1 molar solution of the acid HQ is 3 . The value of the ionization constant, Ka of this acid is :

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

Three reactions involving $\mathrm{H}{}_2\mathrm{PO}{}_4{}^{-}$ are given below:
(i) $\mathrm{H}{}_3\mathrm{PO}{}_4+\mathrm{H}{}_2\mathrm{O}\to \mathrm{H}{}_3\mathrm{O}{}^{+}+\mathrm{H}{}_2\mathrm{PO}{}_4{}^{-}$
(ii) $\mathrm{H}{}_2\mathrm{PO}{}_4{}^{-}+\mathrm{H}{}_2\mathrm{O}\to \mathrm{HPO}{}_4{}^{2-}+\mathrm{H}{}_3\mathrm{O}{}^{+}$
(iii) $\mathrm{H}{}_2\mathrm{PO}{}_4{}^{-}+\mathrm{OH}{}^{-}\to \mathrm{H}{}_3\mathrm{PO}{}_4+\mathrm{O}{}^{2-}$

In which of the above does $\mathrm{H}{}_2\mathrm{PO}{}_4{}^{-}$ act as an acid?

In aqueous solution the ionization constants for carbonic acid are
${\mathrm{K}}_1=4.2\times 10^{-7}$ and ${\mathrm{K}}_2=4.8\times 10^{-11}$
Select the correct statement for a saturated 0.034 M solution of the carbonic acid.

Solubility product of silver bromide is $5.0\times 10^{-13}$. The quantity of potassium bromide (molar mass taken as $120\mathrm{g}\mathrm{of}{\mathrm{mol}}^{-1}$) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is

At $25^{\circ }\mathrm{C}$, the solubility product of $\mathrm{Mg}(\mathrm{OH}{)}_2$ is $1.0\times 10^{-11}$. At which pH, will ${\mathrm{Mg}}^{2+}$ ions start precipitating in the form of $\mathrm{Mg}(\mathrm{OH}{)}_2$ from a solution of $0.001\mathrm{M}$ ${\mathrm{Mg}}^{2+}$ ions?

Solid $\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ is gradually dissolved in a $1.0\times 10^{-4}\mathrm{M}{\mathrm{Na}}_2{\mathrm{CO}}_3$ solution. At what concentration of ${\mathrm{Ba}}^{2+}$ will a precipitate begin to form? $({\mathrm{K}}_{\mathrm{sp}}$ …

The equilibrium constants $K_{P_1}$ and $K_{P_2}$ for the reactions $X\rightleftharpoons 2Y$ and $Z\rightleftharpoons P+Q$, respectively are in the ratio of $1:9$. If the degree of dissociation of $X$ and $Z$ be equal then the ratio of total pressure at these equilibria i …

For the following three reactions $\mathrm{a},\mathrm{b}$ and c , equilibrium constants are given:
a. $\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2(\mathrm{g});{\mathrm{K}}_1$
b. …