How many questions from Equilibrium appear in JEE?

Equilibrium has appeared in 163 of the last 186 JEE Main and JEE Advanced papers — about 88% of them — contributing 199 questions in total across those papers.

Is Equilibrium an important chapter for JEE?

Judged by how often it is actually tested, it appears in roughly 88% of papers. Chapters above about 50% are effectively guaranteed to show up every session, so they repay thorough preparation; lower-frequency chapters are better treated as targeted revision.

Where do these Equilibrium questions come from?

Every question is from an official JEE Main or JEE Advanced paper, transcribed from the original paper and tagged to this chapter. Answers follow the official answer key.

Equilibrium JEE Previous Year Questions with Answers

Q1·ChemistrySingle correctJEE Main 2026

Consider the following reactions in which all the reactants and products are present in gaseous state

2xy \rightleftharpoons x_2 + y_2

K_1 = 2.5 \times 10^5

xy + \frac{1}{2}z_2 \rightleftharpoons xyz

K_2 = 5 \times 10^{-3}

The value of

K_3

for the equilibrium

\frac{1}{2}x_2 + \frac{1}{2}y_2 + \frac{1}{2}z_2 \rightleftharpoons xyz

is:

(A) $2.5 \times 10^{-3}$
(B) $2.5 \times 10^{3}$
(C) $1.0 \times 10^{-5}$
(D) $5 \times 10^{-3}$

Q2·ChemistryNumericalJEE Main 2026

Solid carbon, CaO and

CaCO_3

are mixed and allowed to attain equilibrium at T K.

CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)

K_{p_1} = 0.08

atm

C(s) + CO_2(g) \rightleftharpoons 2CO(g)

K_{p_2} = 2

atm The partial pressure of CO is __________

\times 10^{-1}

atm

Q3·ChemistrySingle correctJEE Main 2026

One mole each of He and A(g) are taken in a 10 L closed flask and heated to 400 K to establish the following equilibrium. A(g) ⇌ B(g).

K_c

for this reaction at 400 K is 4.0. The partial pressures (in atm) of He and B(g) are respectively (at equilibrium) (Assume He, A(g) and B(g) behave as ideal gases) (Given: R = 0.082 L atm K⁻¹ mol⁻¹)

(A)3.28, 2.624
(B)2.624, 3.28
(C)3.28, 0.656
(D)0.656, 6.56

Q4·ChemistryNumericalJEE Main 2026

In a closed flask at 600 K, one mole of

\mathrm{X_{2}Y_{4}(g)}

attains equilibrium as given below :

\mathrm{X_{2}Y_{4}}(g) \rightleftharpoons 2\mathrm{XY_{2}}(g)

At equilibrium, 75%

\mathrm{X_{2}Y_{4}(g)}

was dissociated and the total pressure is 1 atm. The magnitude of

\Delta_{r}G^{\ominus}

(in kJ mol

^{-1}

) at this temperature is __________. (Nearest Integer) (Given : R = 8.3 J mol

^{-1}

K

^{-1}

; ln 10 = 2.3, log 2 = 0.3, log 3 = 0.48, log 5 = 0.69, log 7 = 0.84)

Q5·ChemistrySingle correctJEE Main 2026

Given is a concentrated solution of a weak electrolyte

A_{x}B_{y}

of concentration 'c' and dissociation constant 'K'. The degree of dissociation is given by :

(A) $\left[K \times c^{x+y-1} x^{x} y^{y}\right]^{x+y}$
(B) $\left(\frac{K}{c^{x+y-1} x^{x} y^{y}}\right)^{\frac{1}{x+y}}$
(C) $\left(\frac{c^{x+y-1} x^{x} y^{y}}{K}\right)^{x+y}$
(D) $\left(\frac{c^{x+y-1} x^{x} y^{y}}{K}\right)^{\frac{1}{x+y}}$

Q6·ChemistrySingle correctJEE Main 2026

M_3A_2

is a sparingly soluble salt of molar mass

y

g mol

^{-1}

and solubility

x

g L

^{-1}

. The ratio of the molar concentration of the anion (

A^{3-}

) to the solubility product of the salt is

(A) $\frac{1}{54} \cdot \frac{y^4}{x^4}$
(B) $\frac{y^5}{108x^4}$
(C) $108 \cdot \frac{x^5}{y^5}$
(D) $\frac{1}{108} \cdot \frac{y^4}{x^4}$

Q7·ChemistrySingle correctJEE Main 2026

Arrange the following resultant mixtures in increasing order of their pH values A. 10 mL 0.2 M Ca(OH)

_2

+ 25 mL 0.1 M HCl B. 10 mL 0.01 M H

_2

SO

_4

+ 10 mL 0.01 M Ca(OH)

_2

C. 10 mL 0.1 M H

_2

SO

_4

+ 10 mL 0.1 M KOH Choose the correct answer from the options given below:

(A) $B < C < A$
(B) $C < A < B$
(C) $C < B < A$
(D) $A < C < B$

Q8·ChemistrySingle correctJEE Main 2026

The reaction A(g) ⇌ B(g) + C(g) was initiated with the amount 'a' of A(g). At equilibrium it is found that the amount of A(g) remaining is (a − x) at a total pressure of p. The equilibrium constant

K_p

of the reaction can be calculated from the expression :

(A) $\frac{x^{2}}{a^{2} + x^{2}} \times p$
(B) $\frac{x^{2}}{a^{2} - x^{2}} \times p$
(C) $\frac{a + x^{2}}{x^{2}} \times p$
(D) $\frac{a^{2} - x^{2}}{x^{2}} \times p$

Q9·ChemistryNumericalJEE Main 2026

The values of pressure equilibrium constant recorded at different temperatures for the following equilibrium reaction have been given below

A(g) \rightleftharpoons B(g) + C(g)

The magnitude of

\frac{\Delta H^\circ}{R}

calculated from the above data is _____. (Nearest integer)

$\frac{1}{T}$ (K $^{-1}$ )	$\log_{10} K_p$
0.05	3.5
0.06	2.5
0.07	1.5

Q10·ChemistryNumericalJEE Main 2026

For the following reaction at 50 °C and at 2 atm pressure,

2\mathrm{N_{2}O_{5}}(g) \rightleftharpoons 2\mathrm{N_{2}O_{4}}(g) + \mathrm{O_{2}}(g)

\mathrm{N_{2}O_{5}}

is 50% dissociated. The magnitude of standard free energy change at this temperature is

x

.

x

= ______ J mol

^{-1}

[Nearest integer]. Given:

R

= 8.314 J mol

^{-1}

K

^{-1}

, log 2 = 0.30, log 3 = 0.48, ln 10 = 2.303, °C + 273 = K

Q11·ChemistrySingle correctJEE Main 2026

At

T(K)

, the equilibrium constant of

A_2(g) + B_2(g) \rightleftharpoons C(g)

is

2.7 \times 10^{-5}

. What is the equilibrium constant for

\frac{1}{3}A_2(g) + \frac{1}{3}B_2(g) \rightleftharpoons \frac{1}{3}C(g)

at the same temperature?

(A) $(2.7 \times 10^{-5})^3$
(B) $6 \times 10^{-2}$
(C) $\sqrt{2.7 \times 10^{-5}}$
(D) $3 \times 10^{-2}$

Q12·ChemistrySingle correctJEE Main 2026

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)? (

pK_{a}

value of acetic acid is 4.75).

(A)7.0
(B)4.75
(C)3.5
(D)4.82

Q13·ChemistryNumericalJEE Main 2026

The pH of a solution obtained by mixing 5 mL of 0.1 M

NH_4OH

solution with 250 mL of 0.1 M

NH_4Cl

solution is _______

\times 10^{-2}

. (Nearest integer) Given:

pK_b(NH_4OH) = 4.74

\log 2 = 0.30

\log 3 = 0.48

\log 5 = 0.70

Q14·ChemistrySingle correctJEE Main 2026

At

25^{\circ}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}

,

pK_a = 3.3

,

\alpha << 1

(A)(a) 0.7 (b) 2.0
(B)(a) 2.0 (b) 3.3
(C)(a) 1.1 (b) 2.2
(D)(a) 3.0 (b) 2.2

Q15·ChemistrySingle correctJEE Main 2026

The first and second ionization constants of a weak dibasic acid

H_2A

are

8.1 \times 10^{-8}

and

1.0 \times 10^{-13}

respectively. 0.1 mol of

H_2A

was dissolved in 1 L of 0.1 M HCl solution. The concentration of

HA^-

in the resultant solution is:

(A)0.1 M
(B) $9.53 \times 10^{-6}$ M
(C) $8.1 \times 10^{-8}$ M
(D) $1.0 \times 10^{-13}$ M

Q16·ChemistrySingle correctJEE Main 2026

The solubility product constants of

\mathrm{Ag_{2}CrO_{4}}

and

\mathrm{AgBr}

are

32x

and

4y

respectively at 298 K. The value of

\left(\frac{\text{molarity of } \mathrm{Ag_{2}CrO_{4}}}{\text{molarity of } \mathrm{AgBr}}\right)

can be expressed as :

(A) $\frac{2\sqrt[3]{x}}{y}$
(B) $2\sqrt{\frac{x}{y}}$
(C) $\sqrt{\frac{x}{y}}$
(D) $\frac{\sqrt[3]{x}}{\sqrt{y}}$

Q17·ChemistrySingle correctJEE Main 2026

Consider a weak base 'B' of pK

_{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 25ºC. The values of 'x' and 'y' respectively are: [Given: log 2 = 0.3010, log 3 = 0.4771, log 5 = 0.699]

(A)x | y 11.1 | 88.9
(B)x | y 42.7 | 57.3
(C)x | y 14.3 | 85.7
(D)x | y 85.7 | 14.3

Q18·ChemistryNumericalJEE Main 2026

Consider the dissociation equilibrium of the following weak acid HA

\rightleftharpoons

H

^{+}

(aq)

+

A

^{-}

(aq) If the pKa of the acid is 4, then the pH of 10 mM HA solution is ________. (Nearest integer) [Given : The degree of dissociation can be neglected with respect to unity]

Q19·ChemistrySingle correctJEE Main 2026

Observe the following equilibrium in a 1 L flask.

A(g) \rightleftharpoons B(g)

At T(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 T(K) to establish the equilibrium again. The new equilibrium concentrations (in M) of A and B are respectively.

(A)0.367, 0.275
(B)0.53, 0.4
(C)0.742, 0.557
(D)0.557, 0.418

Q20·ChemistrySingle correctJEE Main 2026

Consider the following gaseous equilibrium in a closed container of volume “V” at T(K).

\text{P}_{2}(\text{g}) + \text{Q}_{2}(\text{g}) \rightleftharpoons 2\text{PQ}(\text{g})

2 moles each of

\text{P}_{2}(\text{g})

,

\text{Q}_{2}(\text{g})

and PQ (g) are present at equilibrium. Now one mole each of ‘

\text{P}_{2}

’ and ‘

\text{Q}_{2}

’ are added to the equilibrium keeping the temperature at T(K). The number of moles of

\text{P}_{2}

,

\text{Q}_{2}

and PQ at the new equilibrium, respectively , are -

(A)2.67, 2.67, 2.67
(B)1.21, 2.24, 1.56
(C)1.66, 1.66, 1.66
(D)2.56, 1.62, 2.24

Q21·ChemistryNumericalJEE Main 2026

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_2S}

. The pH at which the metal sulphide YS will form as a precipitate is ______ (Nearest integer) (Given :

\mathrm{K_{sp}\left(XS\right)=1\times10^{-22}}

at 25°C,

\mathrm{K_{sp}\left(YS\right)=4\times10^{-16}}

at 25°C,

\mathrm{[H_2S]}

= 0.1M in solution,

\mathrm{K_{a1} \times K_{a2}}

(

\mathrm{H_2S}

) =

1.0 \times 10^{-21}

, log 2 = 0.30, log 3 = 0.48, log 5 = 0.70)

Q22·ChemistrySingle correctJEE Main 2026

Consider the general reaction given below at 400 K xA(g) ⇌ yB(g) 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 K

_c

= 28.62 appropriate units The value of x and y in (i) and (ii) respectively are:

(A)(i) 3, 1 ; (ii) 3, 1
(B)(i) 4, 1 ; (ii) 4, 1
(C)(i) 1, 3 ; (ii) 2, 1
(D)(i) 1, 2 ; (ii) 2, 1

Q23·ChemistryNumericalJEE Main 2026

X

_{2}

(g) + Y

_{2}

(g) ⇌ 2Z(g) X

_{2}

(g) and Y

_{2}

(g) are added to a 1 L flask and it is found that the system attains the above equilibrium at T(K) with the number of moles of X

_{2}

(g) , Y

_{2}

(g) and Z(g) being 3, 3 and 9 mol respectively (equilibrium moles). Under this conditions of equilibrium, 10 mol of Z(g) is added to the flask and the temperature is maintained at T(K). Then the number of moles of Z(g) in the flask when the new equilibrium is established is ______. (Nearest integer).

Q24·ChemistryNumericalJEE Main 2026

For the following gas phase equilibrium reaction at constant temperature, NH

_3

(g) ⇌

\frac{1}{2}

N

_2

(g) +

\frac{3}{2}

H

_2

(g) 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

(x \times 10^{-2})^{-1/2}

. The value of x is ______ (Nearest integer)

Q25·ChemistryNumericalJEE Main 2026

Dissociation of a gas A

_2

takes place according to the following chemical reactions. At equilibrium, the total pressure is 1 bar at 300K. A

_2

(g) ⇌ 2A(g) The standard Gibbs energy of formation of the involved substances has been provided below: Substance |

\Delta G_f^{\circ}

/ kJ mol

^{-1}

A

_2

| −100.00 A | −50.832 The degree of dissociation of A

_2

(g) is given by (x × 10

^{-2}

)

^{1/2}

where x = __________. (Nearest integer). [Given : R = 8 J mol

^{-1}

K

^{-1}

, log 2 = 0.3010, log 3 = 0.48]

Q26·ChemistrySingle correctJEE Main 2026

Which of the following mixture gives a buffer solution with pH = 9.25 ? Given :

pK_b

(

NH_4OH

) = 4.75

(A)0.2M $NH_4OH$ (0.4 L) + 0.1M HCl (1L)
(B)0.2M $NH_4OH$ (0.5 L) + 0.1M HCl (0.5 L)
(C)0.5M $NH_4OH$ (0.2 L) + 0.2M HCl (0.5 L)
(D)0.4M $NH_4OH$ (1 L) + 0.1M HCl (1L)

Q27·ChemistryNumericalJEE Main 2026

The first and second ionization constants of

\text{H}_{2}\text{X}

are

2.5 \times 10^{-8}

and

1.0 \times 10^{-13}

respectively. The concentration of

\text{X}^{2-}

in 0.1 M

\text{H}_{2}\text{X}

solution is _______

\times 10^{-15}

M. (Nearest Integer)

Q28·ChemistryNumericalJEE Advanced 2025

At 25°C, the concentration of

H^+

ions in

1.00 \times 10^{-3}

M aqueous solution of a weak monobasic acid having acid dissociation constant

(K_a)

of

4.00 \times 10^{-11}

is

X \times 10^{-7}

M. The value of X is ______. Use: Ionic product of water

(K_w) = 1.00 \times 10^{-14}

at 25°C.

Q29·ChemistryNumericalJEE Advanced 2025

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 X

\times

10

^{-6}

mol dm

^{-3}

. The value of X is _____. Use: Solubility product constant (

K_{sp}

) of barium iodate = 1.58

\times

10

^{-9}

.

Q30·ChemistryIntegerJEE Main 2025

The equilibrium constant for decomposition of

H_2O(g)

\left(H_2O(g)\rightleftharpoons H_2(g)+\dfrac{1}{2}O_2(g),\ \Delta G^\circ=92.34\ kJ\,mol^{-1}\right)

is

8.0\times10^{-3}

at 2300 K and total pressure at equilibrium is 1 bar. Under this condition, the degree of dissociation (

\alpha

) of water is ___

\times10^{-2}

(nearest integer value). [Assume

\alpha

is negligible with respect to 1]

Q31·ChemistryIntegerJEE Main 2025

One litre buffer solution was prepared by adding 0.10 mol each of

NH_3

and

NH_4Cl

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:

pK_b

of

NH_3=4.745

and

\log_{10}3=0.477

)

Q32·ChemistrySingle correctJEE Main 2025

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

)

(A)reduce to 0.5
(B)increase to 1.3
(C)remain same
(D)increase to 2

Q33·ChemistryIntegerJEE Main 2025

The pH of a 0.01 M weak acid HX (

K_a=4\times10^{-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\times10^{-4}

M. The value of

x

is ______ (nearest integer).

Q34·ChemistryIntegerJEE Main 2025

x mg of

Mg(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:

Mg(OH)_2

is assumed to dissociate completely in

H_2O

)

Q35·ChemistrySingle correctJEE Main 2025

In the following system,

PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)

at equilibrium, upon addition of xenon gas at constant T \& p, the concentration of:

(A) $PCl_5$ will increase
(B) $Cl_2$ will decrease
(C) $PCl_5$ , $PCl_3$ \& $Cl_2$ remain constant
(D) $PCl_3$ will increase

Q36·ChemistrySingle correctJEE Main 2025

Given below are two statements. Statement I: A catalyst cannot alter the equilibrium constant

(K_{eq})

of a reaction, temperature remaining constant. Statement II: A homogenous catalyst can change the equilibrium composition of a system, temperature remaining constant. In the light of the above statements, choose the correct answer from the options given below:

(A)Statement I is false but Statement II is true
(B)Both Statement I and Statement II are true
(C)Both Statement I and Statement II are false
(D)Statement I is true but Statement II is false

Q37·ChemistrySingle correctJEE Main 2025

If equal volumes of

AB_2

and

XY

(both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of

AY_2

at 300 K? (Given

K_{sp}

at 300 K for

AY_2=5.2\times10^{-5}

)

(A) $3.6\times10^{-3}$ M $AB_2$ , $5.0\times10^{-4}$ M $XY$
(B) $2.0\times10^{-4}$ M $AB_2$ , $0.8\times10^{-4}$ M $XY$
(C) $2.0\times10^{-2}$ M $AB_2$ , $2.0\times10^{-2}$ M $XY$
(D) $1.5\times10^{-4}$ M $AB_2$ , $1.5\times10^{-3}$ M $XY$

Q38·ChemistrySingle correctJEE Main 2025

Consider the following chemical equilibrium of the gas phase reaction at a constant temperature:

A(g)\rightleftharpoons B(g)+C(g)

. If

p

being the total pressure,

K_p

is the pressure equilibrium constant and

\alpha

is the degree of dissociation, then which of the following is true at equilibrium?

(A)If $p$ value is extremely high compared to $K_p$ , $\alpha\approx1$
(B)When $p$ increases $\alpha$ decreases
(C)If $K_p$ value is extremely high compared to $p$ , $\alpha$ becomes much less than unity
(D)When $p$ increases $\alpha$ increases

Q39·ChemistryIntegerJEE Main 2025

Consider the following equilibrium,

CO(g)+2H_2(g)\rightleftharpoons CH_3OH(g)

. 0.1 mol of CO along with a catalyst is present in a 2 dm

^3

flask maintained at 500 K. Hydrogen is introduced into the flask until the pressure is 5 bar and 0.04 mol of

CH_3OH

is formed. The

K_p^\circ

is ______

\times10^{-3}

(nearest integer). (Given

R=0.08

dm

^3

bar K

^{-1}

mol

^{-1}

; assume only methanol is formed and the system follows ideal gas behaviour.)

Q40·ChemistrySingle correctJEE Main 2025

Consider the equilibrium

CO(g)+3H_2(g)\rightleftharpoons CH_4(g)+H_2O(g)

. If the pressure applied over the system increases by two fold at constant temperature then (A) Concentration of reactants and products increases. (B) Equilibrium will shift in forward direction. (C) Equilibrium constant increases since concentration of products increases. (D) Equilibrium constant remains unchanged as concentration of reactants and products remain same. Choose the correct answer from the options given below:

(A)(A) and (B) only
(B)(A), (B) and (D) only
(C)(B) and (C) only
(D)(A), (B) and (C) only

Q41·ChemistrySingle correctJEE Main 2025

At temperature T, compound AB

_2

(g) dissociates as

AB_2(g)\rightleftharpoons AB(g)+\dfrac{1}{2}B_2(g)

having degree of dissociation x (small compared to unity). The correct expression for x in terms of

K_p

and p is:

(A) $\sqrt[3]{\dfrac{2K_p}{p}}$
(B) $\sqrt{\dfrac{2K_p}{p}}$
(C) $\sqrt[3]{\dfrac{2K_p^2}{p}}$
(D) $\sqrt{K_p}$

Q42·ChemistrySingle correctJEE Main 2025

A weak acid HA has degree of dissociation x. Which option gives the correct expression of

pH=pK_a

?

(A) $\log(1+2x)$
(B) $\log\left(\frac{1-x}{x}\right)$
(C)0
(D) $\log\left(\frac{x}{1-x}\right)$

Q43·ChemistrySingle correctJEE Main 2025

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:

(A)Volume of system increases.
(B)Liquid phase disappears completely.
(C)The amount of ice decreases.
(D)The solid phase (ice) disappears completely.

Q44·ChemistrySingle correctJEE Main 2025

Arrange the following in increasing order of solubility product: Ca(OH)

_2

, AgBr, PbS, HgS.

(A)PbS < HgS < Ca(OH) $_2$ < AgBr
(B)HgS < PbS < AgBr < Ca(OH) $_2$
(C)Ca(OH) $_2$ < AgBr < HgS < PbS
(D)HgS < AgBr < PbS < Ca(OH) $_2$

Q45·ChemistryIntegerJEE Main 2025

37.8 g N₂O₅ was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K:

2N_2O_5(g)\to 2N_2O_4(g)+O_2(g)

. The total pressure at equilibrium was found to be 18.65 bar. Then,

K_p=

_______

\times10^{-2}

[nearest integer]. Assume N₂O₅ to behave ideally under these conditions. Given : R = 0.082 bar L mol⁻¹ K⁻¹

Q46·ChemistrySingle correctJEE Main 2025

For the reaction,

H_2(g) + I_2(g) \rightleftharpoons 2HI(g)

, the attainment of equilibrium is predicted correctly by:

(A)(1)
(B)(2)
(C)(3)
(D)(4)

Q47·ChemistrySingle correctJEE Main 2025

Ksp for Cr(OH)₃ is

1.6\times10^{-30}

. What is the molar solubility of this salt in water?

(A) $\sqrt[4]{\dfrac{1.6\times10^{-30}}{27}}$
(B) $1.8\times10^{-10}$
(C) $\sqrt[3]{1.8\times10^{-30}}$
(D) $\sqrt{1.6\times10^{-30}}$

Q48·ChemistrySingle correctJEE Main 2025

pH of water is 7 at

25^\circ

C. If water is heated to

80^\circ

C, it's pH will :

(A)Decrease
(B)Remains the same
(C) $H^+$ concentration increases, $OH^-$ concentration decreases
(D)Increase

Q49·ChemistryIntegerJEE Main 2025

If 1 mM solution of ethylamine produces pH = 9, then the ionization constant (

K_b

) of ethylamine is

10^{-x}

. The value of x is _______ (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]

Q50·ChemistrySingle correctJEE Main 2025

Which of the following happens when NH₄OH is added gradually to the solution containing 1M A³⁺ and 1M B³⁺ ions ? Given :

K_{sp}[A(OH)_3]=9\times10^{-10}

and

K_{sp}[B(OH)_3]=27\times10^{-18}

at 298 K.

(A)B(OH)₃ will precipitate before A(OH)₃
(B)A(OH)₃ and B(OH)₃ will precipitate together
(C)A(OH)₃ will precipitate before B(OH)₃
(D)Both A(OH)₃ and B(OH)₃ do not show precipitation with NH₄OH

Q51·ChemistrySingle correctJEE Main 2025

Consider the reaction

X_2Y(g)\rightleftharpoons X_2(g)+\tfrac12 Y_2(g)

. The equation representing correct relationship between the degree of dissociation

(x)

of

X_2Y(g)

with its equilibrium constant

K_p

is __________. Assume

x

to be very very small.

(A) $x=\sqrt{\dfrac{2K_p}{p}}$
(B) $x=\sqrt[3]{\dfrac{2K_p^2}{p}}$
(C) $x=\sqrt{\dfrac{K_p}{2p}}$
(D) $x=\sqrt[3]{\dfrac{K_p}{p}}$

Q52·ChemistrySingle correctJEE Main 2025

The molar solubility(s) of zirconium phosphate with molecular formula

(Zr^{4+})_3(PO_4^{3-})_4

is given by relation:

(A) $\left(\frac{K_{sp}}{6912}\right)^{1/7}$
(B) $\left(\frac{K_{sp}}{5348}\right)^{1/6}$
(C) $\left(\frac{K_{sp}}{8435}\right)^{1/7}$
(D) $\left(\frac{K_{sp}}{9612}\right)^{1/3}$

Q53·ChemistrySingle correctJEE Main 2025

A vessel at 1000 K contains CO₂ at a pressure of 0.5 atm. Some of the CO₂ is converted into CO on addition of graphite. If the total pressure at equilibrium is 0.8 atm, then Kp is:

(A)0.18 atm
(B)1.8 atm
(C)0.3 atm
(D)3 atm

Q54·ChemistrySingle correctJEE Main 2024

For a sparingly soluble salt

AB_2

, the equilibrium concentrations of

A^{2+}

ions and

B^{-}

ions are

1.2\times10^{-4}

M and

0.24\times10^{-3}

M, respectively. The solubility product of

AB_2

is:

(A) $0.069\times10^{-12}$
(B) $6.91\times10^{-12}$
(C) $0.276\times10^{-12}$
(D) $27.65\times10^{-12}$

Q55·ChemistrySingle correctJEE Main 2024

Given below are two statements: Statement (I): A buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities. Statement (II): Blood is naturally occurring buffer solution whose pH is maintained by

\text{H}_2\text{CO}_3/\text{HCO}_3^-

concentrations. In the light of the above statements, choose the correct answer from the options given below.

(A)Statement I is false but Statement II is true
(B)Both Statement I and Statement II is true
(C)Both Statement I and Statement II is false
(D)Statement I is true but Statement II is false

Q56·ChemistrySingle correctJEE Main 2024

For the given hypothetical reactions, the equilibrium constants are as follows:

X\rightleftharpoons Y

;

K_1=1.0

;

Y\rightleftharpoons Z

;

K_2=2.0

;

Z\rightleftharpoons W

;

K_3=4.0

. The equilibrium constant for the reaction

X\rightleftharpoons W

is:

(A) $6.0$
(B) $12.0$
(C) $8.0$
(D) $7.0$

Q57·ChemistrySingle correctJEE Main 2024

At

-20\,^{\circ}

C and 1 atm pressure, a cylinder is filled with equal number of

H_2

,

I_2

and

HI

molecules for the reaction

H_2(g) + I_2(g) \rightleftharpoons 2HI(g)

. The

K_P

for the process is

x\times10^{-1}

. The value of

x

is: (Given:

R=0.082

L atm K

^{-1}

mol

^{-1}

)

(A)2
(B)1
(C)10
(D)0.01

Q58·ChemistrySingle correctJEE Main 2024

The ratio

\dfrac{K_P}{K_C}

for the reaction:

CO_{(g)} + \dfrac{1}{2}O_{2(g)} \rightleftharpoons CO_{2(g)}

is:

(A) $(RT)^{1/2}$
(B) $RT$
(C) $1$
(D) $\dfrac{1}{\sqrt{RT}}$

Q59·ChemistrySingle correctJEE Main 2024

The following reaction occurs in the blast furnace where iron ore is reduced to iron metal:

\text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 2\text{Fe}(l) + 3\text{CO}_2(g)

. Using Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium.

(A)Addition of $\text{Fe}_2\text{O}_3$
(B)Addition of $\text{CO}_2$
(C)Removal of CO
(D)Removal of $\text{CO}_2$

Q60·ChemistrySingle correctJEE Main 2024

The equilibrium constant for the reaction

\text{SO}_3(g)\rightleftharpoons\text{SO}_2(g)+\tfrac{1}{2}\text{O}_2(g)

is

K_C=4.9\times10^{-2}

. The value of

K_C

for the reaction

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

given below is

(A)4.9
(B)41.6
(C)49
(D)416

Q61·ChemistryNumericalJEE Main 2024

K_a

for

CH_3COOH

is

1.8\times10^{-5}

and

K_b

for

NH_4OH

is

1.8\times10^{-5}

. The pH of ammonium acetate solution will be ___

Q62·ChemistrySingle correctJEE Main 2024

Solubility of calcium phosphate (molecular mass, M) in water is

W_g

per 100 mL at

25^{\circ}

C. Its solubility product at

25^{\circ}

C will be approximately:

(A) $10^7\left(\dfrac{W}{M}\right)^3$
(B) $10^7\left(\dfrac{W}{M}\right)^5$
(C) $10^3\left(\dfrac{W}{M}\right)^5$
(D) $10^5\left(\dfrac{W}{M}\right)^5$

Q63·ChemistrySingle correctJEE Main 2024

A_{(g)}\rightleftharpoons B_{(g)}+\dfrac{C}{2}_{(g)}

. The correct relationship between

K_P

and equilibrium pressure P is

(A) $K_P=\dfrac{\alpha^{3/2}P^{1/2}}{(2+\alpha)^{1/2}}$
(B) $K_P=\dfrac{\alpha^{3/2}P^{1/2}}{(2+\alpha)^{1/2}(1-\alpha)}$
(C) $K_P=\dfrac{\alpha^{1/2}P^{3/2}}{(2+\alpha)^{3/2}}$
(D) $K_P=\dfrac{\alpha^{1/2}P^{1/2}}{(2+\alpha)^{3/2}}$

Q64·ChemistryNumericalJEE Main 2024

Consider the following reaction at 298 K.

\dfrac{3}{2}O_{2(g)}\rightleftharpoons O_{3(g)}

.

K_P=2.47\times10^{-29}

.

\Delta_r G^\ominus

for the reaction is ______ kJ. (Given R = 8.314 JK

^{-1}

mol

^{-1}

)

Q65·ChemistrySingle correctJEE Main 2024

For the given reaction, choose the correct expression of

K_C

from the following :-

Fe^{3+}_{(aq)}+SCN^-_{(aq)}\rightleftharpoons (FeSCN)^{2+}_{(aq)}

(A) $K_C=\dfrac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^-]}$
(B) $K_C=\dfrac{[Fe^{3+}][SCN^-]}{[FeSCN^{2+}]}$
(C) $K_C=\dfrac{[FeSCN^{2+}]}{[Fe^{3+}]^2[SCN^-]^2}$
(D) $K_C=\dfrac{[FeSCN^{2+}]^2}{[Fe^{3+}][SCN^-]}$

Q66·ChemistryNumericalJEE Main 2024

The pH at which

Mg(OH)_2

[K_{sp}=1\times10^{-11}]

begins to precipitate from a solution containing

0.10\,M

Mg^{2+}

ions is ___

Q67·ChemistryNumericalJEE Main 2024

The pH of an aqueous solution containing 1M benzoic acid (

pK_a=4.20

) and 1M sodium benzoate is 4.5. The volume of benzoic acid solution in 300 mL of this buffer solution is ______ mL.

Q68·ChemistryNumericalJEE Main 2024

For the reaction

N_2O_4(g)\rightleftharpoons 2NO_2(g)

,

K_p=0.492

atm at 300 K.

K_c

for the reaction at same temperature is ______

\times10^{-2}

. (Given : R = 0.082 L atm mol

^{-1}

K

^{-1}

)

Q69·ChemistryNumericalJEE Main 2024

The following concentrations were observed at 500 K for the formation of

NH_3

from

N_2

and

H_2

. At equilibrium

[N_2]=2\times10^{-2}

M,

[H_2]=3\times10^{-2}

M and

[NH_3]=1.5\times10^{-3}

M. Equilibrium constant for the reaction is ___

\times10^{-2}

.

Q70·ChemistrySingle correctJEE Main 2024

Given below are two statements: Statement (I): Aqueous solution of ammonium carbonate is basic. Statement (II): Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on

K_a

and

K_b

value of acid and the base forming it. In the light of the above statements, choose the most appropriate answer from the options given below:

(A)Both Statement I and Statement II are correct
(B)Statement I is correct but Statement II is incorrect
(C)Both Statement I and Statement II are incorrect
(D)Statement I is incorrect but Statement II is correct

Q71·ChemistrySingle correctJEE Advanced 2023

On decreasing the pH from 7 to 2, the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from

10^{-4}\ \mathrm{mol\ L^{-1}}

to

10^{-3}\ \mathrm{mol\ L^{-1}}

. The

\mathrm{pK_a}

of HX is

(A)3
(B)4
(C)5
(D)2

Q72·ChemistrySingle correctJEE Main 2023

Which of the following statement(s) is/are correct? (A) The pH of

1 \times 10^{-8}

M HCl solution is 8. (B) The conjugate base

H_2PO_4^-

is

HPO_4^{2-}

. (C)

K_w

increases with increase in temperature. (D) When a solution of weak monoprotic acid is titrated against a strong base at half neutralisation point,

pH = \frac{1}{2}pK_a

. Choose the correct answer from the option given below.

(A)(B), (C), (D)
(B)(A), (D)
(C)(A), (B), (C)
(D)(B), (C)

Q73·ChemistryNumericalJEE Main 2023

20 mL of 0.1 M NaOH is added to 50 mL of 0.1 M acetic acid solution. The pH of the resulting solution is ____

\times 10^{-2}

(Nearest integer). Given: pKa

(CH_3COOH) = 4.76

.

Q74·ChemistryNumericalJEE Main 2023

25.0\,mL

of

0.050\,M\,Ba(NO_{3})_{2}

is mixed with

25.0\,mL

of

0.020\,M\,NaF

.

K_{sp}

of

BaF_{2}

is

0.5\times10^{-6}

at

298\,K

. The ratio of

[Ba^{2+}][F^{-}]^{2}

and

K_{sp}

is _____ (Nearest integer).

Q75·ChemistryNumericalJEE Main 2023

An analyst wants to convert 1L HCl of pH = 1 to a solution of HCl at pH 2. The volume of water needed to do this dilution is _________ mL. (Nearest Integer)

Q76·ChemistryNumericalJEE Main 2023

One mole of an ideal gas at 350K is in a 2.0 L vessel of thermally conducting walls, which are in contact with the surroundings. It undergoes isothermal reversible expansion from 2.0L to 3.0L against a constant pressure of 4 atm. The change in entropy of the surroundings

(\Delta S)

is _________ J K

^{-1}

(Nearest integer). Given: R = 8.314 J K

^{-1}

mol

^{-1}

.

Q77·ChemistryNumericalJEE Main 2023

A mixture of 1 mole of

H_2O

and 1 mole of CO is taken in a 10 litre container and heated to 725 K. At equilibrium 40% of water by mass reacts with carbon monoxide according to the equation:

CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g)

. The equilibrium constant

K_C \times 10^2

for the reaction is __________. (Nearest integer)

Q78·ChemistryNumericalJEE Main 2023

4.5 moles each of hydrogen and iodine are heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for

H_2(g)+I_2(g)\rightleftharpoons 2HI(g)

is ____.

Q79·ChemistryNumericalJEE Main 2023

\text{A}(g)\rightleftharpoons 2\text{B}(g)+\text{C}(g)

. For the given reaction, if the initial pressure was

450

mm Hg and the pressure at time t is

720

mm Hg at constant temperature T and constant volume V, the fraction of

\text{A}(g)

decomposed under these conditions is

x\times10^{-1}

. The value of x is _______ (nearest integer).

Q80·ChemistryNumericalJEE Main 2023

The number of incorrect statement/s involving equilibria in physical process from the following is _________. (A) Equilibrium is possible only in a closed system at a given temperature. (B) Both the opposing processes occur at the same rate. (C) When equilibrium is attained at a given temperature, the value of all its parameters becomes equal. (D) For dissolution of solids in liquids, the solubility is constant at a given temperature.

Q81·ChemistryNumericalJEE Main 2023

The titration curve of weak acid vs. strong base with phenolphthalein as indicator) is shown below. The

K_{phenolphthalein} = 4 \times 10^{-10}

. Given:

\log 2 = 0.3

. The number of following statements which is/are correct about phenolphthalein is ____ A. It can be used as an indicator for the titration of weak acid with weak base. B. It begins to change colour at

pH = 8.4

C. It is a weak organic base D. It is colourless in acidic medium

Q82·ChemistryNumericalJEE Main 2023

The solubility product of

BaSO_4

is

1\times10^{-10}

at 298 K. The solubility of

BaSO_4

in

0.1

M

K_2SO_4(aq)

solution is ____

\times10^{-9}

g L

^{-1}

(nearest integer). Given: Molar mass of

BaSO_4

is

233

g mol

^{-1}

.

Q83·ChemistrySingle correctJEE Main 2023

Given below are two statements: Statement I: Methyl orange is a weak acid. Statement II: The benzenoid form of methyl orange is more intense/deeply coloured than the quinonoid form. In the light of the above statements, choose the most appropriate answer from the options given below:

(A)Statement I is correct but Statement II is incorrect
(B)Statement I is incorrect but Statement II is correct
(C)Both Statement I and Statement II are incorrect
(D)Both Statement I and Statement II are correct

Q84·ChemistrySingle correctJEE Main 2023

Given below are two statements: Statement I: In redox titration, the indicators used are sensitive to change in pH of the solution. Statement II: In acid-base titration, the indicators used are sensitive to change in oxidation potential. In the light of the above statements, choose the most appropriate answer from the options given below.

(A)Both Statement I and Statement II are correct
(B)Statement I is incorrect but Statement II is correct
(C)Statement I is correct but Statement II is incorrect
(D)Both Statement I and Statement II are incorrect

Q85·ChemistryNumericalJEE Main 2023

The equilibrium composition for the reaction

PCl_3 + Cl_2 \rightleftharpoons PCl_5

at 298 K is given below.

[PCl_3]_{eq} = 0.2

mol

L^{-1}

,

[Cl_2]_{eq} = 0.1

mol

L^{-1}

,

[PCl_5]_{eq} = 0.40

mol

L^{-1}

. If 0.2 mol of

Cl_2

is added at the same temperature, the equilibrium concentration of

PCl_5

is ____

\times 10^{-2}

mol

L^{-1}

. (Given:

K_c

for the reaction at 298 K is 20)

Q86·ChemistrySingle correctJEE Main 2023

For a concentrated solution of a weak electrolyte

(K_{eq}=

equilibrium constant

)

A_2B_3

of concentration

c

, the degree of dissociation

\alpha

is:

(A) $\left(\dfrac{K_{eq}}{108c^{4}}\right)^{1/5}$
(B) $\left(\dfrac{K_{eq}}{6c^{2}}\right)^{1/2}$
(C) $\left(\dfrac{K_{eq}}{5c^{4}}\right)^{1/5}$
(D) $\left(\dfrac{K_{eq}}{25c^{4}}\right)^{1/3}$

Q87·ChemistryNumericalJEE Main 2023

The value of

\log K

for the reaction

A\rightleftharpoons B

at

298\,K

is _____. (Nearest integer) Given:

\Delta H^\circ=-54.07\,kJ\,mol^{-1},\,\Delta S^\circ=10\,J\,K^{-1}\,mol^{-1}

. (Take

2.303\times8.314\times298=5705

)

Q88·ChemistrySingle correctJEE Main 2023

The effect of addition of helium gas to the following reaction in equilibrium state, is:

PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)

(A)helium will deactivate $PCl_5$ and reaction will stop.
(B)the equilibrium will shift in the forward direction and more of $Cl_2$ and $PCl_3$ gases will be produced.
(C)the equilibrium will go backward due to suppression of dissociation of $PCl_5$ .
(D)addition of helium will not affect the equilibrium.

Q89·ChemistryNumericalJEE Main 2023

For the equilibria (i)

\text{X(g)}\rightleftharpoons \text{Y(g)}+\text{Z(g)}

,

K_{p_1}=3

and (ii)

\text{A(g)}\rightleftharpoons 2\text{B(g)}

,

K_{p_2}=1

. If the degree of dissociation and initial concentration of both the reactants

\text{X(g)}

and

\text{A(g)}

are equal, then the ratio of the total pressure at equilibrium

\left(\tfrac{p_1}{p_2}\right)

is equal to

x:1

. The value of

x

is _______ (Nearest integer).

Q90·ChemistryNumericalJEE Main 2023

For reaction:

SO_2(g) + \frac{1}{2}O_2(g) \rightleftharpoons SO_3(g)

,

K_p = 2 \times 10^{12}

at

27^{\circ}C

and 1 atm pressure. The

K_c

for the same reaction is ___

\times 10^{13}

. (Nearest integer) (Given

R = 0.082\ L\,atm\,K^{-1}\,mol^{-1}

)

Q91·ChemistrySingle correctJEE Main 2023

Incorrect statement for the use of indicators in acid-base titration is:

(A)Methyl orange may be used for a weak acid vs weak base titration.
(B)Phenolphthalein is a suitable indicator for a weak acid vs strong base titration.
(C)Methyl orange is a suitable indicator for a strong acid vs weak base titration.
(D)Phenolphthalein may be used for a strong acid vs strong base titration.

Q92·ChemistryNumericalJEE Main 2023

At 298 K, the solubility of silver chloride in water is

1.434\times10^{-3}

g L

^{-1}

. The value of

-\log K_{sp}

for silver chloride is _________ (Given mass of Ag is 107.9 g mol

^{-1}

and mass of Cl is 35.5 g mol

^{-1}

)

Q93·ChemistryNumericalJEE Main 2023

Consider the equilibrium

2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)

,

\Delta H=-190

kJ. The number of factors from the following which will increase the yield of

SO_3

at equilibrium is _______: A. Increasing temperature, B. Increasing pressure, C. Adding more

SO_2

, D. Adding more

O_2

, E. Addition of catalyst.

Q94·ChemistryNumericalJEE Main 2023

600

mL of

0.01

M HCl is mixed with

400

mL of

0.01

M H

_2

SO

_4

. The pH of the mixture is _________

\times10^{-2}

. (Nearest integer) [Given log 2 = 0.30, log 3 = 0.48, log 5 = 0.69, log 7 = 0.84, log 11 = 1.04]

Q95·ChemistryNumericalJEE Main 2023

At

298\,K

N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g),\,K_1=4\times10^5

N_2(g)+O_2(g)\rightleftharpoons 2NO(g),\,K_2=1.6\times10^{12}

H_2(g)+\dfrac12 O_2(g)\rightleftharpoons H_2O(g),\,K_3=1.0\times10^{-13}

Based on above equilibria, the equilibrium constant of the reaction,

2NH_3(g)+\dfrac52 O_2(g)\rightleftharpoons 2NO(g)+3H_2O(g)

is _____

\times10^{-33}

(Nearest integer).

Q96·ChemistryNumericalJEE Main 2023

Water decomposes at 2300 K: H

_2

O(g)

\rightarrow

H

_2

(g) +

\dfrac{1}{2}

O

_2

(g). The percent of water decomposing at 2300 K and 1 bar is ________ (Nearest integer). Equilibrium constant for the reaction is

2 \times 10^{-3}

at 2300 K.

Q97·ChemistryNumericalJEE Main 2023

Millimoles of calcium hydroxide required to produce 100 mL of the aqueous solution of pH 12 is

x \times 10^{-1}

. The value of

x

is ________ (Nearest integer). Assume complete dissociation.

Q98·ChemistrySingle correctJEE Main 2023

When the hydrogen ion concentration

[H^+]

changes by a factor of

1000

, the value of pH of the solution

(A)increases by 2 units
(B)increases by 1000 units
(C)decreases by 2 units
(D)decreases by 3 units

Q99·ChemistryNumericalJEE Main 2023

A litre of buffer solution contains 0.1 mole of each of

NH_3

and

NH_4Cl

. On the addition of 0.02 mole of HCl by dissolving gaseous HCl, the pH of the solution is found to be _______

\times10^{-3}

(nearest integer). (Given:

pK_b(NH_3)=4.745

,

\log 2=0.301

,

\log 3=0.477

, T = 298 K)

Q100·ChemistryNumericalJEE Main 2023

If the

pK_a

of lactic acid is

5

, then the pH of

0.005

M calcium lactate solution at

25\,^\circ C

is _________

\times10^{-1}

(Nearest integer)

Q101·ChemistryNumericalJEE Main 2023

The dissociation constant of acetic acid is

x\times10^{-5}

. When 25 mL of 0.2 M

\text{CH}_3\text{COONa}

solution is mixed with 25 mL of 0.02 M

\text{CH}_3\text{COOH}

solution, the pH of the resultant solution is found to be equal to 5. The value of

x

is _______ .

Q102·ChemistryIntegerJEE Advanced 2022

Concentration of

\mathrm{H_2SO_4}

and

\mathrm{Na_2SO_4}

in a solution is 1 M and

1.8 \times 10^{-2}

M, respectively. Molar solubility of

\mathrm{PbSO_4}

in the same solution is

\mathrm{X} \times 10^{-\mathrm{Y}}

M (expressed in scientific notation). The value of Y is____. [Given : Solubility product of

\mathrm{PbSO_4}\left(\mathrm{K_{sp}}\right) = 1.6 \times 10^{-8}

. For

\mathrm{H_2SO_4}

,

\mathrm{K_{a_1}}

is very large and

\mathrm{K_{a_2}} = 1.2 \times 10^{-2}

]

Q103·ChemistryNumericalJEE Advanced 2022

A solution is prepared by mixing 0.01 mol each of

\mathrm{H_2CO_3}

,

\mathrm{NaHCO_3}

,

\mathrm{Na_2CO_3}

, and NaOH in 100 mL of water. pH of the resulting solution is ________. [Given:

p\mathrm{Ka_1}

and

p\mathrm{Ka_2}

of

\mathrm{H_2CO_3}

are 6.37 and 10.32, respectively;

\log 2 = 0.30

]

Q104·ChemistrySingle correctJEE Main 2022

200 mL of 0.01 M HCl is mixed with 400 mL of 0.01M H

_{2}

SO

_{4}

. The pH of the mixture is ____.

(A)1.14
(B)1.78
(C)2.34
(D)3.02

Q105·ChemistrySingle correctJEE Main 2022

A compound 'X' is a weak acid and it exhibits colour change at pH close to the equivalence point during neutralization of NaOH with CH

_{3}

COOH. Compound 'X' exists in ionized form in basic medium. The compound 'X' is :

(A)methyl orange
(B)methyl red
(C)phenolphthalein
(D)erichrome Black T

Q106·ChemistryNumericalJEE Main 2022

If the solubility product of PbS is 8 ×

10^{-28}

, then the solubility of PbS in pure water at 298 K is x ×

10^{-16}

mol

L^{-1}

. The value of x is ________. (Nearest Integer) [Given

\sqrt{2}

= 1.41]

Q107·ChemistryNumericalJEE Main 2022

K

_a

for butyric acid (C

_3

H

_7

COOH) is 2 × 10

^{-5}

. The pH of 0.2 M solution of butyric acid is ___ × 10

^{-1}

. (Nearest integer) [Given log 2 = 0.30]

Q108·ChemistryNumericalJEE Main 2022

At 600K, 2 mol of NO are mixed with 1 mol of

\mathrm{O_2}

.

2\mathrm{NO_{(g)}} + \mathrm{O_2(g)} \rightleftharpoons 2\mathrm{NO_2(g)}

The reaction occurring as above comes to equilibrium under a total pressure of 1 atom. Analysis of the system shows that 0.6 mol of oxygen are present at equilibrium. The equilibrium constant for the reaction is _____. (Nearest integer).

Q109·ChemistryNumericalJEE Main 2022

At 310 K, the solubility of

CaF_{2}

in water is

2.34 \times 10^{-3}

g /100 mL. The solubility product of

CaF_{2}

is ___

\times 10^{-8}

(mol/L)^{3}

. (Given molar mass :

CaF_{2}

= 78 g

mol^{-1}

)

Q110·ChemistrySingle correctJEE Main 2022

The Plot of pH-metric titration of weak base NH

_{4}

OH vs strong acid HCl looks like:

(A)(A)
(B)(B)
(C)(C)
(D)(D)

Q111·ChemistrySingle correctJEE Main 2022

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. It doesn't dissociate in basic medium. In the light of the above statements, choose the most appropriate answer from the options given below :

(A)Both A and R are true and R is the correct explanation of A
(B)Both A and R are true but R is NOT the correct explanation of A.
(C)A is true but R is false
(D)A is false but R is true

Q112·ChemistryNumericalJEE Main 2022

At 298 K, the equilibrium constant is 2 × 10

^{15}

for the reaction : Cu(s) + 2Ag

^{+}

(aq) ⇌ Cu

^{2+}

(aq) + 2Ag(s) The equilibrium constant for the reaction

\frac{1}{2}

Cu

^{2+}

(aq) + Ag(s) ⇌

\frac{1}{2}

Cu(s) + Ag

^{+}

(aq) is x × 10

^{-8}

. The value of x is________. (Nearest Integer)

Q113·ChemistrySingle correctJEE Main 2022

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

pK_{b}

(

NH_{3}

) = 4.74; Molar mass of

NH_{3}

= 17 g

mol^{-1}

; Molar mass of

NH_{4}Cl

= 53.5 g

mol^{-1}

)

(A)53.5 g
(B)72.3 g
(C)107.0 g
(D)126.0 g

Q114·ChemistrySingle correctJEE Main 2022

20 mL of 0.1 M

NH_{4}OH

is mixed with 40 mL of 0.05 M HCl. The pH of the mixture is nearest to: (Given:

K_{b}(NH_{4}OH) = 1 \times 10^{-5}

, log 2 = 0.30, log 3 = 0.48, log 5 = 0.69, log 7 = 0.84, log 11 =1.04)

(A)3.2
(B)4.2
(C)5.2
(D)6.2

Q115·ChemistrySingle correctJEE Main 2022

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

(A)0.01 M KCl
(B)0.01 M HCl
(C)0.01 M $AgNO_3$
(D)Deionised water

Q116·ChemistrySingle correctJEE Main 2022

4.0 moles of argon and 5.0 moles of 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 : R = 0.082L atm K

^{-1}

mol

^{-1}

]

(A)2.25
(B)6.24
(C)12.13
(D)15.24

Q117·ChemistrySingle correctJEE Main 2022

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of

\frac{[CH_3CH_2COO^-]}{[CH_3CH_2COOH]}

required to make buffer is ………. Given : K

_a

(CH

_3

CH

_2

COOH) = 1.3 × 10

^{-5}

(A)0.03
(B)0.13
(C)0.23
(D)0.33

Q118·ChemistryNumericalJEE Main 2022

pH value of 0.001 M NaOH solution is_______.

Q119·ChemistryNumericalJEE Main 2022

2NOCl(g) ⇌ 2NO(g) +

Cl_{2}

(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 mol/L. The equilibrium constant at 30°C is _______ ×

10^{-4}

.

Q120·ChemistryNumericalJEE Main 2022

40° of HI undergoes decomposition to

H_2

and

I_2

at 300 K.

\Delta G^{\ominus}

for this decompostion reaction at one atmosphere pressure is_________ J

mol^{-1}

. [nearest integer] (Use R = 8.31 J

K^{-1}

mol^{-1}

; log 2 = 0.3010. In 10 = 2.3, log 3 = 0.477)

Q121·ChemistryNumericalJEE Main 2022

50 mL of 0.1 M

CH_{3}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 :

pK_{a}

(

CH_{3}COOH

) = 4.76) log 2 = 0.30 log 3 = 0.48 log 5 = 0.69 log 7 = 0.84 log 11 = 1.04

Q122·ChemistrySingle correctJEE Main 2022

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 NH

_3

and as a base with H

_2

S. In the light of the above statements choose the correct answer from the options given below :

(A)Both A and R are true and R is the correct explanation of A.
(B)Both A and R are true but R is NOT the correct explanation of A.
(C)A is true but R is false.
(D)A is false but R is true.

Q123·ChemistryNumericalJEE Main 2022

The standard free energy change (ΔG°) for 50% dissociation of

N_2O_4

into

NO_2

at 27°C and 1 atm pressure is −x J

mol^{-1}

. The value of x is _________. (Nearest Integer) [Given : R = 8.31 J

K^{-1}

mol^{-1}

, log 1.33 = 0.1239 ln 10 = 2.3]

Q124·ChemistrySingle correctJEE Main 2022

The K

_{sp}

for bismuth sulphide (Bi

_2

S

_3

) is 1.08

\times

10

^{-73}

. The solubility of Bi

_2

S

_3

in mol L

^{-1}

at 298 K is

(A)1.0 $\times$ 10 $^{-15}$
(B)2.7 $\times$ 10 $^{-12}$
(C)3.2 $\times$ 10 $^{-10}$
(D)4.2 $\times$ 10 $^{-8}$

Q125·ChemistryNumericalJEE Main 2022

PCl

_5

dissociates as PCl

_5

(g)

\rightleftharpoons

PCl

_3

(g) + Cl

_2

(g) 5 moles of PCl

_5

are placed in a 200 litre vessel which contains 2 moles of N

_2

and is maintained at 600 K. The equilibrium pressure is 2.46 atm. The equilibrium constant K

_p

for the dissociation of PCl

_5

is_____

\times

10

^{-3}

. (nearest integer) (Given: R = 0.082 L atm K

^{-1}

mol

^{-1}

: Assume ideal gas behaviour)

Q126·ChemistrySingle correctJEE Main 2022

For a reaction at equilibrium

A(g)\rightleftharpoons B(g)+\dfrac{1}{2}C(g)

the relation between dissociation constant (K), degree of dissociation (

\alpha

) and equilibrium pressure (p) is given by :

(A) $K=\dfrac{\alpha^{\frac{1}{2}}p^{\frac{3}{2}}}{\left(1+\dfrac{3}{2}\alpha\right)^{\frac{1}{2}}(1-\alpha)}$
(B) $K=\dfrac{\alpha^{\frac{3}{2}}p^{\frac{1}{2}}}{(2+\alpha)^{\frac{1}{2}}(1-\alpha)}$
(C) $K=\dfrac{(\alpha p)^{\frac{3}{2}}}{\left(1+\dfrac{3}{2}\alpha\right)^{\frac{1}{2}}(1-\alpha)}$
(D) $K=\dfrac{(\alpha p)^{\frac{3}{2}}}{(1+\alpha)(1-\alpha)^{\frac{1}{2}}}$

Q127·ChemistryNumericalJEE Main 2021

The molar solubility of Zn(OH)

_{2}

in 0.1 M NaOH solution is x × 10

^{-18}

M. The value of x is ______ (Nearest integer) (Given : The solubility product of Zn(OH)

_{2}

is 2 × 10

^{-20}

)

Q128·ChemistryNumericalJEE Main 2021

\mathrm{A_3B_2}

is a sparingly soluble salt of molar mass M (g mol

^{-1}

) and solubility x g L

^{-1}

. The solubility product satisfies

\mathrm{K_{sp}} = a\left(\dfrac{\mathrm{x}}{\mathrm{M}}\right)^{5}

. The value of

a

is ____. (Integer answer)

Q129·ChemistryNumericalJEE Main 2021

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

]

Q130·ChemistryNumericalJEE Main 2021

When 5.1 g of solid NH

_{4}

HS is introduced into a two litre evacuated flask at 27°C, 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K

_{p}

for the reaction at 27°C is x × 10

^{-2}

. The value of x is _____ . (Integer answer) [Given R = 0.082 L atm K

^{-1}

mol

^{-1}

]

Q131·ChemistryNumericalJEE Main 2021

The number of moles of

NH_3

, that must be added to 2 L of 0.80 M

AgNO_3

in order to reduce the concentration of

Ag^+

ions to

5.0 \times 10^{-8}

M (

K_{formation}

for

[Ag(NH_3)_2]^+ = 1.0 \times 10^8

) is ________ . (Nearest integer) [Assume no volume change on adding

NH_3

]

Q132·ChemistryNumericalJEE Main 2021

The equilibrium constant

K_c

at 298 K for the reaction

A + B \rightleftharpoons C + D

is 100. Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1M, the equilibrium concentration of D is ______

\times 10^{-2}

M. (Nearest integer)

Q133·ChemistryNumericalJEE Main 2021

The

OH^-

concentration in a mixture of 5.0 mL of

0.0504\ M\ NH_4Cl

and 2 mL of

0.0210\ M\ NH_3

solution is

x \times 10^{-6}

M. The value of x is ________. (Nearest integer) [Given

K_w = 1 \times 10^{-14}

and

K_b = 1.8 \times 10^{-5}

]

Q134·ChemistrySingle correctJEE Main 2021

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, choose the most appropriate answer from the options given below:

(A)Statement I is false but Statement II is true
(B)Statement I is true but Statement II is false
(C)Both Statement I and Statement II are true
(D)Both Statement I and Statement II are false

Q135·ChemistryNumericalJEE Main 2021

PCl_5 \rightleftharpoons PCl_3 + Cl_2

K_C

= 1.844 3.0 moles of

PCl_5

is introduced in a 1L closed reaction vessel at 380K. The number of moles of

PCl_5

at equilibrium is_________

\times 10^{-3}

. (Round off to the Nearest integer)

Q136·ChemistryNumericalJEE Main 2021

The conductivity of a weak acid HA of concentration 0.001 mol L

^{-1}

is

2.0 \times 10^{-5}

S cm

^{-1}

. If

\Lambda_m^o

(HA) = 190 S cm

^2

mol

^{-1}

, the ionization constant (

K_a

) of HA is equal to ________

\times 10^{-6}

(Round off to the nearest integer)

Q137·ChemistryNumericalJEE Main 2021

Assuming that Ba(OH)

_2

is completely ionized in aqueous solution under the given conditions the concentration of H

_3

O

^{+}

ions in 0.005 M aqueous solution of Ba(OH)

_2

at 298 K is ___________

\times

10^{-12}

mol L

^{-1}

. (nearest integer)

Q138·ChemistryNumericalJEE Main 2021

For the reaction A + B

\rightleftharpoons

2C The value of equilibrium constant is 100 at 298K. If the initial concentration of all the three species is 1M each, then the equilibrium concentration of C is x

\times 10^{-1}

M. The value of x is__________. (Nearest integer)

Q139·ChemistryNumericalJEE Main 2021

Value of

K_p

for the equilibrium reaction

\mathrm{N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}}

at 288 K is 47.9. The

K_c

for this reaction at same temperature is __________. (Nearest integer) (R = 0.083 L bar K

^{-1}

mol

^{-1}

)

Q140·ChemistryNumericalJEE Main 2021

2SO

_2

(g) + O

_2

(g) ⇌ 2SO

_3

(g) In an equilibrium mixture, the partial pressures are

P_{SO_3}

= 43kPa ;

P_{O_2}

= 530 Pa and

P_{SO_2}

= 45kPa . The equilibrium constant

K_p

= ______________

\times 10^{-2}

(Nearest integer)

Q141·ChemistrySingle correctJEE Main 2021

A solution is 0.1 M in

\mathrm{Cl}^-

and 0.001 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_{sp}}\left(\mathrm{AgCl}\right) = 1.7 \times 10^{-10}\ \mathrm{M^2}

and

\mathrm{K_{sp}}\left(\mathrm{Ag_2CrO_4}\right) = 1.9 \times 10^{-12}\ \mathrm{M^3}

. Select correct statement from the following :

(A) $\mathrm{Ag_2CrO_4}$ precipitates first because the amount of $\mathrm{Ag}^+$ needed is low.
(B) $\mathrm{Ag_2CrO_4}$ precipitates first as its $\mathrm{K_{sp}}$ is low.
(C) $\mathrm{AgCl}$ will precipitate first as the amount of $\mathrm{Ag}^+$ needed to precipitate is low.
(D) $\mathrm{AgCl}$ precipitates first because its $\mathrm{K_{sp}}$ is high.

Q142·ChemistryNumericalJEE Main 2021

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) = 4.74]

Q143·ChemistryNumericalJEE Main 2021

The solubility of CdSO

_{4}

in water is 8.0 × 10

^{-4}

mol L

^{-1}

. Its solubility in 0.01 M H

_{2}

SO

_{4}

solution is ______ × 10

^{-6}

mol L

^{-1}

. (Round off to the Nearest integer) (Assume that solubility is much less than 0.01 M)

Q144·ChemistryNumericalJEE Main 2021

0.01 moles of a weak acid

\mathrm{HA}(\mathrm{K_a} = 2.0 \times 10^{-6})

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 degree of dissociation <<1]

Q145·ChemistryNumericalJEE Main 2021

Consider the reaction N

_{2}

O

_{4}

(g)

\rightleftharpoons

2NO

_{2}

(g). The temperature at which K

_{C}

= 20.4 and K

_{P}

= 600.1, is_____K. (Round off to the Nearest Integer). [Assume all gases are ideal and R = 0.0831 L bar K

^{-1}

mol

^{-1}

]

Q146·ChemistryNumericalJEE Main 2021

Two salts A

_{2}

X and MX have the same value of solubility product of 4.0 × 10

^{-12}

. The ratio of their molar solubilities i.e.

\frac{S(A_{2}X)}{S(MX)}

= _______. (Round off to the Nearest Integer).

Q147·ChemistryNumericalJEE Main 2021

Sulphurous acid (H

_{2}

SO

_{3}

) has Ka

_{1}

= 1.7 × 10

^{-2}

and Ka

_{2}

= 6.4 × 10

^{-8}

. The pH of 0.588 M H

_{2}

SO

_{3}

is _________. (Round off to the Nearest Integer)

Q148·ChemistryNumericalJEE Main 2021

A homogeneous ideal gaseous reaction AB

_{2(g)}

⇌ A

_{(g)}

+ 2B

_{(g)}

is carried out in a 25 litre flask at 27°C. The initial amount of AB

_2

was 1 mole and the equilibrium pressure was 1.9 atm. The value of K

_p

is x × 10

^{-2}

. The value of x is ________. [R = 0.08206 dm

^3

atm K

^{-1}

mol

^{-1}

]

Q149·ChemistryNumericalJEE Main 2021

The pH of ammonium phosphate solution, if

pk_a

of phosphoric acid and

pk_b

of ammonium hydroxide are 5.23 and 4.75 respectively, is_______________.

Q150·ChemistrySingle correctJEE Main 2021

The solubility of Ca(OH)2 in water is : [Given : The solubility product of Ca(OH)2 in water = 5.5×10

^{-6}

]

(A)1.11 ×10 $^{-6}$
(B)1.77 ×10 $^{-6}$
(C)1.77×10 $^{-2}$
(D)1.11×10 $^{-2}$

Q151·ChemistrySingle correctJEE Main 2021

The solubility of AgCN in a buffer solution of pH = 3 is x. The value of x is: [Assume: No cyano complex is formed; K

_{sp}

(AgCN) = 2.2 × 10

^{-16}

and K

_{a}

(HCN) = 6.2 × 10

^{-10}

]

(A)0.625 × 10 $^{-6}$
(B)1.6 × 10 $^{-6}$
(C)2.2 × 10 $^{-16}$
(D)1.9 × 10 $^{-5}$

Q152·ChemistryNumericalJEE Main 2021

At 1990 K and 1 atrm pressure, there are equal number of

\mathrm{Cl_2}

molecules and

\mathrm{Cl}

atoms in the reaction mixture. The value of

\mathrm{K_p}

for the reaction

\mathrm{Cl_{2(g)}} \rightleftharpoons \mathrm{2Cl_{(g)}}

under the above conditions is

x \times 10^{-1}

. The value of x is _________. (Rounded off to the nearest integer)

Q153·ChemistryNumericalJEE Main 2021

The solubility product of

PbI_{2}

is 8.0 ×

10^{-9}

. The solubility of lead iodide in 0.1 molar solution of lead nitrate is x ×

10^{-6}

mol/L. The value of x is _________(Rounded off to the nearest integer) [Given

\sqrt{2} = 1.41

]

Q154·ChemistryNumericalJEE Advanced 2020

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

pK_{b}

of the base? The neutralization reaction is given by

B + HA \rightarrow BH^{+} + A^{-}

.

Q155·ChemistryNumericalJEE Advanced 2020

Consider the reaction A ⇌ B at 1000 K. At time t', the temperature of the system was increased to 2000 K and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of A was maintained at 1 bar. Given below is the plot of the partial pressure of B with time. What is the ratio of the standard Gibbs energy of the reaction at 1000 K to that at 2000 K?

Q156·ChemistryNumericalJEE Advanced 2020

An acidified solution of 0.05 M

Zn^{2+}

is saturated with 0.1 M

H_{2}S

. What is the minimum molar concentration (M) of

H^{+}

required to prevent the precipitation of ZnS ? Use

K_{sp}

(ZnS) =

1.25 \times 10^{-22}

and Overall dissociation constant of

H_{2}S

,

K_{NET} = K_{1}K_{2} = 1 \times 10^{-21}

Q157·ChemistrySingle correctJEE Main 2020

Arrange the following solutions in the decreasing order of pOH (1) 0.01 M HCl (2) 0.01 M NaOH (3) 0.01 M

CH_3COONa

(4) 0.01 M NaCl

(A)(1) > (3) > (4) > (2)
(B)(1) > (4) > (3) > (2)
(C)(2) > (3) > (4) > (1)
(D)(2) > (4) > (3) > (1)

Q158·ChemistrySingle correctJEE Main 2020

The value of K

_C

is 64 at 800 K for the reaction N

_2

(g) + 3H

_2

(g) ⇌ 2NH

_3

(g) The value of K

_C

for the following reaction is: NH

_3

(g) ⇌

\frac{1}{2}

N

_2

(g) +

\frac{3}{2}

H

_2

(g)

(A) $\frac{1}{64}$
(B)8
(C) $\frac{1}{4}$
(D) $\frac{1}{8}$

Q159·ChemistrySingle correctJEE Main 2020

For the reaction

Fe_2N(s) + \dfrac{3}{2}H_2(g) = 2Fe(s) + NH_3(g)

(A) $K_c = K_p(RT)$
(B) $K_c = K_P(RT)^{-1/2}$
(C) $K_c = K_P(RT)^{1/2}$
(D) $K_c = K_P(RT)^{3/2}$

Q160·ChemistryNumericalJEE Main 2020

If the solubility product of AB

_2

is 3.20 × 10

^{-11}

M

^3

, then the solubility of AB

_2

in pure water is __________ × 10

^{-4}

mol L

^{-1}

. [Assuming that neither kind of ion reacts with water]

Q161·ChemistryNumericalJEE Main 2020

For a reaction X + Y = 2Z, 1.0 mol of X, 1.5 mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0 mol L

^{-1}

. The equilibrium constant of the reaction is __________

\dfrac{x}{15}

. The value of x is __________.

Q162·ChemistrySingle correctJEE Main 2020

For the equilibrium A

\rightleftharpoons

B, the variation of the rate of the forward (a) and reverse (B) reaction with time is given by:

(A)(A)
(B)(B)
(C)(C)
(D)(D)

Q163·ChemistrySingle correctJEE Main 2020

If the equilibrium constant for

A \rightleftharpoons B + C

is

K^{(1)}_{(eq)}

and that of

B + C \rightleftharpoons P

is

K^{(2)}_{(eq)}

, the equilibrium constant for

A \rightleftharpoons P

is:

(A) $K^{(1)}_{(eq)}K^{(2)}_{(eq)}$
(B) $K^{(1)}_{(eq)} / K^{(1)}_{(eq)}$
(C) $K^{(1)}_{(eq)} + K^{(2)}_{(eq)}$
(D) $K^{(2)}_{(eq)} - K^{(1)}_{(eq)}$

Q164·ChemistrySingle correctJEE Main 2020

100 mL of 0.1 M HCl is taken in a beaker and to it 100 mL of 0.1 M NaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?

(A)(A)
(B)(B)
(C)(C)
(D)(D)

Q165·ChemistrySingle correctJEE Main 2020

An acidic buffer is obtained on mixing:

(A)100 mL of 0.1 M HCl and 200 mL of 0.1 M NaCl
(B)100 mL of 0.1 M HCl and 200 mL of 0.1 M CH $_3$ COONa
(C)100 mL of 0.1 M CH $_3$ COOH and 100 mL of 0.1 M NaOH
(D)100 mL of 0.1 M CH $_3$ COOH and 200 mL of 0.1 M NaOH

Q166·ChemistrySingle correctJEE Main 2020

The solubility product of Cr(OH)

_3

at 298 K is

6.0 \times 10^{-31}

. The concentration of hydroxide ions in a saturated solution of Cr(OH)

_3

will be :

(A) $(18 \times 10^{-31})^{1/4}$
(B) $(4.86 \times 10^{-29})^{1/4}$
(C) $(18 \times 10^{-31})^{1/2}$
(D) $(2.22 \times 10^{-31})^{1/4}$

Q167·ChemistrySingle correctJEE Main 2020

The K

_{sp}

for the following dissociation is 1.6

\times

10

^{-5}

PbCl

_{2}

(s)

\rightleftharpoons

Pb

^{2+}

(aq) + 2Cl

^{-}

(aq) Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb(NO

_{3}

)

_{2}

and 100 mL 0.4 M NaCl?

(A)Not enough data provided
(B)Q > K $_{sp}$
(C)Q < K $_{sp}$
(D)Q = K $_{sp}$

Q168·ChemistrySingle correctJEE Main 2020

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

(A)XY, 2 $\times$ 10 $^{-5}$ M $^{3}$
(B)XY $_{3}$ , 1 $\times$ 10 $^{-9}$ M $^{3}$
(C)XY $_{2}$ , 4 $\times$ 10 $^{-9}$ M $^{3}$
(D)X $_{2}$ Y, 2 $\times$ 10 $^{-9}$ M $^{3}$

Q169·ChemistryNumericalJEE Main 2020

Two solutions A and B, each of 100 L was made by dissolution of 4g of NaOH and 9.8 g of H

_2

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

Q170·ChemistryNumericalJEE Main 2020

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 ½ mL of 5 M NaOH is added. The pH of the solution is __________ [Given: p

K_a

of acetic acid = 4.75, molar mass of acetic acid = 60 g/mol, log 3 = 0.4771] Neglect any changes in volume.

Q171·ChemistryNumericalJEE Advanced 2019

For the following reaction, the equilibrium constant K

_{c}

at 298 K is 1.6

\times

10

^{17}

Fe

^{2+}

(aq) + S

^{2-}

(aq)

\rightleftharpoons

FeS(s) When equal volumes of 0.06 M Fe

^{2+}

(aq) and 0.2 M S

^{2-}

(aq) solutions are mixed, the equilibrium concentration of Fe

^{2+}

(aq) is found to be Y

\times

10

^{-17}

M. The value of Y is ……… .

Q172·ChemistrySingle correctJEE Main 2019

The molar solubility of Cd(OH)

_2

is 1.84

\times

10

^{-5}

M in water. The expected solubility of Cd(OH)

_2

in a buffer solution of pH = 12 is :

(A)6.23 $\times$ 10 $^{-11}$ M
(B)1.84 $\times$ 10 $^{-9}$ M
(C) $\frac{2.49}{1.84} \times 10^{-9}$ M
(D)2.49 $\times$ 10 $^{-10}$ M

Q173·ChemistrySingle correctJEE Main 2019

What is the molar solubility of Al(OH)

_3

in 0.2 M NaOH solution? Given that, solubility product of Al(OH)

_3

= 2.4

\times

10

^{-24}

:

(A)3 $\times$ 10 $^{-19}$
(B)12 $\times$ 10 $^{-21}$
(C)12 $\times$ 10 $^{-23}$
(D)3 $\times$ 10 $^{-22}$

Q174·ChemistrySingle correctJEE Main 2019

In which one of the following equilibria, K

_p

≠ K

_c

?

(A)2NO(g) ⇌ N $_2$ (g) + O $_2$ (g)
(B)2C(s) + O $_2$ (g) ⇌ 2CO(g)
(C)NO $_2$ (g) + SO $_2$ (g) ⇌ NO(g) + SO $_3$ (g)
(D)2HI(g) ⇌ H $_2$ (g) + I $_2$ (g)

Q175·ChemistrySingle correctJEE Main 2019

Consider the following statements (a) The pH of a mixture containing 400 mL of 0.1 M

H_2SO_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

K_a = 10^{-5}

has a pH = 5. the degree of dissociation of this acid is 50%. (d) The Le Chatelier's principle is not applicable to common-ion effect. The correct statements are:

(A)(a) and (b)
(B)(a), (b) and (c)
(C)(b) and (c)
(D)(a), (b) and (d)

Q176·ChemistrySingle correctJEE Main 2019

The pH of a 0.02 M NH

_4

Cl solution will be [given K

_b

(NH

_4

OH) = 10

^{-5}

and log 2 = 0.301]

(A)2.65
(B)5.35
(C)4.35
(D)4.65

Q177·ChemistrySingle correctJEE Main 2019

For the reaction,

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

\Delta_H = -57.2

kJ mol

^{-1}

and

\mathrm{K}_\mathrm{C} = 1.7 \times 10^{16}

Which of the following statement is INCORRECT?

(A)The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
(B)The equilibrium will shift in forward direction as the pressure increase.
(C)The equilibrium constant decreases as the temperature increases.
(D)The addition of inert gas at constant volume will not affect the equilibrium constant.

Q178·ChemistrySingle correctJEE Main 2019

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?

(A)(a)
(B)(c)
(C)(d)
(D)(b)

Q179·ChemistrySingle correctJEE Main 2019

If solubility product of

Zr_3(PO_4)_4

is denoted by

K_{SP}

and its molar solubility is denoted by S, then which of the following relation between S and

K_{SP}

is correct?

(A) $S = \left(\dfrac{K_{SP}}{6912}\right)^{1/7}$
(B) $S = \left(\dfrac{K_{SP}}{144}\right)^{1/6}$
(C) $S = \left(\dfrac{K_{Sp}}{929}\right)^{1/9}$
(D) $S = \left(\dfrac{K_{SP}}{216}\right)^{1/7}$

Q180·ChemistrySingle correctJEE Main 2019

For the following reactions, equilibrium constants are given:

S(s)+O_{2}(g)\rightleftharpoons SO_{2}(g);K_{1}=10^{52}

2S(s)+3O_{2}(g)\rightleftharpoons 2SO_{3}(g);K_{2}=10^{129}

The equilibrium constant for the reaction

2SO_{2}(g)+O_{2}(g)\rightleftharpoons 2SO_{3}(g)

is:

(A) $10^{77}$
(B) $10^{25}$
(C) $10^{181}$
(D) $10^{154}$

Q181·ChemistrySingle correctJEE Main 2019

In a chemical reaction

A + 2B \underset{}{\overset{K}{\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

(A)4
(B)16
(C)1/4
(D)1

Q182·ChemistrySingle correctJEE Main 2019

Two solids dissociate as follows

A(s)\rightleftharpoons B(g)+C(g); K_{p_1}=x\ atm^2

D(s)\rightleftharpoons C(g)+E(g); K_{p_2}=y\ atm^2

The total pressure when both the solids dissociate simultaneously is

(A) $\sqrt{x+y}$ atm
(B) $2(\sqrt{x+y})$ atm
(C) $(x+y)$ atm
(D) $x^2+y^2$ atm

Q183·ChemistrySingle correctJEE Main 2019

If Ksp of Ag2CO3 is

8\times10^{-12}

, the molar solubility of Ag2CO3 in 0.1 M AgNO3 is :

(A) $8\times10^{-12}$ M
(B) $8\times10^{-11}$ M
(C) $8\times10^{-10}$ M
(D) $8\times10^{-13}$ M

Q184·ChemistrySingle correctJEE Main 2019

Consider the reaction

N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)

The equilibrium constant of the above reaction is

K_3

. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that

P_{NH_3} \ll P_{total}

at equilibrium)

(A) $\dfrac{3^{3/2}K_p^{1/2}P^2}{16}$
(B) $\dfrac{K_p^{1/2}P^2}{16}$
(C) $\dfrac{K_p^{1/2}P^2}{4}$
(D) $\dfrac{3^{3/2}K_p^{1/2}P^2}{4}$

Q185·ChemistrySingle correctJEE Main 2019

For the equilibrium 2H

_2

O

\rightleftharpoons

H

_3

O

^+

+ OH

^-

, the value of

\Delta G^0

at 298 K is approximately:

(A)100 kJ mol $^{-1}$
(B) $-$ 80 kJ mol $^{-1}$
(C)80 kJ mol $^{-1}$
(D) $-$ 100 kJ mol $^{-1}$

Q186·ChemistrySingle correctJEE Main 2019

The values of K

_{p}

/K

_{c}

for the following reactions at 300 K are respectively: (At 300 K, Rt = 24.62 dm

^{3}

atm mol

^{-1}

) N

_{2}

(g) + O

_{2}

(g) = 2NO(g) N

_{2}

O

_{4}

(g) = 2NO

_{2}

(g) N

_{2}

(g) + 3H

_{2}

(g) = 2NH

_{3}

(g)

(A)1, 24.62 dm $^{3}$ atm mol $^{-1}$ , 606.0 dm $^{6}$ atm $^{2}$ mol $^{-2}$
(B)1, 24.62 dm $^{3}$ atm mol $^{-1}$ , 1.65 $\times$ 10 $^{-3}$ dm $^{-6}$ atm $^{-2}$ mol $^{2}$
(C)1, 4.1 $\times$ 10 $^{-2}$ dm $^{-3}$ atm $^{-1}$ mol, 606.0 dm $^{6}$ atm $^{2}$ mol $^{-2}$
(D)24.62 dm $^{3}$ atm mol $^{-1}$ , 606.0 dm $^{6}$ atm $^{2}$ atm $^{2}$ mol $^{-2}$ , 1.65 $\times$ 10 $^{-3}$ dm $^{-6}$ atm $^{-2}$ mol $^{2}$

Q187·ChemistrySingle correctJEE Main 2019

A mixture of 100 m mol of Ca(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 OH

^{-}

in resulting solution, respectively are (Molar mass of Ca(OH)

_{2}

, Na

_{2}

SO

_{4}

and CaSO

_{4}

are 74, 143 and 136 g mol

^{-1}

respectively; K

_{sp}

of Ca(OH)

_{2}

is 5.5

\times

10

^{-6}

)

(A)1.9 g, 0.28 mol L $^{-1}$
(B)13.6 g, 0.28 mol L $^{-1}$
(C)1.9g, 0.14 mol L $^{-1}$
(D)13.6 g, 0.14 mol L $^{-1}$

Q188·ChemistrySingle correctJEE Main 2019

Consider the following reversible chemical reactions:

A_2(g) + B_2(g) \underset{}{\overset{K_1}{\rightleftharpoons}} 2AB(g)

.......(1)

6AB(g) \underset{}{\overset{K_2}{\rightleftharpoons}} 3A_2(g) + 3B_2(g)

.......(2) The relation between K

_1

and K

_2

is

(A) $K_1K_2 = \frac{1}{3}$
(B) $K_2 = K_1^{3}$
(C) $K_2 = K_1^{-3}$
(D) $K_1K_2 = 3$

Q189·ChemistrySingle correctJEE Main 2019

20 mL of 0.1 M H

_{2}

SO

_{4}

is added to 30 mL of 0.2 M NH

_{4}

OH solution. The pH of the resultant mixture is [pk

_{b}

of NH

_{4}

OH = 4.7]

(A)5.2
(B)9.0
(C)5.0
(D)9.4

Q190·ChemistrySingle correctJEE Advanced 2018

Dilution processes of different aqueous solutions, with water, are given in LIST-I. The effects of dilution of the solutions on

[H^{+}]

are given in LIST-II. (Note: Degree of dissociation (

\alpha

) of weak acid and weak base is << 1; degree of hydrolysis of salt <<1;

[H^{+}]

represents the concentration of

H^{+}

ions) Match each process given in LIST-I with one or more effect(s) in LIST-II. The correct option is

LIST-I	LIST-II
P.(10 mL of 0.1 M NaOH + 20 mL of 0.1 M acetic acid) diluted to 60 mL	1.the value of $[H^{+}]$ does not change on dilution
Q.(20 mL of 0.1 M NaOH + 20 mL of 0.1 M acetic acid) diluted to 80 mL	2.the value of $[H^{+}]$ changes to half of its initial value on dilution
R.(20 mL of 0.1 M HCl + 20 mL of 0.1 M ammonia solution) diluted to 80 mL	3.the value of $[H^{+}]$ changes to two times of its initial value on dilution
S.10 mL saturated solution of $Ni(OH)_{2}$ in equilibrium with excess solid $Ni(OH)_{2}$ is diluted to 20 mL (solid $Ni(OH)_{2}$ is still present after dilution).	4.the value of $[H^{+}]$ changes to $\frac{1}{\sqrt{2}}$ times of its initial value on dilution
	5.the value of $[H^{+}]$ changes to $\sqrt{2}$ times of its initial value on dilution

(A)P $\rightarrow$ 4; Q $\rightarrow$ 2; R $\rightarrow$ 3; S $\rightarrow$ 1
(B)P $\rightarrow$ 4; Q $\rightarrow$ 3; R $\rightarrow$ 2; S $\rightarrow$ 3
(C)P $\rightarrow$ 1; Q $\rightarrow$ 4; R $\rightarrow$ 5; S $\rightarrow$ 3
(D)P $\rightarrow$ 1; Q $\rightarrow$ 5; R $\rightarrow$ 4; S $\rightarrow$ 1

Q191·ChemistryNumericalJEE Advanced 2018

The solubility of a salt of weak acid (AB) at pH 3 is

Y \times 10^{-3}

mol

L^{-1}

. The value of Y is ___. (Given that the value of solubility product of AB (

K_{sp}

)

= 2 \times 10^{-10}

and the value of ionization constant of HB (

K_{a}

)

= 1 \times 10^{-8}

)

Q192·ChemistryMultiple correctJEE Advanced 2017

For a reaction taking place in a container in equilibrium with its surroundings, the effect of temperature on its equilibrium constant

K

in terms of change in entropy is described by

(A)With increase in temperature, the value of $K$ for exothermic reaction decreases because entropy change of the system is positive
(B)With increase in temperature, the value of $K$ for endothermic reaction increases because unfavourable change in entropy of the surroundings decreases
(C)With increase in temperature, the value of $K$ for endothermic reaction increases because the entropy change of the system is negative
(D)With increase in temperature, the value of $K$ for exothermic reaction decreases because favourable change in entropy of the surrounding decreases

Q193·ChemistrySingle correctJEE Advanced 2016

Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2}(g) \rightleftharpoons 2X(g)

The standard reaction Gibbs energy,

\Delta_{r}G^{0}

, of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus,

\beta_{equilibrium}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{-1}

mol^{-1}

) The equilibrium constant

K_{p}

for this reaction at 298 K, in terms of

\beta_{equilibrium}

, is

(A) $\dfrac{8\beta_{equilibrium}^{2}}{2-\beta_{equilibrium}}$
(B) $\dfrac{8\beta_{equilibrium}^{2}}{4-\beta_{equilibrium}^{2}}$
(C) $\dfrac{4\beta_{equilibrium}^{2}}{2-\beta_{equilibrium}}$
(D) $\dfrac{4\beta_{equilibrium}^{2}}{4-\beta_{equilibrium}^{2}}$

Q194·ChemistrySingle correctJEE Advanced 2016

Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2}(g) \rightleftharpoons 2X(g)

The standard reaction Gibbs energy,

\Delta_{r}G^{0}

, of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus,

\beta_{equilibrium}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{-1}

mol^{-1}

) The INCORRECT statement among the following, for this reaction is

(A)Decrease in the total pressure will result in formation of more moles of gaseous X
(B)At the start of the reaction, dissociation of gaseous $X_{2}$ takes place spontaneously
(C) $\beta_{equilibrium} = 0.7$
(D) $K_{c} < 1$

Q195·ChemistryMultiple correctJEE Advanced 2015

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\,^{\circ}

C was measured for the beaker and its contents (

\mathbf{Expt.\ 1}

). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (

-57.0

kJ mol

^{-1}

), this experiment could be used to measure the calorimeter constant. In a second experiment (

\mathbf{Expt.\ 2}

), 100 mL of 2.0 M acetic acid (

K_{a} = 2.0 \times 10^{-5}

) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to

\mathbf{Expt.\ 1}

) where a temperature rise of

5.6\,^{\circ}

C was measured. (Consider heat capacity of all solutions as 4.2 J g

^{-1}

K

^{-1}

and density of all solutions as 1.0 g mL

^{-1}

) The pH of the solution after

\mathbf{Expt.\ 2}

is

(A)2.8
(B)4.7
(C)5.0
(D)7.0

Q196·ChemistryMultiple correctJEE Advanced 2015

The % yield of ammonia as a function of time in the reaction

\mathrm{N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)}

,

\Delta H < 0

at (P,

T_{1}

) is given below: If this reaction is conducted at (P,

T_{2}

), with

T_{2} > T_{1}

, the % yield of ammonia as a function of time is represented by

(A)(A)
(B)(B)
(C)(C)
(D)(D)

Q197·ChemistryMultiple correctJEE Advanced 2013

The initial rate of hydrolysis of methyl acetate (1 M) by a weak acid (HA, 1M) is 1/100

^{th}

of that of a strong acid (HX, 1M), at 25

^{\circ}

C. The

K_a

of HA is

(A) $1 \times 10^{-4}$
(B) $1 \times 10^{-5}$
(C) $1 \times 10^{-6}$
(D) $1 \times 10^{-3}$

Q198·ChemistryMultiple correctJEE Advanced 2013

The

K_{sp}

of

\mathrm{Ag_2CrO_4}

is

1.1 \times 10^{-12}

at 298K. The solubility (in mol/L) of

\mathrm{Ag_2CrO_4}

in a 0.1M

\mathrm{AgNO_3}

solution is

(A) $1.1 \times 10^{-11}$
(B) $1.1 \times 10^{-10}$
(C) $1.1 \times 10^{-12}$
(D) $1.1 \times 10^{-9}$

Q199·ChemistryMultiple correctJEE Advanced 2013

The thermal dissociation equilibrium of

\mathrm{CaCO_3(s)}

is studied under different conditions.

\mathrm{CaCO_3(s)} \rightleftharpoons \mathrm{CaO(s)} + \mathrm{CO_2(g)}

For this equilibrium, the correct statement(s) is(are)

(A) $\Delta H$ is dependent on T
(B)K is independent of the initial amount of $\mathrm{CaCO_3}$
(C)K is dependent on the pressure of $\mathrm{CO_2}$ at a given T
(D) $\Delta H$ is independent of the catalyst, if any

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