Consider the equilibrium 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:

Statement (A) is correct: Increasing pressure by compressing the volume increases active mass/concentration (c = n/V) for both reactants and products instantly. Statement (B) is correct: The reaction has Delta ng = 2 - 4 = -2. Increasing pressure shifts equilibrium towards the direction of fewer gaseous moles, which is the forward path. Statement (C) is incorrect: Equilibrium constant (K) is exclusively temperature-dependent and does not alter with pressure changes. Statement (D) is correct: Confirms that equilibrium constant remains unchanged. Always remember: pressure changes shift positions but NEVER alter the value of the equilibrium constant Kc or Kp. Only temperature changes can change K. Class 11 Chemistry: Equilibrium

Consider the equilibrium 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 i

Statement (A) is correct: Increasing pressure by compressing the volume increases active mass/concentration (c = n/V) for both reactants and products instantly. Statement (B) is correct: The reaction has Delta ng = 2 - 4 = -2. Increasing pressure shifts equilibrium towards the direction of fewer gaseous moles, which is the forward path. Statement (C) is incorrect: Equilibrium constant (K) is exclusively temperature-dependent and does not alter with pressure changes. Statement (D) is correct: Con

Consider the equilibrium 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:

Statement (A) is correct: Increasing pressure by compressing the volume increases active mass/concentration (c = n/V) for both reactants and products instantly. Statement (B) is correct: The reaction has Delta ng = 2 - 4 = -2. Increasing pressure shifts equilibrium towards the direction of fewer gaseous moles, which is the forward path. Statement (C) is incorrect: Equilibrium constant (K) is exclusively temperature-dependent and does not alter with pressure changes. Statement (D) is correct: Confirms that equilibrium constant remains unchanged. Always remember: pressure changes shift positions but NEVER alter the value of the equilibrium constant Kc or Kp. Only temperature changes can change K. Class 11 Chemistry: Equilibrium

Consider the equilibrium 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 i

Statement (A) is correct: Increasing pressure by compressing the volume increases active mass/concentration (c = n/V) for both reactants and products instantly. Statement (B) is correct: The reaction has Delta ng = 2 - 4 = -2. Increasing pressure shifts equilibrium towards the direction of fewer gaseous moles, which is the forward path. Statement (C) is incorrect: Equilibrium constant (K) is exclusively temperature-dependent and does not alter with pressure changes. Statement (D) is correct: Con

Consider the equilibrium If the pressure applied over the system increases by two fold at constant temperature then…

Year	2026	2025	2024	Total
Questions	10	17	8	35

Q30 jee_main_2025_28_jan_evening Solubility Product

Arrange the following in increasing order of solubility product:

Ca(OH)₂, AgBr, PbS, HgS

A. $PbS < HgS < Ca(OH)₂ < AgBr$ $PbS < HgS < Ca(OH)_{2} < AgBr$
B. $HgS < PbS < AgBr < Ca(OH)₂$ $HgS < PbS < AgBr < Ca(OH)_{2}$
C. $Ca(OH)₂ < AgBr < HgS < PbS$ $Ca(OH)_{2} < AgBr < HgS < PbS$
D. $HgS < AgBr < PbS < Ca(OH)₂$ $HgS < AgBr < PbS < Ca(OH)_{2}$

Solution

Related Formula

The solubility product constant ( $Kₛₚ$ $K_{sp}$) reflects the equilibrium position of a sparingly soluble salt in water.

Core Logic

Based on standard literature $Kₛₚ$ $K_{sp}$ values at $298 K$ $298\text{ K}$:

$HgS$ $HgS$: $\approx 4 \times 10⁻⁵³$ $\approx 4 \times 10^{-53}$ (extremely insoluble, Group IIB cation analysis)
$PbS$ $PbS$: $\approx 8 \times 10⁻²⁸$ $\approx 8 \times 10^{-28}$ (highly insoluble, Group IIA cation analysis)
$AgBr$ $AgBr$: $\approx 5 \times 10⁻¹³$ $\approx 5 \times 10^{-13}$ (sparingly soluble halide salt)
$Ca(OH)₂$ $Ca(OH)_2$: $\approx 5.5 \times 10⁻⁶$ $\approx 5.5 \times 10^{-6}$ (moderately soluble base)

Step 1: Arrangement

Comparing these $Kₛₚ$ $K_{sp}$ orders:

4 \times 10⁻⁵³ < 8 \times 10⁻²⁸ < 5 \times 10⁻¹³ < 5.5 \times 10⁻⁶

Hence, the correct increasing sequence is: $HgS < PbS < AgBr < Ca(OH)₂$ $HgS < PbS < AgBr < Ca(OH)_2$.

Pattern Recognition

Sulphides of heavy transition metals like $Hg²⁺$ $Hg^{2+}$ and $Pb²⁺$ $Pb^{2+}$ have exceptionally small $Kₛₚ$ $K_{sp}$ values compared to halides or hydroxides. Among sulphides, $HgS$ $HgS$ is famously known to have one of the lowest solubility products found in inorganic qualitative analysis.

Chapter Mix

Class 11 Chemistry: Equilibrium

Q jee_main_2025_29_jan_morning Degree of Dissociation and Equilibrium Constant

At temperature

T

, compound

AB2(g)

dissociates as:

AB2(g) leftharpoons AB(g) + (1)/(2)B2(g)

having a degree of dissociation

x

(

x ll 1

). The correct expression for

x

in terms of

Kₚ

and total pressure

p

is:

x = ((2Kₚ²)/(p))1/3

A. $[3] 2Kₚp$ $\sqrt[3]{\frac{2K_{p}}{p}}$
B. $[4] 2Kₚp$ $\sqrt[4]{\frac{2K_{p}}{p}}$
C. $[3] 2Kₚ²p$ $\sqrt[3]{\frac{2K_{p}^{2}}{p}}$
D. $Kₚ$ $\sqrt{\mathrm{K_p}}$

Solution

Related Formula

Kₚ = pAB \cdot pB₂1/2pAB₂

Core Logic

Consider the equilibrium reaction setup:

State	$AB2(g)$ $\mathrm{AB}_{2(g)}$	$leftharpoons$ $\rightleftharpoons$	$AB(g)$ $\mathrm{AB}_{(g)}$	$+$ $+$	$(1)/(2)B2(g)$ $\frac{1}{2}\mathrm{B}_{2(g)}$
Initial moles:	$1$ $1$		$0$ $0$		$0$ $0$
Equilibrium moles:	$1 - x$ $1 - x$		$x$ $x$		$(x)/(2)$ $\frac{x}{2}$

Total equilibrium moles:

ntotal = 1 - x + x + (x)/(2) = 1 + (x)/(2)

Since $x ll 1$ $x \ll 1$, total moles $ntotal \approx 1$ $n_{\text{total}} \approx 1$ and $(1 - x) \approx 1$ $(1 - x) \approx 1$.

Partial pressures:

pAB₂ \approx p

pAB \approx x p

pB₂ \approx (x)/(2) p

Substituting into $Kₚ$ $K_p$:

Kₚ = (x p) \cdot ((x p)/(2))1/2p = x \cdot ((x p)/(2))1/2 = x3/2 p1/2\sqrt(2)

Squaring both sides and solving for $x$ $x$:

Kₚ² = (x³ p)/(2) x³ = (2Kₚ²)/(p)

x = 3\sqrt((2Kₚ²)/(p))

Pattern Recognition

For $Δ ng = 0.5$ $\Delta n_g = 0.5$ involving degree of dissociation $x ll 1$ $x \ll 1$, tracking total pressure approximations ensures an immediate analytical solution without full polynomial expansion.

Chapter Mix

Class 11 Chemistry: Chemical Equilibrium

Q90 jee_main_2024_01_february_morning Hydrolysis of Salts

Kₐ

for

CH₃COOH

is

1.8 \times 10⁻⁵

and

Kb

for

NH₄OH

is

1.8 \times 10⁻⁵

. The pH of ammonium acetate solution will be

Numerical Answer. Answer: 7 to 7

Solution

Related Formula

For a salt of weak acid and weak base (like ammonium acetate):

pH = (1)/(2) (pKw + pKₐ - pKb)

Core Logic

Ammonium acetate ( $CH₃COONH₄$ $CH_3COONH_4$) is a salt formed from a weak acid ( $CH₃COOH$ $CH_3COOH$) and a weak base ( $NH₄OH$ $NH_4OH$). Given: $Kₐ = 1.8 \times 10⁻⁵$ $K_a = 1.8 \times 10^{-5}$ $Kb = 1.8 \times 10⁻⁵$ $K_b = 1.8 \times 10^{-5}$

Since $Kₐ = Kb$ $K_a = K_b$, taking the negative logarithm gives $pKₐ = pKb$ $\mathrm{p}K_a = \mathrm{p}K_b$.

Step 1: Calculate pH

pH = pKw + pKₐ - pKb2

Substitute $pKₐ = pKb$ $\mathrm{p}K_a = \mathrm{p}K_b$:

pH = pKw2

At standard temperature (298 K), $pKw = 14$ $\mathrm{p}K_w = 14$.

pH = (14)/(2) = 7

Pattern Recognition

If $Kₐ = Kb$ $K_a = K_b$ for a weak acid-weak base salt, the hydrolysis of cation and anion perfectly balance out, making the resulting solution exactly neutral (pH = 7) regardless of the concentration of the salt.

Chapter Mix

Class 11 Chemistry: Equilibrium

Q jee_main_2024_29_january_evening Equilibrium Constant Calculation

The following concentrations were observed at

500 K

for the formation of

NH₃

from

N₂

and

H₂

. At equilibrium:

[N₂] = 2 \times 10⁻² M

,

[H₂] = 3 \times 10⁻² M

, and

[NH₃] = 1.5 \times 10⁻² M

. Equilibrium constant for the reaction is ________.

Numerical Answer. Answer: 417 to 417

Solution

Related Formula

N₂(g) + 3H₂(g) leftharpoons 2NH₃(g)

Kc = [NH₃]²[N₂][H₂]³

Core Logic

Substituting the given equilibrium concentrations into the equilibrium constant expression:

Kc = (1.5 \times 10⁻²)²(2 \times 10⁻²) \times (3 \times 10⁻²)³

Evaluating the values step-by-step:

Kc = 2.25 \times 10⁻⁴(2 \times 10⁻²) \times (27 \times 10⁻⁶)

Step 1: Final Arithmetic Integration

Kc = 2.25 \times 10⁻⁴54 \times 10⁻⁸ = (2.25)/(54) \times 10⁴ = 0.041666 \times 10⁴ \approx 416.67

Rounding to the nearest integer yields 417.

Pattern Recognition

Pay close attention to the cubic exponent in the denominator derived from the hydrogen stoichiometric coefficient ( $3$ $3$). Small calculation errors here can significantly alter the result.

Chapter Mix

Class 11 Chemistry: Chemical Equilibrium

Q76 jee_main_2024_27_jan_morning Salt Hydrolysis

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

Kₐ

and

Kb

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

Solution

Related Formula

pH of a weak acid-weak base salt system:

pH = 7 + (1)/(2)(pKₐ - pKb)

Core Logic

Ammonium carbonate, $(NH₄)₂CO₃$ $(\text{NH}_4)_2\text{CO}_3$, is formed from a weak acid ( $H₂CO₃$ $\text{H}_2\text{CO}_3$, $Kₐ \approx 4.3 \times 10⁻⁷$ $K_a \approx 4.3 \times 10^{-7}$) and weak base ( $NH₄OH$ $\text{NH}_4\text{OH}$, $Kb \approx 1.8 \times 10⁻⁵$ $K_b \approx 1.8 \times 10^{-5}$). Since $Kb > Kₐ$ $K_b > K_a$, the aqueous medium accumulates an excess of hydroxyl particles over hydronium, forming a basic system ( $pH > 7$ $\text{pH} > 7$). Both statements are structurally accurate descriptions.

Chapter Mix

Class 11 Chemistry: Equilibrium

Solution & Explanation

Core Logic

Pattern Recognition

Chapter Mix

Reference Study Guides

More Equilibrium Previous-Year Questions — Page 6

Solution

Related Formula

Core Logic

Step 1: Arrangement

Pattern Recognition

Chapter Mix

Solution

Related Formula

Core Logic

Pattern Recognition

Chapter Mix

Solution

Related Formula

Core Logic

Step 1: Calculate pH

Pattern Recognition

Chapter Mix

Solution

Related Formula

Core Logic

Step 1: Final Arithmetic Integration

Pattern Recognition

Chapter Mix

Solution

Related Formula

Core Logic

Chapter Mix

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