AIIMS Chemistry Equilibrium Class 11 Questions

When 0.05 M dimethyl amine is dissolved in 0.1 M NaOH solution then the percentage dissociation of dimethyl amine is: (K_b (CH₃)₂NH = 5 x 10⁻⁴)

The compound, Sr(OH)₂ has max. solubility in acidic solution that is at low pH as shown below. Sr(OH)₂ → Sr²⁺ + 2OH⁻ It gives high amount of hydroxide ions which are neutralized by the high amount of H⁺ ions.

The value of ionic product of water increases with temperature.

For the endothermic reaction A₂ → 2A, which of the following will increase yield of monomer?

Assertion: $\text{H}_2\text{O}$ shows atmospheric nature. Reason: According to Bronsted theory, it acts as acid with $\text{NH}_3$ and a base with $\text{H}_2\text{S}$.

For the forward chemical reaction, A + B ⇌ C, The rate of reaction is, Kₑ = [C]/[A][B] And for reverse chemical reaction, C ⇌ A + B, The rate of reaction is, Kₑ = [A][B]/[C] Thus, Kₑ = 1/Kₑ

The reaction in pure water is given as, XB₂ → X²⁺ + 2B⁻ The solubility product for the reaction is, Kₛₚ = 4 × 3 × S × (0.001)² S = 4 × 3 × 10⁶

The dissociation is given as, Kₐ = [H⁺]²/C = (3.6×10⁻⁴)²/0.02 = 6.48×10⁻⁶

For the reaction: $$\text{H}_2(\text{g}) + \text{CO}_2(\text{g}) \rightleftharpoons \text{CO}(\text{g}) + \text{H}_2\text{O}(\text{g})$$ If the initial concentration of $[\text{H}_2] = [\text{CO}_2]$ and $x\text{ mol/L}$ of hydrogen is consumed at equilibrium, the correct expression of $k_p$ is:

Calculate the degree of hydrolysis and $\text{pH}$ of $0.02\text{ M}$ ammonium cyanide ($\text{NH}_4\text{CN}$) at $298\text{ K}$ ($K_a \text{ of HCN} = 4.99 \times 10^{-9}$, $K_b \text{ of NH}_4\text{OH} = 1.77 \times 10^{-5}$)

Assertion (A): Adding an inert gas to the dissociation equilibrium of $\text{N}_2\text{O}_4$ at constant temperature and pressure increases the dissociation. Reason (R): Due to the addition of the inert gas, the molar concentration of reactants and products decreases.

‘a’ moles of PCl₅ are heated in a closed container to equilibrate PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) at pressure of p atm. If x moles of PCl₅ dissociate at equilibrium, then

Consider the reaction equilibrium Ice ⇌ Water – x kcal The favourable conditions for forward reaction are

Which has the highest pH?

$\frac{K_p}{K_c}$ for following reaction will be $\text{CO}_{(g)} + \frac{1}{2}\text{O}_{2(g)} \rightarrow \text{CO}_{2(g)}$

At 60° and 1 atm, N₂O₄ is 50% dissociated into NO₂ then Kₚ is

Kₛₚ of CaSO₄·5H₂O is 9 × 10⁻⁶, find the volume for 1 g of CaSO₄ (M.wt. = 136).

Which of the following is not a characteristic of equilibrium?

25 mL, 0.2 M Ca(OH)₂ is neutralised by 10 mL of 1 M HCl. Then pH of resulting solution is

What is the pH of 0.01 M glycine solution? For glycine Ka₁ = 4.5×10⁻³ and Ka₂ = 1.7×10⁻¹⁰ at 298 K.

Assertion: The equilibrium constant is fixed and a characteristic for any given chemical reaction at a specified temperature. Reason: The composition of the final equilibrium mixture at a particular temperature depends upon the starting amount of reactants.

pH of a 0.01 M solution (Kₐ = 6.6 × 10⁻⁴)

A vessel of one litre capacity containing 1 mole of SO₃ is heated till a state of equilibrium is attained. 2SO₃(g) ⇌ 2SO₂(g) + O₂(g). At equilibrium, 0.6 moles of SO₂ had formed. The value of equilibrium constant is

The equilibrium constant for mutarotation of α-D Glucose ⇌ β-D Glucose is 1.8. What percentage of α form remains at equilibrium?

Assertion: Ice ⟶ water, if pressure is applied water will evaporate. Reason: Increases of pressure pushes the equilibrium towards the side in which number of gaseous molecule increases.

Assertion: In an acid-base titration involving strong base and a weak acid, methyl orange can be used as an indicator. Reason: Methyl orange changes its colour in pH range of 7 to 9.

Assertion: According to Le⁻Chatelier’s principle addition of heat to an equilibrium solid ⇌ liquid results in decrease in the amount of solid. Reason: Reaction is endothermic, so on heating forward reaction is favoured.

The pH of the solution obtained on neutralisation of 40 mL 0.1 M NaOH with 40 mL 0.1 M CH₃COOH is

Assertion : Mixture of CH₃COOH and CH₃COONH₄ is an example of acidic buffer. Reason : Acidic buffer contains equimolar mixture of weak acid and its salt with weak base.

Assertion : The equilibrium constant is fixed and a characteristic for any given chemical reaction at a specified temperature. Reason : The composition of the final equilibrium mixture at a particular temperature depends upon the starting amount of reactants.

40 ml of 0.1 M ammonia solution is mixed with 20 ml of 0.1 M HCl. What is the pH of the mixture? (pKₐ of ammonia solution is 4.74)

Assertion : Sb₂S₃ is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to S²⁻ ions reduces the solubility of Sb₂S₃.

When 10 ml of 0.1 M acetic acid (pKₐ = 5.0) is titrated against 10 ml of 0.1 M ammonia solution (pKₐ = 5.0), the equivalence point occurs at pH

For reaction, 2NOCl (g) ⇌ 2NO (g) + Cl₂ (g), Kc at 427°C is 3 x 10⁻⁶ L·mol⁻¹. The value of Kp is nearly

Among the following the dissociation constant is highest for

For the equilibrium H₂O(l) ⇌ H₂O(g) at 1 atm and 298 K,

What is the pH of 0.01 M glycine solution? For glycine, Kₐ₁ = 4.5 × 10⁻³ and Kₐ₂ = 1.7 × 10⁻¹⁰ at 298 K?

Of the following which change will shift the reaction towards the product? I₂(g) ⇌ 2I(g) ΔHᵒ (298 K) = +150 kJ

Assertion : The pKₐ of acetic acid is lower than that of phenol. Reason : Phenoxide ion is more resonance stabilised.

Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl. Reason : Kₛₚ of AgCl < Kₛₚ of AgBr

Which one of the following is not a buffer solution?

In which of the following acid-base titration, pH is greater than 8 at equivalence point?

Assertion : BaCO₃ is more soluble in HNO₃ than in plain water. Reason : Carbonate is a weak base and reacts with the H⁺ from the strong acid, causing the barium salt to dissociate.

Assertion : Increasing pressure on pure water decreases its freezing point. Reason : Density of water is minimum at 273 K.

At 80°C, distilled water has concentration equal to 1 × 10⁻⁶ mole/litre. The value of Kw at this temperature will be:

The pH of solution containing 0.10 M sodium acetate and 0.03 M acetic acid is (pKa for CH₃COOH = 4.57)

The solubility of CuBr is 2 × 10⁻⁴ mol/L at 25°C. The Ksp value for CuBr is

Which of the following is strongest Bronsted base?

When the temperature of reactions will increase then the effect on pH value will

The pH of aqueous solution of ammonium formate is (pKₐ of HCOOH = 3.8 and pK_b of NH₃ = 4.8)