NEET Chemistry Equilibrium Class 11 Questions

The solubility of BaSO₄ in water is 2.42 × 10⁻³ g L⁻¹ at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO₄ = 233 g mol⁻¹)

Kₐ, Kₓ and Kₑ are the respective ionisation constants for the following reactions. H₂S ⇌ H⁺ + HS⁻ HS⁻ ⇌ H⁺ + S²⁻ H₂S ⇌ 2H⁺ + S²⁻ The correct relationship between Kₐ, Kₓ and Kₑ is

If K₁ and K₂ are the respective equilibrium constants for the two reactions XeF₆(g) + H₂O(g) ⇌ XeOF₄(g) + 2HF(g) XeO₄(g) + XeF₆(g) ⇌ XeOF₄(g) + XeO₃F₂(g) The equilibrium constant of the reaction XeO₄(g) + 2HF(g) ⇌ XeOF₄(g) + H₂O(g) will be

What will be the solubility of AgCl in 0.05 M NaCl aqueous solution if solubility product of AgCl is 1.5 × 10⁻¹⁰?

PCl₅, PCl₃ and Cl₂ are at equilibrium at 500 K in a closed container and their concentrations are 0.8 × 10⁻³ mol L⁻¹, 1.2 × 10⁻³ mol L⁻¹ and 1.2 × 10⁻³ mol L⁻¹ respectively. The value of Kc for the reaction : PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) will be:

For the following reaction: NO(g) + O₃(g) ⟶ NO₂(g) + O₂(g) The value of Kc is 8.2 x 10⁴. What will be the value of Kc for the reverse reaction?

In which of the following reactions, the equilibrium remains unaffected on addition of small amount of argon at constant volume?

The solubility of AgCl(s) with solubility product 1.6 × 10⁻¹⁰ in 0.1 M NaCl solution would be

Which of the following will produce a buffer solution when mixed in equal volumes?

In a qualitative analysis, Bi³⁺ is detected by appearance of precipitate of BiO(OH)(s). Calculate pH when the following equilibrium exists at 298 K. BiO(OH)(s) ⇌ BiO⁺(aq) + OH⁻(aq), K = 4 × 10⁻¹⁰ (Given : log2 = 0.3010)

At 298 K, a certain buffer solution contains equal concentrations of X⁻ and HX, Kb for X⁻ is 10⁻¹⁰. What is the pH of this buffer solution?

Given below are certain reactions. Identify the reaction for which Kₚ ≠ Kc.

Phosphoric acid ionizes in three steps with their ionization constant values Kₐ₁, Kₐ₂ and Kₐ₃, respectively, while K is the overall ionization constant. Which of the following statements are true? A. log K = log Kₐ₁ + log Kₐ₂ + log Kₐ₃ B. H₃PO₄ is a stronger acid than H₂PO₄⁻ and HPO₄²⁻. C. Kₐ₁ > Kₐ₂ > Kₐ₃ D. Kₐ₁ = (Kₐ₃ + Kₐ₂) / 2 Choose the correct answer from the options given below:

For the reaction A(g) ⇌ 2B(g), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K. [Given : R = 0.0831 L atm mol⁻¹ K⁻¹] Kₚ for the reaction at 1000 K is

Higher yield of NO in N₂(g) + O₂(g) ⇌ 2NO(g) can be obtained at [ΔH of the reaction = + 180.7 kJ mol⁻¹] A. higher temperature B. lower temperature C. higher concentration of N₂ D. higher concentration of O₂ Choose the correct answer from the options given below:

For the reaction 2A ⇌ B + C, Kc = 4×10⁻³. At a given time, the composition of reaction mixture is: [A] = [B] = [C] = 2×10⁻³ M. Then, which of the following is correct?

In which of the following equilibria, Kp and Kc are NOT equal?

Consider the following reaction in a sealed vessel at equilibrium with concentrations of N₂ = 3.0 × 10⁻³ M, O₂ = 4.2 × 10⁻³ M and NO = 2.8 × 10⁻³ M. 2NO(g) ⇌ N₂(g) + O₂(g) If 0.1 mol L⁻¹ of NO(g) is taken in a closed vessel, what will be the degree of dissociation (α) of NO(g) at equilibrium?

The equilibrium concentrations of the species in the reaction A + B ⇌ C + D are 2, 3, 10 and 6 mol L⁻¹, respectively at 300 K. ΔG° for the reaction is (R = 2 cal / mol K)

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is ______. [Given pKₐ of CH₃COOH = 4.57]

3O₂(g) ⇌ 2O₃(g) for the above reaction at 298 K, Kc is found to be 3.0 × 10⁻⁵⁹. If the concentration of O₂ at equilibrium is 0.040 M then concentration of O₃ in M is

The pKₐ of dimethylamine and pKₐ of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethylammonium acetate solution is :

Find out the solubility of Ni(OH)₂ in 0.1 M NaOH. Given that the ionic product of Ni(OH)₂ is 2 × 10⁻¹⁵.

Conjugate bases for Bronsted acids H₂O and HF are ________.

Which will make basic buffer?

The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber’s process is ______.

pH of a saturated solution of Ca(OH)₂ is 9. The solubility product (Kₛₚ) of Ca(OH)₂ is

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations: i. 60 mL 10 M HCl + 40 mL 10 M NaOH ii. 55 mL 10 M HCl + 45 mL 10 M NaOH iii. 75 mL 5 M HCl + 25 mL 5 M NaOH iv. 100 mL 10 M HCl + 100 mL 10 M NaOH pH of which one of them will be equal to 1?

The solubility of BaSO₄ in water is 2.42 × 10⁻³ g L⁻¹ at 298 K. The value of its solubility product (Ksp) will be (Given : molar mass of BaSO₄ = 233 g mol⁻¹)

Which one of the following conditions will favour maximum formation of the product in the reaction? A₂(g) + B₂(g) ⇌ X₂(g); ΔH = −x kJ

A 20 litre container at 400 K contains CO₂(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value, will be (Given that: SrCO₃(s) ⇌ SrO(s) + CO₂(g), Kₚ = 1.6 atm)

Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 × 10⁻⁴ mol L⁻¹. Solubility product of Ag₂C₂O₄ is:

MY and NY₃, two nearly insoluble salts, have the same Ksp values of 6.2 × 10⁻¹³ at room temperature. Which statement would be TRUE in regard to MY and NY₃?

If the value of an equilibrium constant for a particular reaction is 1.6 × 10¹², then at equilibrium the system will contain ______.

The Ksp of Ag₂CrO₄, AgCl, AgBr and AgI are respectively, 1.1 × 10⁻¹², 1.8 × 10⁻¹⁰, 5.0 × 10⁻¹³ and 8.3 × 10⁻¹⁷. Which one of the following salts will precipitate last if AgNO₃ solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na₂CrO₄?

Acidity of diprotic acids in aqueous solutions increases in the order:

For the reversible reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat The equilibrium shifts in forward direction

Which of the following salts will give the highest pH in water?

Which of the following statements is CORRECT for the spontaneous adsorption of a gas?

Accumulation of lactic acid (HC₃H₅O₃), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociated. The value of dissociation constant, Kₐ, for this acid will be:

At 100°C the Kw of water is 55 times its value at 25°C. What will be the pH of neutral solution? (log 55 = 1.74)

The dissociation constant of a weak acid is 1 × 10⁻⁵. In order to prepare a buffer solution with a pH = 5, the [salt]/[Acid] ratio should be:

The values of Ksp of CaCO₃ and CaC₂O₄ are 4.7 × 10⁻⁹ and 1.3 × 10⁻⁹ respectively at 25°C. If the mixture of these two is washed with water, what is the concentration of Ca²⁺ ions in water?