AIPMT-PRELIMS Chemistry Equilibrium Class 11 Questions

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product (Kₛₚ) of Ba(OH)₂ is

A buffer solution is prepared in which the concentration of NH₃ is 0.30 M and the concentration of NH₄⁺ is 0.20 M. If the equilibrium constant, Kb for NH₃ equals 1.8 × 10⁻⁵, what is the pH of this solution?

For the reaction N₂(g) + O₂(g) ⇌ 2NO(g), the equilibrium constant is K₁. The equilibrium constant is K₂ for the reaction 2NO(g) + O₂(g) ⇌ 2NO₂(g). What is K for the reaction NO₂(g) ⇌ ½ N₂(g) + ½ O₂(g)?

In a buffer solution containing equal concentration of B⁻ and HB, the Kb for B⁻ is 10⁻¹⁰. The pH of buffer solution is

What is [H⁺] in mol/L of a solution that is 0.20 M in CH₃COONa and 0.10 M in CH₃COOH? Ka for CH₃COOH = 1.8 × 10⁻⁵.

In which of the following reactions, Kₚ and Kc are not equal?

If pH of a saturated solution of Ba(OH)₂ is 12, the value of its Kₛₚ is

The dissociation constants for acetic acid and HCN at 25°C are 1.5 × 10⁻⁵ and 4.5 × 10⁻¹⁰ respectively. The equilibrium constant for the equilibrium CN⁻ + CH₃COOH ⇌ HCN + CH₃COO⁻ would be:

The ionization constant of ammonium hydroxide is 1.77 × 10⁻⁵ at 298 K. Hydrolysis constant of ammonium chloride is:

What is the [OH⁻] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)₂?

The dissociation equilibrium of a gas AB₂ can be represented as : 2AB₂(g) ⇌ 2AB(g) + B₂(g) The degree of dissociation is 'x' and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kₚ and total pressure P is -

If the concentration of OH⁻ ions in the reaction, Fe(OH)₃(s) ⇌ Fe³⁺(aq) + 3OH⁻(aq) is decreased by \( \frac{1}{4} \) times, then equilibrium concentration of Fe³⁺ will increase by -

Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture ?

The value of equilibrium constant of the reaction, HI(g) ⇌ 1/2 H₂(g) + 1/2I₂(g) is 8.0. The equilibrium constant of the reaction, H₂(g) + I₂(g) ⇌ 2HI(g) will be -

The value of Kₚ and Kₚ for the reactions X ⇌ Y + Z and A ⇌ 2B are in ratio of 9 : 1. If degree of dissociation of X and A be equal, then total pressure at equilibrium (1) and (2) are in the ratio :

A weak acid, HA, has a Kₐ of 1.00 × 10⁻⁵. If 0.100 mole of this acid dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to

The following equilibrium constants are given: $$\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3 ; K_1$$ $$\text{N}_2 + \text{O}_2 \rightleftharpoons 2\text{NO} ; K_2$$ $$\text{H}_2 + \frac{1}{2}\text{O}_2 \rightleftharpoons \text{H}_2\text{O} ; K_3$$ The equilibrium constant for the oxidation of $\text{NH}_3$ by oxygen to give $\text{NO}$ is

Calculate the pH of a solution at 25°C that contains 1×10⁻¹⁰ M of hydronium ions, i.e., H₃O⁺.

For the reaction, CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l), ΔH = -170.8 kJ mol⁻¹ Which of the following statements is not true?

Which of the following pairs constitutes a buffer?

The hydrogen ion concentration of a 10⁻⁸ M HCl aqueous solution at 298 K (Kw = 10⁻¹⁴) is:

At 25°C, the dissociation constant of a base, BOH, is 1.0 × 10⁻¹². The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be:

What is the correct relationship between the pHs of isomolar solutions of sodium oxide (pH₁), sodium sulphide (pH₂), sodium selenide (pH₃) and sodium telluride (pH₄)?

Equilibrium constants K₁ and K₂ for the following equilibria: NO(g) + (1/2)O₂ ⇌ NO₂(g) and 2NO₂(g) ⇌ 2NO(g) + O₂(g) are related as:

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10⁻¹¹. Its solubility (in moles/litre) is:-

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In⁻) forms of the indicator by the expression -

Which one of the following compounds is not a protonic acid :

In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the above condition in the end :

The reaction quotient (Q) for the reaction : N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is given by Q = [NH₃]² / [N₂][H₂]³ . The reaction will proceed from right to left if :

The solubility product of AgI at 25°C is \( 1.0 \times 10^{-16} \text{ mol}^2 \text{ L}^{-2} \). The solubility of AgI in \( 10^{-4} \text{ N} \) solution of KI at 25°C is approximately (in \( \text{mol L}^{-1} \)):

The following equilibria are given: \( \text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3, \text{K}_1 \) \( \text{N}_2 + \text{O}_2 \rightleftharpoons 2\text{NO}, \text{K}_2 \) \( \text{H}_2 + \frac{1}{2}\text{O}_2 \rightleftharpoons \text{H}_2\text{O}, \text{K}_3 \) The equilibrium constant of the reaction \( 2\text{NH}_3 + \frac{5}{2}\text{O}_2 \rightleftharpoons 2\text{NO} + 3\text{H}_2\text{O} \) in terms of \( \text{K}_1, \text{K}_2 \) and \( \text{K}_3 \) is:

Reaction BaO₂ (s) ⇌ BaO (s) + O₂(g); ΔH = + ve. In equilibrium condition. Pressure of O₂ is depends on :-

Solubility of MX₂ – type electrolytes is 0.5 × 10⁻⁴ Mole/lit. then find out Kₛₚ of electrolytes :-

Which has highest pH :-

Solution of 0.1 N NH₄OH and 0.1 N NH₄Cl has pH 9.25, Then find out pkb of NH₄OH :-

In HS⁻, I⁻, R–NH₂, NH₃ order of proton excepting tendency will be:-

Ionisation constant of CH₃COOH is 1.7 × 10⁻⁵ and concentration of H⁺ ions is 3.4 × 10⁻³. Then find out initial concentration of CH₃COOH molecules :-

Solubility of Ag₂S salt is 3.5 × 10⁶ then find out solubility product :-

Equilibrium constant Kp for following reaction : MgCO₃(s) ⇌ MgO(s) + CO₂(g)

Correct relation b/w dissociation constant's of a di-basic acid:

For a any reversible reaction. If increases concentration of reactants. Then effect on equilibrium constant:

Conjugate acid of NH₂⁻ :

Which statement is wrong about pH and H⁺