Ionic Equilibrium - Class 12 MCQ

Which equilibrium can be decribed as Lewis acid-base reaction but not Bronsted acid-base reaction?

The correct representation for the solubility product constant of Ag₂CrO₄ is:

The correct statement for the equilibrium is:
HCIO₄ + H₂O  ⇌ H₃O⁺ + CIO^-₄
 

The rapid change of pH near the stochiometric point of an acid-base titration is the basic of indicator detection. pH of the solution is related to the ratio of the  concentration of conjugate acid (HIn) and base (In^- ) form of the indicator by the expression:

One litre of water contains 10^-7 mole H⁺ ions. Degree of ionisation of water is:    

If  CuSO₄ + 5H₂O (s)  ⇌ CuSO₄ . 3H₂O(S) + 2H₂O(v)K_p = 1.086 * 10^-4  atm² at 25⁰C. The efflorescent nature of  CuSO₄ 5H₂O can be noticed when vapour pressure of H₂O in atmosphere is:

The equilibrium constant for the reaction, 3C₂H₂  ⇌ C₆H₆ ,is 4.0 at T.K. If the equilibrium concentration of C₂H₂ is 0.5 mol/litre, the concentration of C₆H₆ is:    

40% of a mixture of 0.2 mole of N2 and 0.6 mole of H2 react to give NH3 according to the equation, N₂(g) + 3h₂(g)  ⇌2NH₃ (g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is:

When 20 g of CaCO₃ were put into 10 litre flask and heated to 8000C, 35% of CaCO₃ remained unreacted at equilibrium. Kp for decomposition of CaCO₃ is:    

The value of K_p1 and K_p2 for the reactions
X  ⇌ Y+Z ..(1)
A  ⇌ 2b ....(2)
are in the ration 9 : 1. If degree of dissociation of X and A be equal, them total pressure at equilibrium (1) and (2) are in the ratio:

At constant temperature in one litre vessel, when the reaction, 2SO₃(g)→2SO₂(g)+O₂(g) is at equilibrium, the SO₂ concentration is 0.6 M, initial concentration of SO₃ is 1 M. The equilibrium constant is:    

HCOOH  ⇌ HCOO^- + H⁺; K_s = 1.7*10^-4
The ionization of formic acid is represented above. Calculate [H⁺] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:

When NaCI is added gradually to the saturated solution of AgCI then which of the following plot is correct?

What is the molar solubility of AgBr in 0.1 M Na₂S₂O₃?

The solubility product of different sparingly soluble salts are:
(i) XY = 4x10^-20    
(ii) X₂Y = 3.2x10^-11    
(iii)  XY₃ = 2.7 x 10^-31
The increasing order of solubility is:

An aqueous solution of hydrogen sulphide shows the equilibrium,
H₂S ⇌ H⁺ +HS^-
If dilute hydrochloric acid is added to an aqueous solution of hydrogen sulphide without any change in temperature, then:

The equilibrium constant for decomosition of Hbr at 500 K and 700 K are 10^-10 and 10^-5 respectively. The reaction is:    

The reaction quotient (Q) for the reaction is given by:
N₂(g)+3H₂(g) ⇌ 2NH₃;

The reaction will proceed from right to left if:

Which of the following gas phase reaction has K_p less than K_c?

For the gaseous phase reaction, 2NO ⇌ N₂ + O₂, ΔH° = -43.5 kcal mol^-1 which statement is correct for,
N₂(g)+O₂(g) ⇌ 2NO(g) ?

The volume of the reactions vessel containing an equilibrium mixture in the reaction.
SO₂Cl₂ (g) ⇌ SO₂(g)+Cl₂(g)
is increased. When equilibrium is restablished.

100ml of 1N NH₄OH (K_b=5x10^-5) is neutralized to equivalence point by 1N HCl. The PH of solution at equivalence point is

Number of H⁺ ions present in 10 mL of a solution of pH =  3 is:

To 100 mL of 0.1 M AgNO₃ solution solid K₂SO₄ is added. The concentration of K₂SO₄ that shows the precipitation is,(K_sp for Ag₂SO₄ = 6.4 x 10^-5 M)

The composition of an acidic buffer mixture made up of HA and NaA of total molarity 0.29 having pH = 4.4 and K_a = 1.8 x 10^-5 in terms of concentration of salt and acid respectively is:     

At 25⁰ C, K_b for a base BOH is 1.0 x 10^-12. The [OH^- ] in 0.01 M aqueous solution of base is:
 

Which of the following is a buffer solution?