Class 11 Chemistry Chapter 7 Equilibrium MCQ Questions with Answer

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Equilibrium Class 11 MCQ Question with Answer

Class 11 Chemistry MCQ with answers are given here to Chapter 7 Equilibrium. These MCQs are based on the latest CBSE board syllabus and relate to the latest Class 11 Chemistry syllabus. By Solving these Class 11 MCQs, you will be able to analyze all of the concepts quickly in the chapter and get ready for the Class 11 Annual exam.

Learn Class 11 Equilibrium MCQs with answers pdf free download according to the latest CBSE and NCERT syllabus. Students should prepare for the examination by solving CBSE Class 11 Chemistry Equilibrium MCQ with answers given below

Question 1. The values of Kp₁ and Kp₂ for the reactions, X ⇌ Y + Z …(i) A ⇌ 2B …(ii) are in the ratio 9 : 1. If degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and ii) are in the ratio                                       
(a) 36 : 1
(b) 1 : 1
(c) 3 : 1
(d) 1 : 9

Question 2. If the concentration of OH– ions in the reaction Fe(OH)₃(s) ⇌ Fe³⁺_(aq) + 3OH– _(aq) is decreased by 1/4 times, then equilibrium concentration of Fe³⁺ will increase by                           
(a) 64 times
(b) 4 times
(c) 8 times
(d) 16 times.

Question 3. In liquid-gas equilibrium, the pressure of vapours above the liquid is constant at                           
(a) constant temperature
(b) low temperature
(c) high temperature
(d) none of these.

Question 4. The reaction, 2A_(g) + B_(g) ⇌ 3C_(g) + D_(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is easured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression                               
(a) [(0.75)³(0.25)] ÷ [(1.00)²(1.00)]
(b) [(0.75)³(0.25)] ÷ [(0.50)²(0.75)]
(c) [(0.75)³(0.25)] ÷ [(0.50)²(0.25)]
(d) [(0.75)³(0.25)] ÷ [(0.75)²(0.25)]

Question 5. Which of the following statements is correct for a reversible process in a state of equilibrium?                   
(a) ΔG° = –2.30 RT log K
(b) ΔG° = 2.30 RT log K
(c) ΔG = –2.30 RT log K
(d) ΔG = 2.30 RT log K

Question 6. Which one of the following conditions will favour maximum formation of the product in the reaction A_2(g) + B_2(g) ⇌ X2_(g), ΔrH = –X kJ ?                         
(a) Low temperature and high pressure
(b) Low temperature and low pressure
(c) High temperature and high pressure
(d) High temperature and low pressure

Question 7. If the value of equilibrium constant for a particular reaction is 1.6 × 1012, then at equilibrium the system will contain                             
(a) mostly products
(b) similar amounts of reactants and products
(c) all reactants
(d) mostly reactants. 

Question 8. 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 aseous mixture under the aforesaid condition in the end?                                             
(a) 20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
(b) 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
(c) 20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen
(d) 20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen

Question 9. For the reversible reaction, N_2(g) + 3H_2(g) ⇌ 2NH_3(g) + heat The equilibrium shifts in forward direction     
(a) by increasing the concentration of NH3(g)
(b) by decreasing the pressure
(c) by decreasing the concentrations of N2(g) and H2(g)
(d) by increasing pressure and decreasing emperature.

Question 10. KMnO4 can be prepared from K₂MnO₄ as per the reaction,3MnO₄ 2– + 2H₂O  ⇌  2MnO4 – + MnO₂ + 4OH– The reaction can go to completion by removing OH– ions by dding                                             
(a) CO₂
(b) SO₂
(c) HCl
(d) KOH

Question 11. For any reversible reaction, if we increase concentration of the reactants, then effect onequilibrium constant                                         
(a) depends on amount of concentration
(b) unchange
(c) decrease
(d) increase. 

Question 12. A 20 litre container at 400 K contains CO_2(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 he movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value, will be (Given that : SrCO_3(s) ⇌  SrO(s) + O_2(g), K_p = 1.6 atm)                                   
(a) 10 litre
(b) 4 litre
(c) 2 litre
(d) 5 litre

Question 13. In which of the following equilibrium Kc and Kp are not equal?                               
(a) 2NO^(g) ⇌ N_2(g) + O_2(g)
(b) SO_2(g) + NO_2(g) ⇌ SO_3(g) + NO_(g)
(c) H2_(g) + I_2(g) ⇌ 2HI_(g)
(d) 2C_(s) + O2(g)  ⇌ 2CO_2(g) 

Question 14. Aqueous solution of which of the following compounds is the best conductor of electric current?              
(a) Hydrochloric acid, HCl
(b) Ammonia, NH₃
(c) Fructose, C₆H1₂O₆
(d) Acetic acid, C₂H4O₂

Question 15. Aqueous solution of acetic acid contains                                                 
(a) CH₃COO^– and H⁺
(b) CH₃COO^–, H₃O⁺ and CH₃COOH
(c) CH₃COO^–, H₃O⁺ and H⁺
(d) CH₃COOH, CH₃COO^– and H⁺

Question 16. According to Le Chatelier’s principle, adding heat toa solid and liquid in equilibrium will cause the             
(a) temperature to increase
(b) temperature to decrease
(c) amount of liquid to decrease
(d) amount of solid to decrease.

Question 17. Which one of the following information can be obtained on the basis of Le Chatelier principle?                 
(a) Dissociation constant of a weak acid
(b) Entropy change in a reaction
(c) Equilibrium constant of a chemical reaction
(d) Shift in equilibrium position on changing value of a constraint

Question 18. The pH of a 0.1 M solution of NH₄ OH (having Kb = 1.0 x 10^-5 ) is equal to
(a) 10
(b) 6
(c) 11
(d) 12     

Question 19. The pH ofa solution obtained by mixing 50 mL of 1 N HCl and 30 mL of 1 N NaOH is (log 2.5 = 0.3979)
(a) 3.979
(b) 0.6021
(c) 12.042
(d) 1.2042     

Question 20. Conjugate base for Bronsted acids H₂O and HF are                                                   
(a) H3O⁺ and H₂F⁺, respectively
(b) OH^– and H₂F^+, respectively
(c) H₃O⁺ and F^–, respectively
(d) OH^– and F^–, respectively.

Question 21. The value of DH for the reaction X_2(g) + 4Y_2(g) ⇌ 2XY_4(g) is less than zero.Formation of XY_4(g) will be favoured at                                             
(a) high temperature and high pressure
(b) low pressure and low temperature
(c) high temperature and low pressure
(d) high pressure and low temperature.

Question 22. Which of the following solutions will have pH = 9 at 298 K? 
(a) 1 X 10^-9 M HCl solution
(b) 1 x 10^-5 M NaOH solution
(c) 1 X 10^-9 M KOH solution
(d) Both (a) and (b)     

Question 23. pH of a 0.0001 M HCI solution is 
(a) 4.0
(b) 2 .0
(c) 6 .0
(d) 7.0           

Question 24. pH of an aqueous solution containing 10^-8 mol /L of HCI is 
(a) 8
(b) 10
(c) 6.96
(d) 12   

Question 25. Calculate the pH of a solution in which hydrogen ion concentration is 0.005 g-equi /L. 
(a) 2.3
(b) 2 .8
(c) 2 .9
(d) 2.6       

Question 26. The approximately pH of0.005 molar sulphw·ic acid is
(a) 0.005
(b) 2 
(c) 1
(d) 0.01     

Question 27. 100 mL of 0.015 M HCI solution is mixed with 100 mL of 0.005 M HCI. What is the pH of the resultant solution?
(a) 2.5
(b) 1.5 
(c) 2
(d) 1     

Question 28. Hydroxyl ion concentration of 10^-2 M HCl is 
(a) 1 x 10¹ mol dm^-3
(b) 1 x 10^-12 mol dm^-3
(c) 1 x 10^-1 mol dm^-3
(d) 1 x 10^-14 mol dm^-3     

Question 29. 100 mL of 0.01 M solution of NaOH is diluted to 1dm³ . What is the pH of the diluted solution? 
(a) 12
(b) 11
(c) 2
(d) 3     

Question 30. Calculate pOH of 0.001 M NH₄OH, when it is 1% dissociated in the solution.
(a) 5
(b) 2.96
(c) 9.04
(d) 11.4     

Question 31. What will be the pH value of0.05M Ba (OH)₂ solution?
(a) 12
(b) 13 
(c) 1
(d) 12.96       

Question 32. Which solution has pH equal to 10? 
(a) 10^-4 M KOH
(b) 10-¹⁰ M KOH
(c) 10^-10 M HCI
(d) 10^-4 M HCl         

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Question 33. A 0.01 M ammonia solution is 5% ionised, its pH will be
(a) 11.80
(b) 10.69 
(c) 7.22
(d) 12 .24       

Question 34. Which of the following cannot act both as Bronsted acid and as Bronsted base ?                                         
(a) HCO₃ ^–
(b) NH₃
(c) HCl
(d) HSO^– ₄ 

Question 35. The pH value of 1/1000 N KOH solution is
(a) 3
(b) 10^-11
(c) 2
(d) 11       

Question 36. Reaction BaO_2(s)  ⇌ BaO_(s) + O_2(g); ΔH = +ve. In equilibrium condition, pressure of O₂ depends on           
(a) increase mass of BaO₂
(b) increase mass of BaO
(c) increase temperature on equilibrium
(d) increase mass of BaO₂ and BaO both. 

Question 37. Which of the following molecules acts as a Lewis acid?                                             
(a) (CH₃₎₂O
(b) (CH₃)₃P
(c) (CH₃)₃N
(d) (CH₃)₃B 

Question 38. Which one of the following statements is not true?                                                     
(a) Among halide ions, iodide is the most powerful reducing agent.
(b) Fluorine is the only halogen that does not show a variable oxidation state.
(c) HOCl is a stronger acid than HOBr.
(d) HF is a stronger acid than HCl. 

Question 39. Which one of the following compounds is not a protonic acid?                                                   
(a) B(OH)₃
(b) PO(OH)₃
(c) SO(OH)₂
(d) SO₂(OH)₂ 

Question 40. Which of the following fluoro-compounds is mostlikely to behave as a Lewis base?                                     
(a) BF₃
(b) PF₃
(c) CF₄
(d) SiF₄

Question 41. Which is the strongest acid in the following?                                                 
(a) HClO₄
(b) H2SO₃
(c) H2SO₄
(d) HClO₃

Question 42. Which one of the following molecular hydrides acts as a Lewis acid?                                                       
(a) NH₃
(b) H₂O
(c) B₂H₆
(d) CH₄

Question 43. The strongest conjugate base is                                         
(a) SO₄ ^2–
(b) Cl–
(c) NO₃ ^–
(d) CH₃COO^– 

Question 44. Which of the following is not a Lewis acid?                                                           
(a) SiF₄
(b) C₂H₄
(c) BF3
(d) FeCl₃

Question 45. Repeated use of which one of the following fertilizers would increase the acidity of the soil?                       
(a) Ammonium sulphate
(b) Superphosphate of lime
(c) Urea
(d) Potassium nitrate

Question 46. Which of these is least likely to act as a Lewis base?                                         
(a) BF3
(b) PF3
(c) CO
(d) F–

Question 47. In HS–, I–, R – NH₂, NH₃ order of proton accepting tendency will be                                                           
(a) I^– > NH₃ > R – NH2 > HS^–
(b) NH_{3 >} R ^– NH₂ > HS^– > I^–
(c) R ^– NH₂ > NH₃ > HS^– > I^–
(d) HS^– > R ^– NH₂ > NH₃ > I^–

Question 48. Conjugate acid of NH2 – is                                                 
(a) NH₄OH
(b) NH₄ ⁺
(c) NH₂ ^–
(d) NH₃ 

Question 49. Which compound is electron deficient?                                                     
(a) BeCl₂
(b) BCl₃
(c) CCl₄
(d) PCl₅ 

Question 50. 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.       
(a) 2 × 10^–13 M
(b) 2 × 10^–8 M
(c) 1 × 10^–13 M
(d) 1 × 10⁸ M

Question 51. The pH of 0.01 M NaOH_(aq) solution will be                                                     
(a) 7.01
(b) 2
(c) 12
(d) 9

Question 52. 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)                                             
(a) 7.00
(b) 7.87
(c) 5.13
(d) 6.13

Question 53. Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?                                             
(a) BaCl₂
(b) AlCl₃
(c) LiCl
(d) BeCl₂

Question 54. The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N + H) in a 0.10 M aqueous pyridine solution (Kb for C₅H₅N = 1.7 × 10^–9) is                           
(a) 0.0060%
(b) 0.013%
(c) 0.77%
(d) 1.6% 

Question 55. 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 issociation constant, Ka, for this acid will be                                                         
(a) 1.4 × 10^–5
(b) 1.4 × 10^–4
(c) 3.7 × 10^–4
(d) 2.8 × 10^–4

Question 56. What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?   
(a) 2.0
(b) 7.0
(c) 1.04
(d) 12.65 

Question 57. Which of the following salts will give highest pH in water?                                                     
(a) KCl
(b) NaCl
(c) Na₂CO₃
(d) CuSO₄ 

Question 58. What is [H⁺] in mol/L of a solution that is 0.20 M in CH₃COONa and 0.10 M in CH₃COOH? (K_a for CH₃COOH = 1.8 × 10^–5)                                           
(a) 3.5 × 10^–4
(b) 1.1 × 10^–5
(c) 1.8 × 10^–5
(d) 9.0 × 10^–6 

Question 59. The ionization constant of ammonium hydroxide is 1.77 × 10^–5 at 298 K. Hydrolysis constant of ammonium chloride is                                             
(a) 6.50 × 10^–12
(b) 5.65 × 10^–13
(c) 5.65 × 10^–12
(d) 5.65 × 10^–10 

Question 60. The hydrogen ion concentration of a 10^–8 M HCl aqueous solution at 298 K (Kw = 10–14) is                         
(a) 1.0 × 10^–8 M
(b) 1.0 × 10^–6 M
(c) 1.0525 × 10^–7 M
(d) 9.525 × 10^–8 M 

Question 61. 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                               
(a) 1.0 × 10–5 mol L^–1
(b) 1.0 × 10–6 mol L^–1
(c) 2.0 × 10–6 mol L^–1
(d) 1.0 × 10–7 mol L^–1 

Question 62. 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?                                                 
(a) 0.40 M
(b) 0.0050 M
(c) 0.12 M
(d) 0.10 M

Question 63. Which has highest pH?                                                 
(a) CH₃COOK
(b) Na₂CO₃
(c) NH₄Cl
(d) NaNO₃

Question 64. Ionisation constant of CH₃COOH is 1.7 × 10^–5 and concentration of H⁺ ions is 3.4 × 10^–4. Then find out initial concentration of CH₃COOH molecules.                                       
(a) 3.4 × 10^–4
(b) 3.4 × 10^–3
(c) 6.8 × 10^–4
(d) 6.8 × 10^–3

Question 65. Calculate the pOH of a solution at 25°C that contains 1 × 10^–10 M of hydronium ions, i.e. H₃O⁺.               
(a) 4.000
(b) 9.000
(c) 1.000
(d) 7.000 

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