MCQ Questions For Class 11 Chemistry Chapter 7 Equilibrium

Please refer to MCQ Questions Equilibrium for Chapter 7 Class 11 Chemistry given below. All MCQ questions are provided with answers. These MCQ Questions for Class 11 Chemistry are designed based on the chapters given in your CBSE NCERT Textbook for Class 11 Chemistry. These MCQ Questions are expected to come in your class 11 Board exams.

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

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

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

Question. 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         

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

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

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

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

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

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

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

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

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

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

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

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

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

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

Question. 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. 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 

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

Question. 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