Please refer to Chapter 7 Equilibrium MCQ Class 11 Chemistry with answers below. These multiple-choice questions have been prepared based on the latest NCERT book for Class 11 Chemistry. Students should refer to MCQ Questions for Class 11 Chemistry with Answers to score more marks in Grade 11 Chemistry exams. Students should read the chapter Equilibrium and then attempt the following objective questions.

MCQ Questions Class 11 Chemistry Chapter 7 Equilibrium

The Equilibrium MCQ Class 11 Chemistry provided below covers all important topics given in this chapter. These MCQs will help you to properly prepare for exams.

Question. What is the pH of a 10⁻⁴M OH⁻ solution at 330 K, if K_w at 330 K is 10^−13.6? 
(a) 4
(b) 9.0
(c) 10
(d) 9.6         

Question. How many litres of water must be added to 1 L of an aqueous solution of HCl with a pH of 1 to  reate an aqueous solution with pH of 2? 
(a) 0.1 L
(b) 0.9 L
(c) 2.0 L
(d) 9.0 L         

Question. The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionisation constant, K_a of the acid is 
(a) 3 × 10⁻¹
(b) 1 × 10⁻³ 
(c) 1 × 10⁻⁵      
(d) 1 × 10⁻⁷   

Question. Three reactions involving H₂PO₄^– are given below:
I. H₃PO₄ + H₂O → H₃PO⁺ + H₂O₄^–
II. H₂PO^–₄ + H₂O → HPO₄^2- + H₃O⁺
III. H₂PO^–₄ + OH^– → H₃PO₄ + O^2–
In which of the above does H2PO₄^– act as an acid?
(a) Only II        
(b) Both I and II
(c) Only III
(d) Only I 

Question. Dissociation constant of a weak acid is 1 × 10^−4. Equilibrium constant of its reaction with strong base is
(a) 1 × 10⁻⁴
(b) 1 × 10¹⁰        
(c) 1 × 10⁻¹⁰
(d) 1 ×10⁴     

Question. The pH of the neutralisation point of 0.1 N ammonium hydroxide with 0.1 N HCl is
(a) 8
(b) 6       
(c) 7  
(d) 9     

Question. NaOH is a strong base. What will be pH of 5.0 × 10⁻²M NaOH solution ? (log 2= 0.3) 
(a) 14.00
(b) 13.70
(c) 13.00
(d) 12.70       

Question. An acid HA ionises as HA ⇌ ^H+ A⁻  The pH of 1.0 M solution is 5. Its dissociation constant would be
(a) 1 × 10⁻¹⁰       
(b) 5.0
(c) 5 × 10⁻⁸
(d) 1 × 10⁻⁵     

Question. The solubility product of BaSO₄ is 1.5 ×10⁻⁹. The precipitation in a 0.01 M Ba²⁺ solution will start on adding H₂SO₄ of concentration.
(a) 10⁻⁹ M
(b) 10⁻⁸ M
(c) 10⁻⁷ M
(d) 10⁻⁶ M       

Question. Solubility product of silver bromide is 5.0 × 10⁻¹³ . The quantity of potassium bromide (molar mass taken as 120 g mol⁻¹) to be added to 1 L of 0.05 M solution of silver nitrate to start the precipitation of AgBr is
(a) 1.2 × 10⁻¹⁰ g
(b) 1.2 × 10⁻⁹ g     
(c) 6.2 × 10⁻⁵ g
(d) 5.0 × 10⁻⁸ g    

Question. What will be the degree of ionisation of 0.05 M acetic acid if its pKa value is 4.74 ?
(a) 0.019%
(b) 1.9%      
(c) 3.0%
(d) 4.74%       

Question. pH of 0.005 M calcium acetate (pK_a of CH₃COOH 4.7) = is
(a) 7.04
(b) 9.37
(c) 9.26
(d) 8.37     

Question. The pK_a of a weak acid, HA is 4.80. The pK_b of a weak base BOH is 4.78. The pH of an aqueous solution of the corresponding salt BA will be
(a) 7.01      
(b) 9.22
(c) 9.58
(d) 4.79      

Question. HX is a weak acid (K_a =10⁻⁵ ) . It forms a salt NaX (0.1M) on reacting with caustic soda. The degree of hydrolysis of NaX is
(a) 0.01%        
(b) 0.0001%
(c) 0.1%
(d) 0.5%      

Question. pK_a of a weak acid (HA) and pK_b of a weak base (BOH) are 3.2 and 3.4 respectively. The pH of their salt (AB) solution is 
(a) 7.2
(b) 6.9         
(c) 7.0
(d) 1.0     

Question. The pK_w of a neutral solution at 50°C is 13.36, what would be the pH of the solution at this temperature?
(a) 7.63
(b) 7.00
(c) 6.68        
(d) 7.96      

Question. The ionic product of water at 310 K is 2.7 ×10⁻¹⁴. What is the pH of neutral water at this temperature?
(a) 7.0
(b) 5.98
(c) 6.78       
(d) 4.58      

Question. Number of (OH)⁻ in 1 mL solution of pH = 13 is
(a) 1 × 10⁻¹³
(b) 6.00 × 10⁷
(c) 6.00 × 10¹³
(d) 6.02  × 10¹       

Question. 5 Solid Ba(NO₃)₂ is gradually dissolved in a 1.0 × 10⁻⁴ M Na₂CO₃ solution. At which concentration of Ba²⁺, precipitate of BaCO₃ begins to form?
(K_sp for BaCO₃ = 5.1 × 10⁻⁹)
(a) 5.1 × 10⁻⁵ M      
(b) 7.1 × 10⁻⁵ M
(c) 4.1 × 10⁻⁵ M
(d) 8.1 × 10⁻² M       

Question. The solubility product of a binary weak electrolyte is 4 x 10^-10 at 298 K. Its solubility (in mol dm^-3) at the same temperature is
(a) 4 x 10^-5
(b) 2 x 10^-5
(c) 8 x 10^-10
(d) 16 x 10^-20       

Question. Passing H₂S gas into a mixture of Mn²⁺, Ni²⁺, Cu²⁺ and Hg²⁺ ions in an acidified aqueous solution precipitatesQuestion
(a) CuS and HgS
(b) MnS and CuS 
(c) MnS and NiS
(d) NiS and HgS         

Question. In IL saturated solution of AgCl [K_sp(AgCI) = 1.6 x 10^-10] 0.1 mole of CuCl [K_sp(CuCl) = 1.0x 10^-6] is added. The resultant concentration of Ag⁺ in the solution isl . 6 x 10^-x . The value of xis 
(a) 3
(b) 5
(c) 7
(d) 9   

Question. The solubility of CaF² is s mol/L. Then, solubility product is 
(a) S²
(b) 4S³
(c) 4S²
(d) S³       

Question. The K_sp for Cr (OH)₃ is 1.6x 10^-30 . The molar solubility of this compound in water is 
(a) 2√1.6 x 10^-30
(b)  4√1.6 x 10^-30
(c)  4√1.6 x 10^-30/27
(d) 1.6 x 10³⁰/27     

Question. H₂ Sis gassed into 1 dm³ of a solution containing 0.1 mole of Zn²⁺ and 0.01 mole of Cu²⁺ till the sulphide ion concentration reaches 8.1 x 10^-19 mole. Which one of the following statement is correct? (K_sp of ZnS and CuS are 3 x 10^-22 and 8 x 10^-36 , respectively) 
(a) Only ZnS precipitates
(b) Both CuS and ZnS precipitate
(c) Only CuS precipitates
(d) No precipitation occurs     

Question. The solubility of Ca₃ (PO₄)₂ h in water is y mole / L. Its solubility product is 
(a) 6Y⁴
(b) 36Y⁴
(c) 64Y⁵
(d) 108Y⁵       

Question. Solubility product of silver bromide is 5.0x 10^-13 • The quantity of potassium bromide (molar mass taken as 120 gmol^-1) to be added to 1 L of 0.05 Msolution of silver nitrate to start the precipitation of AgBr is 
(a) 1.2 x 10^-10 g
(b) 1.2 x 10^-9 g
(c) 6.2 x 10^-5 g
(d) 5.0 x 10^-8 g     

Question. At25°C, thesolubility product of Mg (OH)₂ is 1.0 x 10^-11 . At which pH, will Mg²⁺ ions start precipitating in the form of Mg (OH)₂ from a solution of 0.001 M Mg²⁺ ions ?
(a) 9
(b) 10
(c) 11
(d) 8   

Question. The solubility of AgCl in 0.2 M NaCl solution is (K_sp of AgCl = 1.20 x 10^-10 ) 
(a) 6.0 x 10^-10 M
(b) 0.2 M
(c) 1.2 x 10^-10 M
(d) 0.2 x 10^-10 M     

Question. The expression for the solubility product of Ag₂CO₃ will be 
(a) K_sp = s²
(b) K_sp= 4s³
(c) K_sp = 27s⁴
(d) K_sp = s     

Question. 1 dm3 solution containing 10^-5 moles each of Cl^– ions and CrO^2-₄ ions is treated with 10^-4 moles of silver nitrate. Which one of the following observations is made? 
(K_spAg₂CrO₄ = 4 X 10^-12) (K_spAgCl = 1 x 10^-10)
(a) Precipitation does not occur 
(b) Silver chromate gets precipitated first
(c) Silver chloride gets precipitated first
(d) Both silver chromate and silver chloride start precipitating simultaneously         

Question. If K_sp of Ag₂S is 10^-17, then the solubility of Ag₂S in 0.1 M solution ofN a 2 Swill be 
(a) 10^-8
(b) 5x 10^-9
(c) 10^-15
(d) 10^-16     

Question. Which of the following has the highest value of solubility product? 
(a) CuS
(b) Bi₂S₃
(c) CdS
(d) ZnS     

Question. The solubility product of Hg₂I₂ is equal to 
(a) [Hg²⁺₂][I^–]
(b) [Hg²⁺][I^–]
(c) [Hg²⁺₂][I^–]²
(d) [Hg²⁺][I^–]²       

Question. The molar solubility (in mol L⁻¹) of a sparingly soluble salt MX₄ is S. The corresponding solubility product is K_sp.S is given in terms of K_sp by the relation.
(a) S = (K_sp / 128)^1/4
(b) S = ( 128 K_sp )^1/4 
(c) S = ( 256 K_sp )^1/5
d) S = (K_sp / 256 )^1/5           

Question. A solution which is10 ⁻³ M each inMn²⁺ , Fe²⁺ , Zn²⁺ and Hg²⁺ is treated with10⁻¹⁶ M sulphide ion. If K_sp of MnS, FeS, ZnS and HgS are10⁻¹⁵,10⁻²³,10⁻²⁰ and10⁻⁵⁴ respectively, which one will precipitate first?
(a) FeS
(b) MgS
(c) HgS              
(d) ZnS      

Question. The solubility of a sparingly soluble salt, AB₂ in water is 1.0 × 10⁻⁵ mol L⁻¹. Its solubility product will be
(a) 4 × 10⁻¹⁰
(b) 1 × 10⁻¹⁵
(c) 1 × 10⁻¹⁰
(d) 4 × 10⁻¹⁵       

Question. At 25°C, the solubility product of Mg (OH)₂ is 1.0 ×10⁻¹¹. At which pH, will Mg²⁺ ions start precipitating in the form of Mg (OH)₂ from a solution of 0.001 M Mg²⁺ ions?
(a) 9
(b) 10     
(c) 11
(d) 8   

Question. 0.1 mole of CH₃NH₂ (K_b = 5 ×10⁻⁴ )  is mixed with 0.08 mole of HCl and diluted to one litre. What will be the H+ concentration in the solution?
(a) 8 × 10⁻² M
(b) 8 × 10⁻¹¹ M          
(c) 1.6 × 10⁻¹¹ M 
(d) 8 × 10⁻⁵ M     

Question. The solubility of PbCl₂ is
(a) √K_sp
(b) (K_sp)^1/3
(c) (K_sp /4)^1/3          
(d) (8 K_sp)^1/2     

Question. A weak acid (HA) is 4% ionised at 1 M. Per cent ionisation is 1% in the presence of A^–. The concentration of A⁻ is
(a) 0.04 M
(b) 0.16 M     
(c) 0.02 M  
(d) 0.10 M     

Question. An aqueous solution contains an unknown concentration of Ba²⁺ . When 50 mL of a 1 M solution of Na₂SO₄ is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO₄ is 1 × 10⁻¹⁰. What is the original concentration of Ba²⁺? 
(a) 5 × 10⁻⁹ M
(b) 2 × 10⁻⁹ M
(c) 1.1 × 10⁻⁹ M      
(d) 1.0 × 10⁻¹⁰ M      

Question. Solubility product constant (K_sp)  of salts of types MX, MX₂ and M₃X at temperatureT are 4.0 ×10⁻⁸, 3.2 ×10⁻¹⁴ and 2.7 ×10⁻¹⁵ respectively. Solubilities (mol dm⁻³) of the
salts at temperature ‘T’ are in the order
(a) MX > MX₂ > M₃X 
(b) M₃ X > MX₂ >MX 
(c) MX₂ > M₃X > MX
(d) MX > M₃X > MX₂       

Question. Which of the following will produce a buffer solution when mixed in equal volumes?
(a) 0.1 mol dm⁻³ NH₄OH and 0.1 mol dm⁻³ HCl
(b) 0.05 mol dm⁻³ NH₄OH and 0.1 mol dm⁻³ HCl
(c) 0.1 mol dm⁻³ NH₄OH and 0.05 mol dm⁻³ HCl      
(d) 0.1 mol dm⁻³ CH₄COONa and 0.1 mol dm⁻³ NaOH       

Question. The precipitate of CaF₂ (K_sp = 1.7 × 10⁻¹⁰ ) is obtained when equal volumes of the following are mixed
(a) 10⁻⁴ M Ca²⁺ + 10⁻⁴ M F⁻
(b) 10⁻² M Ca²⁺ + 10⁻³ M F⁻
(c) Both (a) and (b)
(d) None of these       

Question. The solubility of AgI in NaI solution is less than that in pure water because
(a) AgI forms complex with NaI
(b) of common ion effect
(c) solubility product of AgI is less
(d) the temperature of the solution decreases       

Question. The silver ion in a solution is precipitated by addition of chloride ion. The final volume of solution is 500mL. What should be the concentration of C^l– ion if not more than 0.10 mg of Ag+ ion remains unprecipitated?
(K_sp (AgCl) =1.0 ×10^–10 )
(a) 5.4 × 10^–5 M   
(b) 1.9 × 10^–6 M
(c) 5.4 × 10^–4 M
(d) 1.9 × 10^–7      

Question. The degree of ionisation of 1.0 M weak acid, HA is 0.5%. If 2 mL of 1.0 M HA solution is diluted to 32 mL, the degree of ionisation of the acid and H₃O⁺ ion concentration in the resulting solution will be respectively.
(a) 0.02 and 3.125 × 10⁻⁴  
(b) 0.02 and 1.25 × 10⁻³    
(c) 1.25 10⁻³.× and 0.02 
(d) 0.02 and 8.0 × 10⁻¹²     

Question. How do we differentiate between Fe³⁺ and Cr³⁺ in group III?
(a) By taking excess of NH₄OH 
(b) By increasing NH₄⁺ ion concentration
(c) By decreasing OH⁻ ion concentration
(d) Both (b) and (c)         

Question. The K_sp for Cr(OH)₃ is 1 . 6 × 10⁻³⁰. The molar solubility of this compound in water is
(a) ²√1.6 × 10⁻³⁰
(b)⁴√1.6 × 10⁻³⁰
(c) ⁴√1.6 × 10⁻³⁰/27 
(d) 1.6 × 10⁻³⁰/27     

Question. Which one of the following statements is not true?
(a) The conjugate base of H PO₄⁻ is HPO₄²⁻
(b) pH + pOH = 14 for all aqueous solutions
(c) The pH of 1 × 10⁻⁸ M HCl is 8   
(d) α = √K_v for a weak electrolyte     

Question. SO₃ (g) ⇌ SO₂ (g) + 1/2 O₂ ( g)
The equilibrium constant for the above reaction is Kc = 4.9 x 10^-2 . The value of Kc for the reaction
2SO₂ (g) + O₂ (g) ⇌ 2SO₃ (g) will be 
(a) 416
(b) 2.40 x 10^-3
(c) 9.8 x 10^-2
(d) 4.9 x 10^-2     

Question. l mole of N₂O₄ (g) at 300 Kis kept in a closed container under 1 atm. It is heated to 600 K when 20% by mass of N₂O₄ (g )decomposes to NO₂ (g ). The resultant pressure is 
(a) 1.2 atn1
(b) 2.4 atm
(c) 2.0 atm
(d) 1.0 atm       

Question. N₂ + O₂ ⇌ 2NO + Heat
In the above gaseous reversible reaction, if pressure is increased, then the equilibrium constant would be
(a) unchanged 
(b) increased
(c) decreased
(d) sometimes increased, sometimes decreased       

Question. Consider the following equilibrium in a closed container,
                        N₂O₄ (g) ⇌ 2NO₂(g)
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statement holds true regarding the equilibrium constant (K_P) and degree of dissociation(α)? 
(a) Neither K_P nor α changes
(b) Both K_P and α change
(c) K_PP changes butα does not
(d) K_PKP does not change but α changes   

Question. The equilibrium constant of a reaction is 300. If the volume of reaction flask is tripled, then the equilibriurn constant is 
(a) 300
(b) 600
(c) 900
(d) 100     

Question. In the reaction, H₂ + I₂ ⇌ 2HI
In a 2 L flask, 0.4 mole of each H₂ and I₂ are taken. At equilibrium, 0.5 moles of HI are formed. What will be the value of equilibtium constant K_c? 
(a) 20.2
(b) 25.4
(c) 0.284
(d) 11.11     

Question. Two moles of PCl₅ were heated in a closed vessel of 2 L. At equilibriurn, 40% of pCl₅ is dissociated into PCl₃ and Cl₂ . The value of equilib1ium constant is 
(a) 0.53
(b) 0.267
(c) 2.63
(d) 5.3       

Question. The chemical equilibrium of a reversible reaction is not influenced by
(a) pressure
(b) catalyst
(c) concentration of the reactants
(d) temperature     

Question. 56 g of nitrogen and 8 g of hydrogen gas are heated in a closed vessel. At equilibrium, 34 g of ammonia are present. The equilibtium number of moles of nitrogen, hydrogen and ammonia respectively are 
(a) 1,2,2
(b) 2,2,1
(c) 1,1,2
(d) 2,1,2       

Question. Which of the following is not a characteristic property of chemical equilibrium ? 
(a) Rate of forward reaction is equal to rate of backward reaction at equilibriurn
(b) After reaching the chemical equilibrium, the concentrations of reactants and products remain unchanged with time
(c) For A (g) ⇌ B (g),K_c is 10^-2 . If this reaction is carried out in the presence of catalyst, the value of K_c decreases
(d) After reaching the equilibrium, both forward and backward reactions continue to take place     

Question. A monoprotic weak acid (HA) is ionised 5% in 0.1 M aqueous solution. What is the equilibrium constant for its ionisation ? 
HA(aq) + H₂O(/) ⇌ H₃O⁺ (aq)+ A^– (aq)
(a) 2.63 x 10⁴
(b) 2.63 x 10³
(c) 2.63 x 10^-4
(d) 2.63 x 10^-3     

Question. The equilibrium reaction that is not influenced by volume change at constant temperature is 
(a) H₂(g)+ I₂(g) ⇌ 2HI (g)
(b) N₂(g) + 3H2(g) ⇌ 2NH₃ (g)
(c) N₂O₄ (g) ⇌  2NO₂(g)
(d) 2NO(g) + O₂(g) ⇌ 2NO₂(g)     

Question. At a given temperature, the equilibrium constant for the reaction of
PCl₅ ⇌ PCl₃ + Cl₂ is 2.4 x 10^-3 . At the same temperature, the equilibrium constant for the reaction
PCI₃ (g)+ Cl₂ (g) ⇌ PCI₅ (g) is
(a) 2.4 X 10^-3
(c) 4.2 x 10²
(b) – 2.4 x 10^-3
(d) 4.8 x 10^-2         

Question. Which of the following is correct for the reaction ?
     N₂(g)+3H₂(g) ⇌ 2NH₃ (g)
(a) K_P = K_c 
(b) K_P < K_c 
(c) K_P > K_c 
(d) Pressure is required to predict the correlation     

Question. For the reaction, 
      2NO₂ (g) ⇌ 2NO(g)+ O₂ (g)
       (K_c = 1.8 x 10^-6 at 184° C)
        (R = 0. 00831 kJ/mol K)
When KP and K_c are compared at 184 ° C, it is found that
(a) whether K_p is greater than, less than or equal to K_c depends upon the total gas pressure
(b) K_p = K_c
(c) K_p is less than K_c
(d) K_p is greater than K_c       

Question. An amount of solid NH₄ HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atrn pressure. Ammonium hydrogen sulphide decomposes to yield NH₃ and H₂S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH₄HS decomposition at this temperature is 
(a) 0.11
(b) 0.17
(c) 0.18
(d) 0.30     

Question. In which of the following reactions is K_P < K_c ?
(a) I₂(g) ⇌ 2I(g) 
(b) 2BrCl(g) ⇌ Cl₂(g) + Br₂ (g)
(c) CO(g)+ 3H₂ (g) ⇌ CH₄ (g)+ H₂O(g)
(d) All of the above     

Question. What will be the value of pH of 0.01 mol dm⁻³ CH₃COOH  ? (K_a = 1.74 × 10⁻⁵) [log 4.17 = 0.6201]
(a) 3.4    
(b) 3.6
(c) 3.9
(d) 3.0   

Question. The solubility of AgBrO₃ in an aqueous solution ofNaBrO₃ (as compared to that in water) is
(a) the same
(b) more
(c) less
(d)unpredictable due to a new chemical reaction       

Question. What would be the pH of a solution obtained by mixing 5g of acetic acid and 7.5 g of sodium acetate and making the volume equal to 500 mL?
(K_a = 1.75 × 10⁻⁵, pK_a = 4.76 ) 
(a) pH = 4.70
(b) pH < 4.70
(c) pH of solution will be equal to pH of acetic acid
(d) 4.76 < pH < 5.0       

Question. The pK_a of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid ionised is
(a) 4.5
(b) 2.5
(c) 9.5       
(d) 7.0    

Question. 2.5 mL of 2/5 M weak monoacidic base (K_b =1 × 10⁻¹² at 25°C) is titrated with 2/15 M HCl in water at 25°C. The concentration of H+ at equivalence point is (K_w =1 × 10⁻¹⁴ at 25°C)
(a) 3.7 × 10⁻¹³ M
(b) 3.2 × 10⁻⁷ M
(c) 3.2 × 10⁻² M  
(d) 2.7 × 10⁻² M      

Question. 1 MNH₄OH  and 1M HCl are mixed to make total volume of 300 mL. If pH of the mixture is 9.26 and pK_a [NH₄⁺ ] = 9.26 then volume ratio of NH₄OH  and HCl will be
(a) 1 : 1
(b) 1 : 2
(c) 2 : 1  
(d) 3 : 1   

Question. An aqueous solution of 1 M NaCl and 1 M HCl is
(a) not a buffer but pH < 7      
(b) not a buffer but pH > 7
(c) a buffer with pH < 7
(d) a buffer with pH > 7      

Question.  The pH values of 0.1 M solution of HCl, CH₃ COOH , NH4Cl and CH3COONa will have the order
(a) HCl < CH₃ COOH < NH₄ Cl < CH₃COONa      
(b) CH₃COOH < NH₄Cl < CH₃COOH < HCl 
(c) NH₄Cl < CH₃COOH < CH₃COOH < HCl 
(d) All will have same pH value      

Question. Hydroxyl ion concentration [OH⁻ ] in the case of sodium acetate can be expressed as (where, K_a is dissociation constant of CH₃COOH and C is the concentration of sodium acetate)
(a) [OH⁻] = (CK_w K_a)^1/2
(b) [OH⁻] = C.K_w √K_a
(c) [OH⁻] = { C . K_w/Ka }^1/2         
(d) [OH⁻] = C.K_a .K_w      

Question. 1 dm³ solution containing10⁻⁵ moles each of Cl⁻ ions and CrO₄^2– ions is treated with10⁻⁴ moles of silver nitrate. Which one of the following observation is made?
( K_spAg₂CrO₄ = 4× 10⁻¹² ) , (K_sp AgCl =1×10⁻¹⁰ ) 
(a) Precipitation does not occur
(b) Silver chromate gets precipitated first
(c) Silver chloride gets precipitated first     
(d) Both silver chromate and silver chloride start precipitating simultaneously      

Question. Of the given anions, the strongest Bronsted base is
(a) ClO⁻      
(b) ClO₃⁻
(c) ClO₂⁻
(d) ClO₄⁻     

Question. Four species are listed below:
I. HCO³⁻
II. H₃O⁺
III. HSO₄⁻
IV. HSO₃F
Which one of the following is the correct sequence of theiracidic strength?
(a) IV<II<III<I
(b) II<III<I<IV
(c) I<III< II<IV      
(d) III<I<IV<II      

Question. A solution of monoprotic weak acid has ionisation constant K_a. What is the minimum concentration C in terms of K_a, such that the concentration of the undissociated acid can be equated to C within a 10% limit of error. [Assume that activity coefficient correction are negligible.]
(a) 45Ka
(b) 10Ka
(c) 90Ka 
(d) 80Ka       

Question. What will be the pH of a buffer solution prepared by dissolving 30 g of Na₂CO₃ in 500 mL of an aqueous solution containing 150 mL of 1 M HCl?
[K_a for HCO₃⁻ = 5.63 × 10⁻¹¹]
(a) 10.197  
(b) 8.089
(c) 9.858
(d) 6.400     

We hope you liked the above Equilibrium MCQ Class 11 Chemistry. In case you have any questions please put them in the comments box below and our teachers will provide you a response.