JEE Chemistry Equilibrium MCQs Set C

Refer to JEE Chemistry Equilibrium MCQs Set C provided below available for download in Pdf. The MCQ Questions for Full Syllabus Chemistry with answers are aligned as per the latest syllabus and exam pattern suggested by JEE (Main), NCERT and KVS. Multiple Choice Questions for Equilibrium are an important part of exams for Full Syllabus Chemistry and if practiced properly can help you to improve your understanding and get higher marks. Refer to more Chapter-wise MCQs for JEE (Main) Full Syllabus Chemistry and also download more latest study material for all subjects

MCQ for Full Syllabus Chemistry Equilibrium

Full Syllabus Chemistry students should refer to the following multiple-choice questions with answers for Equilibrium in Full Syllabus.

Equilibrium MCQ Questions Full Syllabus Chemistry with Answers

 

 

Question: Which of the following statements about pH and H+ ion concentration is incorrect?

  • a) A solution of the mixture of one equivalent of each of CH3COOH and NaOH has a pH of 7
  • b) pH of pure neutral water is not zero
  • c) Addition of one drop of concentrated HCl in NH4OH solution decreases pH of the solution
  • d) None of these

Answer: A solution of the mixture of one equivalent of each of CH3COOH and NaOH has a pH of 7

 

Question: H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because

  • a) presence of HCl decreases the sulphide ion concentration
  • b) solubility product of group II sulphides is more than that of group IV sulphides
  • c) presence of HCl increases the sulphide ion concentration
  • d) sulphides of group IV cations are unstable in HCl

Answer: presence of HCl decreases the sulphide ion concentration

 

Question: A salt ‘X’ is dissolved in water of pH = 7. The salt is made resulting solution becomes alkaline in nature. The salt is made

  • a) A weak acid and strong base
  • b) A weak acid and weak base
  • c) A strong acid and weak base
  • d) A strong acid and strong base

Answer: A weak acid and strong base

 

Question: Aqueous solution of ferric chloride is acidic due to

  • a) hydrolysis
  • b) polarization
  • c) ionization
  • d) dissociation

Answer: hydrolysis

 

Question: The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffer solution of HA in which 50% of the acid is ionized is

  • a) 9.5
  • b) 4.5
  • c) 7.0
  • d) 2.5

Answer:  9.5

 

Question:

  • a) 9.43
  • b) 8.73
  • c) 9.08
  • d) 11.72

Answer: 9.43

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: Which of the following pairs constitutes a buffer?

  • a) HNO2 and NaNO2
  • b) HNO3 and NH4NO3
  • c) NaOH and NaCl
  • d) HCl and KCl

Answer: HNO2 and NaNO2

 

Question:  Buffer solutions have constant acidity and alkalinity because

  • a) these give unionised acid or base on reaction with added acid or alkali
  • b) acids and alkalies in these solutions are shielded from attack by other ions
  • c) they have large excess of H+ or OH ions
  • d) they have fixed value of pH

Answer: these give unionised acid or base on reaction with added acid or alkali

 

Question: The buffering action of an acidic buffer is maximum when its pH is equal

  • a) pKa
  • b) 7
  • c) 5
  • d) 1

Answer:  pKa

 

Question:  When a buffer solution, sodium acetate and acetic acid is diluted with water

  • a) H+ ion concentration remains unaltered
  • b) OH ion conc. increases
  • c) H+ ion concentration increases
  • d) Acetate ion concentration increases

Answer: H+ ion concentration remains unaltered

 

Question: The product of ionic concentration in a saturated solution of an electrolyte at a given temperature is constant and is known as

  • a) Solubility product
  • b) Ionic product of the electrolyte
  • c) Ionization constant
  • d) Dissociation constant

Answer: Solubility product

 

Question:  The Ksp for Cr(OH)3 is 1.6 × 10–30. The solubility of this compound in water is

  • a)

  • b)

  • c)

  • d)

Answer:

 

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) 10
  • b) 8
  • c) 9
  • d) 11

Answer: 10

 

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

  • a) 5.0 × 10–7
  • b) 5.0 × 10–6
  • c) 3.3 × 10– 7
  • d) 4.0 × 10–6

Answer:  5.0 × 10–7

 

Question: If s and S are respectively solubility and solubility product of a sparingly soluble binary electrolyte then

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a) Solubility product of As2S3 is less than that of ZnS
  • b) Enough As+3 are present in acidic medium
  • c) Zinc salt does not ionise in acidic medium
  • d) Solubility product changes in presence of an acid

Answer: Solubility product of As2S3 is less than that of ZnS

 

Question:

  • a) 5.1 × 10–5 M
  • b) 4.1 × 10–5 M
  • c) 7.1 × 10–8 M
  • d) 8.1 × 1–7 M

Answer: 5.1 × 10–5 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 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is

  • a) 1.2 × 10–9 g
  • b) 5.0 × 10–8 g
  • c) 1.2 × 10–10 g
  • d) 6.2 × 10–5 g

Answer:  1.2 × 10–9 g 

 

More Questions....................................

 

Question:

  • a) 10
  • b) 8
  • c) 9
  • d) 11

Answer: 10

 

Question:  Read the following statements carefully and choose the correct answer

(i) Water and water vapour remain in equilibrium position at atmospheric pressure (1.013 bar) and at 100°C in a closed vessel.
(ii) The boiling point of water is 100°C at 1.013 bar pressure
(iii) Boiling point of the liquid depends on the atmospheric pressure.
(iv) Boiling point depends on the altitude of the place; at high altitude the boiling point increases

  • a) (i), (ii) and (iii) are correct
  • b) only (iii) is correct
  • c) (i), (iii) and (iv)
  • d) (i), (ii) and (iv) are correct

Answer: (i), (ii) and (iii) are correct

 

Question:

  • a) (i), (ii) and (iv) are correct
  • b) (i) , (iii) and (iv)
  • c) (i), (ii) and (iii) are correct
  • d) only (iii) is correct

Answer: (i), (ii) and (iv) are correct

 

Question:  Identify the CORRECT statements below regarding chemical equilibrium:

(i) All chemical reactions which are in equilibrium are irreversible.
(ii) Equilibrium is achieved when the forward reaction rate equals the reverse reaction rate.
(iii) Equilibrium is achieved when the concentrations of reactants and product remain constant.
(iv) Equilibrium is dynamic in nature

  • a) (i), (ii), (iii) and (iv) are correct
  • b) (i), (ii) and (iii) are correct
  • c) only (ii) is correct
  • d) (i), (ii) and (iv) are correct

Answer: (i), (ii), (iii) and (iv) are correct

 

Question: Read the following statements and choose the correct option.

(i) The value of equilibrium constant is independent of initial concentrations of the reactants and products.
(ii) Equilibrium constant is temperature dependent
(iii) The equilibrium constant for the reverse reaction is equal to the inverse of the equilibrium constant for the forward reaction.
(iv) The equilibrium constant for the reverse reaction is equal to the equilibrium constant for the forward reaction.

  • a) (i), (ii) and (iii) are correct
  • b) only (iii) is correct
  • c) (i), (iii) and (iv)
  • d) (i), (ii) and (iv) are correct

Answer: (i), (ii) and (iii) are correct

 

Question:

  • a) (i) , (iii) and (iv)
  • b) (i), (ii) and (iii) are correct
  • c) only (iii) is correct
  • d) (i), (ii) and (iv) are correct

Answer: (i) , (iii) and (iv)

 

Question:

  • a) (i), (ii) and (iii) are correct
  • b) (i) and (ii)
  • c) (ii) and (iii) are correct
  • d) only (iii) is correct

Answer: (i), (ii) and (iii) are correct

 

Question:  Read the following statements and choose the correct option

(i) Most of the acids taste sour
(ii) Acids turns blue litmus paper into red
(iii) Bases turns red litmus paper blue
(iv) Bases taste bitter and feel soapy

  • a) All statements are correct
  • b) (i), (ii) and (iii) are correct
  • c) (i), (iii) and (iv)
  • d) (i), (ii) and (iv) are correct

Answer: All statements are correct

 

Question: Which of the following statements are correct ?

(i) Strong acids have very weak conjugate bases
(ii) Weak acids have very strong conjugate bases
(iii) Strong bases have strong conjugate acids
(iv) Weak bases have weak conjugate acids

  • a) (i) and (ii)
  • b) (ii) and (iv)
  • c) (i) and (iii)
  • d) (iii) and (iv)

Answer: (i) and (ii)

 

Question: Which of the following statement(s) is/are correct ?

(i) Water has ability to act both as an acid and a base
(ii) In pure water one H2O molecule donate proton and acts an acid and another water molecule accepts a proton and acts as a base.

  • a) Both (i) and (ii)
  • b) Only (i)
  • c) Neither (i) nor (ii)
  • d) Only (ii)

Answer: Both (i) and (ii)

 

Question:

  • a) (i), (ii) and (iv)
  • b) (ii) and (iii)
  • c) (i) and (iv)
  • d) (i) and (iv)

Answer: (i), (ii) and (iv)

 

Question:  Read the following statements and choose the correct option

(i) Ka (ionization constant) is a measure of the strength of the acids
(ii) Smaller the value of Ka, the stronger is the acid
(iii) Ka is a dimensionless quantity

  • a) Statements (i) and (iii) are correct
  • b) Statements (i), (ii) and (iii) are correct
  • c) Statements (ii) and (iii) are correct
  • d) Statements (i) and (ii) are correct

Answer: Statements (i) and (iii) are correct

 

Question:

  • a) Both (i) and (ii)
  • b) Only (i)
  • c) Neither (i) nor (ii)
  • d) Only (ii)

Answer: Both (i) and (ii)

 

Question: Which of the following statements are correct ?

(i) The extent of dissociation of an acid depends on the strength and polarity of the H –– A bond (where A is an electronegative element.)
(ii) As the strength of H–A bond increases, the energy required to break the bond decreases.
(iii) As the electronegativity difference between the atoms H and A increases, acidity increases

  • a) (i) and (iii)
  • b) (i) and (ii)
  • c) (ii) and (iii)
  • d) (i), (ii) and (iii)

Answer:  (i) and (iii)

 

Question:

  • a) A – (q), B – (r), C – (p)
  • b) A – (p), B – (r), C – (q)
  • c) A – (r), B – (q), C – (p)
  • d) A – (p), B – (q), C – (r)

Answer: A – (q), B – (r), C – (p)

 

Question:

  • a) A – (q) ; B – (s) ; C – (r) ; D – (p)
  • b) A – (s) ; B – (q) ; C – (p) ; D – (r)
  • c) A – (r) ; B – (s) ; C – (q) ; D – (p)
  • d) A – (p) ; B – (r) ; C – (q) ; D – (s)

Answer: A – (q) ; B – (s) ; C – (r) ; D – (p)

 

Question:

  • a) A – (q), B – (r), C – (p)
  • b) A – (r), B – (q), C – (p)
  • c) A – (p), B – (r), C – (q)
  • d) A – (q), B – (p), C – (r)

Answer:  A – (q), B – (r), C – (p)

 

Question:

  • a) A – (q), B – (p), C – (s), D – (r)
  • b) A – (p), B – (q), C – (r), D – (s)
  • c) A – (r), B – (p), C – (s), D – (q)
  • d) A – (s), B – (q), C – (p), D – (r)

Answer: A – (q), B – (p), C – (s), D – (r)

 

Question:

  • a) A – (r), B – (s), C – (q), D – (p)
  • b) A – (s), B – (p), C – (q), D – (r)
  • c) A – (q), B – (s), C – (r), D – (p)
  • d) A – (p), B – (q), C – (r), D – (s)

Answer: A – (r), B – (s), C – (q), D – (p)

 

Question:

  • a) A – (q), B – (p), C – (r)
  • b) A – (p), B – (r), C – (q)
  • c) A – (r), B – (q), C – (p)
  • d) A – (p), B – (q), C – (r)

Answer: A – (q), B – (p), C – (r)

 

Question:

  • a) A – (r), B – (s), C – (p), D – (q)
  • b) A – (s), B – (p), C – (q), D – (r)
  • c) A – (r), B – (p), C – (s), D – (q)
  • d) A – (q), B – (r), C – (p), D – (s)

Answer: A – (r), B – (s), C – (p), D – (q)

 

Question:

  • a) A – (q), B – (s), C – (p), D – (r)
  • b) A – (r), B – (p), C – (q), D – (s)
  • c) A – (s), B – (q), C – (p), D – (r)
  • d) A – (s), B – (q), C – (p), D – (r)

Answer:   A – (q), B – (s), C – (p), D – (r)

 

Question:

  • a) Assertion is correct, reason is correct; reason is a correct explanation for assertion
  • b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • c) Assertion is correct, reason is incorrect
  • d) Assertion is incorrect, reason is correct.

Answer: Assertion is correct, reason is correct; reason is a correct explanation for assertion

 

Question:

  • a) Assertion is correct, reason is correct; reason is a correctexplanation for assertion
  • b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • c) Assertion is correct, reason is incorrect
  • d) Assertion is incorrect, reason is correct

Answer: Assertion is correct, reason is correct; reason is a correctexplanation for assertion

 

Question:

  • a) Assertion is incorrect, reason is correct
  • b) Assertion is correct, reason is incorrect
  • c) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • d) Assertion is correct, reason is correct; reason is a correct explanation for assertion.

Answer: Assertion is incorrect, reason is correct

 

Question:

  • a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.
  • b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • c) Assertion is correct, reason is incorrect
  • d) Assertion is incorrect, reason is correct.

Answer:  Assertion is correct, reason is correct; reason is a correct explanation for assertion.

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d) None of These

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d) None o these

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d) None of these

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: Two moles of PCl5 were heated in a closed vessel of 2L. At equilibrium 40% of PCl5 is dissociated into PCl3 and Cl2. The value of equilibrium constant is

  • a) 0.267
  • b) 5.3
  • c) 0.53
  • d) 2.63

Answer: 0.267

 

Question:  PCl5 is dissociating 50% at 250°C at a total pressure of P atm. If equilibrium constant is Kp, then which of the following relation is numerically correct ?

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a) 5.82 × 10–2 atm
  • b) 38.8 × 10–2 atm
  • c) 1.94 × 10–2 atm
  • d) 7.66 × 10–2 atm

Answer: 5.82 × 10–2 atm

 

Question:

are in the 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) 36 : 1
  • b) 3 : 1
  • c) 1 : 9
  • d) 1 : 1

Answer: 36 : 1

 

Question:

  • a)

  • b)

  • c)

  • d) All of these

Answer:

 

Question:

  • a) K will remain same
  • b) K will decrease
  • c) K will increase
  • d) K will increase initially and decrease when pressure is very high

Answer: K will remain same

 

Question:

  • a) Adding F2
  • b) Increasing the volume of the container
  • c) Increasing the temperature
  • d) None of these

Answer: Adding F2

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: In HS, I, RNH2 and NH3, order of proton accepting tendency will be

  • a)

  • b)

  • c)

  • d) None of these

Answer:

 

Question: Which equilibrium can be described as an acid-base reaction using the Lewis acid-base definition but not using the Bronsted-Lowry definition?

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: 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 ?

  • a) 3.7 × 10–4 M
  • b) 1.11× 10–3 M
  • c) 1.11 × 10–4 M
  • d) 3.7 × 10– 3 M

Answer: 3.7 × 10–4 M

 

Question: The pH of 10–10 M NaOH solution is nearest to

  • a) 7
  • b) – 10
  • c) 6
  • d) 4

Answer: 7

 

Question: 100 mL of 0.04 N HCl aqueous solution is mixed with 100 mL of 0.02 N NaOH solution. The pH of the resulting solution is:

  • a) 2.0
  • b) 1.0
  • c) 1.7
  • d) 2.3

Answer: 2.0

 

Question: 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 ?

  • a) 3.7 × 10–4 M
  • b) 1.11× 10–3 M
  • c) 1.11 × 10–4 M
  • d) 3.7 × 10– 3 M

Answer:  3.7 × 10–4 M

 

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) 6.13
  • b) 7.87
  • c) 7.00
  • d) 5.13

Answer: 6.13

 

Question:  Ionisation constant of CH3COOH is 1.7 × 10–5 if concentration of H+ ions is 3.4 × 10–4M, then find out initial concentration of CH3COOH molecules

  • a) 6.8 × 10–3M
  • b) 3.4 × 10–4M
  • c) 3.4 × 10–3M
  • d) 6.8 × 10–4M

Answer: 6.8 × 10–3M

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a) 3.0 × 104
  • b) 3.0 × 10– 5
  • c) 3.0 × 10– 4
  • d) 3.0 × 105

Answer: 3.0 × 104

 

Question: If degree of dissociation of pure water at 100°C is 1.8 × 10–8, then the dissociation constant of water will be (density of H2O = 1 gm/cc)

  • a) 1.8 × 10–14
  • b) 1 × 10–14
  • c) 1 × 10–12
  • d) 1.8 × 10–12

Answer: 1.8 × 10–14

 

Question:  Ionisation of weak acid can be calculated by the formula

  • a) Both
  • b)

  • c)

  • d) None of these

Answer: Both

 

Question: Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH ?

  • a) BaCl2
  • b) CaCl2
  • c) MgCl2
  • d) SrCl2

Answer:  BaCl2

 

Question:

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a)

  • b)

  • c) Both
  • d) None of these

Answer:

 

Question:

  • a)

  • b)

  • c)

  • d) None of these

Answer:

 

Question:

  • a) 1.386×10–10
  • b) 1.12×10–11
  • c) 3.16×10–10
  • d) 1.45×10–9

Answer: 1.386×10–10

 

Question: pH scale was introduced by

  • a) Sorensen
  • b) Lowry
  • c) Arrhenius
  • d) Lewis

Answer: Sorensen

 

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