Preparation and solution of 1st year Chemistry MCQs are considered tough enough. MCQs of chemistry are not such simple as other's books. Chemistry MCQs need a special and comprehensive explanation for solutions. So, here you are given a concept review of the most important mcqs of chemistry class 11.
Download or Preview 1st year Chemistry MCQs with answers to Chapter 8 Chemical Equilibrium. These mcqs are also important for the preparation of the Entrance exam UHS NMDCAT and UET.
1st Year Chemistry mcqs Importance
It is a tough and difficult task to solve 1st Year Chemistry mcqs. Students
must need full conceptual knowledge of 1st-year chemistry mcqs for excellent
marks in Chemistry 11. All the important MCQs related to Chapter 8 Chemical Equilibrium of 1st-year Chemistry are here for you. These questions are taken from past
papers of 1st-year chemistry of all Punjab Board of Pakistan as ;
Bahawalpur Board
D.G.Khan Board
Faisalabad Board
Gujranwala Board
Lahore Board
Multan Board
Rawalpindi Board
Post is created and designed with intense care and diligence.
These questions (MCQs) are top repetitive in 1st year Chemistry Past Papers. Each
question has a detailed answer explanation. In this way, you learn 1st year chemistry mcqs chapter 8 Chemical Equilibrium easily.
Study Smart & Splendid Marks
F.sc part 1 Students face big difficulties while preparing for Chemistry Multiple Choice Questions (MCQs). Good News! mhbeducator.com
offers you, the easiest and smartest way to prepare for 1st year chemistry mcqs. In this post, you
can view and download the 1st year chemistry chapter 8 Chemical Equilibrium mcqs. 1st year chemistry mcqs with answers pdf of all chapters click the link below the post. This
content is very helpful for weak students and also helpful for those
students that are better at 1st-year chemistry exam preparation. These
Questions are based on the current Chemistry 11 syllabus according
to Punjab Textbook Board.
About This Chapter
Chapter no. 8 "Chemical Equilibrium" of 1st-year chemistry
enables the students to learn.
- Reversible reactions
- Irreversible reactions
- Equilibrium state
- Law of mass action
- Equilibrium constant expression for some important reactions
- Relationships between equilibrium constants
- Applications of equilibrium constants
- Le-Chateliers Principle
- Applications of chemical equilibrium in the industry
- Ionic product of water
- Ionization constant of acids (Ka)
- Ionization constant of bases(kb)
- Lowery Bronsted acid and base concept
- Common Ion effect
- Buffer solutions
- Henderson's equation for acidic buffers
- Buffer capacity
- Solubility product
- Applications of solubility product
This Post "1st-year Chemistry Chapter 8 Chemical Equilibrium mcqs from past papers" covers all important MCQs that are top repetitive
in past papers relevant to the above-mentioned topics.
👉For Answers to the following questions click the show answer button.
1. Law of mass action was derived by Guldberg and Waage:
(A) 1906
(B) 1909
(C) 1846
(D) 1864
(D) 1864
2. For which system does the equilibrium Kc has units of (Conc.)-1
(A) N2 + 3H2 ↔ 2NH3
(B) 2NO2 ↔ N2O4
(C) H2 + I2 ↔ 2HI
(D) 2HF ↔ H2+ F2
(C) H2 + I2 ↔ 2HI
3. Which one affects the value of Kc?
(A) Catalyst
(B) Pressure
(C) Temperature
(D) Concentration
(C) Temperature
4. Equilibrium constant for gaseous medium is represented by
(A) Kp
(B) Ka
(C) Kb
(D) Kx
(A) Kp
5. The optimum temperature for the synthesis of NH3 by Haber's process is:
(A) 200℃
(B) 300℃
(C) 400℃
(D) 500℃
(C) 400℃
6. The aquas solution of BCl3 is cloudy: cloudiness of BCl3 can be cleared by
(A) Addition of water
(B) Addition of BiCl3
(C) Addition of AlCl3
(D) Addition of BiCl3 and H2O
(D) Addition of BiCl3 and H2O
7. When the Kc value is small, the equilibrium position is
(A) Towards left
(B) Towards right
(C) Remains unchanged
(D) None of these
(A) Towards left
8. pH of Milk is
(A) 6.5
(B) 8.5
(C) 10.5
(D) 12.5
(A) 6.5
9. pH of pure water is:
(A) 6.5
(B) 8.5
(C) 7.0
(D) 8.0
(C) 7.0
10. The term pH was introduced by:
(A) Thomson
(B) Goldsmith
(C) Sorenson
(D) Henderson
(C) Sorenson
11. The pH of 10-3 mol dm-3 of an aqueous solution of H2SO4 is:
(A) 3.0
(B) 2.7
(C) 4.0
(D) 4.7
(B) 2.7
12. The value of the ionic product (kw) of water at 25°C
(A) 3 ✕ 10-14
(B) 1 ✕ 10-14
(C) 0.11 ✕ 10-14
(D) 0.30 ✕ 10-14
(B) 1 ✕ 10-14
13. The sum of pKa and pKb is:
(A) 1
(B) 0
(C) 7
(D) 14
(D) 14
14. Strength of an acid is determined from the value of:
(A) Kw
(B) Kc
(C) Ka
(D) Kp
(C) Ka
15. pH of human blood is
(A) 3.5
(B) 5.35
(C) 7.35
(D) 8.35
(B) 5.35
16. The solubility product of AgCl is 2.0 ✕ 10-10 mol2 dm-6. The maximum concentration of Ag+ ions in the solution is:
(A) 2 ✕ 10-10 mol dm-3
(B) 1.41 ✕ 10-5 mol dm-3
(C) 1 ✕ 10-10 mol dm-3
(D) 4 ✕ 1020 mol dm-3
(D) 4 ✕ 1020 mol dm-3
17. An excess of Aqueous AgNO3 is added to the Aqueous BaCl2 solution, and the precipitate is removed. The filtrate contains:
(A) Ba+2, NO3- and Cl- ions
(B) Ba+2 and NO3- only
(C) Ag+2 and NO3- only
(D) All of above
(A) Ba+2, NO3- and Cl- ions
18. The nature of an aqueous solution of ammonia is :
(A) Acidic
(B) Basic
(C) Neutral
(D) Amphoteric
(D) Amphoteric
19. Which is used as catalyst in Haber Process for NH3 gas manufacture?
(A) Iron
(B) Copper
(C) Carbon
(D) Silver
(A) Iron
20. In modern Haber Process plants, the temperature maintained during the process is:
(A) 400℃ - 500℃
(B) 100℃ - 200℃
(C) 200℃ - 300℃
(D) 500℃ - 600℃
(A) 400℃ - 500℃
0 Comments