MCQs On Ionic Equilibrium For NEET pdf
Multiple Choice Questions On Ionic Equilibrium For Class 12
Hello Students, how are you all hope you all will be well, in this Page we have shared with you more than 20 Important MCQs on ionic equilibrium class 12 with answers which is helpful for various entrance exam preparation. This ionic equilibrium class 12 Mcq pdf will help you enhance your performance in entrance exams like NEET and JEE. mcq on ionic equilibrium in chemistry is an important chapter for Class 10, 11, and Class 12 Students.
Ionic Equilibrium MCQs questions and answers are provided here with answers and detailed explanations of each question. These Ionic Equilibrium MCQs are important from the NEET as well as various types of exams. By practicing our Mcq on Ionic equilibrium class 12 pdf students will get acquainted with the key concepts which must be prepared to score high marks in the objective type questions in any exam.
Important points about Ionic equilibrium
- Chemical equilibria are important in numerous biological and environmental processes. For example, equilibria involving O2 molecules and the protein hemoglobin play a crucial role in the transport and delivery of O2 from our lungs to our muscles.
- The double half arrows indicate that the processes in both directions are going on simultaneously.
- The mixture of reactants and products in the equilibrium state is called an equilibrium mixture.
- Equilibrium can be established for both physical processes and chemical reactions. The reaction may be fast or slow depending on the experimental conditions and the nature of the reactants.
- Some important aspects of equilibrium involving physical and chemical processes are dealt with in this unit along with the equilibrium involving ions in aqueous solutions which is called ionic equilibrium.
- All substances that conduct electricity in aqueous solutions are called electrolytes.
- Acids, bases, and salts are electrolytes and the conduction of electricity by their aqueous solutions is due to anions and cations produced by the dissociation or ionization of electrolytes in aqueous solution.
- The strong electrolytes are completely dissociated. In weak electrolytes, there is an equilibrium between the ions and the unionized electrolyte molecules.
- According to Arrhenius, acids give hydrogen ions while bases produce hydroxyl ions in their aqueous solutions.
- Brönsted-Lowry on the other hand, defined an acid as a proton donor and a base as a proton acceptor.
Multiple Choice Questions On Ionic Equilibrium For Class 12
1. What is the pH of a 0.10 M solution of barium hydroxide, Ba (OH)2?
A) 11.31
B) 11.7
C) 13.30
D) None of these
Answer: C
2. Which of the following oxides is not expected to react with sodium hydroxide?
A) CaO
B) SiO2
C) BeO
D) B2O3
Answer: A
3. In a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant will___________
A) Also be Doubled
B) Be Halved
C) Remain the Same
D) Become One-Fourth
Answer: C
4. Among the following the weakest Bronsted base is__________
A) F–
B) Cl–
C) Br–
D) I–
Answer: D
5. Among the following hydroxides, the one which has the lowest value of Ksp at ordinary temperature (about 25°C ) is___________
A) Mg (OH)2
B) Ca(OH)2
C) Ba(OH)2
D) Be(OH)2
Answer: D
6. When two reactants A and B are mixed to give products C and D, the concentration quotient (Q) at the initial stage of the reaction
A) Is zero
B) Decreases with time
C) Is independent of time
D) Increases with time.
Answer: D
7. For the chemical reaction3X (g) + Y (g) ⇌ X3Y (g) the amount of X3Y at equilibrium is affected by_______
A) Temperature and pressure
B) Pressure only
C) Temperature only
D) Temperature, pressure, and catalyst.
Answer: A
8. For the chemical reaction:2A + BC, the units of Kp is________
A) atm-2
B) atm-3
C) atm-1
D) Dimensionless
Answer: A
9. 1 mole of N2 and 2 moles of H2 are allowed to react in a 1 dm³ vessel. At equilibrium 0.8 mole of NH3 is formed. The concentration of H2 in the vessel is
A) 0.6 mole
B) 0.8 mole
C) 0.2 mole
D) 0.4 mole.
Answer: B
10. For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be_______
A) halved
B) doubled
C) the same
D) one fourth
Answer: C
11. The pH of 10-8 M HCl is__________
A) 8
B) 7
C) between 7 and 8
D) between 6 and 7
Answer: D
12. In equilibrium constant expression, the concentration of products is taken in/on the_______
A) right side
B) left side
C) numerator
D) denominator
Answer: C
13. What is the representation of a reversible reaction?
A) single arrow
B) double arrows
C) bar
D) none of above
Answer: B
14. Which of the following is the correct representation of “active mass”?
A) ( )
B) { }
C) [ ]
D) none of above
Answer: C
15. In an exothermic reversible reaction increase in temp shifts the equilibrium to___________
A) reactant side
B) product side
C) remains unchanged D) none
Answer: A
16 Units of Kw are_______
A) mole dm–3
B) mole2 dm–3
C) mole2 dm–6
D) mole2 dm–3
Answer: A
17. Law of mass action was presented by_____
A) Henderson
B) Lewis
C) Guldberg and Waage
D) Arrehenius
Answer: C
18. The unit of Kc for reaction
N2 + O2 2NO
A) mol dm–3
B) mol–1 dm3
C) mol–2 dm6
D) no units
Answer: d
19. PH of pure water is_____
A) 3.2
B) 4.2
C) 7.0
D) 0
Answer: C
20. When pressure is applied to the given equilibrium ice water which of the following will happen__________
A) more ice will be formed
B) more water will be formed
C) equilibrium will not be disturbed
D) Water well-formed
Answer: D