This set of Class 11 Chemistry Chapter 7 Multiple Choice Questions & Answers (MCQs) focuses on “Ionic Equilibrium in Solution”.
1. CH3COOH \(\rightleftharpoons\) CH3COO– + H+ is in __________________
a) ionic equilibrium
b) chemical equilibrium
c) dynamic equilibrium
d) physical equilibrium
Explanation: The equilibrium that is attained between the ionized molecules and the ions in the solution of weak electrolyte is called Ionic Equilibrium. CH3COOH \(\rightleftharpoons\) CH3COO– + H+ is an example; CH3COO– and H+ are ions.
2. Electrolytes conduct electricity.
Explanation: Chemical substances which can conduct electricity in their Aqua state or in the molten state are called electrolytes. The conduction of current through the electrolyte is due to the movement of Ions, hence the above statement is true.
3. Which of the following may not be a strong electrolyte?
a) hydrochloric acid
b) sulfuric acid
c) nitric acid
Explanation: Electrolytes which dissociate almost completely into constituent ions in aqueous solutions are known as strong electrolytes. Therefore ammonia is not a strong electrolyte because it can’t dissociate completely.
4. All organic acids except sulfonic acid are _____________ electrolytes.
d) neither strong nor weak
Explanation: Electrolytes which dissociate into a lesser extent in aqua solution are called weak electrolytes. All organic acids except sulfonic acids and bases like Ammonia, Ammonium hydroxide, amines, etc are weak electrolytes.
5. Can nonelectrolytes conduct electricity?
d) cannot say
Explanation: Michael Faraday classified substances into two categories; one is electrolytes and nonelectrolytes, nonelectrolytes do not dissociate into ions in a solution. So they do not conduct electricity.
6. Sugar solution __________ electricity.
a) do not conduct
c) depends on the type of sugar
d) cannot say
Explanation: Aqueous solution of sugar does not conduct electricity, but Aqueous solution of sugar conducts electricity. This is because the aqueous solution of sugar is a nonelectrolyte, whereas the salt solution is an electrolyte.
7. Which of the following is in Ionic Equilibrium?
a) 2AgI + Na2S \(\rightleftharpoons\)Ag2S + 2NaI
b) 4 NH3 + 5 O2 \(\rightleftharpoons\)4 NO + 6 H2O
c) TiCl4 + 2 H2O \(\rightleftharpoons\)TiO2 + 4 HCl
d) H2O + H2O \(\rightleftharpoons\)H3O+ + OH–
Explanation: Only H2O + H2O \(\rightleftharpoons\)H3O+ + OH– is in ionic equilibrium. As the equilibrium established between the unionized molecules and the ions in the solution of weak electrolytes is known as Ionic Equilibrium.
8. What is the degree of dissociation for strong electrolytes?
c) less than 1
d) greater than 1
Explanation: Degree of dissociation is the fraction of the total number of molecules which dissociate into constituent ions, it is represented by the symbol ɑ. As a strong electrolyte dissociate completely, it values is 1.
9. Degree of dissociation does not depend on which of the following factors?
a) nature of the solute
b) nature of the solvent
Explanation: Values of the degree of dissociation or degree of ionization depends upon the following factors: 1) the nature of the solute, 2) the nature of the solvent 3) concentration and 4) temperature of the solution.
10. K in K = Cα2/1 – ɑ represents ___________
a) dissociation constant
b) molar concentration
c) degree of dissociation degree of ionization
d) degree of ionization
Explanation: The above equation represents Ostwald’s dilution law, where K is the dissociation constant, C is the molar concentration of the solution and ɑ is a degree of dissociation or degree of ionization of the solution.
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