This set of Class 11 Chemistry Chapter 7 Multiple Choice Questions & Answers (MCQs) focuses on “Solubility Equilibria of Sparingly Soluble Salts”.
1.The degree of dissociation of Ammonium hydroxide increases in the presence of Ammonium Chloride because of ______________
a) solubility product
b) common Ion effect
c) hydrolysis of the salt
d) mixed salts
View Answer
Explanation: Common Ion effect is defined as the separation of the dissociation of a weak electrolyte by the addition of a strong electrolyte having some common ion. Therefore the degree of dissociation of Ammonium hydroxide decreases in the presence of Ammonium Chloride due to common Ion effect.
2. Common Ion effect can be used in which of the following cases?
a) cloth making
b) alcohol purification
c) quantitative analysis
d) qualitative analysis
View Answer
Explanation: Common Ion effect is used in the purification of common salt, salting out of soap and qualitative analysis. In qualitative analysis, Ammonium Hydroxide is added in the presence of Ammonium Chloride to avoid the precipitation of V group radicals.
3. Hydroxide Ion concentration in calcium hydroxide and barium Hydroxide is an example of ______________ solution.
a) isochoric solution
b) isohydric solutions
c) hypo solution
d) hyper solution
View Answer
Explanation: In the solution of two electrolytes, if the common ions’ concentration (Hydroxide Ion concentration in calcium hydroxide and barium hydroxide solution) is equal, then on mixing there is zero change in the degree of association in both of the electrolytes, such solutions are called isohydric solutions.
4. For the dissociation of an electrolyte AxBy, Ksp is given as [Ay+]x[Bx+]y. What is Ksp?
a) solubility product
b) soluble product
c) solution product
d) solvent product
View Answer
Explanation: Solubility product Ksp is defined as the product of the concentrations of the ions of the salt in its standard solution at a given temperature raised to the power of the ions produced by the dissociation of 1 mole of the salt.
5. Precipitate is formed if ionic product is ______________
a) greater than the solubility product
b) less than the solubility product
c) equal to the solubility product
d) independent of the solubility product
View Answer
Explanation: The concept of solubility product helps in predicting the formation of the precipitate. In general, if the ionic product is greater than the solubility product, the precipitate is formed and if the ionic product is less than the solubility product, the precipitate is not formed.
6. Solubility product can be used in predicting the solubility of a sparingly soluble salt.
a) true
b) false
View Answer
Explanation: Yes, we can predict the solubility of a sparingly soluble salt, for example, consider the reaction; AxBy = xAy+ + yBx+, the solubility of a sparingly soluble salt is given by xx.yy.sx+y, knowing the values of Ksp, x and y, the solubility of the salt can be calculated.
7. A salt is soluble is the solubility is ______________
a) less than 0.01 M
b) in between 0.01 M and 0.1 M
c) greater than 0.01 M
d) greater than 0.1 M
View Answer
Explanation: A salt is soluble if the solubility is greater than 0.1 M. A salt is slightly soluble if the solubility is between 0.01 M and 0.1 M and the salt is sparingly soluble if the solubility is less than 0.01 M.
8. If Ksp of a salt A2B3 is given by 1 x 10-25. Then find the solubility of the salt?
a) 10-3
b) 10-4
c) 10-5
d) 10-8
View Answer
Explanation: For the salt AxBy, (AxBy = xAy+ + yBx+), the solubility of a sparingly soluble salt is given by xx.yy.sx+y. Ksp = xx.yy.sx+y, where x = 2 and y = 3; Ksp = 108S5 = 1 x 10-25. S = 10-5. The solubility of the salt is given by 10-5.
9. The solubility for the salts of the type AB3 is given by _______________
a) (Ksp 27)1/4
b) (Ksp/27)1/5
c) (Ksp/27)3/4
d) (Ksp/27)1/4
View Answer
Explanation: For the salt AxBy, (AxBy = xAy+ + yBx+), the solubility of a sparingly soluble salt is given by xx.yy.sx+y. Ksp = xx.yy.sx+y, where x = 1 and y = 3; Ksp = 27S4, by rearranging, we get solubility denoted by S as (Ksp/27)1/4.
10. Both the solubility product and ionic product are applicable to all types of solutions.
a) true
b) false
View Answer
Explanation: Solubility of the product is only applicable to the saturated solutions, whereas an ionic product is applicable to all types of solutions. It is because the formation of a precipitate is dependent on the solubility product.
Sanfoundry Global Education & Learning Series – Chemistry – Class 11.
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