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NEET Exam  >  NEET Tests  >  Daily Test for NEET Preparation  >  Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - NEET MCQ

Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - NEET MCQ


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10 Questions MCQ Test Daily Test for NEET Preparation - Test: Solubility Equilibria of Sparingly Soluble Salts (August 2)

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Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 1
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Common Ion effect can be used in which of the following cases?

Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 1
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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 2
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The degree of dissociation of Ammonium hydroxide increases in the presence of Ammonium Chloride because of ______________

Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 2
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.
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Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 3
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For the dissociation of an electrolyte AxBy, Ksp is given as [Ay+]x[Bx+]y. What is Ksp?

Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 3
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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 4
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Hydroxide Ion concentration in calcium hydroxide and barium Hydroxide is an example of ______________ solution.
Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 4
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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 5
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A salt is soluble is the solubility is ______________
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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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 6
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Precipitate is formed if ionic product is ______________
Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 6
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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 7
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If Ksp of a salt A2B3 is given by 1 x 10-25. Then find the solubility of the salt?
Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 7
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.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 8
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Which of the following statements is true regarding the solubility product (Ksp) of a sparingly soluble salt?
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The statement that is true regarding the solubility product (Ksp) of a sparingly soluble salt is that "Ksp is a constant value and is independent of temperature and pressure." Ksp is a constant at a given temperature and does not change with variations in pressure. It characterizes the equilibrium between the solid salt and its ions in a saturated solution at a specific temperature.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 9
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The solubility of a sparingly soluble salt is primarily influenced by which of the following factors?
Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 9
The solubility of a sparingly soluble salt is primarily influenced by the presence of common ions and the pH of the solution. Common ions can lead to the common ion effect, which reduces the solubility of the salt. Additionally, the pH of the solution can affect the solubility because some salts are more soluble in acidic or basic conditions.
Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 10
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The solubility for the salts of the type AB3 is given by _______________
Detailed Solution for Test: Solubility Equilibria of Sparingly Soluble Salts (August 2) - Question 10
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.
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