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Solubility and Solubility Product MCQ - Practice Questions with Answers
Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET
Quick Facts
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Solubility and Solubility Product is considered one the most difficult concept.
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33 Questions around this concept.
Solve by difficulty
pH of a saturated solution of is 9. The solubility product
of
is:
The solubility of in water is
at 298 K. The value of its solubility product (Ksp) will be
(Given molar mass of )
Using the Gibbs energy change, , for the following reaction,
The of
in water at
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The pH of a saturated solution of is
. The value of the solubility product
of
is :
Identify the correct order of solubility in aqueous medium:
Find out the solubility of in
. Given that the ionic product of
is
.
The solubility of with solubility product in
solution would be:
and
two nearly insoluble salts, have the same
values of
at room temperature. Which statement would be true in regard of
and
?
Identify the correct order of solubility in aqueous medium:
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Download EBookThe are respectively,
. Which one of the following salts will precipitate last if
solution is added to the solution containing equal moles of
?
Concepts Covered - 1
Solubility and Solubility Product
Solubility
It is the weight of solute present in 100 ml of solvent. It is denoted by 's' and is expressed in mol per litre or gm per litre. The number of moles of solute in 1 L of saturated solution is known as molar solubility.
Solubility decreases with the increase in concentration of common ion. It increases with temperature and increases in case the ions formed from the sparingly soluble salt undergo some sort of reaction like complexation.
Example, The solubility of AgCl in water in presence of AgNO3
Solubility increases due to complex ion formation. For example, AgCl has more solubility in ammonia due to complex formation
Solubility Product: It is the product of the molar concentrations of ions of an electrolyte in a saturated solution at a particular temperature. It is denoted by Ksp or S.
General Representation
Relation between Solubility(s) and Solubility Product (Ksp)
s 0 0
- xs ys
Solubility Product and Precipitation
- If Ksp ≈ Ionic product
The solution is saturated and for precipitation, more solute is to be added. - If Ionic product > Ksp
The solution is supersaturated so easily precipitated. - If Ionic product < Ksp
The solution is unsaturated so no precipitation takes place.
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