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Question: Arrange in correct order of increasing solubility of \[AgCl\] in: A) Water B) \[0.1{\text{ }}M{...

Arrange in correct order of increasing solubility of AgClAgCl in:
A) Water
B) 0.1 M NaCl0.1{\text{ }}M{\text{ }}NaCl
C) 0.1 M BaCl20.1{\text{ }}M{\text{ }}BaC{l_2}
D) 0.1 M NH30.1{\text{ }}M{\text{ }}N{H_3}
a. A<B<C<DA < B < C < D
b. B<C<D<AB < C < D < A
c. C<B<D<AC < B < D < A
d. C<B<A<DC < B < A < D

Explanation

Solution

Solubility depends upon many factors, some of these factors are its dissociation in solvent, the ability to form a complex with the solvent and the presence of a common ion. The presence of common ions decreases the solubility and formation of complexes increases solubility.

Complete step by step answer:
Let’s start with discussing the solubility case wise.
Case 1:
In case 1 we are having the water, Water being a common solvent and AgClAgCl being an ionic salt it will easily dissolve into the water. So, let’s take water as the base and measure the solubility of other cases with the reference of water.
Case 2:
In case 2 we are having 0.1 M NaCl0.1{\text{ }}M{\text{ }}NaCl, in this case due to the presence of a common ion that is Cl−C{l^ - } the solubility of the AgClAgCl will be less than that of water.
Case 3:
In case 3 we are having 0.1 M BaCl20.1{\text{ }}M{\text{ }}BaC{l_2}, in this case due to the presence of a common ion i.e. Cl−C{l^ - } the solubility of AgClAgCl will be less than that of water. Since the amount of Cl−C{l^ - } ion will be twice as much as 0.1 M NaCl0.1{\text{ }}M{\text{ }}NaCl, hence the solubility of AgClAgCl will be less as compared to solubility of AgClAgCl in 0.1 M NaCl0.1{\text{ }}M{\text{ }}NaCl.
Case 4:
In case 4 we are having 0.1 M NH30.1{\text{ }}M{\text{ }}N{H_3}, in this case a complex between the AgClAgCl and NH3N{H_3} will be formed. The complex will be [Ag(NH3)2]Cl\left[ {Ag{{\left( {N{H_3}} \right)}_2}} \right]Cl and due to this complex formation the solubility of AgClAgCl will be increased and the solubility of AgClAgCl in 0.1 M NH30.1{\text{ }}M{\text{ }}N{H_3} will be more than that of water.

Hence, the answer to this question is option d. C<B<A<DC < B < A < D .

Note:
The concept of solubility is majorly used to check how much a particular salt or compound is soluble in the solvent or not. Solubility is of utmost importance when you are trying to achieve a solution as if you want a solution of 1M but 1 mole of substance is not soluble in 1L of water then we need to think of some alternative way. Hence the concept of solubility is must to understand.