Respuesta :
Answer: option C. in a solution that is 0.20 M in KNO₃.
Explanation:
This question deals with the common ion effect.
Any presence in a solution of a common ion with the solute will decrease its solubility and here you can find why.
AgCl (silver chloride) is highly insoluble in water.
Its solubility equation is given by this equilibrium equation:
AgCl(s) ⇄ Ag⁺(aq) + Cl⁻(aq)
The constant for this equilibrim is called constant of solubility product and is indicated as Ksp:
- Ksp = [Ag⁺][Cl⁻]
Then, any increase of the product ions (on the right side of the equilibrium equation), will result, according to Le Chatelier's principle in a shift of the equilibrium toward the left side, this is in an increase of the AgCl(s), meaning that less AgCl will be soluble.
Let's see in which of the given solutions is AgCl most soluble
A. Solution 0.20 M in CaCl₂
CaCl₂ is a ionic compound which also ionizes in solution, given Ca²⁺ and Cl⁻ ions. So, you can see that it will increase the concentration of Cl⁻, which means that the equlibrium AgCl(s) ⇄ Ag⁺(aq) + Cl⁻(aq), will be shifting to the left, decreasing the solubility of silver chloride.
B. Solution 0.20 M in AgNO₃
AgNO₃ is also a ionic salt which dissociates in water giving Ag⁺ and NO₃ ions. So, it will increase Ag⁺ ions, also shifting the equilibrium AgCl(s) ⇄ Ag⁺(aq) + Cl⁻(aq) to the left, decreasing the solubility of silver chloride.
C. Solution 0.20 M in KNO₃
Since KNO₃ has no common ions with AgCl, it will not affect the equilibrium equation in the same manner and you can expect that AgCl is most soluble in KNO₃.
Solubility is the property of the substance to get dissolved in a solution. silver chloride is most soluble in a solution of 0.20 M potassium nitrate.
What is the common ion effect?
When a soluble compound is added that contains a common ion as that of the precipitate to the solution decreases the solubility of the precipitate.
Silver chloride is insoluble in an aqueous solution and its solubility equation can be given as:
[tex]\rm AgCl(s) \leftrightarrow Ag^{+}(aq) + Cl^{-}(aq)[/tex]
Constant of solubility product for the equilibrium reaction can be given as:
[tex]\rm Ksp = [Ag^{+}][Cl^{-}][/tex]
The equilibrium will shift towards the left side when there is an increase in the ions of the product. This will result in decreased solubility of silver chloride solution.
The solution of 0.20 M Potassium nitrate has no common ion effect with silver chloride and will not affect the equilibrium constant reaction.
Therefore, silver chloride is most soluble in option C. 0.20 M Potassium nitrate solution.
Learn more about the common ion effect here:
https://brainly.com/question/4090548
