Problem: In which of the following aqueous solutions would you expect AgCl to have the lowest solubility? Choose one answer. a. 0.020 M KCl b. pure water c. 0.015 M NaCl d. 0.020 M BaCl2 e. 0.020 M AgNO3

FREE Expert Solution

We’re being asked to determine in which solvent AgCl would be least soluble in.


The common ion effect states that the solubility of a salt is lower in the presence of a common ion. This means if there is a higher concentration of a common ion present, the less soluble a compound will be. The dissociation of AgCl in water is as follows:


The chloride ion, Cl, has a charge of –1. Silver then has a charge of +1:

AgCl(s)  Ag+(aq) + Cl(aq)


Among the given choices, pure water and 0.020 M AgNO3 don't contain common ions so the solubility of AgCl is not lowered in those.


We’ll now determine which between the remaining solutions have higher Cl concentration: a higher Cl (common ion) concentration will lead to lower solubility of AgCl.


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Problem Details

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility? Choose one answer. 

a. 0.020 M KCl 

b. pure water 

c. 0.015 M NaCl 

d. 0.020 M BaCl2 

e. 0.020 M AgNO3

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