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.
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
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Samoylenko's class at TEXAS.