All the questions on this quiz deal with the following solutions.
Solution A: 40.0 mL of 0.500 M AlCl3 Solution B: 60.0 mL of 1.000 M Ag2SO4
Treat the solubilities of these solutions as would be determined from the solubility rules in
the text. In reality, things are more complicated, as silver forms a AgCl2-
ion in high chloride concentrations, which causes the precipitate to redissolve, giving lower yields
than predicted. Also, in reality, Silver sulfate is a weak electrolyte and will not form a
1M solution, but we will treat it as a strong electrolyte, in accordance with our solubility rules.
This is an important concept to understand, that is, these solubility rules are a simplification of things.
During the second semester of this course we will introduce the more advanced concept of Solubility
Constants, which will allow us to deal rigorously with the actual concentrations of ionic compounds in aqueous
What are the respective aluminum and chloride concentrations in solution A?