A beaker contains 0.010 M AgNO₃(aq). Separate samples of AgBr(s) (Ksp=5.0×10−13) and Ag₂CrO₄(s) (Ksp=1.1×10−12) are added to this solution at 25 °C.
(a) Calculate the percent decrease in molar solubility for AgBr compared with its solubility in pure water.
(b) Calculate the percent decrease in molar solubility for Ag₂CrO₄ compared with its solubility in pure water.
(c) Identify which salt experiences the greater relative suppression of solubility and justify your choice with the calculated values.