posted by yab0yMark94 on .
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0290 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate?What percentage of the Ca2 (aq) can be separated from the Ag (aq) by selective precipitation?
Do you have the corresponding Ksp values?
CaSO4 Ksp= 4.93E^-5
Ag2SO4 Ksp= 1.20E^-5
Ag2SO4 will begin to ppt when
Ksp = (Ag^+)^2(SO4^2-) is exceeded.
(SO4^2-) = Ksp/(Ag^+)^2
(SO4^2-) = Ksp/(0.290)^2
Solve for SO4^2- and substitute into Ksp for CaSO4. Solve for Ca^2+