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?
3 answers
Do you have the corresponding Ksp values?
CaSO4 Ksp= 4.93E^-5
Ag2SO4 Ksp= 1.20E^-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+
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+
1 answer