chemistry
posted by Justin on .
A solution is saturated with Ag2CrO4. a) Calculate [CrO4^2] in this saturated solution. b) What mass of AgNO3 must be added to 0.635 L of the solution to reduce [CrO4^2] to 1.0* 10^8M?

Let x = solubility Ag2CrO4
Ag2CrO4(s) ==> 2Ag^+ + CrO4^2
.....x..........2x.......x
Ksp = (Ag^+)^2(CrO4^2)
Substitute from the chart above and solve for x
b.
Use the same Ksp expression. Substitute what you want CrO4^2 to be an solve for (Ag^+). That will give you Ag^+ in moles/L. Convert to moles in 0.635 L, then g AgNO3 = moles x molar mass AgNO3.