Calculate the mass of solid AgNo3 that can be added to 2.0 L of 0.10M K2CrO4 solution in order to just start precipitation?

Answer 1

Ag2CrO4 ==> 2Ag^+ + CrO4^2-
Ksp = (Ag^)^2(CrO4^2-)
mols CrO4^2- = mols x L = ?
Substitute into Ksp expression and solve for (Ag^+). That is (AgNO3). Convert M to mols in the 2.0 L and convert to grams. g = mols x molar mass. Post your work if you get stuck.

Answer 2

2AgNO3(aq) + K2CrO4(aq) ==> Ag2CrO4(s) + 2KNO3(aq)

Ag2CrO4(s) ===> 2Ag^+ CrO4^^2-

Ksp = [Ag^+]^2[CrO4^2-]

Ksp = (2x)^2(0.1)