[defang]

An experimenter makes up a solution of 0.375 mol Na2CO3, 0.125 mol Ca(NO3)2, and 0.200 mol Ag2CO3 in 2.000 L of water solution.  Note any precipitations that occur, write a balanced equation for each.  Then, calculate the molarities of each ion in the solution.  (CaCO3: Ksp = 4.8X10-9, Ag2CO3: Ksp = 8.1X10-12)

Here is what i have done:
Ca2+  + CO3^2- = CaCO3
2Ag+  + CO3^2- = Ag2CO3

Can anyone help me what I should do next?  THANKS!

I believe the answers are [Ca2+] = 6.4X10^-8 and [Ag+] = 1.04x10^-5

[Borek]

At first you may safely assume only Na2CO3 is a source of CO3(2-) ions. Ca(2+) removes part of the CO3(2-) from the solution, still a lot of these ions is left. Thus you may use their final concentration to calculate Ca(2+) and Ag+ in saturated solution.