Will a precipitate form when 65.0 ml of 0.0200 m ag2so4 is mixed with 50.0 ml of 0.00500 m k2co3? (ksp for silver carbonate is 8.00 x 10–12).

We have to calculate the Ksp of Ag2CO3 value to compare it with the given value to know if Ag2CO3 will be precipitate or not.
when Ksp = [Ag+]^2[CO3-]
when 2 mol of Ag+ gives 1 mol Ag2SO4
and no.of moles of Ag2SO4 = volume * molarity
                                                = 65 ml/1000 * 0.02M = 0.0013 moles
∴ no.of moles of Ag+ = 2 x 0.0013 = 0.0026 moles
and when 1 mol of CO3- gives 1 mol K2CO3
and no.of moles of K2CO3 = volume * molarity
                                              = 50 ml/1000 * 0.005 M = 0.00025 moles
∴no of moles of CO3- = 0.00025 * 1 = 0.00025 moles
∴Ksp = (0.0026)^2 * (0.00025)
         = 1.69x10^-9
by comparing this value with the given value 
∴ Ag2CO3 would be precipitated.

How do we find the answer?