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.