How do I solve this AP Chemistry problem on precipitation?

Question

Can Ce (IO3)3 precipitate when adding together 100mL of 1.0×10^-2 M Ce (NO3)3 and 200mL of 2.0×10^-3 M KIO3?

 

Ksp=1.9×10^-10

Answer 1

Final volume of solution = 100 ml + 200 ml = 300 ml = 0.3 L

Ce(NO₃)₃ + 3KIO₃ ==> Ce(IO₃)₃ + 3KNO₃

Find moles Ce(IO₃)₃ produced:

moles Ce(NO₃)₃ = 0.1 L x 1.0x10^-2 mol/L = 1.0x10^-3 moles 

moles KIO₃ = 0.2 L x 2x10^-3 mol/L = 4x10^-4 moles = LIMITING REACTANT

moles Ce(IO₃)₃ formed = 1/3 x 4x10^-4 moles = 1.3x10^-4 moles

Final [Ce(IO₃)₃ = 1.3x10^-4 mol/0.3 L = 4.4x10^-4 M

Q = [Ce³⁺][IO₃^-]³

Q = (4.4x10^-4)(4.4x10^-4)³ = 3.75x10^-14

Q < Ksp therefore NO PRECIPITATE FORMS