A question on chemical equlibrium...?

A student mixes 0.250 L of 1.8x10-3 M Mg(NO3)2 solutin with 0.150 L of 0.60 M NaCO3 solution to give a final volume of 0.400 L. Determine the concentration of Mg2+ after mixing, the concentration of CO3 2- after mixing, whether or not a percipitate of MgCO3 will form under these conditions.

Answer:
Moles Mg2+ = 0.250 x 1.8 x 10^-3 = 0.00045
Moles CO32- = 0.150 x 0.60 = 0.090
[Mg2+] = 0.00045 / 0.400 = 0.00112 M
[CO32-] = 0.090 / 0.40 = 0.225 M
Ksp of MgCO3 = 3.5 x10^-8
0.00112 x 0.225 = 2.52 x 10^-4
This ion product is highter than the value of Ksp so it would not correspond tp an equilibrium situation and precipitation should occur
you should make the prob simpler so that people can answer you

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