Likely, sulfate... but you would have to do the experiment yourself to verify this.
...And this reaction is given by...
$"Na"_2"SO"_4(aq) + "MgCl"_2(aq) -> "NaCl"(aq) + "MgSO"_4(s)$
$s_(MgSO_4) ~~ "35.1 g/100 mL water"$ at$25^@ "C"$ which is quite high. But contrary to common expectation, by boiling, the solubility decreases.
Magnesium sulfate is one of the only examples I can think of that . You can read more about this , but in short...
Increasing the temperature for
$"MgSO"_4(aq)$ shifts the equilibrium between crystallization and [dissolution + solvation], towards crystallization, because .$DeltaH ~~ -"91.2 kJ/mol"$ .
As for the others...
$s_(Mg(HCO_3)_2) = "0.077 g/100 mL water"$ at$25^@ "C"$
$s_(MgCO_3) = "0.0139 g/100 mL water"$ at$25^@ "C"$
$s_(Mg(NO_3)_2) = "large"$ at$25^@ "C"$
And the first two clearly precipitate at room temperature and pressure. Where on Wikipedia did I get this data?