We're being asked to determine the volume of 0.116 M Na2CO3 needed to precipitate 99% of Mg from 1 L of 0.1 M Mg(NO)3
Writing the reaction for when solid MgCO3 breaks into ions:
MgCO3 (s) ⇌ Mg2+aq) + CO32-(aq)
** Since it has a solubility product constant, we can consider MgCO3 as a solid.
We need to find 1% Mg2+ left since 99% are already precipitated, therefore the concentration of Mg2+ is:
What volume of 0.116 M sodium carbonate solution is required to precipitate 99% of the Mg from 1.00 L of 0.100 M magnesium nitrate solution?
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