Assume we have a solution that contains 0.050 mol/L of Ba2+ and 0.050 mol/L Mg2+

Question

Assume we have a solution that contains 0.050 mol/L of Ba2+ and 0.050 mol/L Mg2+. Calculate the concentration of Ba2+ left in solution at the point that Mg2+ just begins to precipitate. Assume the solution volume (and thus the ion concentration) do not change as we add carbonate ion. The Ksp of barium carbonate is given in table 1 of the experiment 212 handout (8.1x10^-9). The Ksp of magnesium carbonate is 4.0x10-5. write balanced chemical equations and Ksp expressions for each of the salts as part of your solution

Explanation / Answer

let the concentration of Co3 2- required be x.

x*0.05=4*10^-5

so x=8*10^-4 M

so,

[Ba2+]*8*10^-4=8.1*10^-9

or [Ba2+]=1.0125*10^-5 M

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