What is the concentration of the Mg2 ion in solution when [CO3-2] = 0.25M given that the

Ksp= 6.82 x 10-6 for the following reaction

MgCO3-------->Mg +. CO32-

Ksp = (Mg^2+)(CO3^2-)

Substitute 0.25M for CO3^2- and solve for Mg^2+

To find the concentration of the Mg2+ ion in solution, we can use the solubility product constant (Ksp) and the stoichiometry of the reaction.

The given equation for the reaction is:
MgCO3 ⇌ Mg2+ + CO32-

The Ksp expression for this reaction is:
Ksp = [Mg2+][CO32-]

We are given the value of Ksp (6.82 x 10^-6) and the concentration of the CO32- ion (0.25 M). We need to find the concentration of the Mg2+ ion.

To find the concentration of Mg2+, we rearrange the Ksp expression as follows:
[Mg2+] = Ksp / [CO32-]

Plugging in the given values:
[Mg2+] = (6.82 x 10^-6) / (0.25)

Simplifying:
[Mg2+] = 2.728 x 10^-5 M

Therefore, the concentration of the Mg2+ ion in solution when [CO32-] = 0.25 M is 2.728 x 10^-5 M.