Calculate Mg2+ & CO3 2- Concentration in Magnesium Carbonate Solution

[egg]

Hi need a bit of help with a question!
the solubility product of magnesium carbonate is 10^ -7.5. Calculate the concentration of Mg2+ and CO3 2- expected in a saturated solution assuming activity of both ions is 1.0
cheers in advance!

 

[Hootenanny]

Can you start by writing an expression for the solubility product of MgCO_{3}? I'll give you a hint as well;

assuming activity of both ions is 1.0

What does this tell you about the relative concentrations of the Mg^{2+} and CO_{3}^{2-}. It may also helpful if you where to write out an equation of the dissociation of the ions.

~H

 

[egg]

cheers for the reply hootenanny,
i wrote the initial question in a bit of a hurry yesterday and forgot to say i have NO idead what to do with the info!
I know the relative concentrations of the ions will be equal and think that the dissociation is
MgCO3 <=> Mg^2+ & CO3^2-
Think the expression you mean is Ksp=(aMg^2+)(aCO3^2-)/aMgCO3 but not too sure where to go now, do i replace the ions and the Ksp with the values i know and rearrange to find activity of MgCO3? if i do this what does it tell me?
This is a question in a past exam paper we've been given and I'm sure we weren't shown how to do it! My exams next week and this is the only question that's been causing us grief!

 

[Hootenanny]

MgCO3 <=> Mg^2+ & CO3^2-

Yeah, this is correct. You are also correct with your K_sp expression;

K_{sp} = \frac{[Mg^{2+}][CO_{3}^{2-}]}{[MgCO_{3}]}

This is something of a trick question really. The square brackets mean concentration of whatever is inside the square brackets. Now, as you correctly said in your equation, once dissociated the concentration of Mg^{2+} and CO_{3}^{2-} will be equal, so we can re-write the above K_sp expression as;

K_{sp} = \frac{[Mg^{2+}]^2}{[MgCO_{3}]}

Do you follow this?

As MgCO_{3} is only slightly soluble, once the above equation has reached equilibrium adding further solid will not cause any equilibrium shift as the solution is saturated. Therefore, the equation becomes;K_{sp} = [Mg^{2+}]^{2}

Do you follow?

Now, consider how the concentration relates to the solubility product. What happens if the concentrations are greater, less than and equal to K_sp?~H

 

[egg]

think I'm starting to understand a bit better now! can i now rearrange Ksp=[Mg^2+]^2 to
SQRT Ksp=[Mg^2+] or SQRT10^-7.5 in which case the concentration of the ions will be 10^-3.75 ??

 

[Hootenanny]

Your logic is correct, but you might want to check your arithmetic, I get it to be 1.78x10^-4 mol.dm^-3

~H

 

[egg]

yeah that's it, 1.78x10^-4 is the same as 10^-3.75! Thank you loads for the help, just need to revise a ton of other stuff for this exam!
Thanks again!

 

[Hootenanny]

yeah that's it, 1.78x10^-4 is the same as 10^-3.75! Thank you loads for the help, just need to revise a ton of other stuff for this exam!
Thanks again!

O yeah, didn't spot that No problem.

~H