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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!!

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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!!

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Hootenanny

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egg said:assuming activity of both ions is 1.0

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

~H

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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 thats been causing us grief!

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Hootenanny

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egg said:MgCO3 <=> Mg^2+ & CO3^2-

Yeah, this is correct. You are also correct with your K

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

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 [itex]Mg^{2+}[/itex] and [itex]CO_{3}^{2-}[/itex] will be equal, so we can re-write the above K

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

Do you follow this?

As [itex]MgCO_{3}[/itex] 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;

[tex]K_{sp} = [Mg^{2+}]^{2}[/tex]

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

~H

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SQRT Ksp=[Mg^2+] or SQRT10^-7.5 in which case the concentration of the ions will be 10^-3.75 ???????

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Hootenanny

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~H

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Thanks again!

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Hootenanny

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egg said:

Thanks again!

O yeah, didn't spot that No problem.

~H

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