Are the Two Statements About Ksp and Solubility Consistent?

[mooncrater]

Homework Statement

I read this line in my textbook:
"$PbS,CdS$ are precipated in dilute solution only due to higher $K_{sp}$"
And I googled about the relation between solubility and $K_{sp}$ and I found that:
"More is the $K_{sp}$ of a salt more it is soluble in a solution(I think water)"
So are the two statements in accordance to each other?If no then which one is wrong?

Homework Equations

The Attempt at a Solution

I am confused. I do think that one of these lines should be wrong and I would prefer the first one. But I am not sure about it because of which I have asked it here.

 

[x86]

Like any equilibrium constant, for the reaction aA + bB <===> cC + dD, K = [C]^c[D]^d/ ([A]^a^b).

Therefore, if your reaction is solid <===> solute then a higher Ksp will mean that more solute will dissolve in the solution. (Note that in the equilibrium constant you don't include the solids, so in this case Ksp = [solute])

I'm also confused about the first statement, but I know the above is true

 

[mooncrater]

Therefore, if your reaction is solid <===> solute then a higher Ksp will mean that more solute will dissolve in the solution.

So, using your statement in this line

"$PbS,CdS$ are precipated in dilute solution only due to $higher$ $K_{sp}$"

I may say that instead of $higher$ it should be $lower$.
What do you think?

 

[x86]

Yes, that makes sense. If Ksp is really low then there will be very low solubility.

 

[James Pelezo]

You may already know this, but be careful using Ksp as an indication of solubility. You can use Ksp to compare solubility only if the salt ionization ratios are the same. If not, you'll need to use the solubility equation for the ionization ratio. Here's an example where you can get into trouble... Consider single salt saturated aqueous solutions of MgCO₃ (Ksp = 1 x 10^-5) and BaF₂ (Ksp = 1 x 10^-6). Is MgCO₃ more soluble than BaF₂ because it has a larger Ksp-value? NO!

Solubility of MgCO₃ = (Ksp)^1/2 = (1x10^-5)^1/2 = 0.0032M b/c MgCO₃ has a 1:1 ionization ratio

Solubility of BaF₂ = (Ksp/4)^1/3 = (1 x 10^-6/4)^1/3 = 0.0063M b/c BaF₂ has a 1:2 ionization ratio

Solubility of BaF₂ > Solubility of MgCO₃ ... Just an FYI...
Have a good day.