1. Limited time only! Sign up for a free 30min personal tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

##K_{sp}## value and solubility

  1. Apr 30, 2015 #1
    1. The problem statement, all variables and given/known data
    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?

    2. Relevant equations

    3. 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.
  2. jcsd
  3. Apr 30, 2015 #2
    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
  4. Apr 30, 2015 #3
    So, using your statement in this line
    I may say that instead of ##higher## it should be ##lower##.
    What do you think?
  5. Apr 30, 2015 #4
    Yes, that makes sense. If Ksp is really low then there will be very low solubility.
  6. May 13, 2015 #5

    James Pelezo

    User Avatar
    Gold Member

    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.:wink:
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?
Draft saved Draft deleted

Similar Discussions: ##K_{sp}## value and solubility
  1. Constant of Solubility (Replies: 1)