Will a precipitate form if a 0.1 M solution of Na2SO4 is added to a solution that is 0.0005M in barium ions?

Question

Ksp BaSO4= 1.1x10^-10. Please show work...

Answer 1

BaSO4 <=> Ba(+2) + SO4(-2)

So Ksp=[Ba(+2)][SO4(-2)]

You will have precipitate formation if
[Ba(+2)][SO4(-2)]>Ksp

Na2SO4 -> 2Na(+) + SO4(-2)
so from the stoichiometry [SO4(-2)]=0.1

Therefore

[Ba(+2)][SO4(-2)] = 5*(10^-4)*0.1= 5*10^-5>Ksp

which means you will have precipitate formation.

Answer 2

yes. The Ksp for barium sulfate is 1.1x10^-10.

You have 5x10^-4 barium concentration, so you will exceed the solubility.

Here is a link to my data source

http://bilbo.chm.uri.edu/CHM112/lectures/BaSO4.htm