Calculate the solubility, in molL―1, of lead sulfate, PbSO4, in a 0.0185 M solution of sodium sulfate, Na2SO4 .
Ksp (PbSO4) = 1.6 x 10―8
I get 8 x 10^-9...but that is not right! Thanks!
2 answers
You need to write a balanced equation for this reaction and write an ice table. since you know ksp.. you can solve for the x value. and plug it back into your ice table. easy stuff.
If I am reading it correctly...
1.6E-8=(2x)^2 (.0185+x)
ignoring the +x (it is small)
x=1.6E-8/(4*.0185)
1.6E-8=(2x)^2 (.0185+x)
ignoring the +x (it is small)
x=1.6E-8/(4*.0185)
3 answers