Problem: The Ksp of PbSO4 is 1.3 x 10-8. Calculate the solubility (in mol/L) of PbSO4 in a 0.0037 M solution of Na2SO4.

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The Ksp of PbSO4 is 1.3 x 10-8. Calculate the solubility (in mol/L) of PbSO4 in a 0.0037 M solution of Na2SO4.


For this problem, we’re being asked to calculate the solubility (in g/L) of PbSO4(s) in 0.0037 M Na2SO4(aq). Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of PbSO4 and Na2SO4 in water are as follows:


PbSO4(s)  Ca2+(aq) + SO42–(aq)

Na2SO4(s)  2 Na+(aq) + SO42–(aq)


Notice that there is a common ion present, SO42–. The common ion effect states that the solubility of a salt is lower in the presence of a common ion.


We can construct an ICE table for the dissociation of PbSO4. Remember that solids are ignored in the ICE table.




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Problem Details

The Ksp of PbSO4 is 1.3 x 10-8. Calculate the solubility (in mol/L) of PbSO4 in a 0.0037 M solution of Na2SO4.

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