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The cations Pb2+(aq) and Ba2+(aq) can be precipitated as almost insoluble sulfates. The Ksp values for...

The cations Pb2+(aq) and Ba2+(aq) can be precipitated as almost insoluble sulfates. The Ksp values for PbSO4(s) and BaSO4(s) are 2.5 × 10−8 and 1.1 × 10−10, respectively.

If you have a solution that is 0.010 mol L-1 in both Pb2+(aq) and Ba2+(aq) ions, and the concentration of SO42-(aq) ions is gradually increased, the less soluble salt will precipitate first.

What is the concentration of the cation (Pb2+ or Ba2+) that precipitates first remains in solution just before the second sulfate salt begins to precipitate?

The answer is 4.4x10^-5
Could you please show working out :)

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