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I'm stuck on this one aswell...

50.0 ml of a 0.0500 M solution of lead (II) nitrate is mixed with 40.0 ml of a 0.200 M solution of sodium iodate at 25°C. Calculate the Pb2+ and IO3- concentrations when the mixture comes to equilibrium. At this temperature the Ksp for lead (II) iodate is 2.6 x 10-13

Write the balanced equation
Pb(NO3)2 + 2NaIO3 ==> Pb(IO3)2 + 2NaNO3
This is a Ksp problem with a common ion. You will need to determine the mols of each reactant from M x L = mols, see how much of the product is formed and which reactant is in excess. After you understand how to do a and b of the previous post you will know how to do this one.

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