# Problem: The solubility of lead(II) bromide, PbBr2, in water is 4.34 g/L. In an aqueous solution an equilibrium exists between the dissolved ions and the solid salt.PbBr2(s) ⇋ Pb2+(aq) + 2 Br -1 (aq)a) write the solubility product expression for this equation. b) calculate the molar concentration and the Ksp ( solubility product constant) for lead(II) bromide.

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The solubility of lead(II) bromide, PbBr2, in water is 4.34 g/L. In an aqueous solution an equilibrium exists between the dissolved ions and the solid salt.

PbBr2(s) ⇋ Pb2+(aq) + 2 Br -1 (aq)

a) write the solubility product expression for this equation.

b) calculate the molar concentration and the Ksp ( solubility product constant) for lead(II) bromide.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp Or if you need more Ksp practice, you can also practice Ksp practice problems .

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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.