# Problem: Given that the ΔG f ° for Pb2+(aq) and Cl −(aq) is −24.3 kJ/mole and −131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).

###### FREE Expert Solution

We’re being asked to determine thedetermine the solubility product, Ksp, for PbCl2(s).

PbCl2(s)  Pb2+(aq) + 2 Cl (aq)

Recall that ΔG˚rxn and K are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

We can use the following equation to solve for ΔG˚rxn:

Step 1: We can easily solve for ΔG˚rxn

Given:

ΔG f ° for Pb2+(aq) =  −24.3 kJ/mol

ΔG f ° for Cl (aq) = −131.2 kJ/mol

ΔG f ° for Cl (aq) = −314.2 kJ/mol

ΔG˚rxn = 27.5 kJ

90% (426 ratings) ###### Problem Details

Given that the ΔG f ° for Pb2+(aq) and Cl (aq) is −24.3 kJ/mole and −131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).

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