Determine the molar solubility of PbSO4 in pure water. Ksp(PbSO4)= 1.82 x 10^-8.

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Question “Determine the molar solubility of PbSO4 in pure water. Ksp(PbSO4)= 1.82 x 10^-8.”

Answer

This problem uses the concept of solubility products

.

With the help of the expression for the solubility product, you can determine the solubility of a compound in pure water. Write the expression of the solubility product for each molecule, then calculate its solubility.

Solubility:

The maximum amount of a solvent that can dissolve a solute and form a solution is called its solubility. It refers to a chemical property that describes the ability of a substance to dissolve in a solvent.

Solubility product

The solubility product is basically the equilibrium between solids, and their respective ions in the solution. The solubility product is the amount of chemical compound that can be dissociated in water.

Exemple:

Below is the dissociation reaction for ionic solid

.

Below is the expression that corresponds to the solubility products.

The following is the balanced chemical equation for dissociation reaction of

:

Below is the expression that corresponds to the solubility products.

…… (1)

Consider the

as the molar solubility for the compound.

As shown below, the molar solubility

is calculated in pure water.

Substitute

for the value of

, and

for the molar solubility

within the equation

.

Ans:

is soluble in pure water at a molar level of

.

Conclusion

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