Give the Ksp expression for magnesium hydroxide, Mg(OH)2.

Ksp = [Mg2+][OH-]2


The concentration of the solid phase remains constant so [Mg(OH)2(s)] is combined with the value of Kc, allowing it to be removed from the Ksp expression.

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What are the typical units for Ksp?

The units for Ksp depend on the specific reaction but often have units such as mol2 dm-6 or mol3 dm-9, depending on the number of ions involved in the equilibrium expression.

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What is the relationship between the ksp value of a salt and its solubility?

The smaller the Ksp value, the lower the solubility of the salt.

Conversely, the larger the Ksp value, the higher the solubility of the salt.

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How can you apply the concept of solubility product to determine the likelihood of a precipitate forming when solutions of barium chloride (BaCl2) and sodium carbonate (Na2CO3) are combined?

Compare the ion product, [Ba2+][CO32-], to the solubility product, Ksp, for barium carbonate, BaCO₃.

If the ion product is greater than Ksp, a precipitate of BaCO3 will form.


If [Ba2+][CO32-] < Ksp, no precipitate will form.

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What is the common ion effect?

The common ion effect is a phenomenon where the solubility of an ionic compound is reduced when it is dissolved in a solution that already contains one of its constituent ions. This decrease in solubility and often leads to the precipitation of the compound.

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Predict and explain whether barium sulfate (BaSO4) exhibits a higher solubility in water or in sulfuric acid (H2SO4).

Barium sulfate (BaSO4) exhibits higher solubility in water.


This is due to the common ion effect: sulfuric acid (H2SO4) provides SO42- ions which are also present in the barium sulfate compound. As a result, the solubility of barium sulfate decreases in the presence of sulfate ions, leading to lower solubility in sulfuric acid.

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