The exothermic dissolution of Mg(OH)X2 in water is represented by the equation above. The Ksp of Mg(OH)X2
is 1.8×10−11. Which of the following changes will increase the solubility of Mg(OH)X2 in an aqueous solution?
Approach
The Ksp of magnesium hydroxide is low. The reactants are favored in the reaction. To increase the solubility,
we need Mg(OH)X2 to dissociate. In other words, we want the equilibrium position to shift to the right.
Decreasing the pH involves adding acid. The hydroxide would be consumed through neutralization with the acid. Since products are being removed, the equilibrium position will shift to the right.
Increasing the pH would likely have an opposite effect and would shift the equilibrium position to the left, decreasing solubility.
NHX3, a weak base, would react with water and produce some hydroxide ions, resulting in a shift in equilibrium position to the left.
Adding Mg(NOX3)X2 would result in increased MgX2+, shifting the equilibrium position to the left.