College Chemistry : Liquids and Solutions
Study concepts, example questions & explanations for College Chemistry
All College Chemistry Resources
Example Questions
Example Question #32 : Solutions, States Of Matter, And Thermochemistry
Consider an aqueous solution that is saturated with 
The magnesium concentration would need to be decreased by a factor of
The magnesium concentration would need to be decreased by a factor of
The magnesium concentration would need to be increased by a factor of
The magnesium concentration would need to be increased by a factor of
The magnesium concentration would need to be increased by a factor of
For this question, we're told that an aqueous solution of magnesium fluoride is saturated. We're then told that the fluoride concentration in the solution is reduced by a factor of two, and we're asked to find how the magnesium concentration would need to change in order to keep the solution saturated.
First, it's important to recall what saturation means. Some substances cannot dissolve in water, whereas others can dissolve readily. In other words, different substances will dissolve to differing degrees in water. The dissolution of a compound in a solvent such as water can be represented by an equilibrium expression. When there is a relatively small amount of solute added, the solution is said to be unsaturated. This means that all of the added solute will dissolve. As more and more solute is added to the water, there will eventually reach a point at which so much solute is present that it can no longer dissolve. When this happens, any additional solute will not dissolve and will instead form a precipitate in the solution. This condition is referred to as supersaturated. Saturation is the "sweet spot" so to speak; it is the point in between unsaturated and supersaturated where the maximum amount of solute has been added to the solution where all of the solute can be in the dissolved form. In other words, saturation refers to the maximum concentration of added solute where there is NO precipitation.
In order to set up an equilibrium expression, we can first write out the reaction in which magnesium fluoride dissolves.
Knowing the reaction, we can now write an equilibrium expression. Remember that pure solids and liquids don't appear in equilibrium expressions! Thus, this expression will only contain the products of the above reaction.
In the above expression, 
Since the equilibrium expression tells us the concentrations necessary to have a saturated solution, we can determine how a change in fluoride concentration would affect the equilibrium. Then, we can determine what changes to magnesium are needed.
If the fluoride concentration were to be cut in half, the 
Certified Tutor
Certified Tutor
All College Chemistry Resources
