Question

A beaker contains an aqueous solution of sodium acetate (NaC2H3O2) of unknown concentration. A few crystals of sodium acetate are added to the beaker. They sink to the bottom of the beaker and remain there unchanged even after further mixing. What can you conclude about the level of saturation of the solution?

a. The solution is supersaturated.
b. The solution is saturated.
c. The solution is unsaturated.
d. It is not possible to determine the level of saturation because you do not know the concentration of the solution.

Answer 1

Answer:

The solution is supersaturated.

Explanation:

A supersaturated solution contains more solute than it can normally hold at a particular temperature. Hence more solute does not dissolve in the solution. Is more sodium acetate is added and the newly added crystals fail to dissolve, we can safely conclude that the solution has become supersaturated hence cannot dissolve anymore solute at that temperature.

Answer 2

Answer:

The answer is: b. The solution is saturated.

Explanation:

If the beaker contains an aqueous solution of sodium acetate with an unknown concentration, the solubility is not known. If a few crystals of sodium acetate are added to the glass. If these crystals sink and remain unchanged and if after mixing, this means that these crystals are not soluble in water, since the solution is saturated. It is not a supersaturated solution because there is no crystal formation before adding them.