When adding more sucrose to a 0.7 M sucrose solution, why does it not dissolve as readily as it did at a lower molarity? a) the ions in the solution interact with the sugar and that interferes with its solubility
b) the solubility of the solute depends on wether the solute has hydroxyl functional groups or not
c) the solute molecules adhere to the polar regions of the water molecules so there is no room for more sucrose molecules
d) hydrogen bonds in the water molecules change the electrical charge of the sugar molecule, which prevents it from dissolving further in the water

c) the solute molecules adhere to the polar regions of the water molecules so there is no room for more sucrose molecules

Explanation:

A solution contains a solvent (water in this case) and a solute (sucrose in this case). A solution can either be saturated or unsaturated depending on whether it can still dissolve a solute or not.

According to this question, the 0.7 M sucrose solution does not dissolve the sucrose (solute) any longer. This implies that the sucrose solution is getting SATURATED. The saturation of the sucrose solution occurs because the amount of solutes is equating the amount of solvent in the solution.

The solubility of a solution depends upon polarity. The solute molecules (sucrose) adhere to the polar regions of the water molecules (solvent). When this occurs to the point where no other sucrose molecule can adhere, the solution becomes SATURATED so there is no room for more sucrose molecules.