# Question #918cb

##### 1 Answer

Start by writing the three equations that you're going to use to solve for the boiling point, freezing point, and vapor pressure of the solution.

*Freezing point depression*

**cryoscopic constant** - depends on the solvent;

**van't Hoff factor** - the number of ions per individual molecule of solute.

In your case, the van't Hoff factor will be equal to **1** because you're dealing with a non-electrolyte.

Plug in your values and solve for

The freezing point of the solution will be

*Boiling point elevation*

**ebullioscopic constant**;

Once again, plug in your values and solve for

The boiling point of the solution will be

*Vapor pressure lowering*

Since you didn't provide the mass of water used to make your solution, I'll assume that you have a **1-kg** sample.

The number of moles of water present in **1000 g** will be

The *mole fraction* of water, which is defined as the number of moles of water divided by the *total number of moles* in the solution, will be

**SIDE NOTE** *Since molality is defined as moles of solute per kg of solvent, the 1 kg of water implies that you have 0.750 moles of sucrose.*

Therefore, the vapor pressure of the solution will be