# Question #5de6f

##### 1 Answer

The freezing point of the solution will be equal to

**SIDE NOTE** *The cryoscopic constant*, *for benzene is actually equal to* *not* *so I solved the problem using the correct value.*

*If you want, you can redo the calculations with the value you have/were given.*

So, you know that you're dealing with a solution containing naphthalene, your solute, and benzene, your solvent. The first thing you need to do is determine the mass of benzene by using its volume and density

The equation for freezing-point depression looks like this

**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'rea dealing with molecular compounds which do not dissociate.

Use naphthalene's molar mass to determine how many moles you're adding to the solution

The solution's molality will thus be

Now you have all you need to solve for

This means that the freezing point of the solution is