# Question #c6afd

##### 1 Answer

#### Answer:

The boiling point of that solution is

#### Explanation:

The equation for *boiling point elevation* looks like this

**ebullioscopic constant**;

In your case, you know that you have a solution that has a molality of **4 molal** an that the ebullioscopic constant of th solvent,

Since no mention of what your solute is, you can assume that the van't Hoff factor will be equal to **1**, which implies that the solute is not an electrolyte.

Plug in your values into the equation and solve for

This means that your solution's boiling point will be *higher* than the boling point of the pure solvent.

Therefore,

I will leave the answer rounded to two sig figs, despite the fact that you only gave one sig fig for the molality of the solution. Thus, the answer will be