Brian has the correct answer.
I'd like to add, however, that in the most general sense, we don't have to take a molar to mean a mole of solute per liter of solution. I've actually seen it used to mean "a mole of stuff per liter of space" for particular values of stuff.
Since the above sentence isn't exactly self-explanatory, let's take a look at a few examples.
Example 1: Water
At 4 °C, water has a density of 1000 g/L. Water has a molar mass of 18.02 g/mol. This means that in a liter of water at 4 °C, there are:
$$
1~\mathrm{L} \cdot 1000 ~\frac{\mathrm{g}}{\mathrm{L}} \cdot \frac{\mathrm{mol}}{18.02 \mathrm{g}} = 55.5 ~\mathrm{mol}
$$
Since there are 55.5 moles of water per liter of water, we can actually say that, at 4 °C, water is 55.5 molar. (See Example 3 on Wikipedia).
Note how this works: there is a certain amount of stuff (in this case, water) per amount of space (one liter, or one cubic decimeter). It doesn't matter that we don't have a solution--since there's stuff, and it takes up space, we can calculate a molarity for it.
Example 2: Ideal gas
An ideal gas takes up 22.4 L per mole, at STP. Taking the inverse of this, we find that it is 0.0446 moles/L. Therefore, the concentration of an idea gas at STP is 0.0446 molar.
Again, there's a certain amount of stuff (one mole of ideal gas) and a certain amount of space (22.4 liters), which allows us to calculate a molarity. The fact that the substance is pure doesn't stop us from writing a concentration for it.
A note of caution
This will NOT work for a measure of concentration like molality, because molality is defined by the amount of solvent used. It also won't usually work for things like normality, since you (usually) need to be in solution to generate ions.