# Problem: What is the molarity of the solution 0.0433 m LiF, if the density is 1.10g/mL?

###### FREE Expert Solution
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###### FREE Expert Solution

We’re being asked to calculate the molarity (M) of a solution of LiF

Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:

We’re given the molality of the solution, 0.0433 m LiF

Recall that the molality (m) is the ratio of the moles of solute and the mass of solvent (in kg):

This means the solution of LiF is:

The steps we need to do for this solution are:

Step 1: Calculate the mass of LiF

Step 2: Calculate the mass of the solution.

Step 3: Convert the mass of the solution to volume (in L).

Step 4: Calculate the molarity of the solution.

99% (297 ratings)
###### Problem Details

What is the molarity of the solution 0.0433 m LiF, if the density is 1.10g/mL?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calculate Molarity concept. You can view video lessons to learn Calculate Molarity. Or if you need more Calculate Molarity practice, you can also practice Calculate Molarity practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofWhat is the molarity of the solution 0.0433 m LiF, if the de...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 6 minutes and 29 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Jiang's class at UHD.