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Calculating Molar Mass

Describes calculations for determining molar mass from changes in boiling or freezing point.

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Calculating Molar Mass

It is possible to calculate quantities like molecular weight from freezing point depression

Credit: Courtesy of the US Marine Corps
Source: http://commons.wikimedia.org/wiki/File:USMC-110329-M-PE262-004.jpg
License: CC BY-NC 3.0

How much antifreeze is needed?

We know that we can put antifreeze into a radiator and keep an engine from freezing up. By knowing how cold it will get and how much water is in the radiator, we can determine how much antifreeze to add to achieve our desired freezing point depression. We can do this because we know what the antifreeze is. Can we switch things around and get some information about the properties of the antifreeze (such as its molecular weight) from the freezing point decrease? It turns out that we can do this fairly easily and accurately.

Changes in melting point and boiling point can be used to determine molecular weight

Credit: Laura Guerin
Source: CK-12 Foundation
License: CC BY-NC 3.0

Changes in temperature.[Figure2]

Calculating Molar Mass

In the laboratory, freezing point or boiling point data can be used to determine the molar mass of an unknown solute. Since we know the relationship between a decrease in freezing point and the concentration of solute, if we dissolve a known mass of our unknown solute into a known amount of solvent, we can calculate the molar mass of the solute. The \begin{align*}K_f\end{align*}Kf or \begin{align*}K_b\end{align*}Kb of the solvent must be known. We also need to know if the solute is an electrolyte or a nonelectrolyte. If the solvent is an electrolyte, you would need to know the number of ions is produced when it dissociates.

Sample Problem: Molar Mass from Freezing Point Depression

38.7 g of a nonelectrolyte is dissolved into 218 g of water. The freezing point of the solution is measured to be -5.53°C. Calculate the molar mass of the solute.

Step 1: List the known quantities and plan the problem.


  • \begin{align*}\Delta T_f=-5.53^\circ \ \text{C}\end{align*}ΔTf=5.53 C
  • mass H2O 218 g = 0.218 kg
  • mass solute = 38.7 g
  • \begin{align*}K_f(\text{H}_2\text{O})=-1.86^\circ \ \text{C}/m\end{align*}Kf(H2O)=1.86 C/m


  • molar mass solute = ? g/mol

Use the freeing point depression \begin{align*}(\Delta T_f)\end{align*}(ΔTf) to calculate the molality of the solution. Then use the molality equation to calculate the moles of solute. Then divide the grams of solute by the moles to determine the molar mass.

Step 2: Solve.

\begin{align*}m=\frac{\Delta T_f}{K_f} &=\frac{-5.53^\circ \text{C}}{-1.86^\circ \text{C}/m}=2.97 \ m\\ \text{mol solute} &= m \times \text{kg H}_2\text{O}=2.97 \ m \times 0.218 \text{ kg} = 0.648 \text{ mol}\\ \frac{38.7 \text{ g}}{0.648 \text{ mol}} &= 59.7 \text{ g/mol}\end{align*}m=ΔTfKfmol solute38.7 g0.648 mol=5.53C1.86C/m=2.97 m=m×kg H2O=2.97 m×0.218 kg=0.648 mol=59.7 g/mol

Step 3: Think about your result.

The molar mass of the unknown solute is 59.7 g/mol. Knowing the molar mass is an important step in determining the identity of an unknown. A similar problem could be done with the change in boiling point.



  1. What do we need to know about the solvent to use this technique?
  2. Will it work with ionizable compounds?
  3. Can we use boiling point elevation to determine molar mass?

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Image Attributions

  1. [1]^ Credit: Courtesy of the US Marine Corps; Source: http://commons.wikimedia.org/wiki/File:USMC-110329-M-PE262-004.jpg; License: CC BY-NC 3.0
  2. [2]^ Credit: Laura Guerin; Source: CK-12 Foundation; License: CC BY-NC 3.0

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