How to Calculate Moles

••• eprouvettes image by Pascal Péchard from

Often in chemistry a solute is added to a solution. One of the most frequent tasks is to determine the concentration of that solute in the solution. This calculation is referred to as the molarity of the solution.

    Learn the equation: M=moles solute/liters solution. "M" represents the molarity, or concentration, of the solute in the solution.

    Convert grams of solute into moles of solute. You will need a periodic table in order to do this. To calculate the moles of solute you will need to divide the weight in grams you have added to the solution by the weight in grams of one mole. For this example, use sodium chloride: NaCl. The weight of one mole, rounded to the nearest tenth, is the atomic weight of sodium, 23g, plus the atomic weight of chorine, 35.5. Therefore one mole of solute would be 58.5g. Assuming for this example that there are 24g of NaCl, the conversion would be: 24/58.5=.41 moles of solute.

    Measure the amount of solution. The solution will be in liters before the final calculation but can be taken in milliliters. In this example, the amount of solution will be 650 mL. Converting this into liters: 0.65 L.

    Calculate the molarity of the solute in the solution: M=moles solute/liters solution. Using the example given: 0.41 moles solute/0.65 liters solution=.63 M--rounded to the nearest hundredth.

    Things You'll Need

    • Calculator
    • Periodic table


    • Keep in mind that molarity simply stands for moles of solute per liter of solution. Round atomic weights according to the specifications you are using.


    • Remember to translate milliliters to liters of solution.

About the Author

This article was written by a professional writer, copy edited and fact checked through a multi-point auditing system, in efforts to ensure our readers only receive the best information. To submit your questions or ideas, or to simply learn more, see our about us page: link below.

Photo Credits

  • eprouvettes image by Pascal Péchard from