How to Find the Mass Percent of an Element or Compound

PDF download Download Article
Learn how to use the mass percent chemical formula
PDF download Download Article

In chemistry, mass percent tells you the percentage of each element that makes up a chemical compound. Finding the mass percent requires the molar mass of the elements in the compound in grams/mole or the number of grams used to make a solution. But finding these variables and the mass percent isn’t as difficult as it may seem! In this article, we’ll walk you through the process of solving for mass percent when given and not given the masses of a compound.

What is the formula for percent by mass?

The formula for percent by mass of a solution is mass percent = (mass of chemical/total mass of compound) x 100 or (%w/w) x 100 .

Section 1 of 2:

Solving for Mass Percent When Given Masses

PDF download Download Article
  1. The basic formula for mass percent of a compound is mass percent = (mass of chemical/total mass of compound) x 100 (also written as (%w/w) x 100 ) . The 100 at the end of the formula turns the value into a percentage. [1]
    • Make sure both values are in grams so they cancel each other out once you solve the equation. If they’re not, convert the values to grams (you can use an online converter tool for help).
    • The mass of the chemical you’re interested in is the mass given in the problem. If the mass isn’t given, refer to the following section about solving for mass percent when the mass is not given.
    • "w/w" refers to weight/weight, also known as mass/mass. It's used in chemistry to express the concentration of a solution or mixture.
  2. When you know the masses of all the elements or compounds being added together, you simply need to add them together to calculate the total mass of the final compound or solution. This will be the denominator in the mass percent calculation. [2]
    • Example 1: What is the percent mass of 5 g of sodium hydroxide dissolved in 100 g of water?
      • The total mass of the compound is the amount of sodium hydroxide plus the amount of water: 100 g + 5 g for a total mass of 105 g .
    • Example 2: What masses of sodium chloride and water are needed to make 175 g of a 15% solution?
      • In this example, you are given the total mass and the percentage you want, but are asked to find the amount of solute to add to the solution. The total mass is 175 g .
    Advertisement
  3. When asked to find the “mass percent,” you’re being asked to find the mass of a particular chemical (the chemical-in-question) as a percentage of the total mass of all elements. Write down the mass of chemical-in-question. This mass will be the numerator in your mass percent calculation. [3]
    • Example 1: The mass of the chemical-in-question is 5 g of sodium hydroxide.
    • Example 2: For this example, the mass of the chemical-in-question is the unknown you’re trying to calculate.
  4. Once you have determined the values for each variable, plug them into the equation: mass percent = (mass of chemical/total mass of compound) x 100. [4]
    • Example 1: (5 g/105 g) x 100.
    • Example 2: We want to rearrange the mass percent equation to solve for the unknown mass of the chemical. So, the new equation would be mass of the chemical = (mass percent x total mass of the compound)/100 , which would be (15 x 175)/100.
  5. Now that the equation is filled in, simply plug the information into your calculator to find the mass percent. Divide the mass of the chemical by the total mass of the compound and multiply by 100. This gives you the mass percent of the chemical. [5]
    • Example 1: (5/105) x 100 = 0.04761 x 100 = 4.761%. Thus, the mass percent of 5 g of sodium hydroxide dissolved in 100 g of water is 4.761% .
    • Example 2: (15 x 175)/100 = (2625)/100 = 26.25 g sodium chloride.
      • The amount of water to be added is simply the total mass minus the mass of the chemical: 175 – 26.25 = 148.75 g water.
    6. Advertisement
Section 2 of 2:

Solving for Percent Mass When Not Given Masses

PDF download Download Article
  1. The basic formula for mass percent of a compound is: mass percent = (molar mass of element/total molecular mass of compound) x 100. The molar mass of a compound is the amount of mass for one mole of an element, while the molecular mass is the amount of mass for one mole of the entire compound. [6] Multiplying by 100 at the end expresses the value as a percentage. [7]
    • Both values have units of grams per mole (g/mol). This means the units will cancel each other out when you solve the equation.
    • When you aren’t given masses, you can find the mass percent of an element within a compound using molar mass.
    • For this tutorial, we’ll be using two example problems:
      • Example 1: Find the mass percent of Hydrogen in a water molecule.
      • Example 2: Find the mass percent of carbon in a glucose molecule.
  2. Write out the chemical formulas for each compound. If you are not given the chemical formulas for each compound, write them out. If you are given the chemical formulas, you can skip this step. [8]
    • Example 1: Write out the chemical formula for water, H2O.
    • Example 2: Write out the chemical formula for glucose, C6H12O6.
    • If you’re not sure what the chemical formulas are for the compounds, don’t hesitate to look them up!
  3. Look up the molecular weight of each element in your chemical formulas on the periodic table . The mass of an element can usually be found underneath the chemical symbol. Write down the masses of every element in the compound. [9]
    • Example 1: Look up the molecular weight of Oxygen, 15.9994; and the molecular weight of Hydrogen, 1.0079. [10]
    • Example 2: Look up the molecular weight of Carbon, 12.0107; Oxygen, 15.9994; and Hydrogen, 1.0079.
  4. Identify how many moles (mole ratio) of each element are in your chemical compounds. The mole ratio is given by the subscript number in the compound (the number of atoms in the compound, indicated by the small number beside the element). Multiply the molecular mass of each element by this mole ratio. [11]
    • Example 1: Hydrogen has a subscript of 2 while oxygen has a subscript of 1. Therefore, multiply the molecular mass of Hydrogen by 2, 1.00794 X 2 = 2.01588; and leave the molecular mass of Oxygen as is, 15.9994 (multiplied by one).
    • Example 2: Carbon has a subscript of 6, hydrogen 12, and oxygen 6. Multiplying each element by its subscript gives you:
      • Carbon (12.0107*6) = 72.0642
      • Hydrogen (1.00794*12) = 12.09528
      • Oxygen (15.9994*6) = 95.9964
  5. Using the masses calculated using the mole ratio, you can calculate the total mass of the compound. This number will be the denominator of the mass percent equation. [12]
    • Example 1: Add 2.01588 g/mol (the mass of two moles of Hydrogen atoms) with 15.9994 g/mol (the mass of a single mole of Oxygen atoms) and get 18.01528 g/mol .
    • Example 2: Add all of the calculated molar masses together: Carbon + Hydrogen + Oxygen = 72.0642 + 12.09528 + 95.9964 = 180.156 g/mol .
  6. When asked to find the “mass percent,” you’re being asked to find the mass of a particular element in a compound, as a percentage of the total mass of all elements. The mass is the mass calculated using the mole ratio. This number will become the numerator in the mass percent equation. [13]
    • Example 1: The mass of hydrogen in the compound is 2.01588 g/mol (the mass of two moles of hydrogen atoms).
    • Example 2: The mass of carbon in the compound is 72.0642 g/mol (the mass of six moles of carbon atoms).
  7. Once you have determined the values for each variable, plug them into the equation mass percent = (molar mass of the element/total molecular mass of compound) x 100. [14]
    • Example 1: (2.01588/18.01528) x 100.
    • Example 2: (72.0642/180.156) x 100.
  8. Now that the equation is filled in, simply solve to calculate the mass percent. Divide the mass of the element by the total mass of the compound and multiply by 100. This gives you the mass percent of the element. [15]
    • Example 1: mass percent = (2.01588/18.01528) x 100 = 0.11189 x 100 = 11.18%. Thus, the mass percent of Hydrogen atoms in a water molecule is 11.18% .
    • Example 2: mass percent = (molar mass of the element/total molecular mass of compound) x 100 = (72.0642/180.156) x 100 = 0.4000 x 100 = 40.00%. Thus, the mass percent of carbon atoms in a molecule of glucose is 40.00% .
    9. Advertisement

Expert Q&A

Search
Add New Question
  • Question
    If a solution is prepared by mixing 50 ml of vinegar into 300 ml of solution, what is the percentage by volume?
    Bess Ruff, MA
    Environmental Scientist
    Bess Ruff is a Scientist based in Sydney, Australia. Her research interests and previous scientific experience include environmental science, geography, biotechnology, mariculture, marine spatial planning, stakeholder engagement, and spatial ecology. She is a Postdoctoral Researcher at University of Sydney and a Project Manager at Offshore Biotechnologies. Prior to her work in Sydney, Bess was a Postdoctoral Researcher for over 2 years at Florida State University. She received a PhD in Geography from Florida State University, with a doctoral dissertation entitled "Culturing a Sustainable Seafood Future: How Governance, Economics, and Society Are Driving the Global Marine Aquaculture Industry”. She received her MA in Environmental Science and Management from the University of California, Santa Barbara in 2016. She has conducted survey work for marine spatial planning projects in the Caribbean and provided research support as a graduate fellow for the Sustainable Fisheries Group.
    Bess Ruff, MA
    Environmental Scientist
    Expert Answer
    You can use the same formula to calculate percentage by volume as you use to calculate percentage by mass. First, calculate the total volume of the solution. Then, divide the volume of the vinegar by the total volume of the solution. Finally, multiply by 100 to get the percentage of vinegar in the total solution. 50 ml + 300 ml = 350 ml for the total volume of the solution. Vinegar percentage = 50/350 = 14 x 100 = 14% vinegar.
    Thanks! We're glad this was helpful.
    Thank you for your feedback.
    If wikiHow has helped you, please consider a small contribution to support us in helping more readers like you. We’re committed to providing the world with free how-to resources, and even $1 helps us in our mission. Support wikiHow
    Yes No
    Not Helpful 11 Helpful 12
  • Question
    How do I determine the mass percentage of salt (NaCl) in a water-salt solution?
    Community Answer
    In order to calculate the mass percentage, you must know how much salt was added to a certain amount of water. For instance, if you added 50 grams of NaCl to 1000 grams of water, that mass percent would be 50/1050 x 100 = 4.76%.
    Thanks! We're glad this was helpful.
    Thank you for your feedback.
    If wikiHow has helped you, please consider a small contribution to support us in helping more readers like you. We’re committed to providing the world with free how-to resources, and even $1 helps us in our mission. Support wikiHow
    Yes No
    Not Helpful 13 Helpful 25
  • Question
    How would I calculate the mass percent of a MgBr2 solution that contains 5.80g of MgBr2 in 45.0g of solution?
    Community Answer
    Similar to the example given above, simply plug the numbers into the mass percent equation. Calculate total mass of the compound: 5.8 + 45 = 50.8. Divide mass of the chemical by mass of the compound and multiply by 100: 5.8/50.8 x 100 = 11.42%.
    Thanks! We're glad this was helpful.
    Thank you for your feedback.
    If wikiHow has helped you, please consider a small contribution to support us in helping more readers like you. We’re committed to providing the world with free how-to resources, and even $1 helps us in our mission. Support wikiHow
    Yes No
    Not Helpful 17 Helpful 14
See more answers
Ask a Question
200 characters left
Include your email address to get a message when this question is answered.
Submit
      Advertisement

      Video

      Tips

      Submit a Tip
      All tip submissions are carefully reviewed before being published
      Name
      Please provide your name and last initial
      Submit
      Thanks for submitting a tip for review!

      You Might Also Like

      How to
      Calculate the Concentration of a Solution
      How to
      Calculate Molarity: Easy Step-by-Step Guide
      How to
      Calculate Vapor Pressure
      How to
      Calculate Molar Mass
      How to
      Calculate Electronegativity
      How to
      Calculate Atomic Mass
      How to
      Calculate Average Atomic Mass (and Use the Result)
      How to
      Calculate the Enthalpy of a Chemical Reaction
      How to
      Calculate Theoretical Yield
      How to
      Calculate Molar Absorptivity
      Enthalpy of Air: Calculating It With & Without Steam Tables
      How to
      Calculate Molecular Weight
      How to
      Calculate Percent Yield in Chemistry
      How to
      Calculate Bond Order in Chemistry
      Advertisement

      References

      1. ↑ https://chem-textbook.ucalgary.ca/version2/review-of-background-topics/measurements-and-data/measurements-in-chemistry/other-units-for-solution-concentrations/
      2. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map:_Introductory_Chemistry_(Tro)/06:_Chemical_Composition/6.06:_Mass_Percent_Composition_of_Compounds
      3. ↑ https://www.geeksforgeeks.org/chemistry/mass-percent-formula/
      4. ↑ https://www.geeksforgeeks.org/chemistry/mass-percent-formula/
      5. ↑ https://www.geeksforgeeks.org/chemistry/mass-percent-formula/
      6. ↑ https://www.webqc.org/mmcalc.php
      7. ↑ https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Quantifying_Nature/Density_and_Percent_Compositions
      8. ↑ https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT:_CHE_201_-_General_Chemistry_I_(Anthony_and_Clark)/Unit_4:_Quantifying_Chemicals/4.2:_Formula_Mass,_Percent_Composition,_and_the_Mole
      9. ↑ https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT:_CHE_201_-_General_Chemistry_I_(Anthony_and_Clark)/Unit_4:_Quantifying_Chemicals/4.2:_Formula_Mass,_Percent_Composition,_and_the_Mole
      1. ↑ http://sciencenotes.org/wp-content/uploads/2015/01/Periodic-Table-Color.png
      2. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/12:_Stoichiometry/12.02:_Mole_Ratios
      3. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map:_Introductory_Chemistry_(Tro)/06:_Chemical_Composition/6.07:_Mass_Percent_Composition_from_a_Chemical_Formula
      4. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map:_Introductory_Chemistry_(Tro)/06:_Chemical_Composition/6.07:_Mass_Percent_Composition_from_a_Chemical_Formula
      5. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map:_Introductory_Chemistry_(Tro)/13:_Solutions/13.05:_Specifying_Solution_Concentration-_Mass_Percent
      6. ↑ https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map:_Introductory_Chemistry_(Tro)/06:_Chemical_Composition/6.07:_Mass_Percent_Composition_from_a_Chemical_Formula

      About This Article

      Article Summary X

      To calculate mass percent, start by identifying the mass of the chemical-in-question. Next, figure out the total mass of the compound by adding together the masses of all of the chemicals used to make that compound. Then, divide the mass of the chemical by the total mass of compound. Multiply the answer you get by 100 to calculate the percentage! To learn how to calculate mass percent when you don't know any of the masses involved, read on!

      Did this summary help you?
      In other languages
      Thanks to all authors for creating a page that has been read 670,313 times.

      Reader Success Stories

      • Sylvester Pyne

        Apr 11, 2018

        "This article is very helpful. i didn't know how to fine mass percent by myself. After going through this ..." more
      More reader stories Hide reader stories
      Share your story

      Did this article help you?

      Advertisement