How To Calculate Mass Percent: 13 Steps (with Pictures) - WikiHow

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Terms of Use wikiHow is where trusted research and expert knowledge come together. Learn why people trust wikiHow How to Find the Mass Percent of an Element or Compound PDF download Download Article Learn how to use the mass percent chemical formula Co-authored by Ronitte Libedinsky, MS and Aly Rusciano

Last Updated: August 8, 2025 Fact Checked

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  • Solving for Mass Percent When Given Masses
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  • When Not Given Masses
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This article was co-authored by Ronitte Libedinsky, MS and by wikiHow staff writer, Aly Rusciano. Ronitte Libedinsky is an Academic Tutor and the Founder of Brighter Minds SF, a San Francisco, California based company that provides one-on-one and small group tutoring. Specializing in tutoring mathematics (pre-algebra, algebra I/II, geometry, pre-calculus, calculus) and science (chemistry, biology), Ronitte has over 10 years of experience tutoring to middle school, high school, and college students. She also tutors in SSAT, Terra Nova, HSPT, SAT, and ACT test prep. Ronitte holds a BS in Chemistry from the University of California, Berkeley, and an MS in Chemistry from Tel Aviv University. There are 10 references cited in this article, which can be found at the bottom of the page. This article has been fact-checked, ensuring the accuracy of any cited facts and confirming the authority of its sources. This article has been viewed 672,000 times.

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.

Steps

Section 1 of 2:

Solving for Mass Percent When Given Masses

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  1. Step 1 Start with the equation mass percent = (mass of chemical/total mass of compound) x 100. 1 Start with the equation mass percent = (mass of chemical/total mass of compound) x 100. 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. Step 2 Find the total mass of the compound. 2 Find the total mass of the compound. 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.
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  3. Step 3 Identify the mass of the chemical-in-question. 3 Identify the mass of the chemical-in-question. 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. Step 4 Plug the variables into the mass percent equation. 4 Plug the variables into the mass percent equation. 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. Step 5 Solve the mass percent equation. 5 Solve the mass percent equation. 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.
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Section 2 of 2:

Solving for Percent Mass When Not Given Masses

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  1. Step 1 Start with the equation mass percent = (molar mass of element/total molecular mass of compound) x 100. 1 Start with the equation mass percent = (molar mass of element/total molecular mass of compound) x 100. 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. Step 2 Write out the... 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. Step 3 Find the mass of each element in the compound on the periodic table. 3 Find the mass of each element in the compound on the periodic table. 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. Step 4 Multiply the masses by the mole ratio. 4 Multiply the masses by the mole ratio. 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. Step 5 Add up the total mass of all the elements in your compounds. 5 Add up the total mass of all the elements in your compounds. 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. Step 6 Identify the mass of the element-in-question. 6 Identify the mass of the element-in-question. 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. Step 7 Plug the variables into the mass percent equation. 7 Plug the variables into the mass percent equation. 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. Step 8 Calculate the mass percent by solving the equation. 8 Calculate the mass percent by solving the equation. 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%.
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Expert Q&A

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  • 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 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 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 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 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
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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
More References (6)
  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

Ronitte Libedinsky, MS Co-authored by: Ronitte Libedinsky, MS Chemistry and Biology Tutor This article was co-authored by Ronitte Libedinsky, MS and by wikiHow staff writer, Aly Rusciano. Ronitte Libedinsky is an Academic Tutor and the Founder of Brighter Minds SF, a San Francisco, California based company that provides one-on-one and small group tutoring. Specializing in tutoring mathematics (pre-algebra, algebra I/II, geometry, pre-calculus, calculus) and science (chemistry, biology), Ronitte has over 10 years of experience tutoring to middle school, high school, and college students. She also tutors in SSAT, Terra Nova, HSPT, SAT, and ACT test prep. Ronitte holds a BS in Chemistry from the University of California, Berkeley, and an MS in Chemistry from Tel Aviv University. This article has been viewed 672,000 times. How helpful is this? Co-authors: 14 Updated: August 8, 2025 Views: 672,000 Categories: Chemistry Calculations Article SummaryX

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?YesNo

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