In order to grasp the concept of molar mass calculations it is important to understand the molar unit. The mole also called mol is the basic unit of measurement in chemistry. By definition, in modern chemistry, one mole represents the number of carbon atoms in exactly 12 grams of carbon 12 isotope. Remember that carbon-12 has an atomic mass of 12 (six neutrons and six protons).

One mole of anything, however, contains 6.0221367E^{23} of that object. This is known as Avogadro's number.

- Examples:
- 1 mole of carbon = 6.0221367E
^{23}carbon atoms - 1 mole of bananas = 6.0221367E
^{23}bananas

(Aren't you glad they don't sell bananas by the mole?)

Obviously it would be impossible to count out 6.0221367E^{23} atoms. Remember, however that 1 mole of carbon-12 = 12 grams = 6.0221367E^{23} atoms. It has been established that 1 mole of any element = the atomic mass of that element expressed in grams. Since magnesium has an atomic mass of 24, one mole of magnesium weighs 24 grams and contains 6.0221367E^{23} atoms of magnesium. A mole of any molecule = the molecular mass of that molecule expressed in grams. In order to determine the weight of one mole of bananas, one would have to get an average weight of a banana and multiply that by 6.0221367E^{23} then we could weigh out that weight of bananas and presto, we would have a mole of bananas. Of course, nobody would ever do that. It just demonstrates that mole of anything = 6.0221367E^{23} and we can measure out a mole of something by counting it or by weighing it out. Since atoms are too small to count, we must weigh out a mole of atoms.

*Molar mass*is a unit that enables scientists to calculate the weight of any chemical substance, be it an element or a compound. Molar mass is the sum of all of the atomic masses in a formula. Once one determines the molar mass of a substance, it will be easy to measure out one mole of that substance.

The molar mass calculation of a substance is complete the following steps (We will use sulfuric acid, H_{2}SO_{4}, as an example):

- Make a list of each element and the number of atoms of each element present in the substance.
- H 2

S 1

O 4

- H 2
- Go to periodic table and determine the atomic mass average (atomic weight) of each element.
- H 1.00794

S 32.066

O 15.9994

- H 1.00794
- Multiply each atomic mass by the number of atoms in the formula.
- H 1.00794 * 2 = 2.015

S 32.066 * 1 = 32.066

O 15.9994 * 4 = 63.998

- H 1.00794 * 2 = 2.015
- Add up the results of step three:
- 2.015+32.066+63.998 = 98.079 = molar mass of sulfuric acid

In this example the results have been rounded off to the correct number of decimal places. (Since the atomic mass average of sulfur given above only has 3 decimal places, accuracy can not be determined beyond that point).

These calculations will be necessary before one can determine the molarity or normality of a solution and many other formulas in stoichiometry (the quantitative relationships between chemical substances in a chemical equation).

- Try these formulas and then compare your results to those you get on the calculator below:
- H
_{2}O - NH
_{3} - C
_{2}H_{4}O_{2} - K
_{2}Cr_{2}O_{7}

Formulas can have a max of two brackets open at the same time, and the molecule of crystallization must be placed last.

**Examples:**- 3BeO.Al2O
_{3}.6(SiO_{2}) = (BeO)3.Al2O3.6(SiO2) - (BaH
_{2}O)_{2}Mn_{5}O_{10}= (BaH2O)2Mn5O10 - (KMgCl
_{3}).6H_{2}O = (KMgCl3).6H2O

- Molarity, Molality and Normality

Introduces stoichiometry and explains the differences between molarity, molality and normality. - Periodic Table of Elements

Provides comprehensive data on the chemical elements including scores of properties, element names in many languages, chemical compounds, most known nuclides. - Anatomy of the Atom

Answers many questions regarding the structure of atoms.

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Roberta Barbalace, Kenneth Barbalace. Molar Mass Calculations and Molecular Weight Calculator. EnvironmentalChemistry.com. 1996. Accessed on-line: 5/3/2016

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