The molar mass of sodium sulfate, Na2SO4, is 142.03554 g/mol. That single number is what connects a mass you can weigh to an amount of substance you can react: one mole is 142.0355 g, and a gram of it is 4.24e+21 formula units. The calculator turns any weighed mass into that count, and reports the amount in moles, millimoles and the mass of a single formula unit alongside it.
The figure comes from the formula. Sodium sulfate is 2 × 22.9898 (Na) + 32.06 (S) + 4 × 15.999 (O), which is 142.03554 g/mol, taking standard atomic weights, and every page here computes that sum rather than quoting it. Oxygen makes up the largest share of the mass: 4 of the 7 atoms in a formula unit are oxygen, and they account for 63.996 g of the 142.0355 g, or 45.06% by mass. The derivation table below breaks the whole molecule down element by element.
The numbers a bench actually uses sit at the millimole scale. One millimole of sodium sulfate is 142.036 mg and one micromole is 142.036 µg, so a balance reading to a milligram places you within 7.04 µmol. A single formula unit weighs 2.3586e-22 g, which is why the count in the gauge runs into the sextillions for any mass you can see.
A drying agent in the laboratory and a filler in powdered detergent. The decahydrate, Glauber salt, is 322.20 g per mole. At 142.0355 g/mol it is heavier than 17 of the 34 salts covered here, and that ranking matters more than it looks: disodium phosphate has a molar mass of 141.9573 g/mol, so a gram of it contains 0.0551% more formula units than a gram of sodium sulfate. Weigh by mass and you are not weighing equal amounts of substance.
Purity is the usual gap between the calculation and the balance. A reagent sold at 98% means 2.8407 g of a nominal 142.0355 g is something else, so for exact work you divide the weighed mass by the assay figure on the certificate. For most purposes the difference is smaller than the error in reading the meniscus, but it is systematic rather than random, so it does not average out.
The formula
m- The mass of sodium sulfate in grams
142.03554- The molar mass of sodium sulfate in g/mol, derived from its formula
N- The number of formula units that mass contains
How it works, step by step
- Enter a mass of sodium sulfate in grams.
- It is divided by the molar mass, 142.03554 g/mol, giving the amount in moles.
- That amount is multiplied by the Avogadro constant, 6.02214076 × 10²³ per mole, to give the number of formula units.
- The panel also reports the amount in moles and millimoles and the mass of one formula unit.
Worked examples
0.5 g of sodium sulfate as a molecule count
0.5 g divided by 142.0355 g/mol is 0.00352025 mol, and multiplying by the Avogadro constant gives 2.12e+21 formula units of sodium sulfate. The same mass is 3.5202 mmol, which is the figure a reaction is actually planned in.
5 g of sodium sulfate as a molecule count
5 g divided by 142.0355 g/mol is 0.0352025 mol, and multiplying by the Avogadro constant gives 2.12e+22 formula units of sodium sulfate. The same mass is 35.202 mmol, which is the figure a reaction is actually planned in.
50 g of sodium sulfate as a molecule count
50 g divided by 142.0355 g/mol is 0.352025 mol, and multiplying by the Avogadro constant gives 2.12e+23 formula units of sodium sulfate. The same mass is 352.02 mmol, which is the figure a reaction is actually planned in.
How to read your score
Frequently asked questions
What is the molar mass of sodium sulfate (Na2SO4)?
It is 142.03554 g/mol. That is the sum of the standard atomic weights of every atom in the formula: 2 × 22.9898 (Na) + 32.06 (S) + 4 × 15.999 (O). One mole of sodium sulfate therefore weighs 142.0355 g, and a gram of it is 7.0405 mmol.
What percentage of sodium sulfate is oxygen?
45.06% by mass. Each formula unit contains 4 oxygen atoms contributing 63.996 g of the 142.0355 g total, so 100 g of sodium sulfate contains 45.06 g of oxygen and a kilogram contains 450.56 g of it.
How many molecules are in one gram of sodium sulfate?
About 4.24e+21. One gram is 0.00704049 mol, and each mole contains 6.02214076 × 10²³ formula units by definition of the mole, so the count is that constant divided by 142.0355.
How much does a single molecule of sodium sulfate weigh?
2.3586e-22 g, which is 142.03554 daltons. It is the molar mass divided by the Avogadro constant, and the number in daltons is numerically the same as the molar mass in g/mol — that equivalence is what makes the mole convenient.
Is molar mass the same as molecular weight?
They are the same number in ordinary use but not the same quantity. Molecular weight, properly relative molecular mass, is a ratio and has no unit: for sodium sulfate it is 142.03554. Molar mass carries grams per mole: 142.03554 g/mol. Because the mole is defined so those agree, you can read one off the other.
Why is the molar mass not a whole number?
Because standard atomic weights are averages over the isotopes found in nature. Oxygen is quoted as 15.999 rather than a whole number for that reason, and the same applies to the other elements here, which is why sodium sulfate comes out at 142.03554 g/mol rather than 142.
Molar mass, composition and mole equivalents of sodium sulfate
| Element | Atoms | Atomic weight | Contribution (g/mol) | By mass |
|---|---|---|---|---|
| Oxygen (O) | 4 | 15.999 | 63.996 | 45.06% |
| Sodium (Na) | 2 | 22.98977 | 45.97954 | 32.37% |
| Sulfur (S) | 1 | 32.06 | 32.06 | 22.57% |
| Total — one mole of sodium sulfate | 142.03554 | 100% |
Standard atomic weights, IUPAC 2021. The contribution column is atoms × atomic weight, and the total is the molar mass this page uses: 142.03554 g/mol.
| Amount | Mass (g) | Mass (mg) | Formula units |
|---|---|---|---|
| 1 µmol | 0.000142036 | 0.142036 | 6.022e+17 |
| 10 µmol | 0.00142036 | 1.42036 | 6.022e+18 |
| 100 µmol | 0.0142036 | 14.2036 | 6.022e+19 |
| 1 mmol | 0.142036 | 142.036 | 6.022e+20 |
| 10 mmol | 1.42036 | 1420.36 | 6.022e+21 |
| 50 mmol | 7.10178 | 7101.78 | 3.011e+22 |
| 100 mmol | 14.2036 | 14,203.6 | 6.022e+22 |
| 250 mmol | 35.5089 | 35,508.9 | 1.506e+23 |
| 500 mmol | 71.0178 | 71,017.8 | 3.011e+23 |
| 750 mmol | 106.527 | 106,527 | 4.517e+23 |
| 1 mol | 142.036 | 142,036 | 6.022e+23 |
| 2 mol | 284.071 | 284,071 | 1.204e+24 |
| 5 mol | 710.178 | 710,178 | 3.011e+24 |
| 10 mol | 1420.36 | 1420355.385600 | 6.022e+24 |
Mass is the amount multiplied by 142.03554 g/mol. The last column is that amount multiplied by the Avogadro constant, 6.02214076 × 10²³ per mole.
| Compound | Formula | Molar mass (g/mol) | Millimoles in 1 g |
|---|---|---|---|
| Ammonium sulfate | (NH4)2SO4 | 132.134 | 7.5681 |
| Monopotassium phosphate | KH2PO4 | 136.0841 | 7.3484 |
| Disodium phosphate | Na2HPO4 | 141.9573 | 7.0444 |
| Sodium sulfate (this page) | Na2SO4 | 142.0355 | 7.0405 |
| Potassium permanganate | KMnO4 | 158.0323 | 6.3278 |
| Copper(II) sulfate | CuSO4 | 159.602 | 6.2656 |
| Iron(III) chloride | FeCl3 | 162.195 | 6.1654 |
Ordered by molar mass. The last column is 1000/M, which is the number a weighed gram actually gives you.