0.6 Gram CuSO4 to Moles Calculator
Convert copper sulfate mass to moles with clarity. Choose formula type, purity, and volume settings. Get stoichiometry results plus clean export files for records.
Convert copper sulfate mass to moles with clarity. Choose formula type, purity, and volume settings. Get stoichiometry results plus clean export files for records.
Moles = effective mass ÷ molar mass
Effective mass is corrected for purity before conversion.
Effective mass = entered mass × purity ÷ 100
For anhydrous CuSO4, the molar mass is about 159.607 g/mol.
For CuSO4·5H2O, the molar mass is about 249.682 g/mol.
Formula units are calculated with Avogadro's constant.
Formula units = moles × 6.02214076 × 1023
When volume is entered, molarity is also calculated.
Molarity = moles ÷ liters of solution
Enter the mass of copper sulfate in grams. The default value is 0.6 g.
Select the correct compound form. Pick anhydrous CuSO4 for dry material. Pick pentahydrate for blue crystals.
Add purity if your sample is not pure. Use 100 for a pure reagent.
Enter solution volume only when you need molarity. Leave it blank for a mole-only conversion.
Choose significant digits, then press the calculate button. The result appears above the form.
Use the CSV or PDF buttons to save the current calculation.
| Sample mass | Compound form | Molar mass | Moles | Formula units |
|---|---|---|---|---|
| 0.6 g | Anhydrous CuSO4 | 159.607 g/mol | 0.003759 mol | 2.263 × 1021 |
| 0.6 g | CuSO4·5H2O | 249.682 g/mol | 0.002403 mol | 1.447 × 1021 |
| 1.0 g | Anhydrous CuSO4 | 159.607 g/mol | 0.006265 mol | 3.772 × 1021 |
| 2.5 g | Anhydrous CuSO4 | 159.607 g/mol | 0.01566 mol | 9.435 × 1021 |
Copper(II) sulfate is often used in school labs, agriculture, plating work, and solution preparation. A mass value alone does not show how many reacting units are present. Moles solve that problem. This calculator changes grams of CuSO4 into moles using the selected molar mass. It also adjusts the answer for purity, hydrate form, and optional solution volume.
Many products labeled copper sulfate are not always anhydrous CuSO4. The common blue crystal form is copper sulfate pentahydrate, written as CuSO4·5H2O. It contains five water molecules in each formula unit. That extra water increases molar mass, so the same 0.6 gram sample gives fewer moles. Choose anhydrous CuSO4 only when the material contains no attached water.
Moles help compare copper sulfate with other reactants in a balanced chemical equation. For example, one mole of CuSO4 contains one mole of copper ions and one mole of sulfate ions after dissociation. The tool also estimates formula units with Avogadro's constant. This is useful when a lesson asks for particles, ions, or concentration.
A reagent may not be completely pure. The purity field reduces the effective reacting mass before the mole conversion. A 95 percent sample means only 95 percent of the entered mass is counted as CuSO4. When volume is supplied in liters, the calculator also reports molarity. That value is moles divided by solution volume.
Use a calibrated balance for mass. Record whether the sample is dry or hydrated. Keep units consistent before comparing results. Very small samples may need scientific notation. Export the result when you need a saved record for worksheets, lab books, or reports. The example table shows common outputs for several sample masses and formula choices.
The main answer is the mole amount. The supporting values explain how it was reached. Effective mass shows the purity correction. Molar mass shows the selected compound basis. Particle count estimates formula units. Molarity appears only when volume is greater than zero. These checks make the conversion transparent and easier to audit. Use rounded results only after final checks.
Using 159.607 g/mol, 0.6 g of anhydrous CuSO4 equals about 0.003759 mol. The value changes if purity is below 100 percent.
CuSO4 pentahydrate has five water molecules attached to each formula unit. This increases molar mass, so the same gram amount gives fewer moles.
It uses 159.607 g/mol for anhydrous CuSO4 and 249.682 g/mol for CuSO4·5H2O. You can also enter a custom molar mass.
Purity reduces the effective mass. For example, 0.6 g at 95 percent purity is treated as 0.57 g of actual CuSO4.
Yes. Enter the solution volume in liters. The calculator divides moles by liters and reports molarity in mol/L.
Formula units are particle counts for ionic compounds. The calculator multiplies moles by Avogadro's constant to estimate them.
Choose anhydrous for dry CuSO4. Choose pentahydrate for blue copper sulfate crystals or products labeled CuSO4·5H2O.
You can download a CSV file for spreadsheet use. You can also download a simple PDF report for printing or record keeping.
Important Note: All the Calculators listed in this site are for educational purpose only and we do not guarentee the accuracy of results. Please do consult with other sources as well.