# Copper Sulfate lab - Minneota Public School

```Name: ____________________________________Period: _____
Date:____________
Formula of a Hydrate Lab
Purpose:
To utilize mole conversions to determine the ratio between copper (II) sulfate
molecules and water of hydration.
Materials:
1 Bunsen burner
1 Clay triangle
1 Crucible
1 Ring stand
1 Electronic Scale
1 Crucible Tong
Copper II Sulfate Hydrate (approx. 5g)
Procedure:
1. Mass crucible (empty)
2. Obtain approximately 5 grams of Copper II sulfate hydrate
3. Put hydrate in crucible and find the mass.
4. Light Bunsen burner
5. Place crucible with copper II sulfate hydrate over Bunsen burner.
6. Place lid on crucible (keeping it slightly cocked open).
7. Heat until blue color is gone.
8. Turn off Bunsen burner and close lid on crucible
9. Let crucible cool until you can handle it.
10. Mass crucible and copper II sulfate anhydrate.
11. Wipe out crucible into waste container and wash out.
12. Clean up lab station.
13. Perform calculations.
Data:
Mass of Empty Beaker(g)
Mass of Beaker &amp; CuSO4 . H2O (g)
Mass of Beaker and CuSO4 (g)
NOTES
Calculations: You must show all work for complete credit.
Determine the mass of Copper II Sulfate Hydrate.
Using the mass of the beaker only and the mass of the beaker with copper II hydrate, determine
the mass of the blue copper II sulfate hydrate.
________________g CuSO4.XH2O
Determine the mass of Copper II Sulfate Anhydrate
Using the mass of the beaker and the mass of the beaker with copper II anhydrate, determine the
mass of the copper II sulfate anhydrate.
_________________g CuSO4
Determine the mass of water lost from Hydrate.
Using the mass of the copper II sulfate hydrate and the mass of the copper II sulfate anhydrate,
determine the mass of water lost from the hydrate.
__________________g H2O
Determine the number of moles of copper II sulfate anhydrate, CuSO4.
Using the mass of copper II sulfate anhydrate and the molar mass from the periodic table,
determine the number of moles of copper II sulfate used in your experiment.
__________________ mol CuSO4
Determine the number of moles of water.
Using the mass of water lost and the molar mass from the periodic table,
determine the number of moles of water of hydration.
__________________ mol H2O
Determine the mole ratio of Copper II Sulfate and Water.
Using the number of moles of copper II sulfate and moles of water,
determine the smallest whole number ratio.
Ratio _____to _____
Write the formula of Copper II Sulfate Hydrate
CuSO4 . _____ H2O
Conclusion
By heating __________ grams of copper II sulfate _______________, it was calculated that
__________ grams of water were lost. With a mass of __________ grams for the anhydrate, it
was determined that the mole ratio of copper II sulfate to water is ___:___. From this, it can be
stated that the formula for the hydrate is _______________.
The actual formula for the hydrate is _______________. Our ratio was ____________ to that of
the actual formula. Potential sources of error in this lab could be ______________________
```