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 & 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 ______________________