Remember: this lab is due on Wednesday October 3, 2012.

Also wear mismatched clothes for tomorrow!

No homework for today except to study for the test on Friday!

            Today, we needed to determine how many moles of water are present in the compound per mole of Copper (II) Sulfate.

Lab Goal: To determine the formula of the hydrated.

Procedure: First, a clean crucible or flask must be readied. Then, add a reasonable amount of blue hydrated copper (II) sulfate to the crucible or flask. Due to the shortage of crucibles, many students received a flask. Instead, the flask is heated over a Bunsen burner, evenly applying minimal heat. The substance must be heated until the substance turns white. Brown indicated overheated. Upon completion, allow the flask to cool and wipe out any with a tissue or paper towel.

Data & Conclusion:

Mass of empty crucible	19.44	17
Mass of crucible with Hydrated Salt	21.43	19.12
Mass of crucible with Anhydrous salt	20.62	18.44

 Calculate the mass of the hydrated salt:

Mass of crucible with hydrated-Mass of empty flask = Hydrated salt

Calculate the mass and moles of the water lost.

       Mass of Hydrated Salt – Mass of Anhydrous salt = Water Loss

`           Mass of the water / Grams of H2O

Calculate the mass and moles of anhydrous salt.

       Mass of crucible with anhydrous salt – Mass of empty flask

            Mass of anhydrous salt / mass of CuSO4 in grams

Calculate the ratio between moles of water and moles of anhydrous salt.

       Moles of H2O : Moles of CuSO4

Claim: What is the formula of the hydrated salt?

Evidence: What data did you use to prove your claim?

Reasoning: If all of the water was not driven off, how would this affect your formula for the hydrated salt? Be specific.

Next Scribe: FaBIAN

Signed -Josh-