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CuSO4 Lab

   

The weight % water in hydrous cupric sulfate is approximately 35%. Some of you had some old cupric sulfate that had already begun to dehydrate due to the extremely dry Nevada climate. Answers between 20 and 40 % are reasonable.

Calculating the formula extra credit.

1.) Recognize that the CuSO4 is many times heavier on a molecule by molecule basis than the H2O.

2.) We need to find a ratio of how many molecules of water to how many molecules of CuSO4 are present.

3.) Recall that if you have a GFW then you have one mole of molecules

4.) Calculate number of moles of H2O present.

1.8 g H20 1 mole H20
  18.02 g H2O

= 0.1 mole H20

5.) Calculate the number of moles of dry CuSO4 present (Subtract the mass water from the mass of  hydrous CuSO4)

3.2 g H20 1 mole CuSO4
  160 g CuSO4

= 0.02 mole CuSO4

6.) Now we have a ratio, but the numbers are awkward. Lets "normalize" them by dividing both by the smallest number.

0.1 mole/ 0.02 mole =  5 (the H2O)

0.02 mole/ 0.02 mole = 1 ( the CuSO4 )

So for every 1 CuSO4 we have 5 H20 or we can write this CuSO4 . 5H20 and its formal name is copper (II) sulfate pentahydrate.