Lab 9: Composition of a Copper Sulfate Hydrate Lab

   In the Composition of a Copper Sulfate Hydrate Lab, my group was required to evaporate water out of copper(II) sulfate hydrate into copper(II) sulfate. This was done by heating copper(II) sulfate hydrate in an evaporating dish. We occasionally stirred and reduced the temperature of the chemical compound to make sure it was not decomposing into copper sulfide.  Eventually the water evaporated out.

1. Calculate the mass of the hydrate used.
40.65 g - 39.84 g = 0.81 g of hydrate

2. Calculate the mass of the water lost.
40.65 g - 40.38 g = 0.27 g of water

3. Calculate the percentage of water in the hydrate.
0.27 g / 0.81 g = 33.33%

4.The accepted value for the percentage of water in this hydrate is 36.0%. Find your percent error and provide a possible explanation for your error.
(33.33% - 36.0%) / 36.0% = -7.42 percent error
There is a percent error because the measurements of the hydrate before and after heating are not precise measurements.

5.
Moles of evaporated water - 0.27/18.01= 0.0150 mol
Moles of copper sulfate - 0.81/159.604= 0.00508 mol
Ratio of Moles - 1.851/0.4192= 4.42

Empirical Formula - 1CuSO4 + 4H2O

Before Heat



After Heat

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