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# 3.09 Molar Mass of Compounds Honors

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## Erichelle Goitia

on 19 June 2014

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#### Transcript of 3.09 Molar Mass of Compounds Honors

3.09 Molar Mass of Compounds Honors
Calculations Continued
4. Subtract the mass of the dehydrated compound from the mass of the hydrate to determine the mass of water that was present in the hydrate.
- 20.037g
5. Convert the mass of water to moles of water.
- 0.1281 moles
6. Convert the mass of dehydrated compound to moles of the compound.
- 1.113
7. Divide by the lowest mole value to get a whole number mole ratio.
- 0.007
Formula: CuSO4*9H2O
Discussion & Conclusion
The purpose of this experiment is to determine the formula of a copper sulfate hydrate by heating it up.

Materials:
hydrate, crucible, balance, bunsen burner, scale

Procedure:
First you measure the mass of the empty crucible and record that mass. Then you should fill the crucible with 3-5 scoops of the hydrate and record that mass as well. Heat the hydrate filled crucible above the bunsen burner for 10 minutes for all of the water to evaporate. Let the crucible cool and then mass the crucible with dehydrated solid inside. Record that mass and finally calculate the formula of the hydrate.
Mass of empty crucible- 19.508g
Mass of crucible & hydrate- 40.4816g
Mass of hydrate- 20.976g
Mass of crucible & dehydrate- 39.955g
Mass of dehydrate- 20.628g

Calculations
1. Obtain the mass of the empty crucible. Obtain the mass of the crucible and the hydrate. Subtraction of the mass of the empty crucible from the mass of the hydrate and crucible gives the mass of the CuSO4 hydrate.
- 20.9736g
2. Heat the hydrate. After heating, record the mass of the crucible and the dehydrated compound.
- 20.447g
3. Subtracting the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 gives you the mass of the dehydrated compound.
- 0.939g
When heating a hydrate the most important thing to keep in mind is the amount of time you heat it for. If not heated long enough I think the mass of the anhydrate would've resulted differently. It would've still been wet causing it to weigh more than the dehydrate. The final mass would effect the calculated formula for the hydrate because the dehydrate would be incorrect. The whole equation would be inaccurate. In conclusion, if everything is performed well, you would end up with the correct formula.
Erichelle Goitia
Molar Mass Lab
Before the heating of the hydrate, it looked like small blue grains. Once I started heating the hydrate over the bunsen burner, its color slowly changed to white and stayed that way after cooling.
Observations
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