Send the link below via email or IMCopy
Present to your audienceStart remote presentation
- Invited audience members will follow you as you navigate and present
- People invited to a presentation do not need a Prezi account
- This link expires 10 minutes after you close the presentation
- A maximum of 30 users can follow your presentation
- Learn more about this feature in our knowledge base article
3.09 Molar Mass of Compounds Honors
Transcript of 3.09 Molar Mass of Compounds Honors
Discussion & Conclusion
Title: 3.09 Lab
Purpose: The purpose of this experiment is to determine the formula of copper sulfate hydrate by it being heated.
The materials were hydrate, crucible, a balance, a bunsen burner, and a scale.
First, measure the mass of the empty crucible. Fill the crucible with 3-5 scoops of the hydrate. Heat the hydrate filled crucible above the bunsen burner for 10 minutes for all of the water to evaporate. Let the crucible cool. Then, then measure the mass of the crucible with the dehydrated solid inside. 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
1. Obtain the mass of the empty crucible, the mass of the crucible and the hydrate. Subtract the mass of the empty crucible from the mass of the hydrate and crucible, which 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. Subtract the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 which, gives the mass of the dehydrated compound. 0.939g
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 the moles of the compound. 1.113
7. Divide by the lowest mole value to get a whole number mole ratio. 0.007
When heating a hydrate keep in mind that the amount of time you heat it makes a difference. If the heating was timed differently the mass of the hydrate would've resulted differently as well. It still would have been wet, which would cause it to weigh more than the dehydrate. The final mass would effect the calculated formula for the hydrate, because the dehydrate would have been incorrect. The whole equation would have been inaccurate. In conclusion, if the lab is performed properly, it will result in the correct formula.
Before heating the hydrate, it looked like tiny blue grains, but when I started heating the hydrate over the bunsen burner, its color slowly changed to white and stayed that way after it cooled.
CuSO4 x 9H2O