Purpose
To understand the properties of a hydrated ionic compound and the process of converting hydrates into anhydrous ionic compounds.
Question
What is the formula of hydrated copper (II) Sulfate, CuSO4 • xH2O?
Hypothesis
When hydrated copper(II) sulfate is heated, the high temperature will cause the water and copper(II) sulfate to decompose forming anhydrous copper(II) sulfate and water (vapour). The reaction which will occur is decomposition.
Materials
1. 400 mL beaker
2. beaker tongs
3. Hot plate
4. Scoopula
5. Electronic balance
6. Glass rod
7. 3g hydrated copper(II) sulfate
8. 3g hydrated barium chloride
9. ceramic bowl (substitute for hot plate)
Procedure
Make a table to record observations. Then, add 3 g of hydrated copper(II) sulfate to the beaker and measure the mass of the beaker with hydrated copper(II) sulfate after measuring the mass of the beaker and stirring rod.
Next, heat the beaker over a hot plate on medium heat until the colour fades into a lighter shade. Remember to stir occasionally, and stop heating after the colour changes. Allow the beaker to cool before measuring the mass of the beaker with anhydrous copper (II) sulfate, and record the mass onto a table. Find the mass of the beaker with anhydrous copper (II) sulfate, and record …show more content…
If the conversion from hydrated ionic compound to anhydrous compound wasn’t complete before recording the observations, then there would still be some water left in the compound which would have an effect on the percent by mass of water. If other groups ended the experiment before or after it would affect their percent by mass. [See table 3]. The differences in the percent composition tells us that our experiment carried on for the longest compared to the two other groups. It would also change the formula because then the mass would also be different. In addition to time, the mass of the hydrated copper (II) sulfate is also more and contributes to the difference in mass and percent
To understand the properties of a hydrated ionic compound and the process of converting hydrates into anhydrous ionic compounds.
Question
What is the formula of hydrated copper (II) Sulfate, CuSO4 • xH2O?
Hypothesis
When hydrated copper(II) sulfate is heated, the high temperature will cause the water and copper(II) sulfate to decompose forming anhydrous copper(II) sulfate and water (vapour). The reaction which will occur is decomposition.
Materials
1. 400 mL beaker
2. beaker tongs
3. Hot plate
4. Scoopula
5. Electronic balance
6. Glass rod
7. 3g hydrated copper(II) sulfate
8. 3g hydrated barium chloride
9. ceramic bowl (substitute for hot plate)
Procedure
Make a table to record observations. Then, add 3 g of hydrated copper(II) sulfate to the beaker and measure the mass of the beaker with hydrated copper(II) sulfate after measuring the mass of the beaker and stirring rod.
Next, heat the beaker over a hot plate on medium heat until the colour fades into a lighter shade. Remember to stir occasionally, and stop heating after the colour changes. Allow the beaker to cool before measuring the mass of the beaker with anhydrous copper (II) sulfate, and record the mass onto a table. Find the mass of the beaker with anhydrous copper (II) sulfate, and record …show more content…
If the conversion from hydrated ionic compound to anhydrous compound wasn’t complete before recording the observations, then there would still be some water left in the compound which would have an effect on the percent by mass of water. If other groups ended the experiment before or after it would affect their percent by mass. [See table 3]. The differences in the percent composition tells us that our experiment carried on for the longest compared to the two other groups. It would also change the formula because then the mass would also be different. In addition to time, the mass of the hydrated copper (II) sulfate is also more and contributes to the difference in mass and percent