Formula of a Hydrate Lab

HAPPY MONDAY!

In class:

We did the Formula Hydrate Lab (hence the title)

*Extra: Be aware of the spirit days this week as it is possible we might get a visit from the "Homecoming Genie" (I have NO idea what that means--but just show your spirit!)

For HW:

This lab (in the carbonless paper notebook of course) is due on wednesday.

DON'T FORGET: Test on Friday--Remember to do those webassigns!

Before Reaction

During Reaction

After Reaction

Let's get started.  So the purpose of this lab was to determine the amount of moles of water that are present in the compound per mole of Copper (II) Sulfate.

EQUATION OF Copper (II) Sulfate: CuSO4 * nH20 we are finding n in the lab)

Basically, we took blue hydrated Copper (II) Sulfate crystals, put them in a test tube, and heated them with a Bunsen burner until they turned white (allowing the water to separate from the substance). Here is a video of the process of the change from hydrated to anhydrous salt:

But, we had to do some weighing too.

1. Finding the mass of the empty test tube
2. Finding the mass of the test tube with hydrated salt
3. Finding the mass of the test tube with anhydrous salt

AND some calculations after you collected TWO trials of the data:

• Calculating the mass of the hydrated salt 
• Calculating the mass and moles of water lost 
• Calculating the mass and moles of anhydrous salt
• calculating the ratio between moles of water and moles of anhydrous salt (this being your n from before)

Make sure to show all your work and answer all the questions at the bottom of the lab sheet!

**Don't forget--you should have used Avagadro's number at some point in your calculations.

Next Scribe will be: Rachel! :)