Hydrate Lab Purpose: Determine the formula of the hydrate compound Copper (II) Sulfate by identifying the amount of water molecules that are attached to a formula unit by evaporating the hydrate in the compound.
https://youtu. be/YI0qaNCBqK4
Background
Hydrates are ionic compounds (salts) that have a definite amount of water (water of hydration) as part of their structure. The water is chemically combined with the salt in a definite ratio. Ratios vary in different hydrates but are specific for any given hydrate.
The formula of a hydrate is represented in a special manner. The hydrate of copper sulfate in this experiment is listed below:

In the formula, the unit formula for the salt appears first, and the water formula is last. The raised dot means that the water is loosely bonded to the salt. The coefficient x stands for the number of molecules of water bonded to one unit of salt. This special formula, like all other formulas, illustrates the law of definite composition.
When hydrates are heated, the "water of hydration" is released as vapor. The remaining solid is known as the anhydrous salt. The general reaction for heating a hydrate is:

Some anhydrous salts can absorb moisture from the air to become hydrated. A common example is silica gel, made from sodium silicate which is usually packaged with optical or electronic devices shipped by boat. The silica gel protects the devices from high humidity.

Materials:
(List in bullet point the materials used and amount of sample needed)

Procedures:
(Listed in numbered format the steps taken for this virtual lab; be thorough)

Data:
Mass of crucible
(thousandth place)
Mass of crucible + CuSO4 hydrate
(thousandth place)
Mass of crucible + CuSO4 anhydride
(thousandth place)
Mass of CuSO4 hydrate
(thousandth place)
Mass of CuSO4 anhydride
(thousandth place)
Moles CuSO4 anhydride

Mass of water loss (hydrate – anhydride)
(thousandth place)
Moles of water loss

Ratio (Divide moles of water by moles of CuSO4)

Percent of water in CuSO4 hydrate
(mass of water / mass of CuSO4 hydrate) x 100%

Describe color before and after applying heat:

Ratio of CuSO4 to H2O: (substitute x with your rounded whole number value)

Discussion questions:
1. What was the actual ratio you obtained (with all significant digits)? What was your rounded ratio to whole numbers? Is your actual ratio higher or lower than the rounded ratio? Research what the actual ratio should be. Is your answer too high or too low? What is the percent error [((theoretical – actual) / theoretical ) x 100]?
2. How would your ratio change if you did not dehydrate the compound fully?
3. Suppose some of the compound fell out of the crucible before heating but after massing. How would that change your ratio?
4. How would your ratio change if the crucible was wet when the hydrated compound was added to it at the beginning of the experiment?
5. How would your ratio relate to another group’s who used the same compound, if you used 2.0 grams and they used 2.5grams?
6. Suggest what might happen if you left the anhydrous compound to sit overnight before weighing it for your data?
7. If you could improve this lab, what you do differently and why? Discuss at least three feasible improvements and why with reference to the other discussion questions and errors. (Note: relate this to #1 and the answers for the other questions).
One Paragraph Reflection: