Lab 4C: Naming a Hydrate

What is a Hydrate?
A "hydrate" is a name given to a compound, formed by the addition of water to the molecule. When writing the formula of a hydrate, first write the original molecule, and attach a "· nH₂O", where "n" is the number of water molecules present in the hydrate. For example, Cobalt(II) chloride hexahydrate is CoCl₂·6H₂O. 


Lab Summary
In our lab over the last two classes, we wasted productively spent most of the class heating and waiting for a crucible to cool. In our first class, we did this process three (for some groups, four) times. The first time, we heated it, using Bunsen burner, ring stand, and pipestem triangle, to eliminate any water already present in the crucible. Between heatings, we also measured, using a centigram, the weight of the crucible. At the first weighing, we discovered the weight of our crucibles. Afterwards, we used another weighing and the first weighing to derive the weight of the hydrate. Finally, after heating the crucible to evaporate the water, we weighed it again, and derived the amount of water that was evaporated through heating.

Results

After being generously given the weight of one mole of the anhydrous compound (the compound to which water was attached in the hydrate) and the formula, we could correctly produce the empirical formula of the original hydrate we were given.

Afterwards, we added a drop of water to the anhydrous salt, and observed it bond, forming a hydrate once again, thus wasting all of our original patience hard work.

To end this sarcastic blog post, below is a picture of some crazy dude burning a hydrate (that contains methane) in his hands. Compliments of Google Image Search. Until next time, stay safe, don't eat in the classroom, and wash your hands. No, seriously.