LAB 4C

LAB 4C FORMULA OF A HYDRATE






Determine the empirical formula of hydrate!
















Hydrate is compound that contains a definite number of water molecules incorporate into crystal structure.


An anhydrous salt is a salt that has been heated up until the water in it evaporates and it usually disenigrates into a powder, but is now anhydrous (Without water).

Procedure

• set up the pipestem triangle, iron ring, stand and bunsen burner
• heat up the crucible and cool it for 3 min
• place the hydrate in the crucible
• heating the crucible and cool it for 5 min
• reheating the crucible 
• note any change that occur

    *record the mass after each step*

Make a table to organize the information we get from experiment. By calculation, we can get the mass of the hydrate, anhydrous salt, and water given off. Since the teacher already gives us mass of one mole of anhydrous salt. It will be very easy to get the answer.

1. calculate the mole of anhydrous salt

mole(anhydrous salt) = mass of anhydrous salt/molar mass of anhydrous salt

2. calculate the mole of water

mole(water) = mass of water given off/ molar mass of water

3. divide each molar amount by the smallest molar amount we get just now

4. scall ratio to wholes number by multiplying

Now we are done!!!