1. COMPOSITION AND FORMULA OF A HYDRATED SALT
By :
aisha al-anssari
haya al-dossari
ghadah al-ghamdi

2. Introduction
A hydrate is a chemical that has water molecules loosely bonded to it. The water molecules are not actually part of the formula, so the formula is written slightly differently. The water can easily be removed from a hydrate just by heating strongly. You will be weighing a hydrate and heating it to remove the water (now called "anhydrous salt") and weigh it again. You can now find the percent of the anhydrous salt and the water. By finding a mol ratio, you can find out how many moles of water there are per mol of anhydrous salt. This number goes just before the H2O in the formula.

3. Objective
Determination of the water of hydration in a hydrated barium chloride salt and using this value to determine the percent composition of a mixture of hydrated barium chloride and sand.

4. Material required Barium chloride dehydrate Crucible and cover Tongs
Clay triangle
Electronic balance
Tripod stand
Burner

5. Procedure Clean and dry a crucible and find its mass on an
accurate balance.

6. Objective Obtain a scoop of the hydrate from your teacher and find the
mass again.

7. Procedure Heat the crucible under moderate heat for 3-5 minutes. Let
the crucible cool and
find its mass again.

8. Procedure
Heat the crucible again under moderate heat for another 2 minutes. Place an inverted beaker over it while cooling. Find its mass again.
Repeat this heating and weighing until the mass doesn't change any more (stays within .05 grams).

9. Conclusion
As the conclusion, by doing the empirical method we can determined the number of moles in the given substance of the element. Moreover this method also help us to find the real molecular formula.