Hydrated Chloride

Purpose: The purpose of this experiment is to determine the number of moles of water molecules of crystallization of a sample of hydrated Barium
Chloride. This can be calculated using Gravimetric Analysis and to indirectly determine the percent composition of a hydrate by taking advantage of its chemical properties.
Introduction:
Gravimetric procedures are analytical methods in which the results are determined from the masses of starting materials and products. These methods differ from volumetric procedures in which the calculations are based on the volumes of standardized solutions used in the procedure. One of the simplest gravimetric procedures involves the heating of a weighed sample to drive off a volatile component. The difference in mass before and after heating provides the mass of the volatile component. Hydrates are examples of compounds that would display this behavior. If the formula of
Once cool, the empty crucible was weighed and approximately 2-3g of Hydrated Barium Chloride was added to the crucible. The crucible and contents were then weighed on a balance and a note of the mass was taken. The crucible was then heated for 15minutes using a blue Bunsen burner flame on the pipe-clay triangle, with the lid partially covering the contents. The crucible was then transferred to the desiccator using tongs. Once cooled, the crucible + contents were re-weighed. This process was repeated, heating for about4 minutes each time, until two successive balances reading were within 0.002g of each other, at this point the contents were at constant mass, and all of the water had been removed. The value of n in BaCl2.nH2O was then