Lab 3 - Emily Bissel MS#1116 Lab Partner: Becca Angell...

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1 mole 18.015 g mol 2.113 g BaCl 2 •2H 2 O 2.646 g sample Emily Bissel MS#1116 Lab Partner: Becca Angell September 19, 2007 Thursday AM Stoichiometry of Hydrated Salts Introduction: In this experiment, various compounds were tested to find whether they were hydrated salts or not. A hydrated salt is a compound which incorporates H 2 O molecules into it’s solid structure. If the compound is a hydrate then the mass would become smaller once the substance was heated because they were efflorescent and therefore lost H 2 O molecules as they moved into the atmosphere. After being heated for a period of time, each salt was placed into the desiccator. Because the substance within the desiccator, known as desiccant, is hygroscopic, water that has not yet been dehydrated from the substance through heating is removed. Once the hydrate has cooled to room temperature, it must be massed and then reheated until there was no longer a mass change, helping to determine the mass of the anhydrous solution. Results: In part one of A, the CoCl 2 •6H 2 O originally appeared to be dark purple. As the heat was added, the hydrate turned a lighter purple and exhibited a crackling sound. Continuing to heat the substance until there was no longer any change resulted in a light blue powder, resulting in cobalt (II) chloride. When water and heat were added, the compound went turned a purple color and darkened into a dark blue. After the compound had cooled for one hour, the compound had returned to its original purple color and
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This lab report was uploaded on 04/16/2008 for the course CHEM 006L taught by Professor Miller during the Spring '08 term at Westmont.

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Lab 3 - Emily Bissel MS#1116 Lab Partner: Becca Angell...

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