Part I

When the hydrate initially dissolved, the water molecules tied up in the hydrate were freed to mix with the rest of the added water. Calculate the number of water molecules set free after the copper(II) chloride dihydrate is dissolved.

Mass CuCl2 2H2O (g)	Volume of Water(mL)	Mass Al (g)	Theoretical mass copper metal created (g)	Mass excess reagent left over (g)	Expected solution color
2.0500 100 g 2.05 g	1.180 102 mL 118 mL	1.00 10-1g 0.1 g	3.53 10-1 0.353 g	1.103 100 1.103 g	Blueish with a copper precipitate

This is the balanced equation 2Al(s) + 3CuCl₂2H₂O(aq) 3Cu(s) + 2AlCl₃(aq) + 6H₂O(l)

Part II

Describe in your own words what is happening on the molecular level as the copper(II) chloride solid dissolves in the water, and as the water from the hydrate dissolves in the water. Is this even possible? Food for Thought: What does the term dissolving mean anyway? Is the dissolving process different for an ionic compound versus a covalent compound?