1) Aluminum sulfate hydrate Al2(SO4)3.xH2O contains 13.63% Al by mass. Calculate x, that is, the number of water molecules associated with each Al2(SO4)3unit.
2) What would happen if a small amount (0.2ml) of water is added to 10.0g of solid anhydrous CuSO4? What happens to the color? Write an equation that describes this process. How is this different from the experiment that you did in the simulation?
2007-01-13 13:24:15 · 3 answers · asked by Rubidium S 1 in Science & Mathematics ➔ Chemistry
1) All you do is...
-Find the molar mass of Al(2) (SO(4))3 without the hydrate.
-Set up a ratio of [mass % Al:unhydrated mass::mass % Al:Hydrated mass]
-You obviously don't know the hydrated mass yet, so that's what you're solving for.
-Once you have the hydrated mass, subtract the mass of the unhydrated Aluminum sulfate.
-The remaining mass is the total mass of the water molecules.
-Now, divide the mass of all of the water molecules by the mass of one water molecule
-This number is x, the number of water molecules that hydrate the aluminum sulfate molecule.
If you need clarification on anything, just e-mail me.
2) When you add water, the color will change... I don't know how this is different from your simulation because I didn't do your simulation.
But you can work out the chemical equation for what's going on... the water will hydrate the CuSO4, but not completely.
2007-01-13 15:11:13 · answer #1 · answered by Jess4352 5 · 1⤊ 0⤋
SOrrrrrrrrrrrrrrrrrrrrrrrry but i cant help I'm only in 6th grade and i don't really even no the definition 4 that SORYYYYYYYYYY
2007-01-13 21:33:53 · answer #2 · answered by Anonymous · 0⤊ 1⤋
holy mother of a cactus! I got no idea, and I'm in Hoors Chemistry!
2007-01-13 21:31:43 · answer #3 · answered by teenwriter_25 2 · 0⤊ 1⤋