I plan to conduct a demonstration lesson on stoichiometry using copper (II) sulfate which i plan to hydrate. Is it as simple as computing for the mass of the anhydrous and adding the mass of 5 moles of water?
2007-01-28 05:29:23 · 2 answers · asked by Marinela C 1 in Science & Mathematics ➔ Chemistry
In principle, yes. However, you may have some trouble getting it to mix properly.
It's easier to do it the other way - weigh out some copper sulfate pentahydrate, then heat it until it's all dull green. Measure the dried sample. The difference should be 5 moles of water (or close - may not drive all of it away).
Leave it out on the counter, especially near a good humidity source like hot steamy water. The stuff should be blue a little while later.
2007-01-28 06:11:51 · answer #1 · answered by fucose_man 5 · 0⤊ 0⤋
to produce hydrated copper sulfate, you would have to dissolve the anhydride and then recrystalize it, which will take some time if you want it to be hydrated. and yes, if you dissolve one mole of copper sulfate, it is just that simple.
2007-01-28 05:33:23 · answer #2 · answered by The Frontrunner 5 · 1⤊ 0⤋