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DutchChemistryBox
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Take a look at this paper:
http://www.sciencedirect.com/science/article/pii/S0304386X11...
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DraconicAcid
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It says it removes the water ligands from the copper and still forms the pentahydrate.......someone's not paying attention.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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12thealchemist
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I have (today) also recreated the experiment, and obtained results consistent with the formation of a trihydrate. A nearly boiling (97*C) saturated
solution of copper sulphate was created, and was then allowed to cool to ~70*C. The liquid was poured off, since some copper sulphate crystals had
formed. I then added ethanol so that ~10% of the total volume was ethanol, and allowed the mixture to cool slightly (about 30 seconds/a minute of
cooling). Again, the liquid was poured off and the small needle-like crystals drained. These were then collected, and dried to a free-flowing powder.
A portion of these were then weighed. The crystals were then heated much more strongly to drive off the water of crystallisation, and left on the
hotplate until white. The white (with a subtle hint of blue) crystals were then reweighed.
The masses are as follows:
Mass needle crystals: 2.675g
Mass anhydrous: 1.990g
Mass of water lost: 0.685g
Moles water: 0.0380
Moles anhydrous CuSO4: 0.0124
Ratio water to copper sulphate: 3.05:1
Therefore, I conclude that I prepared the trihydrate using the above method.
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Eddygp
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Thank you for having a go at this, 12thealchemist!!
there may be bugs in gfind
[ˌɛdidʒiˈpiː] IPA pronunciation for my Username |
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