73.9g NiO + 192.3ml 32% HCl = plate of soggy green crap that WILL NOT DRY.

I noticed that it melts into a thick, clear green liquid when heated and upon cooling crystallizes into a crusty bright green paste with a little extra neon green fluid running around...
How do I get this to a point where it can be accurately measured for subsequent reactions?

Is this NiCl2.6H2O?

[edit]
Ok.. that last little bit finally solidified, I poked it
a few times, doesn't seem to be any more fluid left...
Tastes like green apple jolly ranchers...

Yes it could be your produkt. NiCl2*H2O is indeed green while NiCl2 anhydrous is yellow.
recrystallize it from water 2 or 3 times till it ll be pure.

How would I go about doing that?  Merely dissolve what
I have now in water then... cool the water?  Boil it off?

Dissolve then reduce the volume, cool to half-crystallized then filter?

/me aquires extreme nickel sensitivity due to lack of proper protective handware whilst experimenting.

Dissolve then reduce the volume, cool to half-crystallized then filter?

Yes, but aim for at least a 80% recovery. According to "Purification of Laboratory Chemicals", 4th ed. the crystallization is to be performed from dilute (I assume ~5%) hydrochloric acid to give a pure product. I'd say that a single recrystallization is enough for most purposes.

me aquires extreme nickel sensitivity due to lack of proper protective handware NiCl2 is corrosive

I'm not touchin' that stuff...  I'm going to make my lab
monkey do it.  And by "lab monkey" I'm not humorously
referring to some human lackey, I mean a standard rhesus
monkey.  You'd be surprised how trainable they are.


Report from Joey:

Innovation #2232
Baking a thin layer of sat. NiCl2.6H2O sol'n at 350F in
a 9"x9" square pyrex baking dish results in the flaky
yellow anhydrous form.