artemov - 24-11-2020 at 06:47
I made some nickel chloride solution (using pure nickel coins, H2O2 and HCl) from which I am trying to get the hexahydrate crystals via slow
evaporation in open air.
Unfortunately I just found out that "the nickel chlorides are deliquescent, absorbing moisture from the air to form a solution" (https://en.wikipedia.org/wiki/Nickel(II)_chloride)
Can a hygroscopic salt crystallized via slow evaporation in the open air? If not, what can I do besides heating/boiling the solution, something I am
reluctant to do? Cheers.
CarlSagans_RayGuns - 24-11-2020 at 07:07
Have you tried putting it in a sealed bag with magnesium sulfate desiccant? You might still need a little bit of heat. I dry mine in open air over a
heating pad. Wear a respirator and nitrile gloves, no biggie. You want to avoid breathing the dust.
Tsjerk - 24-11-2020 at 07:22
Hygroscopic salts can only be dried in open air when the relative humidity is below a certain threshold. In a closed container with for example
magnesium sulfate or calcium chloride you will bring down the humidity so far, the salt will dry. Under vacuum the salt dries faster, but with a
little patience any closed container will do.
MidLifeChemist - 24-11-2020 at 08:05
>> If not, what can I do besides heating/boiling the solution, something I am reluctant to do?
Is it because you are worried about the quality of the crystals, or some other reason?
artemov - 24-11-2020 at 08:06
There is still a lot of water currently. I think I will wait for the water/hcl to reduce by a fair amount first before doing the dessicating box
thing. Thanks guy!
MidLifeChemist: for safety reason
[Edited on 24-11-2020 by artemov]