Lancer85 - 28-4-2025 at 03:25
The sulfate salt should be convertible to the HCL salt by double displacement I just need to know a few details before I waste my precious reagent. I
would start by mixing the sulfate with a solution of calcium chloride, calcium sulfate forms, filter it off and then I have a solution of
hydroxylamine hcl mixed with calcium chloride.
1. Should I use an excess of calcium chloride but using an excess will leave contamination in the hydroxylamine hcl.
2. How do I go about getting the hcl salt out of solution?
3. How should I purify the hcl salt in this case.
[Edited on 28-4-2025 by Lancer85]
Precipitates - 29-4-2025 at 19:53
You may be able to recrystallise the HCl salt out of an ethanol solution, given its lower solubility as compared to CaCl2.
But barium chloride would be much better reagent to use, given its negligible solubility in ethanol:
Preparation of hydroxylamine hydrochloride (hydroxylammonium chloride)
Using CaCl2 you will need to recrystallise your HCl salt from an ethanol extraction (?), whereas using barium chloride, your extraction
should only contain the HCl salt.
JackleApp - 30-4-2025 at 17:46
strontium chloride might be an option too.
its solubility is moderately impacted by dissolving alcohols or other solvents into a given solution.
consider this: how much reagent will you waste attempting purification vs just very carefully only converting most of it, giving you a pure
hydrochloride and a contaminated small amount of residual sulfate. this is a sacrifice you make when fractionally crystalizing as well.
hydroxylamine chloride and sulfate seem easy enough to seperate just by rinsing with methanol or ether or a long soak in absolute ethanol.