Tsathoggua favours dealing with the hydrochloride salt. Not highly experienced with either its handling or use, having only done so relatively recently, within a timescale of less than two years, greater than a good few months.
The reason for this, is of course, the danger of hydroxylamine in its freebase form. And compared to the sulfate, which mind you, has never been used by the great ancient amphibian one, if one has to form a freebase for a reaction, such as forming an oxime in the presence of a functional group which one does not want protonated by escaping HCl if based in situ either specifically or via reaction conditions already being sufficiently basic, capturing the escaping HCl, if one were theoretically to use a proton donor which does not depend on amine groups for its basicity, may be too slow, and lower reaction yields.
Seems 'cleaner' than sulfate also, as HCl is gaseous in nature and can, as said, if required in a specific reaction of some sort, be pursuaded, logically speaking, to bugger off elsewhere by driving it off, as long as it isn't highly soluable, with a good affinity for the solvent. Similar to how NH3(g) can be driven off from NH3(aq) leaving water, by heating. The ammonia having a good solubility in water, but not being 'captured' and having a certain quantity, small, compared to however much was originally in the rxn solvent, but nevertheless existant. This is conjectural theory, the latter paragraph, or parts of it from applied logical deduction, not gospel truth obtained by viewing through practical experience, so do not take it as holy writ. Results may differ. Of course, sulfates are not volatile, HCl is...go figure. (aside from certain sulfates, such as esters, Me2SO4, etc. of course, and if THATs being driven off from your reaction, one should be several miles in the opposite fucking direction:D)
From what Tsathoggua has read, the freebase of NHOH is dangerous primarily, when heated. In the cold, and absence of base (again, as stated, seemingly particularly the group I, and he would surmise, group II metal hydroxide bases) the impression Toady gets, is that it is likely to simply sit there and react. However if refluxed (presumably past a certain temperature, or possibly under the influence of vacuum), there may well be a tendency towards explosion if one is unlucky. Most unpleasant if it were to happen in a glass flask with a clandestine chemist standing next to it observing the progress of their currently pursued reaction, whatever it might be. The toad deity HAS read of explosions, while looking up hydroxylamine base, knowing the propensity towards energetic decomposition if it gets pissy, prior to first using the chemical, which occured in plants, after vacuum distillation of large quantities using alkali metal hydroxides to base the stuff prior to industrial scale vac distillation for purification/synthesis purposes (one if he recalls, was an industrial hydroxylamine production/purification factory actually, that did so, and met a rather ugly fate involving a bloody loud noise and a very large, and almost certainly very untidy and messy hole in the ground)
He is pretty glad he was not walking down the road past that one when it went off like a firecracker
Toady wonders....if certain metal salts, transition metal compounds, salts, oxides, ions, he isn't sure, but he recalls, very distantly in the back of his mind, reading something to this effect somewhere online...he may be getting it mixed up with something else, but he may not. He is just throwing it out there for safetys sake, it would be prudent to look it up first to ascertain the accuracy of this prior to using or permitting to exist in a reaction, hydroxylamine base.
. Hydroxylamine salts are stable as far as I know.
May I ask what method you were using to create the Hydroxlamine, you were recovering?
The procedure:
The end results from the effort applied 
bruhl.zip
), let me know!