BlazeBall - 27-4-2011 at 16:32
Would there be any significant reaction between zinc chloride and sodium hypochlorite in an aqueous solution of 0.5% and 0.1% respectively?
Ozone - 27-4-2011 at 19:34
Why don't yout give it a try?
O3
ScienceSquirrel - 28-4-2011 at 06:22
There is no reaction between zinc ions and hypochlorite ions.
Zinc cyanide in waste plating solutions is routinely treated with hypochlorite to destroy the cyanide and free the zinc for precipitation as the
carbonate.
This is then separated out and sent for disposal.
bbartlog - 28-4-2011 at 06:59
In that case though one would expect the zinc to be precipitated as hydroxide by the NaOH present, no? With enough ZnCl2 I bet you could evolve
chlorine gas, too... concentrated, it's acidic. But a 0.5% solution probably wouldn't do the job.
ScienceSquirrel - 28-4-2011 at 07:13
You are right about the hydroxide, that is what drops out;
http://www.wastech.com/pages/zinc-removal
I doubt those solutions would evolve chlorine gas when mixed, they might behave like the chlorine water of old 
AJKOER - 23-5-2011 at 19:35
I would not rule out the possible production of some oxy-chloride which are commonly created with the metals Copper and Lead (which also has an
oxy-nitrate).
Any chance the compound is white, amorphous zinc oxychloride, 2 ZnCl2,3 ZnO.11 H20?
AJKOER - 24-5-2011 at 14:51
Another possibility is:
2 NaClO + ZnCl2 = 2 NaCl + Zn(OCl)2
namely, Zinc Hypochlorite, which exists and per Wikipedia was original reported per the now defunct Groliers' Encyclopedia as being formed by heating
a water solution of ZnCl2 upon which the Zn(OCl)2 solid forms. I suspect the O2 in the water oxidized the ZnCl2. In our case, NaClO is the oxiderizer.
AJKOER - 24-5-2011 at 18:27
I hate to say that I am the best, but honestly, I just came across this reference that establishes that BOTH of my opinions expressed in this thread
(even though one might think there are mutually exclusive) are in fact CORRECT.
REFERENCE
"A comprehensive treatise on inorganic and theoretical chemistry", Volume 2 By Joseph William Mellor
LINK
http://books.google.com/books?id=7XoGAQAAIAAJ&pg=PA274&a...
Extract of Page 274
" A. J. Balard likewise formed a soln. of zinc hypochlorite by the action of hypochlorous acid on zinc oxide. The soln. behaved in an analogous manner
when the attempt was made to concentrate it in vacuo. A. J. Balard also prepared a similar soln. by double decomposition of zinc sulphate and an
excess of calcium hypochlorite. G. Lunge and L. Landolt obtained a soln. of zinc hypochlorite by a process similar to that employed by P. Grouvelle.
They found that some chlorate was formed when working at 15°, and still more at higher temp. The zinc hypochlorite was found to decompose into zinc
chloride or oxychloride and oxygen. Very little chlorate is present in the soln. obtained by decomposing zinc sulphate with a soln. of bleaching
powder. The soln. of zinc hypochlorite is less stable than that of the calcium or magnesium salt. R. Bottger found that hypochlorous acid has no
appreciable action on zinc."
From this it is evident a double replacement with ZnCl2 and NaClO most likely does produce Zn(OCl)2 and further, the Zn(OCl)2 is unstable decomposing
into zinc chloride or oxychloride and oxygen, the latter being my first speculation.
hkparker - 24-5-2011 at 21:36
@AJKOER please don't post multiple times repeatedly, just use the edit function. Also if something accidentally gets posted twice please delete it.
Thanks for the reference.
AJKOER - 25-5-2011 at 04:43
Sorry, I a new guy.
I just figure out how to delete, namely check DELETE box and proceed to re-edit. This apparently works, although normally re-hitting the EDIT button
just puts me in an infinite loop with no-edits.
I will delete this message also for more practice!