Quote: Originally posted by Antiswat | i somewhat randomly found a way to make Ba(ClO3)2 ..
the procedure was following
ammonium tartrate and potassium chlorate is mixed, this produces nearly insoluble potassium tartrate and ammonium chlorate |
Ammonium chlorate has a low solubility itself. (most ammonium salts tend to be very soluble, but ammonium chlorate and perchlorate have anomalously
low solubilities) This is likely to interfere with the separation, since some ammonium chlorate will likely precipitate out with the potassium
tartrate.
Indeed, it is fairly easy to precipitate out ammonium chlorate from a mixture of sodium chlorate and ammonium chloride.
One note of warning for those who may not be aware: NH4ClO3 has a much lower stability than NH4ClO4. Ammonium perchlorate is perfectly safe here, but
there may be some explosion hazard from the NH4ClO3. Because of safety, it is often recommended not to mix ammonium compounds with solutions
of chlorates, but it can be a very useful route to make metal chlorates. I would just suggest using some caution, and to redisolve the ammonium
chlorate precipitate (after separatation) back into another solution of water as soon as possible. Either use the solution quickly, or keep it out of
sunlight.
While many chemistry books recommend keeping certain light-sensitive reactions away from sunlight, what they often fail to mention is that exposed
fluorescent tubes not covered by acrylic diffusor panels are just as bad (I mention this because more and more people are using those awful spiral CFL
bulbs that leak out ungodly ammounts of UV radiation)
[Edited on 10-3-2013 by AndersHoveland] |