In article <
hj3j88+7erb@...>,
halamander <
frog.aye@...> wrote:
> Roger, I think you will find that this is not a particularly effective
> technique. HCl in its native state at room temperature is a gas, what
> you purchase is an aqueous solution of it. I think you will drive the
> HCl out of solution before you evaporate much of the water, thus leaving
> yourself with a weaker soln.
Certainly will.
It's 40 years or so since I did any chemistry but I seem to recall
"drying" organics with anhydrous Calcium Chloride, maybe it would work in
this case. Being a Chloride it would not react with the HCl. However, even
if it works how are you going to ascertain the resulting strength of your
acid?
Better to get the required strength, or higher, in the first instance.
--
Stuart
http://www.torrens.org.uk/ZFC/gallery/winsor.html