Hello,

I have some old Co(NO3)2.6H2O stuff, clumped together. An idea how
much more water (in excess of 6H2O) it could take?

Thanks,
Arman

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On Sep 21, 12:09 am, Rich Murray comcast.net> wrote:

I'm a first-year student in Pharmaceutical sciences with a background
in Chemistry. My professor has posed this question to me:

"To make water-soluble amines more soluble (and thus more orally
bioavailable) medicinal chemists routinely prepare salts but they
avoid HCl salts. Why?"

It has me a bit baffled, since I know that many pharm formulations
utilize HCl salts, as HCl is stable, non-toxic, already present in our
stomach, etc. I can't think of why it would be avoided. This was
from a lecture on ionic equilibrium and pH, but that hasn't seemed to
help my thinking any.

Thanks!

Dear all,

I have water samples (regular, run of the mill dilute river water)
that I plan to analyze for alkali and alkali earth metals using ICP-
OES. Some of these samples are in 1%% HCl matrix, which may cause
corrosion to the equipment and, for all I know, cause interferences.
Would I be better off adding concentrated HNO3 to my samples that are
currently in 1%% HCl or just leaving them as are? I'm hoping that
adding the nitric acid will convert the Cl- to Cl2(g) but I'm not sure
if that will actually happen. My concerns are mainly about
interferences and possible matrix effect of the HCl, but also about
corrosion since I'll be running a lot of samples. Any insight or
advice is warmly appreciated.

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What is "normality", as in a 1N solution? And what are "equivalences"
and "formals"? Why can't we all just use molarity? What are they used
for?

Thanks!

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