[NewCandle] crystallization weight change transients

[Keith Nagel]

Hey Nick,

I've just done some quick searching on alt.chem, and here
are some suggestions besides the usual ones we have been
discussing ( sodium acetate, thiosulfate )

baking soda(?)
calcium gluconate
citric acid

posters claim that most organic salts will readily
form supersaturated solutions, so one could cruise down
all the usual edible suspects. Sugar is mentioned,
but poster claims that it's kind of hard to get it
to crystallize out. I've never worked with this
before, so you've tapped me out on specifics. I
don't even really know where to go to find out,
other than asking practicing chemists and hoping
for a hit. 

I think you're correct about the anhydrous salt,
in yea olde days ( and these days around my lab )
it's usually the case that more complex chemicals
are made up from scratch. If you don't get rid of
all the water, you often end up with mixed hydrates
which make measurement difficult. And as I'm usually
heating off the water anyway, I tend to go all the way and
reduce the salt to the anhydrous state.

BTW, is it just me, or is 21st century America looking
like the Middle Ages with indoor plumbing? Just a thought (grin).

K.

K.

-----Original Message-----
From: newcandle-bounces at ipdiscover.com
[mailto:newcandle-bounces at ipdiscover.com]On Behalf Of Nick Reiter
Sent: Wednesday, September 27, 2006 8:34 PM
To: New energy for the new world.
Subject: Re: [NewCandle] crystallization weight change transients


Hi Keith,

Red Devil is indeed up there on the ones that comes to
mind immediately - and yes, it is my experience (as
well as understanding) that what evolves heat on
solution would absorb it on crystallization.

I was reading about simple binary ionic salts today -
it seems they are typically pretty hard to get into a
supersaturated state.  NaCl apparently has nearly the
same solubility at 100C as it does at 20C.  Not sure
about hydroxides like lye.

I was also thinking sucrose sugar this afternoon.  Now
that would put a chiral twist on the whole matter, eh?

The three parts  hypo-S to 1 part water was how I ran
the first hypo-S run.  Thats what gave me only 2
milligrams of weight loss.  It is far below maximum
solubility though... yesterday, when I was getting the
4 mg type deflections, I was more like 5 to 6 parts
hypo-S to water.  UNLESS way back in the day they were
going with an anhydrous version... the natural
hydrated version is a pentahydrate.  If they were
using anhydrous, 3 to 1 might just about work out to
where I was at by trial and error at maximum.

N

--- Keith Nagel <NewCandleAdmin at ipdiscover.com> wrote:

> Fair enough on the hot air thing.
> 
> As concerns the endothermic crystallization,
> wouldn't
> it be the case that salts that are exothermic on
> dissolution would be endothermic on crystallization?
> The devil we know, comes to mind, although that
> would
> be rather bothersome to work with. How about
> ordinary
> table salt?
> 
> Here's another question. The reference Colin
> provided
> describes a solution of 3 parts by weight of the
> salt
> to one part water. How close are you now to this
> ratio?
> 
> K.
> 


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