Thread View: rec.juggling
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Started by Jay
Sat, 09 Jan 1993 07:36
Coloured flames
Author: Jay
Date: Sat, 09 Jan 1993 07:36
Date: Sat, 09 Jan 1993 07:36
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Does anyone know an easy way to colour flames? We have some: Strontium Chloride, Barium Chloride, Copper Sulphate, and Calcium Sulphate. Unfortunately, hydrocarbons (eg kerosine/parrafin and lamp oil) are not solvents for these compounds. However, some of them are soluble in ethanol (cf methylated spirits) but the flame is barely coloured. Since strontium and barium are supposed to give very bright flames, we were wondering if anyone had done this before. BTW, what's the address of moocow? pyro
Re: Coloured flames
Author: maize
Date: Tue, 12 Jan 1993 17:55
Date: Tue, 12 Jan 1993 17:55
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In article <1ilv9tINNk6n@uniwa.uwa.edu.au>, pyro@gu.uwa.edu.au (Jay) writes:
> Does anyone know an easy way to colour flames?
> We have some:
> Strontium Chloride, Barium Chloride, Copper Sulphate,
> and Calcium Sulphate.
>
> Unfortunately, hydrocarbons (eg kerosine/parrafin and lamp oil) are not
>solvents for these compounds. However, some of them are soluble in ethanol
>(cf methylated spirits) but the flame is barely coloured. Since strontium
>and barium are supposed to give very bright flames, we were wondering if
>anyone had done this before.
>
> BTW, what's the address of moocow?
>
>
>pyro
Moocow is moocow.cogsci.indiana.edu.
Strontium Chloride is listed as being "very slightly soluble" in absolute
ethanol. This is not enough to give good color. I don't like Strontium's
color as much as Lithium. Lithium Chloride at around 3M will give you a
strongly colored red flame.
Throw the Barium Chloride away. It's not soluble and too toxic. Just
use Boric Acid (usually you can get it at a grocery store or drug store).
It is very soluble an produces a good green. Add a little Copper Nitrate
for more intensity.
The sulfates are to be avoided because of the burning sulfur smell
you'll end up with. Calcium's only going to give you a normal flame color
anyway. Copper almost always gives green. It is the ion CuCl that emits
blue -- but it is unstable at temperatures above 1200 oC and degrades into
the green emitter CuOH. By using CuCl2 I always get a green flame until
the torch has almost burnt out -- then for a few seconds the blue color
appears. If you could think of some way to control the flame temp you
could get a great blue color.
This stuff will corrode your wicks and torches. Also don't use different
colors on the same torch. Once you've use a torch for a certain color only
use it for that color from then on. Otherwise you end up with ugly
mixtures of colors.
_______________________________________________________________________
Phillip SanMiguel Purdue
maize@bilbo.bio.purdue.edu Institute for
Molecular "We'll do anything
Bennetzen Lab Plant for funding."
Science
_______________________________________________________________________
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