dubois928

What is the solution percentage in beaker 4 (salt+vinegar=HCl)? Kenneth Anderson

When I burned a few drops of Iodine Tincture on a thin piece of aluminum, a very minute amount of light gray-brown powder was left. What is it? Thanks, Kenneth Anderson

Thanks everyone! You've all been a great help. Kenneth Anderson Well I just tried testing on the potato and remarkably the liquid on the outside, which is supposed to be the phenyl (see first post), turned out to be the H202. It reacted with the potato and created bubbles. Kenneth Anderson

Thanks! Is it possible to remove the orange dye from the h2o2? Possibly through filtration? If not, is the dye inert? Will it affect any experiments I might do with it? Kenneth Anderson

Sorry for bringing up an OLD thread, but I thought that only Americium was used in smoke detectors. Do they make smoke detectors that use Neptunium instead? Where can I get one of these? Or is it simply referring to the fact that americium decays into it? Ken

I also just noticed that the clear liquid I removed is more viscous, I have it in a prescription medication bottle and if I tip it the liquid sticks to the sides and falls back down somewhat slowly. I still have not broken open the glass vial yet. Anyone have any idea which is which? Thanks, Ken

Sorry for the double post, but I'd really like to know if what I made really is a dilute sulfuric acid, or what tests I might do to see if it is. Thanks, Kenneth Anderson

I wanted to get a higher concentration of hydrogen peroxide, so I decided to get it from glow sticks. The H2O2 is supposed to be in the glass vial and the phenyl w/ the dye is supposed to be surrounding it, but it seems that in the case of my glow stick, it's the other way around. Ether that, or the dye is mixed with the H2O2. I have not broken open the glass vial yet. The solution that was surrounding it is clear with an odor like rubbing alcohol. Any ideas on which is which? I'd hate to have the H2O2 have a dye mixed with it. Thanks, Kenneth Anderson

You mean while I was dissolving the chemical in the water? I did have a pretty hot torch flame I was using to help dissolve it; I would heat it until just before it started to boil then remove the flame. But the reaction with the sodium bicarbonate happened at STP. Ken

So then what is it? Just a simple solution? I did find where it mentions that it hydrolyzes to form sulfuric acid: http://www.jtbaker.com/msds/englishhtml/a2856.htm "This material hydrolyzes in water to form sulfuric acid, which is responsible for the irritating effects given below." Ken

Well when I came back to the solution it had formed clear crystals in the bottom of the container that stuck there when I poured the solution out to filter it. I scraped the crystals out and set them aside to dry. I then tried to see if the solution would react with sodium bicarbonate, as sulfuric acid does. It did bubble strongly for a moment then tapered off (I didn't use that much at all). So it seems to be sulfuric acid, at least a diluted one. Any thoughts? Ken

Got a lot of it from an old chemistry set. I read somewhere that it hydrolyzes in water to form a dilute sulfuric acid. Is this true? I have tried it in a small amount of water, heating and mixing along the way. I have it stored for now, but not sure if it worked. Thanks, Ken