Darkblade48

I believe terepthalic acid can be extracted using a simple saponification reaction, with ethylene glycol as the solvent.

Boiling would most likely speed up the decomposition of the peroxide rather than purifying it.

Not magnesium, but manganese (dioxide). Breaking down hydrogen peroxide is much easier than breaking down water, as YT2095 said, you could use manganese dioxide, or failing that, you could use your own blood, as it has an enzyme (I believe it's catalase) that will break down the peroxide to release oxygen. As for hydrogen, dissolving metal in acid is an easy way to generate hydrogen gas.

Nope

Wouldn't the flame temperature be dependent on the portion of the flame you are measuring (i.e. base of flame vs. tip of flame) and the amount of air/fuel ratio you have as well (i.e. lots of oxygen for a little bit of alcohol vs. minimal oxygen for a large volume of alcohol)?

Regarding the comment sunspot made, AFAIK, if you grind popcorn into a paste, it will no longer pop. The reason popcorn pops is because the water in the kernel is heated (while it's in the microwave) and coverts to steam. The steam has no where to go, so the pressure builds up, and when the kernel has too much pressure, it pops, and you get your fluffy, white popcorn.

Most likely not. I believe normal nitrating conditions (of course, you'll need another reagent, not just HNO3 to nitrate the ring) will only give you a maximum of two NO2 groups on the ring.

Some of these questions are better left unanswered unless you do some research yourself

Try performing a Kolbe carboxylation on the phenol first and then carrying out the synthesis of acetominophen with acetic anhydride. It's more efficient, and on top of this, you won't have to worry about nitrating phenol and then having to separate the ortho and para products.

Here's the order that I copied from Wikipedia Functional group Cations e.g. Ammonium Thiocarboxylic acids Selenocarboxylic acids Sulfonic acids Sulfinic acids Sulfenic acids Carboxylic acid derivatives Esters Acyl chlorides Amides Imides Amidines Nitriles Isonitriles Aldehydes Thioaldehydes Ketones Thioketones Alcohols Thiols Selenols Tellurols Hydroperoxides Amines Imines Hydrazines Ethers Thioethers Selenoethers Peroxides Disulfides

I read that and almost spit out my orange juice....

Then you'll probably have to pay a premium for sterilized test tubes, as I don't see those very often. On top of that, once you use your test tubes once, you'll have to throw them away, since they're no longer "pure and clean and not used". I suggest you can donate them to various users of these forums, though.

Agreed. I didn't get hooked on chemistry after seeing some explosion on TV/movies/whatever. This shouldn't be the basis for your chemistry fascination.

Are you asking what will oxidize potassium? Your question is vague

What are you doing that specifically requires new test tubes? I don't see why you can't use old test tubes, just clean them out well with dish detergent or something.

From a reputable chemical supplier...or other sources if you happen to have them.

woelan is correct, this will be nearly impossible to extract a good, pure sample of what you want.

You can just buy Magnesium sulfate, rather than make it from its constituent parts...

I'm not sure what you read, but YT2095 said "Potassium Aluminium Sulphate (AKA Alum/Bitter Alum)"

Well, according to Chemdraw Ultra, the IUPAC name of this molecule is: 3-hydroxy-2-methyl-4H-pyran-4-one