latentheat

http://www.humanmetrics.com/cgi-win/JTypes2.asp I'm INTP (Introverted iNtuitive Thinking Perceiving).

I had something similar happen to me when I stupidly used 120 V AC on a sodium chloride solution. I was using two carbon rods as electrodes. The instant I turned it on, there was arcing like crazy in the beaker and steam pouring out of the beaker. The solution was boiling from the heat created. I unplugged it as quickly as I could. The room smelled horribly of ozone for awhile.

Keep in mind that most chems can act as either in different situations, but that aside, here's some things... Common oxidizing agents: halogens, permanganates, perchlorates, nitrates, peroxides Common reducing agents: active metals, Alkali metals bonded to hydride complexes

An equal mixture of the two optical isomers of a substance: dextrorotary and levorotary. When the optical isomer is important in a particular situation, the name of the chem will include the bolded part. The dextro and levo rotary refer the the direction the molecules rotate plane polarized light.

If that works it would likely result in really, disturbingly fine powder.

You could basically say that ox state just tells you how many bonds have been made, and only reflects lost or gained electrons in ionic bonds.

Calcium carbide is really fun stuff to play with. One time I told my mother to hold a piece of it and she had wet hands, she wanted to kill me

I'd imagine it would react with zinc quite well if the zinc was powdered and mixed in the correct molar ratio with sulfur and ignited. The result would be zinc sulfide.

Barium sulfate is actually given to people in suspension form before various tests on the colon. It's safe because its insoluble.

Carbonates get the pH high enough that you get the slippery feel on your hand. Does anyone know exactly how high the pH can be raised with carbonates?

You could electrolyze a sulfide salt resulting in this rxn occuring at the anode S2- ---> S + 2e- Or you could just buy it at the hardware store in the gardening section or at some pharmacies for treatment of acne. It's dirt cheap.

Sodium bisulfate, sold at every pool supply place as solid pH down chemical. It's basically partially neutralized sulfuric acid.

NaCl + NaHSO4 ---> HCl + Na2SO4 Heat the reactants and collect the HCl(g) in a syringe and then dissolve it in water to get hydrochloric acid.

You could synth copper(II) oxide by reacting sodium carbonate or bicarbonate with copper sulfate. Then roast the copper carbonate ppt. Form the green tetrachlorocuprate(II) complex by adding a small amount of copper sulfate to a saturated soln. of sodium chloride like in my avatar. Drop some aluminum metal into this solution and witness a neat redox reaction that ppts copper metal.

Although what bulldullwraagh is stating could very well get him in trouble if it's not true, it just may in fact be true. Look for a thread concerning kno3.com on another chem forum (I won't name the forum here, but you can figure it out). Jdurg : it's diethylamide probably, because LSD is lysergic acid diethylamide. For unaltered ethanol (not dry though) buy Everclear brand, but it's expensive (alcohol tax).

I think the double replacement reaction that occurs would cause the bicarbonate anion to break down to carbon dioxide and carbonate anion. I've observed this when getting copper carbonate from reacting copper sulfate with sodium bicarbonate. I'm not sure why this happens though.?

It probably is partially caffeine, but you won't get it all unless you basify. Some of the caffeine will remain in solution complexed with the organic acids. If you raise the pH really high the caffeine will go freebase and it will all ppt after awhile, because freebase caffeine is only slightly soluble in cool water. The method Yggdrasil posted is based on this idea.

Not every chem experiment has to have an exact purpose. What's the point of tossing sodium into water, it just makes sodium hydroxide, which you can buy anywhere. Same deal. It's a fun thing to do. Given pure reagents were used, why not consume the product...it's no worse than popping a vivarin or stacker 2.

Thanks for that. Even easier than an a/b extraction.

If you want to post a procedure that would be appreciated. I'm assuming with tea you can leave out the defat step with no problems. My only thing with tea.... how significant is theophylline contamination?

Yes. Lower barometric pressure = larger pressure gradient. Larger pressure gradient = greater air transfer needed to re establish equilibrium = higher winds.

barometric pressure in the center now down to 902 mb. Anyone in new orleans who won't leave will DIE, plain and simple. This is not the time to play games.

I tried extracting caffeine from tea and coffee several times with poor yields. I think my biggest mistake was using naptha - don't use naptha it really sucks at pulling alkaloids out. I'm gonna try it from coffee at some point with a defatting step with toluene (after acidification with HCl), precipitation of tannins w/ calcium ascorbate, basification and pulling out the freebase with chloroform. Think it will work? I know it's really cheap to just buy but it'd be cool to get good yields of relatively pure crystals from plant material. LOL @ dandygurl...I don't think chewing coca leaves is legal in the US bc of the cocaine content. I'd imagine it would be a great cold remedy though. Numbing of the sore throat and nasal decongestant effects from the CNS stimulation. I'm addicted to caffeine, and it will keep you up ALL night in sufficient quantities.