budullewraagh

i believe he was kidding. phosphorus, hands down

favourite metals: gallium, bismuth, osmium/indium, neodymium, cesium, strontium, indium favourite nonmetals: phosphorus, fluorine, bromine, iodine

yes, the enzyme is catalase. it catalyzes the decomposition of hydrogen peroxide, which is indeed formed in the cell sometimes as a product of respiration.

i have to disagree. when i make chlorine gas, i boil bleach. the first salt to precipitate is the Ca(OCl)2. upon further distillation i was left with reasonably pure hypochlorite.

i know how soluble hydrohalic acids are in water. i also know that you can oxidize hydroiodic acid with hydrogen peroxide

h2so4, that isnt true; think of schrodinger's cat. half-life of 210 At is actually 2 minutes. if you get an active enough alpha source you can produce enough of it to see; it's black. in fact, researchers have produced enough to perform some tests on it.

it will result in HI and KCl. the HI+H2O2 will result in I2 and H2O

astatine doesnt exist

mods, please move this to the homework section... and never post homework here

no, you need to acidify, THEN use the peroxide

you could bubble chlorine gas into a bromide solution. you could also use H2SO4. really important factor: MAKE SURE THE H2SO4 IS ONLY 25% OR SO. anything above 30% and youre pushing your luck. you dont want H2S to be evolved. btw, jdurg, while it isnt smart to mix H2SO4 and H2O2, it is smart to do the following: NaBr+H2SO4-->HBr+NaHSO4 2HBr+H2O2-->Br2+2H2O

so you just want to corrode metals? HF, H2SO4, HNO3, HClO4, HMnO4 come to mind

no, HI is definitely reddish. my salt was pure, reagent grade KI. there may have been a few ppm Br, but certainly not enough to produce such a great amount of the red gas. i saw triiodide in the solution, but the H2SO4 dehydrated the products on contact AND reduced to form SO2 and H2S. i definitely saw HI gas though, which can easily be reddish-yellow

oxidizes bacteria, etc?

which reminds me that the hydroiodic acid i have prepared has been yellow. except once when i produced the gas, which happened to be reddish. what do you suppose the red comes from?

"Probably not. NaOCl forms when a solution of sodium hydroxide is exposed to chlorine gas. The chlorine gas then forms sodium hypochlorite." just a little more info on Cl2+NaOH: NaOCl will be formed, but small amounts of NaClO2 will be formed depending on temp. in boiling solution, NaClO3 is formed. "If the reaction occured under basic conditions (NaOH), the making the solution acidic will reverse the reaction forming chlorine gas and sodium hydroxide. This is what Bud and I have each done." second most unintelligent error i have made in my lab work: i titrated my fuming supersaturated HCl with draino. didn't happen to notice that NaOCl was in draino along with the NaOH. and yeah, it neutralized the HCl...but got rid of the anion (via oxidation) in the form of Cl2. and i was doing this right in front of my face. coughed for a good 3 minutes or so. surprisingly, the pulmonary edema that ensued was not so bad, and on my next exposure to Cl2 i wasnt affected too much. "[update] i am now done with the iodine making. IT was smelly, but it worked. I have iodine (i think alot) in a bucket. After collecting the sludge it reeks of chlorine. Due to the fact there still the water left after the chlorine was bubbled through the iodine. WHat is that stuff that was made and why does it reek?" pleeease tell me you have pics. make sure the iodine stays wet; otherwise it will just sublime. it may smell bad due to the chlorine, but probably because of the iodine. i remember my products smelling bad.

that's pretty sick

sodium iodide definitely has been known to be, on occasion, somewhat yellow. it's highly soluble and deliquescent

that sounds like 8th grade to me (just before high school); we did "physical science"

your name refers to nitroglycerin, right? what sort of chem is it that you have done?

i've handled KOH. it's not so bad at all. the powder smells somewhat ammoniacal. it dries the skin and is irritating. wet conc KOH on the other hand is very, very caustic. i got a drop on my arm, didnt notice, then suddenly i felt a crescendo of searing pain. the fact that your KMnO4 was wet and conc plays quite a role in its oxidizing powers when it is placed on something dry

i dont agree, yt; iodine is a lot easier to oxidize than chlorine. i wouldnt be surpirised if you got iodite instead of hypoiodite. of course it depends on how hot the solution is, but i know you can get iodate if you do that in boiling solution.

do you realize that if you went to colombia and said "hi, i'm your new dictator" you'd get shot by a few hundred thousand druglords and their collective possie?

i suggest books before you start playing around with expensive, potentially hazardous chemicals

"The only way to generate chlorine gas from Cl- ions is via electrolysis" or if we're considering HCl, one could use a strong oxidizer such as permanganate, chromate, dichromate, manganate, etc. btw, jdurg, you'd have a bit of HCl gas, plus there's the Cl2. are you sure the stopper isnt corroded by these gases? "how could i utilize the common and cheap NaCl to make me some Cl? also, im not sure wat u were doing in that picture: reacting the hypochlorite in the beaker with something or planning to? planning to distill it and condense the stuff coming out the end?" electrolysis. i put the hypochlorite in the beaker, pulled the funnel up just enough to add the conc HCl and dropped the funnel immediately. Cl2 was produced and brought through the tube under the surface of the I- solution. it works well; there was a very miniscule amount of HCl involved, if any, and the fact that the Cl2 was, to small degree, wet didnt make a difference.. just make sure the tube stays submerged in the I- solution, lest you spew Cl2 into the solution and push the crucible/tube away from one another, leaving you with Cl2 and only the initial amount of I2.