xeluc

Yeah. Dumb...people.. eat it.... And die. If it didn;t happen so often you could give them all Darwin awards. They ARE doing the gene pool a favor..

I've always known iron to create Iron Hydroxide first when expopsed to water. Of course then that loses H's and turns into Fe2O3. Is this correct?

I've heard nasty things about Atropine. I just so happen to have a certain plant that produces the chemical. It has pretty flowers I've heard of cats dieing after eating the leaves. lol.

I for one found that very humorous. Imagine the surprise of your gas leak setting off a primary explosive

I have a question about Nitrogen Triiodide as well. I saw a video of someone detonating some. It was on a ring stand. They used a FEATHER to detonate it. So my question is, How could that NI3 even be PLACED on the ring stand. Very carefullly doesn't cut it for some reason, seeing as the touch of a feather will set it off

there is NaCl in both cups and the salt bridge, yes

You would melt NaCl at 800 C or 600 C with addition of CaCl2. Then you would pass an electrical current through the molten salt. Keep in mind that you can't let the chlorine touch the sodium or the whole apparatus will likely explode. You also can't let the sodium go in contact with water or air as it is VERY reactive. In short, it's almost impossible to do with things you find at home unless your VERY talented.

alright thanks

Could you answer the rest of my questions?

Ok. So I have two cups with NaCl in solution. I have a wide peice of string between them acting as a salt bridge. As expected. I see the blue color of Cu2+ in the solution in the cup that contains the anode. Here is where my question is. Just two seperate cups with electrolyte don't conduct electricity. that means that ions MUST physically flow through the solution to donate, take electrons.....Right? So why is only the Anode blue? Why don't the Cu2+ ions run over to the Cathode? I understand that a salt bridge is suposed to seperate compound created in the Anode and Cathode, but I don't understand how it's seperated. SOMETHING is obviously moving through the bridge. If not Cu2+, then what?

..Google Electrochemistry. Electrolytic cell and Electrolysis are also some good terms.

Alright... thanks a lot.

so, if i have oxygen and copper all the time, will the Cu2+ ions continue to disolve the copper? I put some copper in a 20 ounce bottle with some HCl and Copper Oxide (should disolve into the Cu2+ ion) and nothing really change much throughout the day. I added some H2O2 later to try and get more Cu2+ into solution. After wards, the solution is a little darker green, when the wire is no in HCl, I can see the little bubbles of liquid turn dark, and redisolve when placed ni the HCl. So can I continue to make CuCl2 in this way until not more Cl- Ions are available? (it IS kinda slow though.)

Thanks a lot, your awsome The amount of knowledge I have Amassed in such a short time is really amazing, and most of it is thanks to people like you and YT. ACTUALLY, It is VERY funny that you should mention that, I have also witnessed your dark compound. I didn't have the knowledge I now possess and didn't try to think about it, but now I realize that it's really weird for it to turn so dark when Cu+ ions are colorless... As for an explanation... looks liek your all over it.. I have no idea what else it could be. EDIT: Also, in your experiment where you mixed your brown complex with NaOH... Well I believe that your yellow Precipitate may be Cu2O. It can be anywhere from yellow to red. I have made some that was yellow/ orange. It behaves exactly like the CuO I made when disolved in HCl, Although I do remember it disolving easier. So, I'm jsut offering a hypothesis here, I'm sure you have done much more thinkign about this though. Also, lol... I had to disolve a decent amount of CuO in order to obtain visible Cu2+ ions. See in one of your experiments, you take CuCl2 + HCl + copper wire and throw it in a test tube. It becomes dark (Cu+ and Cu2+) But when it is stoppered, it goes clear. so there must be some reduction going on here. I'm going to attempt something to further my understanding of this... [math] \ce{Cu2+ + Cu -> 2Cu+} [/math] So, is the Copper acting as a reducer? I hope so, it all makes sense to me at least..

One comes out first because it has a lower solubility. Unless they have close solubility levels.. The further apart they are, the easier they are to seperate. As far as I know, the only way to make sure that the other compound does not crystalize is to measure all your stuff. If you have 100 mL of water with 2 different compounds mixed in, calculate how much of each compound will disolve in 100 mL of water at a given temp. Then, evaporate water but make sure you remove crystals before the water level drops enough for the second compound to decide to crystalize out. Or you could just guess at it..

rrrrrr If you have ONLY HCl and Cu+, I don't really see HOW it could happen, but that happens a lot, which is why I ask these questions... I threw the equation together.. I found out that H+ isn't going to be taking any more electrons. Cl- Obviously won't. The way I see it, noone wants Cu+'s electron. So, my guess is that this would not happen. It could be that some other complex is formed as a side reaction that would oxidize it, of course this is jsut a wild guess.. I do beleive H2O2 would do this though, if not, maybe in an acidic solution... So anyway I guess I'm ready for my... Correction

Thanks a lot. I added my grey stuff to some diluted HCl. At frist nothing happened. Then it rapidly cleared up into a crystal clear liquid. After doign this some more, the liquid turned bluish green. After boiling it turned green. Definatly Copper (II) Chloride. Would Copper (I) Oxide Be turned into Copper (I) Chloride on addition of HCl or would the HCl further oxidize Cu+ to Cu2+

So If I cool all the reactants than I should get Cu)OH)2... right? Well, I jsut bought me some HCl I will do some testing tomorrow. Right now I have to worry about what I'm going to do about my radiator that jsut decided to take a shit and spill antifreeze everywhere... EDIT: Also, would you know how to turn CuO into Cu2O? Maybe a strong Oxidizing agent? Hope that doesn't sound stupid, It's a guess. EDIT 2: just realized, I wanna go DOWN an oxidation state. Now I have no idea. Reducer? lol.....

Yeah, all the colors look the same. My blue solution WAS a lot darker. after leaving the precipitate to settle, it lightened up considerably. It is definatly not a Cu2+ solution, the color is much darker. I did this experiment once before and got what I thought was Copper Hydroxide. It does turn dark after heating. But this turned dark right away. There was no heating involved. So how did the Cu(OH)2 Decompose?

what would too much NaOH have produced?

I figured that when I mixed these compounds that I would get a solution of NaCl and a Precipitate of Cu(OH)2. Instead, I have a blue solution, and a dark dark Grey Precipitate. Can anyone explain this? Undoubtably my CuCl2 is slightly contaminated, But only slightly. There is as much grey sediment as I put CuCl2, so I don't think this was due to contaminents. (An Excess of NaOH was used.)

I'd imagine chrome plated steel as the website says that the ceramic is slower at grinding, although produces purer contents. Of course, I'd need to know why Lead is such a horrible Choice. Quartz apparently works ;-)

i mean like.. Cu Fe Ni Zn just the simple ones

I'm sorry if this is obvious.. but can you displace ANY hydroxide with HCl? If so, I can finally do a test I have been wanting to do.

lol... @Jdurg Thanks! I'll try that. Would like. Pat Catans be good? What's a store I could use?