Inorganic Chemistry

I've devised a preliminary experiment for a nickel catalyst. First I make hydrogen through electrolysis and collect it in a test tube. Now this test tube is special because I've rigged it like a mini fuel cell. To stop the hydrogen from coming out of the test tube, I made this little assembly that ressembles the MEA in PEM fuel cells. It's a nickel plate with a plastic sheet under it and a wire connecting the catalyst exposed to the hydrogen to the plastic exposed to the air. Theoretically, the hydrogen should get split by the nickel into its protons and electrons. The protons go through the plastic, but since the electrons can't they take the wire to make it…

I month ago or so I was cooking some Calcium carbonate to make calcium oxide, I was thinking is there a eay way to purify this? Because I've I've been using everyday limestone (thank council workers ) I'm happy to grind up the Oxide then do what ever using water etc then re-cook it again. While Im on the subject of cooking, A while ago I was thikning about cooking Barium carbonate, this needs about 1300C, as far as I know this will break down to Barium peroxide, can anyone confirm this? I can cook this easy (new and improved charcoal cooker, even clay gets melted, lol. ) Anyway I'll be back in a day to read (grrr library comps, lol. )

Do latex gloves stop Mercury from getting absorbed through to skin? Just wondering... if they don't then can someone tell me what type of golves would? And incase you ask no, I'm not using mercury (I only have one sample in my element collection and its sealed, thankfully), I'm just doing some research for school Cheers, Ryan Jones

ok sure we have lots of aluminium oxide around us, drinks cans and such, but how can i get pure aluminium and how can i get so that it will not react with oxygen to for aluminium oxide??? electrolysis??? reducing agent??? and ideas any one???

Anyone has the structure of it? or link? And what is the pH value of this molecule?

I'm trying to find some information on trends in the chemical properties of MgCl2, CaCl2, SrCl2, BaCl2, like their pH, their solubility in water and most important of all on their water of hyrdation but I can't find any relevant information or serious explanations... !!! so if anybody can help i would be really grateful because i have to do my lab write up for tomorrow

who knows how to make silver nitrate out of nitric acid and silver, i mean the exact method eg how much silver to add to how much nitric acid and how to get silver nitrate crystals out of the silver nitrate solution,

How much does graphite plates cost and where can I get them?

Is hydrogen bonding in water the result of the hydrogen bonding to the bonded electrons of oxygen or is it a mutual things due to electrostatic attraction between oxygen and hydrogen. In other words, a one-way potential or a two-way potential.

I was just wondering...Since HNO3 is made from KNO3, would it be possible to do the opposite (HNO3 To KNO3)?

Hi, I was wondering if anyone could help me out here. My chem book says that there are 88 naturally occuring elements... but other places say 90, or 92, or 83! Does anyone know what the 88 are and how they distinguish "naturally occuring" ? Thanks!

today I`ve managed to extract the element Boron from Boric acid, so for those element collectors out there that couldn`t be bothered with Ebay here`s How. 1`st you`ll need a large pyrex test tube (don`t use your best test tube for this, it`s a little messy. add a spatula of boric acid, and then heat it over a bunsen until it starts to bubble, you`ll notice moisture being driven off too, keep this going until the bubbling stops and try to get the mixture around the sides of the bottom of the test tube (this will help later when you try to get it off), the now boron oxide will look similar to the glass. allow it to cool and make sure no water condensation gets back int…

Why does NO+ have a triple bond? The formal charges would be the same with 1 bond and two lone pairs on each atom, so wouldn't it be just as stable?

Ive thought about this before, but never really bothered about it. If the valency of Nitrogen is 3 and oxygen 2, how can the two form NO and NO2? Do they have orbitals that bond together, as between layers of graphite, or exist as dimers, or is there something weird going on? I'd really appreciate someone helping out!

some cars have Nitrous Oxide (N2O or NOS) to boost acceleration, but that stuff hurts your engine ... so i was thinking, wouldn't it be smarter to use pure oxygen (or very high oxygen concentration in air) in a tank and use that for an extra boost.. you know, mix it in the turbo-charger, so that you get the 20PSI mixture of mist gasoline + lots of oxygen = a he!! of a boost:cool: i know it will cause the temp to rise, but hey, you don't use it all the time, and if you get an intercooler it should be good!

Can anybody tell me what primary standard is usually used to standardize NaCl?

Hi, I've got some Sodium percarbonate (oxy plus cleaner, you know the stuff). It was so slow to give off any oxygen at all. So I did some reading in the time I could and its like H2O2. So I think I'll try the same thing you do to get the O2 out of the the peroxide. I added some manganese dioxide (back stuff in batteries) and this worked pretty good. But I only got about 1 balloon full of gas from about 30g (2 scoops) of the sodium percarbonate. And I'm not to sure on how pure this is. Its higher then nomal air but not That high as H2O2 will give you. So to cut to the point, is there a better way to get the O2 out?

The element copper remains a very special element to me. It keeps on giving strange results and I want to post one over here again. It is a really simple experiment, just add two chems to each other. In jsatan's words, I saw a "little thing", which I cannot neglect. The "little thing" here is that the copper (II) chloride turns very dark brown, almost black in the concentrated acid. When water is added, then it dissolves again and the results become predictable again. http://woelen.scheikunde.net/science/chem/riddles/copper+h2so4/index.html If anyone over here has an explanation for the observation, then I would be pleased to know.

Why does Aqua Reiga dissolve Gold but neither of its compoents does? There must be a reason - as far as I knw neither Hydrochloric acid nor Nitric Acid dissolve gold and if they do then they don't to it at any impressive rate. So does anyone had a reason why Aqua Reiga does? Cheers, Ryan Jones

Whats the highest (feasable) concentrations of Hydrochloric, Nitric and Sulphuric Acids? I have Nitric Acid at 70% conc. I have heard you can make Sulphuric Acid 97% conc. by boiling the sulution untill you stop seeing a white smoke. No idea abut Hydrochloric Acid at all... Anyone have any ideas? Cheers, Ryan Jones

In ionic reactions a new ionic compund forms, sometimes a percipetate or just a solid. I want to know why a reaction happens and sometimes doesnt. For example: Silver Nitrate and Sodium Chloride react to make new ionic compounds- silver chloride and Sodium nitrate. But how is it determined if reaction will happen? Are the produced compunds somehow more favorable to make than the starting 2? If you mix NaCl and Kno3 no new compound is formed- why do some react and some dont? EDIT: I guess Nacl and KNO3 do react, but the point being why some dont and some do.

how dan i make phosphorus, the stuff off of matchheads??? i have heard you can make it with urine... anyone else have anying to say??????/

Hi, I was seeing what colours I could get whne I burned some chems with sodium chlorate. I added copper sulphate to this mix with some sugar and it gave me a great blue purple, I noticed a very yellow colour in my mixing dish after I tried the Calcium chloride. So I found out what it was. If I get some Calcium chloride and mix this with copper sulphate it gives me a strange yellow with will turn green ish. but if I add some water it goes clear, the blue and the yellow. Whats going on here?

I make mixtures or KClO3/sucrose for use in my small bang firecrackers. I calculated the enthalpy of reaction for KMnO4 + sucrose and found that it releases slightly more heat than the chlorate mixture. When i lit the permanganate firecracker however, it just went up in flames. I assumed that, due to the large particle size of both my granular permanganate and sucrose, the reaction didn't take place fast enough to burst the container. Would it be possible to stir my mixture in a very little amount of solvent so that the mixture is more intimate? Or can the dissolved permanganate oxidize the sugar in solution? Is permanganate and sucrose simply not a good bursting mi…

If you light thermite, does anyone know of anythin you can do to stop the reaction?? or is 2500+ degrees of molten iron simply unstoppable:confused: