Inorganic Chemistry

I was just wondering if Barium Hydroxide + Ammonium Chloride would be a dangerous endothermic reaction.

I know that when iron crodes, it also means it rusts... however, I thought, as redundant time has gone by, iron will react will oxygen apparantly, but in my textbook, it says it only rusts with oxygen+water...why????

Does anybody know of a safe and easy way to make CS2(l)? I needed to extract sulphur.

Hi there all you fellow chemistry fans! I was recelty reading a chemistry book in school, it was quite new too. I saw a vague reference to 2 chemicals I have never heared of before: Sodium Triiodide ([math]NaI_3[/math]) and Nitrogen Triiodide ([math]NI_3[/math]) Does anyone know what these do and how I would make them? Please note: If they are very dangerous then please say so as I don't want to endanger myself or someone else. Cheers, Ryan Jones

How is oxygen dissolved in water?? Since oxygen is neutral, ie, formed by covalent bond, it shouldn't have any charge, right??

Even acid has OH- ions in it...., but how can we measure how many OH- ions there are... secondly, how can we determine how many ions/molecules a solution can dissolve?? esp with water as the solvent. Eg, how many oxygen molecules, hydrogen ions, halogen ions, etc... can water dissolve? Any help?? thx alot

I hope to receive a liter of triethylamine [MATH]N(C_2H_5)_3[/MATH] next weekend. I would like to make some quaternary ammonium compound by adding a fourth ethyl group to this, such that I get ammonium ion with all four H's replaced by ethyl groups [MATH]N(C_2H_5)_4^+[/MATH]. Such a quaternary ammonium ion is large and fairly unreactive. This opens up ways for preparing salts of complexes (e.g. the triiodide as mentioned in another thread), which are otherwise not accessible. Any organikers out there, who have an idea how such a methyl group can be attached to the triethylamine, perferrably using reagents, which are available for the home-chemist? Does anyone see …

How can you tell which is a stronger reducer? For example, the question was which is the best reducer: Iron, Osmium, Ruthnium or some other metal. The point is, how can you tell? I kno alkali metals are good reducers and as they get bigger they get even better, but does that have a correlation to all of the other metals? btw the answer was Fe

Hi everyone, Xenon(II) Fluoride [math]XeF_2[/math], how did that make it? At GCSE level we were taught that any atom of a group 0 element is stable, it has a full outer election shell. I guessed they would cdut things out to make things more simple but at AS we were taught that some elements E.G. Sulphur could expand their octlet (Speeling is probably wrong). Is it the same principal for doing this with a noble glass? Also can you give me any information on the reactions such as preassure required, catalyst required etc. Are there any elements that have no known compounds at this point in time? Cheers, Ryan Jones

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 n…

How can I do it?

Will SO2(aq) be changed SO4 2- ion [sO2+H2O<->H2SO3, (SO3 2- + H2O->SO4 2- +2e- + 2H+,I2+2e- ->2I-)] and turn iodine solution from brown to colourless?

I would like to do more research in electrochemistry, since I'm doing a project on fuel cells, but where do I start? Any good books? Websites?

i was wondering if i could get potassium from electolysis of salt alternative. i can't mix it with water, because as the potassium gets separated, it will simultaniously react with water. is there anyway i can get it without the use of water??? could i use some other liquid to disolve the potassium chloride in?? like an alcohol or an oil??? is there any other way i can get potassium without going through the hassle of ordering it??????????????

Ive heard from people that hydrofluoric acid is actualy pretty weak, but i know it can dissolve certain types of glass. I thought that the the stronger the halogen, the stronger its acid. Is this true, is this the same for the alkali metals and there bases. Is cesium hydroxide the strongest base known to man?

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.)

Could my trusty old data-book have yet Another error in it? it clearly states that Mg3(PO4)2.4H2O is a Blue monoclinic crystal, since I like "collecting" colored crystals I put a chunk of Mg into some Phoshoric acid to make some. It`s Not blue. in fact if anything it`s a clear to grey liquid without even the slightest hint of blue with a white paper test. I`ve tried to google for it, and there`s no mention of blue there either, anyone have any ideas what it could be on about? or is it just another error (like the MP of NaHSO4 being 6588 kelvin!).

I am working on an overview of the chemistry of many metals. Part of this work is finished by now (first row of transition metals except scandium), and I want to share it with others. It might be that the material is made into a book (or e-book), but for now, it first will be part of my website. I hope you like it. If there are errors or omissions, then I would be pleased to know about that. http://woelen.scheikunde.net/science/chem/solutions

I need a step-by-step guide for calculating the reaction enthalpy of thermite at 2000 degrees celsius. Can somebody help?

For a while, I've been looking for ways to create fe2o3/red iron oxide/ferric oxide, other than scraping it off the bottom of my car. Then I chanced upon a page (which I, of course, can't find again) that suggested the following procedure. First, make a solution of an iron salt in water. Then, add a hydroxide to the solution. The solution should change its colour as a precipitate forms. Upon drying, the precipitate should change its colour to that of rust. So I decided to try some chemicals I have already, namely iron vitriol (sulfate AFAIK) and household ammonia/ammonium hydroxide. The solution was a greenish/milky colour, just as the powder. …

goal: making pure nickel metal method: stripping down dead Ni-Cad batteries, isolating the Nickel mesh plate, washing it to remove most of the KOH, drying it then cracking off the Ni metal from the mesh. adding sulphuric acid to this metal and placing it on a low heater for several days, leaving the excess Ni metal and the subsequent Green Crystals. re-hydrating this now ph neutral material, filtering and then displacing the Nickel with Aluminium inside a magnetic bottle, the Ni metal will stay in the bottle as I pour out the alu sulphate and wash the metal in pure water several times. remove from the magnetic bottle and dry the Nickel as fast as possible to avoid …

1.Can potassium permanganate be used as a bleach? It donates oxygen atoms to the dye. 2.What's the reaction between con. sulphuric acid and ethanedioic acid (COOH)2? Dehydration or CO2 will be given out? When will con. sulphuric acid take out the elements of water of a compound?

why solid ammonium iron(II) sulphate dissolve in dil.sulphuric acid but not in water??

This is a titration experiment, first, we had to standardization of KMnO4 solution.Then i find the Molarity of the KMnO4=0.0279M here are some equations & datas that the book provided: 2 ((MnO4) - ) + 5 (H2O2) + 6 (H+) --> 2 (Mn 2+) + 5 (O2) + 8 (H2O) Concentration of H2O2 is expressed either by %(assuming the density of the solution is1.0g/cm3)or by volume. volume concentration is expressed as the volume of oxygen available from unit volume of the peroxide solution measure at S.T.P according to the equation: 2(H2O2) --> 2(H2O ) + O2 68g 22.4litre at S.T.P. by definiation a 22.4 volume solution contaion 68g/litre 2nd, we had…

If you go to here: http://www.webelements.com/webelements/elements/text/Cr/key.html (it's data about Cr, but that's not really what this is about) And scroll down a bit to the "WebElements Movie" there's an interesting video given to us by Sheffield Uni. I would like to know more about this reaction, focusing on the why part of the 'snakes' being formed (watch the video if you don't know what I mean). I know that traditionally ammonium dichromate makes a volcano effect which is visible here and I'm guessing there were 3 "mercuric" (wouldn't it just be mercury?) thiocyanate pellets as there were 3 'snakes'. Questions: 1) Why do the snakes form? What w…