Inorganic Chemistry

Does anyone know how to make or purchase a basal plane carbon electrode?

If one were to make a solution of NaCl and water, would it be possible to seperate the Na+ and Cl-? I would like to then see if i could somehow run the Na+ through an electric coil to make electricity, and the same with the Cl-. I am thinking this might work becuase if you put a magnet through a wire coil, it makes electricity. Possibly, instead of a magnet, i could use the charges of the Na+ and Cl- to make electricity. I first just need to know if i can seperate the Na+Cl- using magnets.

"investigation of sodamide and of its reaction-products with phosphorus" William Phillips Winter p42-43 The article goes on to say that the reaction of sodium phosphide with water generates small portions of phosphites and hydrogen gas, in addition to the main products of sodium hydroxide and phosphine. Hydrogen sulfide is known to be able to reduce sulfur dioxide (actually sulfurous acid in aqueous solution) at room temperature. Perhaps phophine would similarly be able to reduce phosphorous acid (H3PO3)? It seems apparent that hypophosphorous acid, H3PO2, is reduced by phosphine, PH3, to elemental phosphorous. The selective oxidation of PH3 by aqueous i…

I noticed that in a description of the byproduct of lightning that instead of it giving a discrete formula it was NOx, and NOx compounds can also result from other high energy events and even a microwave to form NO2 or 3, so is there a limit to what the O can be? Or is it just as I increase the energy, I increase the capacity for O? Could I have NO100?

Can anyone tell me any water insoluble colored chemical? Thank you.

Could someone please tell me if it is possible to makes copper sulphate from copper oxide and magnesium sulphate.Thanks

I was doing some Reaserch about various compounds and according to Wikipedia magnesium chloride decomposes if you slowly heat it to about 300 degrees.i was just wondering what it decomposes to because it does not say?

I was just wondering if anyone could help me with a microstate table. It is p1d1. I know there are 60 microstates but I am having trouble actually making the table. Any help would be appreciated. I solved for the ML andMS but I got zero for both MS values, which can't be correct because you will not get 60 microstates. Thanks

Hi, just wondering how to extract magnesium from magnesium silicat (talc). Thanks.

Hello! I have a question. Do I have to deposite the chromium on the glass for silver deposition? Chromium is too dark to make device such as OLED or solar cell. I want to increase transmittance... so............................ Do you have any idea about silver deposition without chromium on the glass? (Lilke surface treatment using solution.) Thank you for your favor

Is it possible to take an alloy (e.g. stainless steel, solder) and separate it into its components? Could you melt each metal out, or what? Help is appreciated.

Hello, I would like to ask if it is possible to know the exact or if not closest voltage and current that a specific acid under specific circumstances produces. For example, how much volts and amperes can a 10 milliliter 10% Acetic Acid (CH3CO2H) produce? The cathode and anode I am going to use are Copper (Cu) and Zinc (Zn) respectively. Is there any formula for this? I also heard that the two metals are the big deal here. But I'm really confused. Thank you.

I just did a sort of manganese-based thermite. I had washed and dried, fine powdered MnO2 from alkaline batteries, and coarse Aluminum powder which was made in a ball mill. Now, the thing wouldn't behave like a normal thermite when I ignited it: The magnesium fuse just went out as soon as it touched the mix (which was expected, I suppose) and I had to hold a blowtorch over it for extended periods of time to get any reaction at all. Here's what happened: When the flame was over an area, that area emitted molten sparks of metal, which collected at the bottom of the flowerpot. Was this newly formed alumina or manganese? I have reason to suspect both, as the powder that resu…

We know that Al tends to form amorphous oxide layer when exposed to atmosphere at room temperature. But what if the reaction of Al and O2 happen in very low pressure and high temperature? will the Al2O3 formed as crystalline?

I was bored and feeling stupid tonight, so I dropped a 9v battery in salt water, hoping to make NaOH. It seemed to work at first, as bubbles of hydrogen were rapidly being formed. But then, I checked back on it a few minutes later, and something blackish was drifting around. Bubbles were still forming (at the anode only, for some reason), so I decanted the solution into a new container. The solution has blackish particles drifting around in a dark green solution. My guess is that the manganese dioxide and potassium hydoxide reacted in solution to make the green solution of potassium manganate, and extra manganese dioxide would explain the black particles. Is this logical,…

how this reaction occur? Cu + 4HNO3 ---conc.----> Cu(NO3)2 + 2H2O + 2NO2 (The Reactants: Copper, 3 Nitric Acid and the Products: Copper II Nitrate, Water and Nitrogen Dioxide) What happened first? And what happened then? Where did the water came from? and where did the nitrogen dioxide came from? And for this reaction Fe+4HNO3 -----dil./heat------> Fe(NO3)3 + 2H2O + NO Where did water came from? and why hydrogen gas is not evolved?? and what happened exactly? Any Help Please

I'm looking for an interesting article on practical applications of hydrogenase or even just glycolysis in general? I'm not looking for anything specific - to be frank, anything will do. I just would like something to show a colleague of mine. However, I just would like it to be from a reputable scientific news source, Thank you.

I had an idea for a reaction to easily produce nitryl fluoride. The reaction has not been tested. (2)CaFeF6 + (22)HNO3 --> (4)Ca[NO3]2 + (4)Fe[NO3]3 + (22)HF + (2)NO2F + O2 Ideally the concentration of the nitric acid used in the reaction should be greater than 98%. Preparing the hexafluoroferrate H2O2 + 6HF + FeO4(-2) --> FeF6(-2) + 4H2O + O2 The H2O2 and HF must be premixed, then added to ferrate solution. A similar reaction is known to occurr for permanganate. After completion of reaction, a solution of calcium nitrate is added, which would cause CaFeF6 to precipitate out. The solution is filtered, and the precipitate is dried. The solution …

I've recently online run into a metal called "ruthenium brass". Specifically, on Amazon. Is this an alloy of brass and ruthenium? It doesn't look like it's ruthenium-plated, because it's lacking the dark gray color. Help would be much appreciated.

Hi, I have 4 questions for you that I need to know how to answer them very well because I have an exam that coming up and I want to be ready for it. First:- http://dl.dropbox.com/u/936463/inorganic/4.jpg Second:- http://dl.dropbox.com/u/936463/inorganic/5.jpg Third:- http://dl.dropbox.com/u/936463/inorganic/7.jpg Fourth:- http://dl.dropbox.com/u/936463/inorganic/8.jpg Thank you so much and God bless you

Hello, I am currently working out the chemical equations to prepare ReCl3 solutions in order to synthesis NaYF4. The following equation is used to prepare the chloride solution: Re2O3 + 6 HCl = 2 ReCl3 + 3 H2O In order to prepare 0.5 mol/L of ReCl3 solution, I divided the equation by 4, then I will add more water to the solution to achieve the required concentration. Going forward with the procedure, I should achieve NaYF4. My question is if I want to synthesis NaYF4:20%Er (this means 80% NaYF4 and 20%NaErF4), should the proportion of metal oxides be 80% Y2O3 and 20% Er2O3? Please help me!

i saw a video on youtube about the making of hydrobromic acid, the guy used potassium bromide and sulphuric acid the set up was a beaker and over head stirrer and then a basic still. to me this seemed a bit ott because the product would require to be sepurated from the residual H2SO4 by using simple displacement chemistry one can make it using hydrochloric acid, this in theory should produce a more pure sample for the HBr can be boiled off and passed through distilled water to produce the acid. equation: KBr(aq) + HCl(aq) --> KCl(aq) + HBr(aq) instead of: KBr(aq) + H2SO4(aq) --> KSO4H + HBr

http://woelen.homesc...uIII/index.html Copper(II) salts can be oxidized to Copper(III) complexes, with the help of a hypochlorite or persulfate oxidizer, sodium hydroxide, and sodium periodate. The complex [Cu(H3IO6)2]-2 is oxidized to [Cu(H3IO6)2(OH)2]-3, which has a very deep brown-red color The composition of these complexes can more simply be thought of as: IO4[-],Cu[+2], IO4[-],(2)OH[-],(2)H2O and IO4[-],Cu[+3],IO4[-],(4)OH[-],(2)H2O Actually, Cu(OH)2 is soluble in concentrated solutions of NaOH showing that copper(II) oxide is actually slightly amphoteric. CsCuCl3, although copper is still in its normal +2 oxidation state, is a …

Many years ago I started a list of zoological exceptions that's now hundreds of items long, so I was bound to notice the exceptional cases when I started to go over my long-forgotten knowledge of chemistry just four months ago. If so many have piled up in such a short period of time then surely there must be many others that only the advanced students or the pros are aware of. This is an invitation to add them to the following list. I doubt that it would ever grow to be as long as the other one, to which additional facts are frequently being added, or even as long as a much shorter one of botanical exceptions. I've been an amateur astronomer ever since 1985 and I…

if i was to form a solution of aqua regia using diluted acids (5 mol nitric and hydrochloric instead of 15 and 12 moles respcetifily) would it still be able to dissolve gold? the reason being is that if the acid is diluted should be some what safer than the 'pure' stuff.