Inorganic Chemistry

how do you make nitric acid using potassium nitrate and sulphuric acid

Hey guys, So, this is going to sound very strange but bear with me... I was wondering if anyone knows of a way to remove the graduations and labeling off of glassware without scratching or destroying the glass. Just because this is such a strange request, I'll explain: It's actually just because I'm so anal about aesthetics I'm thinking of buying some media bottles that have graduations and labels and stuff, and I don't like the way the markings look, so I wanted to remove them. I know that's weird, but it's just how I am... sigh Anyways, thanks for your help! ~Sebastian P.S. Sorry if this is in the wrong section, but I wasn't sure where to put it...

Guys I've got some caustic soda powder... and how can i make a kinda conc. solution of NaOH??? Can i make it by dissolving them with water till it saturates???

I don't expect many hits on this Thread but I have not found the answer to this enquiry. Imagine the scene - an excited Yr 9 class is following up displacement reactions where a more reactive metal will displace a less reactive metal from its compound. For example, the students add magnesium metal to copper sulfate and immediately notice that the copper is precipitated. However, a lot of groups also notice streams of bubbles coming off various reactions and these are discounted as 'side reactions.' by me. Does anyone know if I am right, and if so, what are the side reactions? Any clues will be appreciated.

situation: one is conducting an experiment to deduce the reactivity series of metals based on their reactions with oxygen to supply the oxygen, KMnO4 is heated however, it is heated only AFTER heating the metal which is going to be tested why is the metal heated strongly first before heating potassium permanganate?

Why does low atmospheric pressure cause the oxygen leels in a body of water, like a lake, to rise....or so I am lead to believe? I am an avid angler and it is a commonly held belief that, during low pressure, the oxygen levels rise and push the thermocline down causing fish to seek the bottom of the lake. Does anybody understand the physics or chemistry of this phenomenon. My instinct says that oxygen levels should rise with rising pressure since the atmosphere is 'pushing' more on the water's surface,.but apparently not

please tell me how to prepare SO3 cristals? Can I use H2SO4 and freeze it, or need use SO2 + O2?

I bought a chemistry set for my sons last weekend and the instructions stated that, to do all the experiments, more copper sulphate and aluminium potassium sulphate (APS) would have to be purchased. The copper sulphate is not a problem, but the APS appears to be available in two forms: APS 12-WATER LR and APS 24-water LR. The APS in the chemistry set is 24-water (LR is not mentioned), but the type available from a supplier is 12-WATER LR. Would the 12-WATER LR be okay? Also, can anyone suggest a UK chemical supplier that sells small quantities of chemicals? The smallest weight I've found so far is 500g. Thanks.

While experimenting with primary cells using aluminium, copper, and caustic soda both electrodes begin to gas under certain load conditions. It is common knowledge that the gas from the aluminium electrode must be hydrogen, but bubbles from the copper are larger, non-fizzy, and rise slowly through the elecrolyte. I assume it is oxygen, but researching the reaction between al and naoh gives some confusing answers, but nowhere is the production of oxygen mentioned. The copper does not appear to be consumed, and the electrolyte does not turn bluish. It is as if the "mystery gas" becomes dissolved in the electrolyte then adheres to the copper rather like dissolved air in…

I couldn't find any other ways to make it other than from Wikipedia so I was decided to make sure if it would work first. From wikipedia: Phosphorus trichloride is prepared industrially by the reaction of chlorine with a refluxing solution of white phosphorus in phosphorus trichloride, with continuous removal of PCl3 as it is formed. P4 + 6 Cl2 → 4 PCl3 Industrial production of phosphorus trichloride is controlled under the Chemical Weapons Convention, where it is listed in schedule 3. In the laboratory it may be more convenient to use the less toxic red phosphorus.[5] It is sufficiently inexpensive that it would not be synthesized for laboratory use. If I get…

Finding the lovely, yet rather old thread, you guys have on making copper sulfate, (which actually yields copper hydroxide), I was curious as copper hydroxide is a useful chemical to have around, and as such performed the experiment as prescribed, using copper electrodes, and magnesium sulfate (epsom salt) as an electrolyte. I used about 18 volts initially, however, as batteries burned out, some were replaced, some weren't, I was left with about 12 volts, by the experiment's end, however the results, were not at all as I expected, as the solution turned a soft , pale shade of yellow, while the precipitate was orange. I thought this to be due to an excess of epsom salt, so…

We did these experiments in college to find out what type of ions they contained (anions or cations), but can someone explain to me as to how each of the tests actually work? I really need to know this... Test for chloride ion, Cl-. Known solution is sodium chloride. Test for sulfate ion, SO42-. Known solution is sodium sulfate. Test for hydrogen carbonate ion, HCO3-. Known solution is sodium hydrogen carbonate. Test for phosphate ion, PO4-3-. Known solution is sodium phosphate. there are some more but these will do for now.... I'd really appreciate any help

Hi everyone. I had a question concerning the basicity of nitrogens in Imidazole ( 2 nitrogens) vs the basicity in the 1 nitrogen in Pyrrolidine. I understand that the nitrogen not attached to the hydrogen in Imidazole is the most basic of the 3 because of the lone pair that is in the same plane of the aromatic system. However, I was stuck on the LEAST basic nitrogen of the 3. I know the lone pair of second nitrogen in Imidazole is in the plane of the aromatic system, but not sure about the lone pair of the nitrogen in Pyrrolidine. Any help is greatly appreciated. Thanks!

After doing some experiments using limewater for CO2 testing, my glassware was left with a layer of whitish CaCO3 caked firmly on the inside. I know that hydrochloric acid removes it fine, but I don't want to waste any, as I am running low. Anybody know some other means of removal? Mechanical methods don't work very well as far as I've tried.

Can anyone tell us how to create non-toxic stagnant smoke for use in our experiment to visualize flow through airfoils? We tried using fog machines, however they have very high initial velocity so they affect the flow. Can you help us with some chemical reactions which don't require much heating and produce visible fumes?

is a scale to the 10th of a gram good enough to weigh chemicals powder or does it have to be 100th of a gram?

How to prepare sodium hypochlorite solution in domestic level?

Please haelp me to make my projects on the topic to test the presence of Ni2+ in Chocolate please help me..........

was wondering if anyone could help me, im trying to make flash powder 70/30 potassium perchlorate/aluminum powder, but i accidently ordered the spherical AP instead of the flake, so not im stuck with a pound of potassium perchlorate and a pound of AP 500 mesh spherical, is there any way i could still make this flash powder doable?

I was wondering if anyone had any relatively easy procedures to produce dry ice? any help would be appreciated.

I saw something new today, and it was pretty cool. I'm sure lots of everyone here has heard or seen a demonstration of Sulfur Hexafluoride. I looked at wikipedia and the origional discoverers made it by exposing fluorine to sulfur. You couldn't pay me to do that. But what I'm wondering is if there are any other very dense gasses that are more safe in terms of their production? Maybe something with chlorine or bromine or oxygen or selenium? These are probably not practical for the home chemist, but does anyone know of a very dense, heavy gas similar to sulfur hexafluoride?

I have 35% Food Grade H2O2 on hand, and I'm tired of worrying about it decomposing, but buying stabilized H2O2 is very expensive. I then thought to myself, well, why don't I just stabilize it myself. So, after some searching through Google, I found that the most common stabilizers are Acetanilide (used in USP H2O2), Sodium stannate, phenol (which I don't want to use because it causes cancer, if I recall correctly) and Tetrasodium phosphate (AKA Sodium Pyrophosphate). I also found this :"Colloidal stannate and sodium pyrophosphate (present at 25 - 250 mg/L)" - which gives the approximate quantity of stabilizer per liter, for those two substances. As well, I'm going to assu…

I need your chemistry brain with this one here. There is a person who I came in contact who is studying biology who claims she can make explosive out of a gummi bear (or gave indication to some with sugar) and some mystery substance she is not willing to give up and says I could never figure it out and that the mystery chemical is something you can only acquire from say...a lab. That's the wrong thing to say to me because I HAVE to know. My first thought was potassium chloride (ive seen experiments on the net, seems like a basic intro to a class) but that doesn't seem to like a chemical compound that is hard to acquire. She really placed emphasis on the inability to a…

I was heating magnesium metal and suddenly became really deformed looking and turned black. When I continued to heat this, it then caught fire and left white magnesium oxide, with a little of the black stuff in the center. It can't be mangesium nitride, I tried burning magnesium in pure nitrogen and the resulting powder was yellow. I really have no idea what else magnesium could do, unless there is another metal alloyed with it? It was labeled as lightweight magnesium, but it could have had something else added to improve its strength or other properties. If the formation of this black substance indicates another metal present, any ideas on what this metal is? And when I …

hay every one im doing a research task for chem about the effects of temp, concentration of hcl, surface area of the mg and the presence of a catalyst i have a cupel of questions 1) if there is a catalyst what is it? 2)any general hints and tips? thanx all nb; also any suggestions for a simple method and safety risks for this prac.