Inorganic Chemistry

We are trying to make Sodium Iodide 57% solution using NaOH 50% and crude Iodine. We finish with a pH of the solution of approx 12, when we try to drop the pH to approx 8.5-9, the solution becomes deeply colored. Can someone help with what we are doing wrong?? Thank Johnd

Recently, I lent a friend my small butane torch, it's good for soldering and stuff. It's burns pretty much invisibly during the day, at night with a very pale blue. Anyways, he thought he had put it out, but he hadn't, and he got burned pretty bad. Is there anything I can do to pretty much permanently color the flame? I have access to lots of salts, KCl, NaCl, NaF, KF, even CsF and others. Would making a salt solution, dipping the head of the torch in, and allowing to dry work? How vividly would it color the flame? That is the important part. I can also get my hands on strontium and barium nitrate, as well as their chlorides. And yes, I know fluorides are dangerous, I lik…

For Beau, "My problem is with the >reaction of ammonia solution and silver as both as ion or solid. In >particular I would like to know whether AgOH is possible from the >reaction of limited ammonia solution (being a base) and either >silver ion or solid. I have searched on the internet for AgOH with >no result therefore I thought that when silver is reacted with any >base it either forms a Ag20 precipitate or a Ag(OH)2- ion. I'm also >not sure which one would be the product from limited ammonia. I >understand that in excess ammonia silver will form a complex ammonia >ion but dont know the limited solution. If the product i…

Would it be best to use cold water and bleach, or hot water and bleach, for cleaning our water bottles and water jugs? I've read numerous pages about how to clean water bottles, but haven't found anything yet that clearly states whether cold or hot water and bleach is best for killing the bacteria that collects in water bottles. A friend of mine swears by his method of using a little rice mixed with water, shake it around for half a minute, then rinse. I've tried that, but still have problems with stuff floating around in my water bottles (after they have been rinsed really good, air dried, then filled with filtered water (from our home filter), and then frozen. …

I'm a little unsure on endothermic and exotermic reactions. an endothermic reaction absorbs heat (the product will become hot) and an exothermic reaction gives off heat (the product will become cold) But if i react two products together will exo and endo occur at the same time? Because, for example in a replacement reaction one product gains some more energy and the other loses energy.

Can anyone give me the patented formula (In detail) for producing HYDROGEN from HYDROGEN SULFIDE? Yeah I know it’s one of the easiest ways. But I just want to know the process to reduce the smell. Actually I have to do it in my University Lab so can't have too much space and time. So I am interested to know the total formula in detail.

Hello, I want to study polymorphism and allotropy more extensively.Wikipedia and the web pages I found are too brief. I hope somebody can you help me with some directions to good resources(sites, books or others)? Thanks.

Hey so I know this sounds a little stupid but I need to find an evaporation formula for my current research project. Yes, I have looked around the internet but I keep running into formulas that only deal with homogeneous solutions or just water and I'm not sure if they apply to my case which is a little bit more complicated and I really want some opinions on which formula is best to use for this type of solution and please don't hassle me about how I should know this if I'm conducting research - I'm taking way too many classes to remember everything. Here's what I'm doing and why I'm interested in evaporation: I'm making polythiophene nanoparticles in which I have…

I have a large quantity of WW2 era dental filling pellets, 75% Ag, 25% Sn, in the form of pellets of compressed powdered metals (not an alloy). I see that I can buy 15% HCL at Home Depot. How do I proceed to dissolve the tin away? Do I need to crush the pellets first? I'm not a chemist, and wasn't paying too much attention in freshman chemistry. Any advise would be appreciated.

Hi, sorry if this is a stupid mistake or I should be ignoring Wikipedia, I'd just like clarity. As I understand it, the concentration of H3O+ ions in an acidic solution is denoted by (x^3)+(Ka*(x^2))-((Kw*x)+(C*Ka*x))-(Kw*Ka)=0 (where x is the concentration of H3O+ ions, C is the starting concentration of acid molecules, Ka is the acid dissociation constant and Kw is the auto-ionization constant of water. My question is, assuming that the above is correct (if it's not please correct me), is it safe to describe the concentration of OH- ions in an alkaline solution with (x^3)+(Kb*(x^2))-((Kw*x)+(C*Kb*x))-(Kw*Kb)=0 (where x is now the concentration of OH- ions instea…

If a H+ ion is needed in all acidic compunds and the more H+ ions you have the more acidic something is. If you had a beaker of pure H+ ions, i.e protons, in theory, would this be the most acidic thing possible; and if so would it react even with noble gases and platinum etc.

Hi guys, As we all know most aqua regia are made from 3 parts HCl and 1 part HNO3. Any ideas what happens when we change the composition around to like 1 part HCl to 1 part HNO3 or 1 part HCL to 3 parts HNO3? For what I know the purpose is to make the strong oxidising OCl- My primary guess will be that a less potent aqua regia will result from the change in composition (lesser Cl- ions) Any comments? Please correct me if I'm wrong , thanks

If this true http://www.ahanw.org/forum/topic.asp?TOPIC_ID=602 (that hydrogen burns at 4000F) then wouldn't thermolysis occur when the hydrogen combines when oxygen, since at 4000F water would have the hydrogen separate from the oxygen(it seems impossible since there would be continuous energy being produced if the hydrogen were burned again)?

I was searching for a reaction to know which solution contains CuCl and which solution contains CuCl2... There was a NH3 + CuCl Solution and CuCl2 solution. When i added H2O2 to CuCl solution , dark-brown percipate was fromed.It was like sensitive to air. When it contacted with air its color turned to dark-yellowish-green.The color of this solution was always blue what with brown percipate the bottom. When i added H2O2 to CuCl2 solution , a greenish - white colored percipate was formed.But i have no idea about its sensitivity to air.The Solution wast blue . The firs drops of NH3 formed the blue color as i waited at the surface after mixing it color was gone. …

Not able to understand "The ion electron method of balancing equations for oxidation and redox reactions".. Help!!!

Does anyone know how to obtain stibnite? I need it for a pyrotechnic composition and I do not know how to produce it.

We both know that ferric oxide will react with h2s and could be regenerated by air.Are there any methods onstream to regenerate the spent oxide to original status?For example,how about introducing H2O2 solution or ammonia into the ferric oxide before desulfurization in vessels,since we know the decompostion of H2O2 will produce oxygen.Could this method work efficiently?

1. The problem statement, all variables and given/known data The rate of decomposition of hydrogen peroxide was studied at a particular temperature. H2O2(aq) = H2O (l) + 1/2O2(g) The initial concentration of hydrogen peroxide was 0.200 mol/L. 10.0 s later, it was measured to be 0.196 mol/L. b) 0.500 L of hydrogen peroxide solution was used for the experiment. What mass was lost as O2 bubbled out of solution in this initial 10.0 s interval? 2. The attempt at a solution What I did was. 0.500 L * 0.200 mol/L = 0.1 0.500 L * 0.196 mol/L = 0.098 0.1 - 0.098 = 0.002mol 0.002 * 16 = 0.032 g What I'm doubting is. 0.500 L * 0.196 mo…

Stabilized ammonium nitrate seems the best bet so far, but manufacturing it seems virtually beyond the scope of the kitchen lab. does anybody have any ideas?

Hello! I am trying to translate a paper on inorganic chemistry (specifically a potentiometric study on the interaction betweeen the COMT inhibitor and Mg(II) and Fe(III) ions) from Spanish into English but, since I am not an English native speaker and my knowledge of chemistry is limited, I could really use some help in order to get everything right. I just need someone to check if something sounds "weird" or maybe I've made any grammar or tipographical errors (specially with chemical formulae). I'm sorry for the lack of context but it's two pages long and I thought it would be too much to post it here. Thank you so much! To begin with, my translation of the pa…

Hi everyone! I am an English learner and I would like to know how do people name intermetallic compounds. For example, Mg2Si is "magnesium silicide". Then what is the name of AlCu? How to add "-ide" to copper?

I recently found some Cerium (IV) Oxide as a polishing powder, and have a lot of calcium metal chunks to spare. What is the best way to start this reaction in a thermite-like manner? Should I grind up the Ca into powder, or leave it as these 1 cm chunks? The reaction is: CeO2 + 2Ca -> 2CaO + Ce Molar ratios: 172.115 + 80.156 -> 112.155 + 140.116 (numbers correspond to reactants and products above them) So, for every 17 grams of CeO2, I would use 8 grams of Ca (either powder or chunks) to get 11 grams of CaO and 14 grams of Ce, correct?

I have a question about Ksp and L'Chateliur's Principle. Lets says we have the following: NaCl(s) ----> Na+(aq) + Cl-(aq) If we add more NaCl(s), the equilibrium does now shift since (s) and (l) do not affect Keq. In addition, the reaction does not shift either b/c L'Chateliur's Principle shifts are not affected by (s) or (l). But what about Q. Q is the [P]/[R] at any time. If we add more solid, don't we in fact increase the value of Q. If so, can't we then compare Q and K to see which way the reaction shifts and/or if we can still dissolve more solid? Thanks.

Fellow members, I ask for your help- I add nitric conc to Fe powder slowly. It dissolves after a while, and after cooling/settling, I get most of the Fe to dissolve to clear solution as well as a bunch of ppt (oxidized Fe?). I am trying to first, get all of it to dissolve without the brownish oxide, and second, to get ferric, not ferrous nitrate. Should I use any water anywhere? I can use either one, but prefer ferric. I know now, that there are some pretty sharp guys here, so I am confident I can get some good advice, eh?? Thanks!! Oh, in the end, I prefer the hexahydrate, but nona hydrate is OK too.

I've been trying to figure this out for a while now but all the methods found easily on with google have been tried and rejected. At the Rhenium recycling facility that I work at we have about 54000L of Ammonium thiocyanate solution that contains about 3g/L Re, reduced from 50-60g/L by cooling to -4C. This stuff has been piling up for over a year now and nobody wants to send it out as waste because there is potentially $1mil worth of product tied up in these things. But it is also starting to take up lots of space. I will welcome any suggestions on how to either force the solubility equilibrium to favor Ammonium perrhenate, or reduce the oxidation state of the Re…