Inorganic Chemistry

The chemical compound which conducts electricity in the molten condition or through its aqueous solution with chemical change is called an electrolyte. All the mineral acids, bases and salts are electrolytes in aqueous solutions or molten state. HCl, H2SO4, NaOH, CuSO4 etc, are electrolytes. Electrolyte is an ionic compound. Non-Electrolytes is the compound which do not conduct electricity in molten or in aqueous solutions are non-electrolytes; such as sugar, petrol, benzene etc. Non-Electrolyte is a pure covalent compound.

A mixture containg 1 part by volume of HNO3 ( conc ) and 3 parts by volume of HCl is called agua regia which means royal water. It can dissolve gold and other noble metals due to liberation of chlorine. It forms Hydroauric chloride.

No suitable material, there is no finished product. Want to know 1mA/cm3 surface currents, is low?

So I have another question. Silver iodide, AgI can work as a solid electrolyte. How can electricity pass through the silver iodide? Im thinking that this must have something to do with interstitial sites. We know that iodide ions is much bigger than the silver ions. That means that the silverions can be found in these interstitial sites between the iodide ions. Does that mean that the ions can move around more and "carry" the electricity around?

Hi I have a question about the thiocyanate ion, SCN-. How does it bond to Ca2+ and how does it bond to Hg2+. My guess was that SCN- is a soft base. Hg2+ is a soft acid, so those two go well together. But Ca2+ is a hard acid, so it doesnt go well with SCN-. Is this right?

I am having a hard time washing my gold after two types of gold dissolving methods. One is where I add 70% nitric acid to computer pins to eat away at the metal causing it to release the gold. The other is when I dissolve the gold off of a new set of pins with aqua regia. Both seem to leave a lot of salts behind. In the first method with just nitric acid the salts are so bad I end up loosing a lot of gold flakes trying to rinse the salts out. Any idea how to dissolve the salts so I can wash the gold easily? Also I would really like to know what these salts are. Is it silver chloride? In the second method of using aqua regia on a new set of gold plated computer p…

I'm looking into a process handling an aqueous feed solution containing metal salts as well as up to 30% of a polar organic solvent like acetone or methanol. The goal is to separate out the metal cations by element. So far, I've been able to identify a few promising approaches to the point that I can start building a simple working demo. The problem is, I'm attempting to procure an anion-exchange membrane that can tolerate the organic solvents and I'm at a loss with my current suppliers. Does anybody know of a membrane or membrane supplier that can survive in that environment? Many thanks!

People, A friend asked me (and Im asking yous) the above- hes smelling an awful smell in his shower, and its making him cough like mad. The utility Co here uses chloramines not chlorine. Is here any possible way one can smell chlorine or the other component, ammonia from this basic molecule (meaning the molecule would have to be broken down, I figure)? Thanks

I was wondering why it's the oxides (Nitrogen Oxide, Carbon Dioxide) that are the main causes of global warming? And how does that reason compare to the other gases in terms of not playing a part in global warming?

Am I right in saying that, in an exothermic reaction for example, the reactants have a higher enthalpy, and the products have a lower enthalpy, as seen from the energy profile diagram. But the reactants have a lower bond enthalpy, and the products have a higher bond enthalpy, because a lower amount of energy is required to break the bonds in the reactants, but a higher amount of energy is released when the new bonds are formed. This just confused me as I thought enthalpy and bond enthalpy were the same thing!

In which part of a galvanic cell does the temperature increase, if nothing is attached to use up the electrical energy (other than wire resistance)? I am considering a construction of a galvanic cell like this: http://chemwiki.ucdavis.edu/@api/deki/files/6149/=ZnCu_detail.gif I assume that a galvanic cell without a load will work just like any exothermic reaction. So where does it get warmer? Is it in both the anode and the cathode electroytes? Or is it only the cathode electrolyte that gets warmer? Maybe the anode will even cool down, since energy is required to release electrons from the anode.

Hi, I'm looking for a software package to simulate a process of electrowinning of mixture of transition metals in acidic solution. Thank you. Alex

Hi I am working on a paper on nanoparticles comprising a polymeric component as well as a component of inorganic semiconductors (such as TiO2, ZnO ...). Primarily I am interested in such nanoparticles that are designed to enhance the efficiency of solar cells. What I am looking for is a paper/publication that gives an overview over the chemical methods that are being used to make such nanoparticles. Or any publication on the matter. Any hints or links are greatly appreciated!

Conventionally in elementary chemistry, you really only deal with at most quadruple bonds which typically occur in the carbon group, but I know there are higher bonding states http://en.wikipedia.org/wiki/Sextuple_bond But, what exactly allows this to happen and what creates this limit for other atoms? Let's say you stripped all the electrons from Neon and had just the nuclei, the orbitals would fill according to whatever s2p4... pattern they have in such a way that each orbital would have a net spin of 0, an up by 1/2 and a down by 1/2. However, let's say this nuclei came into contact with another neon atom with 10 electrons, could you then have a dectupple covalent b…

I wanted to buy some Bordeaux mixture (as in the solution of copper sulfate and calcium hydroxide) so that I could precipitate the copper out of it as copper hydroxide (using sodium hydroxide). The Bordeaux Mixture that is on sale here is in powder form, and says 'tetra copper tricalcium sulfate'. In my head it sounds like this is just the dehydrated form, forming a complex, and that it will dissociate into the respective ions again in solution. Since I cannot find any information to confirm or deny this, however, I would just like to ask for some confirmation before I buy it...? Thank you in advance

Hello All! I've been doing a lot of research recently on the synthesis of chlorates and perchlorates (specifically potassium). However, no where have I found a single comprehensive article on how the synthesis of potassium perchlorate is accomplished, and what the differences are between the production of the chlorate and the perchlorate. I know there is a lot of misinformation on the subject out there, and that many people make it more complicated than it needs to be. Therefore, I was hoping for some help on exactly how to produce potassium perchlorate and possible the why behind the different steps. I am looking for the EASIEST and QUICKEST way possible to produce i…

What would be a chemical test to distinguish between sulphurous acid and sulphuric acid? I think Sulphuric acid is an oxidising agent and sulphurous acid is a reducing agent but i am not able to come up with a common test that will distinguish the two.

The rate constant in a rxn rate in based on the Arrhenius equation. In this equation, two factors can change and thus influence "k"-- temp and Ea. I was always taught that temp increases the rate if a rxn and this makes sense based on the Arrhenius eq but Ea is also a factor. Now catalysts increase the rate of a rxn by decreasing the Ea if both the fwd and rev rxn. So can we say that a catalyst influences the rate constant and thus influences the rate of a rxn by increasing the value of "k"?

Trying to see if its possible to make a free Cl aqueous by say, mixing some HCl and nitric conc to genetrate Cl2. Then test with thiosulfate to verify Cl2 content, then standardize. Tips/opinions appreciated.

What is a liquid liquid critical point? I know that a liquid has critical point is when no phase boundary exists between the 2 phases, but it seems based on what Wikipedia says a liquid liquid critical point is when the two fluids can be separated. Why is this so and under what conditions is this possible?

Hello there, it is my first day on these forums today. I am planning a science fair project to do, (a real science lab, with variables and data collection, not just a "demonstration"). I am basically measuring the cold produced by different endothermic reactions, such as adding salt on ice for example. It would be nice if the forum commenters could list a few common endothermic reactions that I would be able to produce using common or household materials, or chemicals commonly avalable inside a labortory. Please note that I am merely 13 years old, so please list chemicals by their names rather then symbols. Thank you very much, and if this is in the wrong section, i …

On someone's blog about h2o2 that I found randomly (sounds stupid, right? I did find it interesting though), I read that you can make exceptionally strong h2o2 with sodium percarbonate. Does anyone know how I could do this, and get a 30-40% concentration? Dilution is allowed, but I don't like the idea of messing with test grade+ HP more than I have to... Anything above 40 just frightens me, it's nasty stuff. Apparently the other product is sodium carbonate, could I remove that with a coffee filter, or would it (the sodium carbonate) dissolve in the solution? Please try to stay on topic, not that you wouldn't. This is meant to be a practical exercise, cost effectiveness is…

Today in the laboratory in my school, I wanted to make a small Ammonium Dichromate volcano. The lab teacher got a very small amount of the substance and then heated it up to see the reaction. She said it is a carcinogen substance, so I got worried about my health. Must I worry? I didn't get in touch with the substance but maybe I inhaled a very small amount of gas while it was burning, and I don't remember I got in touch with the green substance. Can you help me please. The best answer will be chosen. Thanks!

How thick would the layer of bismuth oxide on pure Bi metal need to be to produce green, and what would the progression of colors be as the layer thickens? I think we would apply Fresnell's Equations, but I'm not sure how. The refractive index of Bi2O3 is 2.5/0.4 according to a Chinese distributor of the yellow powder form. I'm not sure if that applies on the thin oxide layer on pure metal. Many thanks to whoever can help me understand. Ernie

I was taught that reactivity increases down a group in Gr 1 and Gr 2 elements, but I never understood why. Would anyone be able to please clarify this? Is the same true for non-metals as well such as the elements in Groups 5, 6, and 7? Thanks.