Inorganic Chemistry

Hi i am 14 years old and need help on a science project for which I need to heat water immediately in a test tube at a temperature as close to 50 degrees centigrade as possible but not more than that and keep the water heated at this temperature only. please advice thanks and regards

I know we can get the relative atomic mass of any two nuclides by just looking up the CODATA. But I'll like to know if anyone has measured atomic mass with a chemical process. Say we analyze the weight composition of ¹H₂¹⁶O to get the relative mass of ¹⁶O/¹H. Or of any other two elements through any chemical process.

Hi I was interested to get some insights on how you would be able to instantly shatter an ice lattice. Instant instense heating of very cold glass for example will cause the lattice to break but i was interested why an ice lattice responds differently. Is there a temperature where it would shatter rather than melt? If not then why? I presume that a shattering can occur if a high intensity electrical impulse is applied to the lattice but I’m not sure how high the voltage would need to be or how it would respond. Does anyone know? And is there any way that the lattice can be shattered otherwise? Any insight by someone would be helpful. Many thanks.

Hi everyone, I have a question regarding Gallium and I know very little about chemistry, so I was hoping this forum could help me out. I have spread a relatively thin layer of gallium across a flat piece of glass, creating a small mirror. I then used a hot-air gun and different settings (the highest being 300°C) and applied heat to small areas of the glass for a maximum of 2 minutes (directly on the side with the layer of gallium). I was hoping for the gallium to form a little droplet and drip down, leaving just the glass at those specific points. This did not happen at all. You could see it liquefy but there was always a layer of gallium still on the glass. Eve…

< I will be posting this Topic in the Organic Chemistry section as well, it is up to moderators or anyone else to get rid of it in any section. > Alright, I know there are a lot people that believe that Silicon-based life is not possible, and there is science to prove a lot of it. However, it is an interesting field and I think we shouldn't discredit it. While it might be improbable for an organism to evolve to be entirely silicon-based (the planet might have to be 1000 C just to start trying) we have the advantage of computers and molecule visualization programs to let us think them up. Now, my proposition is this, if there is any…

Yesterday i was melting stuff in an iron "crucible" for no specific reason. Today I was surprised to have found several different types of crystals growing on top of some silver metal I had left in the crucible the day before. What I'm wondering now is what exactly can this possibly be? In order to get an idea of what it could be I will list everything that has been melted/burned in it: Copper Powder Bismuth Silver Magnesium Borax When I most recently melted stuff in it with a propane torch, the crucible became a glowing hot orange color. Any ideas of what these might be? Also I'm new to this forum and I hope I am actually asking this in the …

Ok, I have some FeCl3 that I have created, and somewhere I heard that this is used to dissolve copper. I took some of my (hopefully) FeCl3, put it in a test tube, and placed some copper inside, and there was no reaction. Does this reaction take a long time, or is what I think is FeCl3 something else (perhaps with lots o' impurities)? While I'm at it, I might as well ask why this reaction works, seeing as copper is a very unreactive metal.

I have made hcl by mixing acetic acid and sodium chloride, but there is a byproduct of sodium acetate, how can I remove this sodium acetate? Btw, I’ve been trying to make a system that turns good waste into electricity ive done it already on a small scale I’ll explain how. Say I have eggshells banana peels and potato chips.I ferment the banana peels to get acetic acid, soak and strain potato chips for salt then make hcl from acetic acid and salt, then I dissolve the eggshells in hcl and add salt, I make calcium chloride, which when dissolves creates heat, when it creates heat I put in a shallow tray with a lid, when the water condenses it drips down over a water mill slow…

If I get aluminum scraps and dissolve it in hcl how do I turn it back into metal and what reactions are happening there? Also is there a chemical that I can rinse through sand to dissolve iron because I found this sand that has tons of iron(I checked with a magnet)

The question is simply to predict the reaction product of S2- and NH4+, and find its equilibrium constant. We have access to the Ka of H2S (which is the Ka of HS-) and the Kb of NH3.second HS- + H2O -> S2- + H3O+ ka = 1.1x10-12 => kb = kw/ka = 9.1.10^sup]-3[/sup] which is the equilibrium constant for the reaction: S2- + H2O -> HS- + OH-NH3 + H2O -> NH4+ + OH- kb = 1.774x10-5 => ka = kw/kb = 5.637x10-10 which is the equilibrium constant for the reaction: NH4+ + H2O -> NH3 + H3O+ Adding those two reactions together, we find: S2- + NH4+ + 2H2O -> HS- + NH3 + OH- + H3O+And so by multiplying the constants, we get 51.3x10-13... Which…

Hey, i was going through the topic 'ionic bond' and read this- I didn't get the thing- how can an ionic bond be covalent? Please explain(with example).

Write the balanced equation for the decomposition of hydrogen peroxide into water and oxygen gas. a. 2H2O2 → 2H2O + O2 Use Hess’ Law to calculate the net energy released. Then calculate the energy in kJ/ mol—this will be the theoretical value: H2 + ½ O2 → H2O ΔH = -286 kJ/ mol H2 + O2 → H2O2 ΔH = -191 kJ/ mol H2O2 + H2 + ½ O2 → H2 + O2 + H2O H= -95 kJ/mol H2O2 → ½ O2 + H2O H= -95 kJ/mol I am not sure what the answer to the second part is. I think that it is either -95 kJ/mol or -190 kJ/mol. I just want to make sure which one it is.

Hello, so I have been trying to calculate the mass of hydrochloric acid needed to produce calcium chloride from calcium carbonate. I have a solution of 30% hydrochloric acid and a 10g of CaCO3, how much acid do I need to react with the CaCO3? And how can one convert the calculated mass of HCl needed into volume (room temperature)? Thanks in advance

when we were going over answers to a homework in class today my teacher had a answer that was different from mine so i asked what i had done wrong. the question reads "the pH of a bicarbonate-carbonic acid bufer is 8.00. calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3-)" (see attached file for pic of the question and my work) . now our work was almost exactly the same but there was one difference which was that when he went to undo the log on the last step, he undid the log as if it was a negative log (EX: 10^-x). he claims that its the right way to do it, and even tho i have found a few other ways to solve the proble…

I am trying to formulate to pH of between 3.0 and 3.4. The slurry starts at about 5.5. I have to add vitamin c as ascorbic acid to the slurry. I would like to use a combination citric acid and ascorbic acid to get the slurry down to my desired range and achieve my label claim for vitamin C. Can someone point me in a direction I can start researching?

Some solvation reactions are quite energetic (either endothermic or exothermic). Does it allow us to create an energy storage (similar to battery) in which energy would be generated when metal atoms pass to a solution through an ion-conducting membrane? If yes, how much energy may we expect to obtain and what about reverse-ability?

does anyone know how to make a simple non-toxic breathable smoke bomb? this would be to study differences in air pressure and other studies like that without harming the enviroment

I’m a noob when it comes to things chemistry. Is the burning point of sodium metal (s) and H20 (l) enough to melt through certain objects? Like a door of wood. Since capillary action doesn’t happen with metals that don’t absorb.... could a design using spit amounts of water on top of raw sodium metal to form a sort of blowtorch. I’m not sure when oxidation comes into play with the metals.... can someone explain?

Dear friend, does anyone know if there exists any study about electrical conductivity of liquid argon? Thank you in advance for any suggestion.

Hi, I was cleaning some of my rusty tools by bathing them in vinager. It was a pretty slow clean as I'm used to leaving it for 2 - 3 days but when I returned I had an unusual reaction which I'm hoping you can tell me what happened? It's got a very unique aroma of copper grease but this wouldn't had corroded the sockets. I think the black cake is copper oxide but what about the red and orange? Any help greatly appreciated.

It is known that chlorine is produced when electrolysis of seawater or sodium chloride solution.My question, what is first produced, or in which form chlorine will be the first evolved; 1- as chlorine gas form that starts to dissolve in the salt solution? or; 2- as an aqueous form which will start to escape the solution after reaching saturation limit?all answers are very much appreciated. Thanks, Shadi

I am attempting to prepare some CuO for various experiments and am running into a bit of a sore problem. I have, on hand, an excess of Copper (II) Sulfate pentahydrate and baking soda, and decided to employ them as precursors to CuO. To my best knowledge, the reaction should resemble this: 2(CuSO4.5H2O) + 4NaHCO3 -> Cu2(OH)2CO3 + 2Na2SO4 + 3CO2 + 11H2O After the reaction was complete (i.e. no more fizzing) , I was left with the precipitate of the basic copper carbonate (Cu2(OH)2CO3). I then washed this precipitate several times and then heated it up to decompose it to CuO, H2O and carbon dioxide. I believe the reaction should go: Cu2(OH)2CO3 + heat -> 2CuO…

How is a correlation coefficient of 0.999992 better than a correlation coefficient of 0.99996 even though both analyses resulted in the same molar absorptivity for the analyte using spectrophotometric analysis? Does 0.999992 result in a higher correlation coefficient than 0.99996? If so, why?

I learnt that copper sulphate changes from blue to a green colour in the presence of iron. please i would like to know the stoichiometry of this reaction. Any help? thank you

Title says it all. I was trying to crystallize some InCl3 and came across something I had never seen before - an inorganic substance 'oiling out'. It was just rolling around in dense oil beads in the acetone at the bottom of my beaker. I evaporated the solvent and washed it with acetone a few more times, and it became more clumpy and granular with each washing. Upon drying, a flame test proved that it had the indium cation in it, so I have little reason to believe that it isn't indium (III) chloride (unless it somehow reacted with the acetone, but I am skeptical of this). Does anyone know what happened to make it behave as an oil? I've never seen that kind…