Hello people, this is my first time using this site. Today I would like to ask if my tin (II) chloride is really tin (II) chloride. I specially bought
this compound to make Tin metal crystals which can be made by Zinc displacement but I am having problems that when ever I put a piece of zinc metal in
there, I see no reaction at all. The zinc is obtained from the Alkaline batteries, at first I used the strips that I obtained from the battery and
when I placed it in the tin chloride solution after some while there was this blue colored solution with some blue participate. The next time I melted
the zinc metal and then I placed it in another solution of tin chloride, this time I saw the zinc gone black and bubbles were trapped on top of it and
transparent crystals were formed beneath the zinc. Also when ever I mix the tin chloride It gave a white suspension. If anyone could help me and is
there any other way to make crystals of tin from the solution without electrolysis? If needed I can post pictures.
[Edited on 26-12-2015 by Bert]elementcollector1 - 20-12-2015 at 09:21
Aluminum foil should work just as well. One reason you may not be seeing much crystal growth is that the zinc's surface area is getting coated with a
layer of tin, preventing further reaction.DemonsHeadshot - 20-12-2015 at 09:40
Thanks, I don't have any aluminium foil on hands right now so will an aluminium can work? The_Davster - 20-12-2015 at 09:44
Try electrochemically too. Tin dendrites grow easy on the cathode. If nothing comes out upon electrolysis you know you have not been provided the
correct material.
Okay well thank you too but I am getting suspension when ever I dissolve the Tin Chloride, could you point it out some how? gdflp - 20-12-2015 at 10:03
Stannous chloride will hydrolyze to some extent in aqueous solution as per the following equation, SnCl<sub>2</sub> +
H<sub>2</sub>O <---> Sn(OH)Cl + HCl. Basic stannous chloride, Sn(OH)Cl is insoluble in water, hence the suspension. As are most
aqueous ionic reactions, this is an equilibrium so adding a few drops of conc. HCl(or any strong acid for that matter) will lower the pH and cause the
tin salts to redissolve.unionised - 20-12-2015 at 10:09
Also Sn(II) will oxidise in the presence of air to give Sn(IV) which is even more prone to falling out of solution as a hydrated oxide. aga - 20-12-2015 at 10:12
DOH !
Thanks for pointing that out gdflp.
A small pot of some heavy orangey brown nastiness has been sitting on my desk for a while.
I tried to make SnCl2 with tin metal and conc HCl.
Boiling it down removed the water, so it's a pot of mostly Sn(OH)Cl.
Chemicals from paint n stuff?
DemonsHeadshot - 22-12-2015 at 06:33
So I was looking for toluene but I couldn't find it any where here so I thought maybe paint thinner contains toluene so could anyone help me on how to
identify different solvents such as MEK,DMF or toluene? I know the smell of acetone but do these also smell? Also I found out that paints have nitro
cellulose so could I possibly recover the nitro cellulose from them?aga - 22-12-2015 at 06:51
There are several threads on paint thinners in this site with details of how to extract the DCM, Toluene etc.
Yes, Toluene smells.
Google is your friend.
Please put these type of unreferenced/unresearched questions in the Beginnings section.
[Edited on 22-12-2015 by aga]DemonsHeadshot - 22-12-2015 at 06:53
Sorry for my mistake, I haven't explored the site much.. Anyways thank you!bismuthate - 22-12-2015 at 12:17
You may want to look of the MSDS of whatever paint you have. aga - 22-12-2015 at 13:19
Sorry for my mistake, I haven't explored the site much.. Anyways thank you!
Exploring this site is quite difficult (as there Soooo Much stuff here) unless you use google with the search term :
site: sciencemadness.org "what you want to know"
I posted something similar to your question a couple of years back
The First thing i wanted was the Toluene.
This turned out to be as simple (thanks to Praixchys) as adding some distilled water and shaking the mixture, then leaving to settle for a few
minutes.
The Toluene is not soluble in water, so you get two layers (phase separation).
Wiki says that toluene has "Density: 866.90 kg/m³" so it's Lighter than water, so it will be the top layer, which you can just pour off.
The Lower layer contains all the other stuff, and you'll have to distill them off, cutting the fraction at the various vapour temperatures you would
see as the distillation proceeds.
If there's any DCM, it will come over first.
Do you have an intended use for your Toluene ?
[Edited on 22-12-2015 by aga]diddi - 22-12-2015 at 20:28
There are plenty of industrial solvents that contain a lot of toluene. go visit your local panel beater (auto painter) and ask if you can buy a bit
from them. check the MSDS as already suggested and then you know which do the job you want best.
DemonsHeadshot's thread of many questions
DemonsHeadshot - 26-12-2015 at 06:25
Hello everyone, today I would like discuss about melting lithium. So far I have melted some miligramic quantities and when melted in an oil (I used
vegetable oil) the oil turns to black and when it is cooled down, it becomes jelly like and the lithium balls don't coalesce each other, any way to
coalesce them?
[Edited on 26-12-2015 by Bert]kecskesajt - 26-12-2015 at 06:26
The vegetable oil reacts with litium to form soap.Mabus - 26-12-2015 at 10:03
Vegetable oil contains triglycerides that react with alkali metals. Use dry mineral oil, in an argon atmospheredeltaH - 26-12-2015 at 10:10
Soap? ... Not so much, but it does make a fantastic grease, so don't throw it away DemonsHeadshot - 26-12-2015 at 10:35
It is pretty nasty to work with, I have some mineral oil but I am never gonna find argon here... Although I melted some pellets with the vegetable oil
so if anyone wanna see pictures of it
Oxalic acid to formic acid?
DemonsHeadshot - 26-12-2015 at 11:05
Is it possible to convert oxalic acid to formic acid by heating oxalic acid with sodium hydroxide?
[Edited on 26-12-2015 by Bert]
[Edited on 26-12-2015 by Bert]aga - 26-12-2015 at 11:20
This an Organic Chemistry question, however there is no procedure, no reference, no homework, no way to repeat your process, so Beginnings is where
you should ask.
Sorry to keep banging on about this kind of thing, just that the forum would look a lot better with Chemistry in the relevant sections and random
questions in Beginnings.Bert - 26-12-2015 at 11:26
No lab report or references, this kind of thing goes in beginnings.
Actually, I'm going to lump ALL your questions into a single thread, until you read the FAQ and get the hang of how things are done here.stygian - 26-12-2015 at 11:27
From 1911 encylopedia article on formic acid:
It may be prepared artificially by the oxidation of methyl alcohol and of formaldehyde; by the rapid heating of oxalic acid (J. GayLussac, Ann. chim.
phys., 1831 [2] 46, p. 218), but best by heating oxalic acid with glycerin, at a temperature of iooI to° C. (M. Berthelot, Ann., 1856, 98, p. 139).
In this reaction a glycerol ester is formed as an intermediate product, and undergoes decomposition by the water which is also produced at the same
time.mayko - 26-12-2015 at 11:31
Heating oxalic acid or its salts can produce carbon monoxide, so this reaction could well be hazardous even if it worked. Heating glycerine and oxalic
acid seems to be the most popular prep, and it's been on my to-do list for a while:
