opfromthestart
Harmless
Posts: 46
Registered: 23-12-2018
Member Is Offline
Mood: tetranitrammmonium chlorate
|
|
Ideas
I have a large interest in chemistry but don't have much access to lab supplies. I was wondering if you guys have any ideas.
Supplies:
1.8L .8M NaClO
1.1L NH4OH
1.4L 2.7M HCl
100g Fe2O3
600g KCl
300mL Acetone
2L 3% H2O2
370mL Iodine(povidone-iodine)
400mL 70% ethanol
1L 91% isopropanol
300g NH4NO3
1.7 kg NaHCO3
450g NaClO3
3.3L 24% CH3OH
22.6kg CaCl2
500g nearly anhydrous MgSO4
20g MnO2
|
|
|
j_sum1
Administrator
Posts: 6220
Registered: 4-10-2014
Location: Unmoved
Member Is Online
Mood: Organised
|
|
I am assuming that this list is what you have, not what you want. It looks like a pretty versatile start. A lot depends on what interests you.
Inorganic is generally a less demanding place to explore.
A lot of people have gotten a lot of enjoyment with copper chemistry. There is an amazing range of salts. Search for "copper carnival" competition and
check out the winning submissions for some procedures.
I have enjoyed disassembly of lantern batteries to extract the elements. There is a lot to be learned from that.
Growing crystals.
Electrolysis, if you have a power supply. Numerous projects possible.
If you can get hold of some Al powder, thermites of various kinds.
Begin an element collection. Plenty of projects there.
Esters.
Depending on equipment available, plant extractions. Caffeine, theobromine, thymol, capsacin, piperine, camphor... Depending on what is around.
Extraction and purification of chems from otc products. You will never regret having some DCM around.
Don't forget that you can add to your supplies using over the counter products. Aspirin, peroxide, essemtial oils, pottery glazes, paint thinner, pool
chems, sulfur from gardening supplies... Many many possibilities.
Edit
Please forgive any typos I missed. I am using a small phone keyboard.
[Edited on 24-12-2018 by j_sum1]
|
|
|
Ubya
International Hazard
Posts: 1232
Registered: 23-11-2017
Location: Rome-Italy
Member Is Offline
Mood: I'm a maddo scientisto!!!
|
|
well if you just want a list of all the possible reactions using those reagents it's quite boring, you have a large interest in chemistry but can't
figure out what to do with that stuff?
plus, you don't have acces to lab supplies, alright but what do you have other than reagents? it's important as some experiments can't be done in just
jars or drinking glasses.
it's quite a broad question, anyway just to give some ideas:
-extracting iodine or iodide salt from the povidone solition
-ferric chloride
-iodine and ammonia to make nitrogen triiodide (make less than a gram of this)
-some esters if you could find acetic acid and sulphuric acid
-sodium carbonate by heating sodium bicarbonate over 80°C
-calcium carbonate from calcium chloride and sodium carbonate
-chlorine gas from MnO2 and HCl
-drink the ethanol
as a general rule first think of an experiment and then get the supply, this way you don't stock kilograms of reagents that won't ever be used
[Edited on 24-12-2018 by Ubya]
---------------------------------------------------------------------
feel free to correct my grammar, or any mistakes i make
---------------------------------------------------------------------
|
|
|
opfromthestart
Harmless
Posts: 46
Registered: 23-12-2018
Member Is Offline
Mood: tetranitrammmonium chlorate
|
|
Thanks for the ideas
About the calcium chloride, i have that just for road salt but bought it thinking i could use it for chem too with processing.
|
|
|
j_sum1
Administrator
Posts: 6220
Registered: 4-10-2014
Location: Unmoved
Member Is Online
Mood: Organised
|
|
CaCl2 can be dehydrated in an oven and is a good dessicant.
If it is road salt qualuty, I would purify it first.
|
|
|
Tsjerk
International Hazard
Posts: 3022
Registered: 20-4-2005
Location: Netherlands
Member Is Offline
Mood: Mood
|
|
I wouldn't start purifying road quality CaCl2, unless you really like recrystallizations, it is OTC in much higher purity in moisture absorpers for a
few bucks. And if you like crystallizations I would go with other compounds.
You could try and separate metals from different coins into the different metals (as metal or as metal salt) you would probably need some more
compounds, but they should be OTC.
Edit: you should try to get some sulfuric acid, it is very versatile. Maybe you can get it as battery acid (get new, not used acid!), or as drain
cleaner. Usually battery acid is clean, but about 6 M, and is drain cleaner contaminated but > 90%. 6 M is contrated enough for most experiments.
[Edited on 24-12-2018 by Tsjerk]
|
|
|
AJKOER
Radically Dubious
Posts: 3026
Registered: 7-5-2011
Member Is Offline
Mood: No Mood
|
|
Prepare HOCl and a precipitate of CaCO3 from 2 NaOCl + CaCl2 + 2 NaHCO3.
The fine precipitate of CaCO3 is photo catalytic (as are carbonates in general in select light releasing an electron and the very acidic carbonate
radical, see https://pubs.acs.org/doi/abs/10.1021/j100909a029?journalCode... and my Acidic Radicals thread at http://www.sciencemadness.org/talk/viewthread.php?tid=94166#... ). Note, with the electron in the presence of an acid source, e- + H+ = •H, the
very powerful hydrogen atom reducing radical (think nascent hydrogen), which will attack NO3- and create OH- and NO2, also •H + ClO3- = OH- +
ClO2,..., and with more •H, even further reduction is possible.
Use the NaOCl or HOCl in a bleach battery to make electric power, Al(OH)3 and some Cl2 (using HOCl).
See my related electro syntheses of CuO (see http://www.sciencemadness.org/talk/viewthread.php?tid=84047#... ), ZnO, Al2(SO4)3,....using a galvanic cell concept (in essence, anodic corrosion
of copper or zinc or..., versus a more noble, say carbon, electrode in a battery cell).
Prepare Singlet Oxygen (see http://www.sciencemadness.org/talk/viewthread.php?tid=31729#... ) which with oxygen may make some very strong (but transient) oxidizing atomic
oxygen that in the presence of, for example, ClO3-, I would speculate could form Cl04-. Source on atomic oxygen: See Eq 4 at http://olab.physics.sjtu.edu.cn/papers/2017/29.Huan%20Yue_PC... , where apparently, O(3P) is created from severe collision quenching of O(1D) atom
with air or oxygen and acts as the major oxidant in the work by Huan Yue and colleagues ‘Exploring the working mechanism of graphene patterning by
magnetic-assisted UV ozonation’. Note, O(3P) is also known as highly reactive ground-state 3P oxygen and a form of atomic oxygen.
Photolysis may also be a path to perchlorates. To quote a source (https://agupubs.onlinelibrary.wiley.com/doi/full/10.1029/200... ):
"[20] A role for water ice as a reaction surface for adsorbed species may be a possible path to perchlorate chemistry. ClO radicals are readily
produced by atmospheric oxidation of chlorine volatiles, and ClO can interact on ice to produce OClO when the ice sublimates [McKeachie et al., 2004].
Chlorine dioxide (the OClO molecule is not to be confused with Cl‐O‐O, which is the chlorine peroxy radical, unfortunately also sometimes called
“chlorine dioxide”) is a possible source of perchlorate because it can react with O3 or O to make chlorine trioxide [Wayne et al., 1995]:"
Followed by:
•OH + •ClO3 = HClO4
And while •ClO is easy formed by the action of a radical (•OH or •CO3-) on the hypochlorite ion in common bleach:
•OH + ClO- = OH- + •ClO
the whole sublimation of •ClO + ice under UV is likely a bridge too far as a path to •OClO radical. However, per another source (https://www.researchgate.net/publication/222104943_Observati... ):
"The ClO + BrO reaction is presently believed to be the only source of OClO in the stratosphere, although several studies show this reaction system to
severely underestimate OClO production in this atmospheric subsystem"
Is a more likely path to the OClO radical, as in an albeit slow reaction:
OCl- + Br- = Cl- + BrO- (see http://old.sustainability.gatech.edu/publications/Ozone_Brom... )
just add hydroxyl radicals (from say the UV photolysis of aqueous N2O or the action of HOCl on Fe(ll) , or the action of microwaves on activated
carbon, ...) to the system and then the atomic oxygen. Speculation? Perhaps or not (see https://www.researchgate.net/publication/250142618_Bromate_c... and https://awwa.onlinelibrary.wiley.com/doi/full/10.5942/jawwa.... ).
[Edited on 25-12-2018 by AJKOER]
|
|
|
opfromthestart
Harmless
Posts: 46
Registered: 23-12-2018
Member Is Offline
Mood: tetranitrammmonium chlorate
|
|
Thank you for the ideas. I will try many of these.
Quote: Originally posted by AJKOER  |
Prepare Singlet Oxygen which with oxygen may make some very strong (but transient) oxidizing atomic oxygen that in the presence of, for example, ClO3-
may form Cl04- . Photolysis may also be a path to perchlorates.
|
Do you have a link for how to do this? I'd rather not trust my own searching.
Also any ideas of reagents that I should have and how to obtain/synthesize them would be useful.
Thanks again.
|
|
|
AJKOER
Radically Dubious
Posts: 3026
Registered: 7-5-2011
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by opfromthestart | Thank you for the ideas. I will try many of these.
| Quote: Originally posted by AJKOER |
Prepare Singlet Oxygen which with oxygen may make some very strong (but transient) oxidizing atomic oxygen that in the presence of, for example, ClO3-
may form Cl04- . Photolysis may also be a path to perchlorates.
|
Do you have a link for how to do this? I'd rather not trust my own searching.
Also any ideas of reagents that I should have and how to obtain/synthesize them would be useful.
Thanks again. |
Yes, a good idea, so I have added some links and source references.
----------------------
For reducing, I recommend in situ creation of the hydrogen atom radical (cited as the major reducing specie by Buxton in solution, see Eq 3 on page 2
at https://pdfs.semanticscholar.org/d696/b35956e38351dd2eae6706...). Chemisorption of the radical on the surface of metals like Zn, Al and Mg with a
limited lifespan is also possible. My prior related comment:
| Quote: Originally posted by AJKOER |
.......
Next, imbue the surface of Mg or Al with the hydrogen atom radical (from the traditional nascent hydrogen generation methods based on say Al/NaOH).
One may assume that the •H radical functional behaves (per its seemingly reversible formation reaction: e- + H+ = •H ) as apparently a (e-,H+)
pair acting on ions. For an example from 'Hydrometallurgy 2008: Proceedings of the Sixth International Symposium', p. 818, a commercial reductive
leaching equation, to quote:
" PbS + 2 •H = Pb + H2S (5) " (see https://books.google.com/books?id=1etfSdk55SYC&pg=PA818&... )
which I view functionally as follows:
Pb(+2)S(2-) + 2 (e-, H+) = Pb + H2S (g)
......
[Edited on 4-10-2018 by AJKOER] |
Although some on this forum, even given the above proposed commercial application of surface active hydrogen radicals, remain skeptics (apparent
current, or want to be, residents of the show me state of Missouri). Although some may actually point to the 'Make Potassium' thread on this very
forum as an illustration of the power of chemisorption of this very radical on the surface of Mg metal, which could account for some reported oddities
when working with different surface forms of the metal in achieving results (for example, per NeonPulse on p.63, "So I did another test last night and
found the fineness and shine of the Mg is really the key factor in my successes" and also per Experimentor, p. 64, "The simplest possible routes I
could find are the Zn/HCl reduction or..", which sounds like a classic nascent hydrogen path). The fact the formation of K is not proportional to the
mass of Mg (but surface area of pure magnesium metal) implies it is not a standard chemical reaction (see comments by S.K. Sadrnezhaad, et al, in
'Kinetics of Silver Dissolution in Nitric Acid..., at http://www.sciencemadness.org/talk/viewthread.php?tid=110811... ).
[Edited on 24-12-2018 by AJKOER]
|
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
