I figured since this is a random experiment threed then I may as well add random notes that I have been keeping here and there within reason of course. Alot of this may not make sence to anyone you but ill attempt to doctor it here and there to make it more readable. Understand much was written in a haste long ago and where written for my eyes and not anyone elses so any questions or corrections feel free to ask.

Cavone removal from Dill oil
28.7 * .15  = 4.305 apiol
28.7 * .552 = 15.8  carvone
28.7 * .166 = 4.7642 bylimonene
28.7 * .037 = .790

30gr h20
3+3+33311 bisulfite 114.2

30grm bs + DA + 50ml h2o

104.06 sBisulfite

15.9994 oxygen
1.00794   hydrogen
32.065 sulfur


81.07114 solfonic acid mol    (=O)-SO2OH


    H
   /
R-C--OH
   \
    SO2Na

Addition of sodium bisulfite- a reaction formed from aldehydes and some ketones
saturated(40%)(aq) solution



Sodium nitrate from Ammonia nitrate and Sodium Bicarbonate
Na           23.00    g/mol
O            16.00    g/mol
C            12.01    g/mol
N            14.01    g/mol
H             1.00    g/mol


03           48.00    g/mol
NO3          62.01    g/mol
NH3          17.03    g/mol


Reagents and Materials            Formula    Molar Weight
-----------------------------------------------------------------------
28.8 grams sodium bicarbonate     NaHCO3     84.007 g/mol
27.5 grams ammonia nitrate        NH4NO3     80.043 g/mol
------

27.5 grams sodium nitrate.        NaNO3      84.990 g/mol

2d attempt
-------------
79.3     grams ammonia nitrate
39.5     grams sodium hydroxide              39.997 g/mol

3d attempt
----------------
79.4 grams ammonia nitrate
83.  grams of sodium bicarbonate


Results
-----------------
1: 27.5 grams sodium nitrate
2:
3: 74   grams sodium nitrate


discussion
----------------
1: product was a bright white when dried after some effort.27.5 grams it a little two high and makes me think that some bicarbonate contamination is in the mix because after a lose of NH3 and a
gain of Na there should be a net lose in the molar weight yet quantitive yeilds where observed.

2:lots of fizzing and very strong ammonia smell. It has come to my attention that the NaOH I was using was a mix of NaOH and KOH so the ratio will
be way to low for my liking so I will attempt another bicarbonate reaction.
After it had dried I added a very small portion of NaOH and the smell of ammonia became appearent so More conversion could be used because as it stands now it is a
mixture of sodium/potassium/ammonia nitrate.
After drying a small amount of NaOH solution was added and the smell of ammonia because quickly appearent so it it obvious that a total conversion did not take place.
Im going to slowly add more and dry and ad more and dry until i no longer smell NH3 from NaOH addition. Smells gone now but it has a hint of urinal smell

3: 2mm crystals precipitated and where dryed but there is some concern with H2O being traped within the crystal structure so i am going to grind it very fine and continue heating it.



Next phase:Sodium Nitrite

CaO        56.0774    g/mol
NaNO3      84.994669  g/mol
NaNO2      68.995267  g/mol

nitrite percent of nitrate = 81.175289%

nitrite = 18.824711% loss in weight

ammonia nitrate
------------------------
Molar mass 80.043 g/mol

Sodium bicarbonate
------------------------
Molar mass 84.007 g/mol



78.5


.980722%

82.38.

61.7 total bicarb
58.7 total NH3NO3
118.8 total weight of reactants


.734462







Urea/ammonia chloride seperation
NH4Cl       29.7 g/100 water at   0 °C
(NH2)2CO   108   g/100 water at (20 °C)


Mercuric Chloride

2.6gr   Hg
52.1gr  h2so4
---Heat--->20 minutes---->large SO2 production and irritating oder
White flat needles crystals on cooling.



Piperine to pipernol weight loss
piperine ----> pipernol = 52.6%
285.33766      150.13144 




Mn(IV) Electrochemical Cell and other

------------------------------------------------------------------------------
H2SO4 = 98.08
MnO2  = 86.94

17.8


{======Neograviton quote=============================================================================================================================
Here is a easy way to do it with Mn(V)sulfate. A way I used many time!

1:First get some MnO2. You can buy it as "Manganese-Black" a pigment for cement and concrete. Thats about 70% MnO2.

2:Then put it in an equimolar amount of H2SO4 (100%) and heat it up. Make it really hot. (>200°C).

3:Let it be there for about half an hour. When I do this, I let The acid become so hot, that white steam comes out.

4:After that, let it cool down. You just have made Mn(V)SO4. It is soluble in 37% H2SO4 (battery acid) with a deep, chocolate like brown color.

5:After that put it 1:1 with the toluene in about 60% H2SO4 (enough H2SO4, so that nearly everything dissolves).

6:Heat (or cool) it to about 50-60°C and stirr it well. After 3-4 hours you will have mostly Benzaldehyd (in my cases about 70%)

7:Distill the Benzaldehyd/Toluene out by a simple steam distillation. (Just boil water out, until there is no oily layer any more)
  When you start boiling that stuff, the color of the liquid becomes sand-like. Thats because the rest of the Mn(V)SO4 breaks down to Mn(II)SO4.

And now the best: just put the liquid in a electrolytic cell (in the anode-part) and put some electricity through it, while stirring.
 The color will chance to chocolate brown once again, and you can use it again!!! About 6 times!
================================================================================================================================================}


100 grams 93% H2SO4 = 93 grams H2SO4 = .9482 mol per 100 grams.


100/.93% = 107.526 grams H2SO4

1.1281 grams 93% H2SO4 per 1 gram MnO2
            95.313 grams MnO2

==============================================================================
------------------------------------------------------------------------------

20 grams MnO2 added to 22 grams H2SO4








Sodium acetate / bisulfate to acetic acid
120.6 sodium bisulfate 66.359%
82.03 sodium acetate.  .2438

25.3700 grams sodium bisulfite
20 grams of sodium acetate = 14 grams acetic acid = 15.35817822 ml acetic acid from 20 grams of pure (anhy)sodium acetate
.2438

sodium acetate -- > acetic acid === 73.2039% weight kept from the conversion/



Ethyl Bromide synthesis

Materials
----------------------------------
NaBr
Molar mass 102.894 g/mol  / 53 = .5150

H2SO4
Molar mass 98.08 g/mol * .5150= 50.5112 grams

C2H6O
Molar mass 46.07 g/mol  * .5150 = 23.726
--------------------------------------------
HBr
Molar mass 80.91 g/mol
--------------------------------------------

==============================
Products
----------
C2H5Br
Molar mass 108.97 g/mol * .5150 = 56.1195

H2O
Molar mass 18.01528(33) g/mol * 2 = 36.03056 * .2526 = 9.10

NaHSO4
Molar mass 120.06 g/mol

==============================================
2NaBr  + H2SO4 = Na2SO4 + 2HBr
2EtOH  + 2HBr  = 2EtBr  + 2H2O
==============================================
Based on 52 gram pack of NaBr
-----------------------------------
52grams NaBr / 1mol NaBr = 50.53%

1mol H2SO4 * 50.53% = 49.55   grams H2SO4 / 2 = 24.775 grams H2SO4
1mol EtOH  * 50.53% = 23.2791 grams EtOH

==============================================
Conclusion
------------------------
IN
---
NaBr  = 52
H2SO4 = 49.559  grams
EtOH  = 23.279 grams

Equals 100.0469 grams
========================
OUT
---
EtBr   = 55.051  grams * 1.14(density)  = 62.7ml
Na2SO4 = 35.886
H2O    =  9.1031grams

Equals  100.0401
==============================================

EtBr boiling point = 102 degrees F
EtOH Bp = 173 degrees F



Dibromoethane

NaBr + H2SO4 = HBr + NaHSO4
HBr + C2H4(OH)2 = H2O + C2H4(Br)2

Materials / Total mass in 396.008
----------------------------------
H2SO4
Molar mass 98.08 g/mol * .5053 = 49.55 grams

NaBr
Molar mass 102.894 g/mol  / 52 grams = 50.53%
--------------------------------------------

Na2SO4
Molar mass 142.04 g/mol (anhydrous)

HBr
Molar mass 80.91 g/mol  * .5053 = 40.883 grams


C2H4(OH)2
Molar mass 62.068 g/mol * .5053 = 31.362 grams 




49.55 grams of H2SO4 and 20 grams of H2O is added to 31.362 grams Ethylene Glycol. 52 grams of finely powdered Sodium Bromide is added and reaction is stirred until sodium bromide is consumed. Dibromoethane distills over at 131-132 °C.
 


EtOH placed into a cold water bath and 130 grams of 45% H2SO4 was added slowly via dropper seringe over a 10 minute period inorder to keep the heat down



KI tablets Iodine extraction
---------------

active
---------
120 pills*
84mg calcium 10.08 grams calcium         : as dibasic phosphate#Solubility: Practically insoluble in water.
32.5 mg = 3900mg KI                             : Solubility in water 128 g/100 ml (6 °C)

Inactive
--------------
dibasic calcium phosphate
steric acid
mod cellouse gum
magnesium stearate.


35.8 grams 150ml Distilled H2o

Time 1:20

200 ml total after addition to wash remaining calcium phosphate.
evaperation reduced to dryness
2.7 grams yeild yellow powder sticky when damp.






Ammonia Methyl Sulfate

50.1 grams of Sulfamic acid
105 ml of MeOH.
Refluxed N? Hours







As you can see much is incomplete due to the fact that I find paper notes more rewarding but now and then I need to figure up a quick number or two and save it there.

Wiki says,

Hydroxylamine can also be produced by the reduction of nitrous acid or potassium nitrate with bisulfite:

HNO2 + 2 HSO3? ? N(OH)(OSO2)22? + H2O ? NH(OH)(OSO2)? + HSO4?
NH(OH)(OSO2)? + H3O+ (100 °C/1 h) ? NH3(OH)+ + HSO4?

Sedits thoughts are, "Thats suppose to be KNO2 not KNO3"

But a spoonful of KNO3 was added to warm water. A spoon of Sodium Bisulfate was added.........Fuck bisulfite, bisulfite.... well that explains it somewhat. Hence the term random. I seen it, I tryed it, I read it wrong..

Oh well,

Anyway bubbles came up and im not quite sure what they where,

Any suggestions?

Yeh I think your right as a different batch of NaNO3 created differently did not react the same.



New experiment:

Some will understand my reason for doing this test......

1ml of Black Mangenese persulfate oxidiser was added to 1ml of HCl. Fumes appeared but its a bit humid so there where fumes from the HCl anyway. As soon as they where mixed though the smell changed from HCl fumes to what seemed like Hypo Chlorate fumes and the smell was strong. It appears that the Mn(IV)sulfate oxidiser is strong enough to oxidise HCl to Hypochlorous acid (HClO) quickly.

The solution after about 20-40 minutes changed from black to yellow and the smell of HClO appeared to drop to almost nothing which strikes me as odd because I would think the smell would persist is indeed HClO was still in solution.

sedit, how do you know that the Cl^- isn't being oxidized to Cl?

That one was pretty recent zz-zhuchila, Full experiment is here. Worked out well Ala getto.
http://127.0.0.1/talk/index.php/topic,32.0.html

Your all more then likely correct in that its oxidising Cl which in H2O like you said it yeilding the HOCl.
It will be easy enough to test as NaCl should yeild the same smell that I was getting. Vesp did you notice the bleach smell when adding the NH4Cl? Im still woundering though if Mn(SO4)2 is even the correct product of the electrosynthesis to begin with. Im starting to wounder if activated MnO2 is the real oxidiser in all of this because there is much black slug that forms when the ozone smell appears, see other threed for toluene oxidation as I was messing around with it a bit last night.


As far as the KNO3 is concerned, yeh Im not going to go any deaper into that as it would just be a waste of material. However I will play some more when I get some Bisulfite to test the correct reaction with.

The black slug is suppose to be the Mn(IV). The smell of ozone though throws me off because I know that when Mn2O7 decomposes to O3. The smell of O3 is strong when the finished oxidiser is run cold.

Just a bit bord so i decided to play with some nitromethane and a mixture of Nickle and copper salts made from a normal nickle coin with a concentration of something on the order of 25% Ni / 75% Cu.

Anyway the dryed salts where dissolved in H2O and HCl dripped in to Dissolve some oxides that where mixed in from prolonged sitting. Slightly heated to drive off HCl and then Some MeOH added. Fine bubbles started to rise and fear of them being Methylchloride I decided to leave this outside for some time followed with a hot water bath to try to remove any MeCl that may be there. I then added Nitromethane streight from the can (This is a random experiment threed get off my back youll get the goods later ) and then added some Aluminum slivers cut from flashing.

It bubbled at an increasing pace and I left it still outside stirring for quite a while. When I came back the Copper had precipitated as well as a black slug presumably Nickle or Aluminum ... or both for that matter.

When all said an done I evaporated off much of the methanol and basifyed with a bit of strong NaOH solution. There was a strong smell of Methylamine.



Results:

The Methylamine could have withease been formed under acidic conditions thue dissolving metal reduction of aluminum so there is not much conclusion. I soon plan on getting some Styrene and pure Nickle salts to try a few more things with it such as condensation of MeNO2 with styrene and attempting to reduce to Phenylethylamine. If it does reduce the nitrostyrene to Phenylethylamine is should prove applicable to use on other simular substrates.

knoevanagel style condensation of nitro alkanes onto styrenes?
i don't think it will happen.
condensation would be misnomer really it would be addition to the double bond.
never heard of nitroalkanes adding to double bonds you have any literature?

Aluminum foil balls prepared for use in an amalgum a while ago was added to Potassium Nitrate, NaOH solution. Faint bubbling forms with no smell until the temperature runs to high then the smell of ammonia becomes extreamly strong as the exothermic runaway takes over. Aluminum reduces nitrates to nitrites under 60 degrees with Ammonia being the product if the temperature climbs to high. I have never heard of discussion of this being performed in a solely aq enviroment though.

My guess would have to be that the same principle could be applyed using Al in MeOH/NaOH + MeNO2 to bail methylamine out of the reaction mixture.

This will be toyed with later I guess. Easy enough to test just mix and wait then smell.

Tiny bit of NaOH and low temperatures it is Vesp... Work up to clear the nitrite from the aluminum compounds don't seem practical right now though so thats the current road block.

Now back to our currently scheduled ADD programing...........

pool EDTA metal chelating solution containing EDTA, Sodium metasilicate, limonene(IIRC), and polysorbate. When Muriatic acid is added to it in equal portions needle like crystals start to precipitate and the smell changes from citrus to the smell of cedar wood. This has me more interested then anything considering I love the smell of cedar. I would have to assume at first guess that it has to do with the Limonene undergoing some form of reaction leading to the smell of cedar. Anyone have a guess as to what?

Also what do you think these crystals(about 1mm -2mm long) are? Are they the hydrolysis product Im after(EDA*(HCl)2) slowly precipitating in this mixture of crap? That would be real nice lemme tell ya, but.... If I learned anything from organic chemistry its if something seems to work with ease you done did it wrong.....