Polverone
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Registered: 19-5-2002
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Mr. Anonymous: improved hydrazine sulfate
Our mysterious friend has sent a chapter from his new novel in progress here for our enjoyment. It seems to be about refinements to his earlier
hydrazine sulfate synthesis.
| Quote: | Hydrazine Sulfate from urea and pool chlorinator is a synthesis which has been previously described. From six recent experiments there has been
discovered and proven several refinements providing significant improvement upon the original process first reported. The improved method is more
economical, and produces a higher yield of better product. The revised proportions of ingredients and temperatures and reaction times are confirmed to
better control the foaming of the reaction mixture. During the series of six experiments small modifications upon the earlier synthesis which is an
OTC adaptation of GB392845 have been evaluated, and the experiments produced consistently good results for each run.
The changes involve a larger batch size, a heavier stirbar, higher initial reaction temperature, and use of HCl for neutralization of the basic sodium
compounds, before using sulfuric acid to precipitate the hydrazine sulfate by a method that improves the yield and quality of the crystals. It has
been discovered that it is useful in the neutralization stage to first use HCl equivalent to approximately the required amount for converting the
theoretical amount of Na2CO3 reaction by-product to NaCl. Then the remaining portion of the neutralization / acidification is accomplished with a much
reduced requirement of H2SO4 for producing the hydrazine sulfate. Using HCl for the bulk of the neutralization is more economical, and it also
eliminates the contamination by hydrated sodium sulfate by-product which is produced at near saturation levels if the entire neutralization /
acidification is done using only H2SO4. Using HCl for the main portion of the neutralization also considerably reduces the total exotherm during the
neutralization. The crystalline form and density of the hydrazine sulfate produced by final acidification using diluted H2SO4 is improved, and it
crystallizes out in better yield, when the acidified reaction mixture containing hydrazine sulfate is predominately a sodium chloride solution,
instead of a mixed solution of sodium chloride also containing large amounts of sodium sulfate. Previously, solutions resulting from the entire
neutralization / acidification done using only H2SO4, could not be cooled down very cold without contaminating the hydrazine sulfate precipitate with
a hydrated sodium sulfate coprecipitate. Six syntheses using the new method have confirmed a purer end product is obtained by making use of HCl for
the first portion of the neutralization, and then using diluted sulfuric acid to complete the neutralization / acidification which precipitates the
desired hydrazine sulfate, consistently resulting in better formed crystals of improved density and purity.
These more dense and better quality hydrazine sulfate crystals perform much better in subsequent reactions where hydrazine is freebased from its
sulfate, requiring only half the previously required amount of added water to create stirrable slurries with NaOH for methanol extraction of the
freebase hydrazine hydrate. The more dense better formed crystals of hydrazine sulfate may be freebased to hydrazine hydrate by portionwise additions
of solid NaOH, the water produced as a by-product of the freebasing being almost sufficient alone for creating a stirrable slurry capable of being
extracted with methanol, taking up the hydrazine hydrate in methanol while leaving behind the sodium sulfate as an insoluble residue. In practice it
has been found that only 10 to 12 ml of added water per mole of hydrazine sulfate is sufficient for the purpose of keeping the mixture in the form of
a slurry able to be extracted easily by methanol in sequential portions which are decanted from the residue until the hydrazine has been effectively
extracted from the insoluble residue of sodium sulfate crystals. Reducing the added water requirement to this small amount in the freebasing of the
hydrazine has eliminated the need for elaborate dehydration schemes using alkoxides to obtain acceptable yields of sodium azide directly from the much
drier methanolic extract of hydrazine hydrate.
For the synthesis of sodium azide, methanolic hydrazine hydrate extract is further basified to slight excess of an equimolar amount of NaOH and
treated in the cold with a slight equimolar excess of isopropyl nitrite (preferable), or equivalent of ethylene glycol dinitrite, to consistently
produce sodium azide directly, in 65 per cent total yield based on the hydrazine sulfate used for the freebasing of hydrazine hydrate into methanol.
The improved freebasing technique using reduced added water provides a useful yield of sodium azide by a process which involves no hazardous
distillations of hydrazine or other added tasks for chemical elimination of excess water. Isopropyl nitrite was found to have a low transesterfication
activity on contact with methanol in thecold, with cooling provided by immersing the azide production flask in an ordinary 0 degrees cold water bath
containing chunks of ice. With this cooling the partial pressure of methyl nitrite from transesterfication of the isopropyl nitrite was sufficiently
low that the back pressure provided by immersing a vent line from the closed apparatus to a depth of sixteen inches into a water filled carboy
prevented any free boiling away of the organic nitrite from the reaction producing sodium azide, until the reaction was very near its endpoint. After
three hours reaction in the cold, the temperature was raised to boil away unreacted nitrite and the back pressure peak upon heating to drive the
reaction to completion was raised to six feet of water, (about two and one half pounds per square inch of back pressure ), maintained for fifteen
minutes, before gradually reducing the back pressure to atmosphere and allowing complete boiling off of any unreacted nitrite. An alternate attempt to
freebase hydrazine hydrate and use isopropanol for the extraction failed because of the stratification of the liquid portion into two layers, leaving
much of the hydrazine hydrate in the heavier more aqueous layer unextracted by the isopropanol. Full details for the synthesis of sodium azide will be
provided in a later communication. This digression simply describes why the improved synthesis of the hydrazine sulfate is of special interest for
producing the hydrazine sulfate in better crystalline form by a method which improves its usefulness particularly as a precursor material for OTC
sodium azide, or when the purpose will be to freebase the hydrazine and extract it with methanol for any other use.
After the HCl / H2SO4 sequenced acidification of the mixture which precipitates hydrazine sulfate, the supernatant sodium chloride solution is far
below saturation so it can be chilled without worry for contaminating the hydrazine sulfate with sodium chloride, and this new method does not produce
the occasional gelation problems of the earlier method when sodium sulfate / sodium chloride solutions containing gelatine are chilled. There is
already indigenous NaCl present in the reaction system from the original manufacture of the sodium hypochlorite solution, as well as additional NaCl
produced
from the decomposition of the sodium hypochlorite in its reaction with urea, so it just makes sense to first cheaply convert the reaction by-product
sodium carbonate to NaCl, and then make a final addition of dilute H2SO4 to precipitate the hydrazine sulfate. That theory has proven correct by the
results of several variations of the example experiment detailed below. The best yield from this synthesis was 236 grams dry weight of pure sparkling
white crystals of hydrazine sulfate, from a total reaction mixture volume after neutralization / acidification of 3250 ml. ( 72 grams of hydrazine
sulfate per liter completed reaction mixture). The range of varying yields for six experiments was 221 grams to 236 grams. After several synthetic
steps are completed, the conversion rate is a minimum 125 grams sodium azide from the chemical conversion of one gallon of 10 per cent sodium
hypochlorite liquid pool chlorinator. The synthesis is cheap in terms of chemicals, but many hours of time and work are required for performing the
various intermediate steps to get from feedstock materials to the desired end product sodium azide. Thankfully, a small quantity of sodium azide goes
a very long way, so performing this synthesis only once provides an anonymous source of sodium azide sufficient for many years of experiments
requiring its use in the synthesis of experimental initiators.
The volume of the foaming at the highest point in only one experiment did not overflow the capacity of the 4 liter Erlenmeyer flask, but did rise to
just about one inch below the beginning of the straight section of the neck of the flask. In the average of several experiments the peak height of
the foaming did rise into the overflow funnel in amounts varying from 500ml to 1000ml exceeding the capacity of flask. Exactly why these variations
occur in the peak volume is unknown, but is probably due to slight variations in the dynamics of the reaction related to small differences in
temperature and also related to variations in the exact composition of the hypochlorite solution which changes from decomposition in storage as it
sits on the shelf. The reduced peak volume for the foaming mixture is not precisely constant. The peak volume of the reaction mixture can vary over a
range of a liter depending upon slight variations in temperature and stirring efficiency and small variations in the measured ingredients. However,
the average peak volume observed for several experiments has been reduced sufficiently to establish that a significantly increased batch size can be
managed in a four liter Erlenmeyer flask without experiencing any troublesome messy overflows due to excessive foaming. Optimum yields have been
obtained using the following proportions and generally it was found that for each one per cent deviation from the described quantities, a two to two
and one half per cent reduction in yields resulted. This optimization is derived from six experiments, so only a few variations were tested, and it
may be possible to perfect the proportions or reaction conditions further, after charting the results of many more experiments. But the procedure
described below has produced consistently good yields and smooth, predictable reactions for the several syntheses which were done in this particular
study.
Anyone wishing to do a charted study of the efficiency of the reaction would want to look at the quantity of gelatine across the range of plus or
minus a tenth gram above and below 2. 5 grams, the urea across a range of plus five grams from 180 grams, and the NaOH across a range of plus ten
grams from 255, adjusting the neutralization equivalents for the HCl requirement accordingly. The effect of a small addition of epsom salt in solution
up to say three grams does have a significant effect in the reaction by creating a colloidal dispersion of magnesium hydroxide, and the effect this
produces is a marked slowing of the color change transition from orange to almost clear, increasing the time duration for the reaction but not
improving yields. The inclusion of epsom salt or the use of ammonium hydroxide as solvent for the urea were both tried separately and in combination,
in an effort to improve the yields, but negative results were produced. In the case of ammonia, the reaction produced a geyser of foam and lowered
yields significantly. The best procedure determined from the results of the series of six experiments is described as follows:
Experimental:
1892 ml to 1900 ml (one half gallon US ) of 10 per cent Sodium Hypochlorite liquid pool chlorinator was placed in a one gallon glass pickle jar and
sealed with a threaded lid, placed into the freezer overnight to chill to 10 below 0 degrees centigrade. A three inch oval 60 gram stirbar was placed
into the jar and to the rapidly stirred cold sodium hypochlorite was added 170 grams of solid fine prilled NaOH poured into the vortex over two
minutes. Stirring is kept vigorous to dissolve suspended particles of NaOH and not allow
accumulation of solid material on the bottom. When all the NaOH was dissolved, the jar was resealed
and returned to the freezer to cool down again for several hours. When the solution was again freezing cold, an additional portion of 85 grams of
solid NaOH was added as before, for a total of 255 grams of solid NaOH, that is two thirds of the total being added in the first portion, and one
third in the second portion. When all of the NaOH is again dissolved, the basified sodium hypochlorite solution is sealed and returned to the freezer
for keeping. It is very important not to allow the sodium hypochlorite to become warm during these solutions of added NaOH. If your freezer cannot
chill the solution cold enough between additions of NaOH, then make smaller additions of NaOH in more than two steps in order to keep the sodium
hypochlorite cold. There is a large exotherm produced by the solution of the NaOH, so the sodium hypochlorite must be very cold at the beginning of
these additions of NaOH in order to absorb the exotherm without becoming warm, which would decompose the thermally unstable hypochlorite, and
significantly reduce the yield of hydrazine.
It is common for NaOH to be packaged in a plastic bottle of 510 grams. This is precisely the amount which would correspond to a gallon of pool
hypochlorite, or two batches of the size described here which can be done conveniently in a 4 liter Erlenmeyer flask.
In a one pint jar having a threaded lid is placed 182 grams of urea and 100 ml hot distilled water. In a second one pint jar having a threaded lid is
placed 2. 5 grams (two and five tenths grams) of gelatine and 100 ml hot distilled water.
A hot water bath and occasional swirling of these containers will assist forming clear solutions. The two solutions are combined in one container
before addition to the chilled hypochlorite solution. Any undissolved urea will dissolve in the combined quantity of water from the warm gelatine
solution, aided by gentle warming and stirring of the combined solutions. There is no need to keep the combined urea / gelatine solutions warm after
everything is dissolved. At this dilution the urea / gelatine mixture will not congeal even standing overnight so long as it is not subjected to cold
temperatures.
On a large stirrer hotplate is placed a 4 liter Erlenmeyer flask having a three inch oval stirbar of sixty grams weight. This weight of stirbar or
larger is recommended to prevent uncoupling in the viscous foam which initially forms in the reaction, and for creating sufficient turbulence to break
up and stir down the foam. A regular 3 inch by 1 / 2 inch octagon or polygon stirbar will uncouple at about 45 percent speed on the stirplate, but the
heavier magnet in the larger 3 inch oval stirbar enables it to remain coupled up to about a 65 per cent speed on the stirplate, which results in much
better stirring when a task like breaking up a viscous foam is required.
In the neck of the 4 liter flask is placed a one gallon plastic funnel whose stem is enlarged with a sleeve bushing cut from a two inch length of one
and five eighths OD, one and one quarter ID, tygon vinyl tubing, for a snug fit in the neck of the flask. The plastic funnel serves as an overflow
reservoir and return path for the foaming which usually exceeds the capacity of the flask during the reaction. The peak reaction volume can sometimes
remain within the flask, perhaps one in five is the chance the foaming reaction will not rise into the overflow space of the funnel, but the overflow
funnel will provide a useful added capacity which is more often going to be needed than the few occasions when it is not reached and partially filled
by the peak volume of foaming reaction mixture. It creates a messy and hazardous spill if an overflow of a hydrazine containing mixture goes pouring
over expensive equipment and contaminates a work area, so a cheap plastic safeguard against this risk is a good sensible precaution which should be
followed without fail every time this hydrazine synthesis is performed. If a large plastic funnel is not on hand, it would likely be sufficient to use
an empty three liter plastic soda bottle having its bottom end cut off with scissors, inverted and the neck of the soda bottle secured to the neck of
the flask with a strip of two inch wide duct tape. I have not tried this, but the foam temperature is mild enough that the thin plastic soda bottle
taped to the flask should work fine used in this way as an improvised overflow / return vessel. A small plastic bowl could be placed in the open end
of the soda bottle to exclude air and vent carbon dioxide escaping from the reaction mixture. The observation I have made is that the reaction should
be started cold, but not too cold, or
the gentle exotherm of the reaction will not smoothly sustain itself as the reaction proceeds on its own.
The thermodynamic curve of the reaction seems to favor beginning the reaction in a synthesis of this quantity, with the hypochlorite solution at about
5 (five) to 8 (eight) degrees centigrade. The foam viscosity caused by the gelatine content is reduced at this above freezing temperature, so the
foaming is easier to break up by rapid stirring, even though the initial reaction rate is slightly higher and more foam is being produced more
rapidly. Since the reaction begins at a higher rate initially, it also occurs that the foaming stage tends to last for a shorter duration, therefore
the foam begins to dissipate earlier, and the total reaction time from beginning to endpoint is reduced, with lower endpoint temperatures. Good yields
were observed with a reaction endpoint temperature of only 85 degrees centigrade. The best yields will generally result if the reaction mixture is
allowed to proceed for 25 minutes before supplemental heating is applied, unless the foam begins to dissipate and reduce in volume on its own at an
earlier time. At any point where the peak height of the foaming reaction begins to fall on its own, then the supplemental heating should be
immediately applied, and the heating begun at a twenty per cent level, ramped in like increments increasing every five minutes to drive the reaction
to completion. No problems with heat induced surge foaming occurred when this approach was used. The reaction proceeds smoothly with no reaction
lagging / surging problems observed.
A good way to estimate the correct pouring temperature for the basified hypochlorite is to remove the jar from the freezer and let it sit while the
apparatus for the synthesis is being assembled. A layer of frost will form on the cold surface of the glass jar. The stirbar is placed into a four
liter Erlenmeyer and the one gallon overflow funnel is inserted snugly into the neck of the flask, placed upon a large stirrer hotplate. Observe the
jar and note the time when the frost finishes melting. About ten minutes after the frost finishes melting, the cold basified hypochlorite is at the
right temperature for pouring through the overflow funnel into the flask. The stirrer should be started at about 40 per cent speed without any
heating, and the combined urea / gelatine solution poured quickly all at once through the overflow funnel into the vortex. The stirring speed should
be immediately raised to about 60 per cent. The funnel is covered with a plastic plate to provide a spatter shield and reduce exposure of the reaction
mixture to air. The reaction initiates immediately and a white foam rises quickly to almost the full capacity of the flask. After about fifteen
minutes, usually the foam begins to subside very slowly, and at twenty minutes the mixture is stirring more freely still with the level of the foam
having diminished further. A gradual slowly darkening in color towards orange will be observed as the minutes pass and the flask may feel slightly
warm to the touch. There will become visible an upwardly spiraling pattern of streaks in the foam from the action of the stirrer and the foam will
gradually stratify into two layers as it breaks up and begins to dissipate. The upper layer of foam will show a more coarse texture to the bubbles and
develop an open cell spongy appearance at the time when the foam is about to dissipate completely. At twenty-five minutes the volume of the mixture
sometimes reduces to 3200 ml, and supplemental heating is applied at a setting of 20 percent in any case. At thirty minutes the volume of foam is down
to 3100 ml, heating is increased to 40 per cent. At thirty-five minutes the volume of foam is reduced to 2900 ml, and heating is increased to 60 per
cent. The color of the mixture is becoming a distinct orange. At forty to fifty minutes, the foam has subsided to a clear transparent dark orange
solution. The stirring is reduced to 20 per cent in order to prevent vortex aeration and foaming caused by excessive stirring, and the heat kept at 80
per cent. Over the next ten minutes the orange color will gradually fade at a visible rate in the completing reaction. The color will fade to a pale
yellow, very light ale colored, almost clear solution and this will indicate the endpoint of the reaction. The reaction mixture is (preferably)
heated an additional five minutes after color fade ceases or optionally may be heated until moisture is condensing on the inner walls of the flask in
the neck area of the flask. The heating is discontinued.
Please note that the description given for time intervals and the behavior of the reaction at a particular time interval are a generalization, and
each reaction proceeds with its own individual variations upon that general theme. There are a range of peak volumes achieved, and time associations
may differ by a few minutes from one reaction to the next. These variations seem to have no adverse effect on the yield. The reaction may be complete
at 55 minutes or it may require twenty or even thirty minutes longer for the next reaction which is attempted to duplicate the reaction just
performed. And yet the yield may be identical for each run, in spite of the evident difference in the dynamics of the two runs. Go figure. The
conclusion at which I have arrived about this anomaly is that the reaction is simply sensitive to small variables which are then amplified in the way
the reaction responds, yet the general reaction proceeds well to produce consistently good results in spite of the reaction rate variations observed.
The overflow funnel is removed and the flask is quickly stoppered to exclude air. Then the flask is removed from the hotplate stirrer, and placed into
a pan of water to help speed the cooling of the contents. The flask should be stoppered, but occasionally during the first few minutes of cooling the
stopper should be dislodged to allow for breaking the vacuum produced as the hot water vapors in the flask condense. If this vacuum break precaution
is not performed, there is a risk of imploding an ordinary wall thickness Erlenmeyer flask. Do not leave the flask open to the air or the hot free
hydrazine solution may be decomposed by excessive contact with the air. There can initially be transients of pressure from effervescing carbon
dioxide, then vacuum from condensing vapors, so loosely stopper the flask and dislodge the stopper occasionally until the pressure variations
stabilize while the mixture is cooling.
After the flask has cooled in the plain water bath for about thirty minutes, it is placed in an ice water bath for about an hour to further cool in
preparation for the neutralization. The exotherm of the neutralization process to follow will cause the cool mixture to gradually heat up until it
becomes hot again. Pre-cooling the reaction mixture will allow the exotherm of neutralization to be absorbed without the mixture becoming excessively
hot or boiling from the heat of neutralization. Limiting the temperature this way helps control the fumes being evolved during the neutralization, and
also results in a consistent size of crystals for the precipitate which forms at the same time peak temperature is being reached.
While the reaction mixture is cooling, measure out a quantity of 650ml of 31. 45 per cent HCl (thirty-one and forty-five hundredths per cent pool
grade muriatic acid, 20 Degrees Baume) and place this 650 ml HCl in a suitable closed container and chill the pre-measured 650 ml of HCl in an ice
bath or in the freezer, in advance of its use for the first part of the neutralization reaction.
Also prepare a diluted sulfuric acid solution as follows : Place 175 ml cold distilled water in a 500 ml Erlenmeyer flask and place the flask in a
shallow pan of cold water. Slowly, (Caution Exothermic!) in four 50 ml portions add to the water a total of 200 ml of H2SO4 drain cleaner of 92. 5 per
cent H2SO4 concentration, swirling the flask after each 50 ml portion is added. After the heat of dilution subsides for a few minutes, place this
flask containing the diluted sulfuric acid in a separate ice water bath or freezer to cool it for later use in the final neutralization.
When the reaction mixture has cooled, the flask is returned to the stirplate and the stirrer is started with no heating. To the rapidly stirred
solution is added dropwise 650 ml of ice cold HCl 31. 45 per cent, at a drip rate of about 3 drops per second. Observe for any excessive foaming from
the neutralization of carbonate, and reduce the drip rate temporarily to reduce any excessive foaming if necessary. Hydrazine is decomposed by air,
and in order to reduce easy exposure to air through the open neck of the flask, I prefer to wind an inch wide strip of paper toweling above the tip of
the addition funnel until the thickness of the strip of paper toweling has formed a snug fit, effecting a one hole stopper which is a loose seal
between the neck of the flask and the funnel discharge tip. This allows the carbon dioxide produced during neutralization to escape, but prevents air
from freely swirling downward into the flask where it would contact the hydrazine. About three paper towels thickness folded back over itself until an
inch wide strip is formed makes a good winding for this packing.
After the HCl addition has been completed, the mixture will have become warm again from the exotherm of the conversion of the basic sodium compounds
to sodium chloride. The valve on the addition funnel is closed, and into the addition funnel is placed the cold diluted sulfuric acid which has been
previously prepared.
To the rapidly stirred mixture is added dropwise the diluted H2SO4 at a drip rate of two drops per second. Observe for any excessive foaming during
the early part of this addition, as was done before with the frst stage of the neutralization, and reduce the drip rate if necessary to control any
transients of excessive foaming. Generally the neutralization is well behaved and goes smoothly. The addition of the first half of the diluted
sulfuric acid will convert all of the freebase hydrazine which is present in the solution into the highly soluble dibasic hydrazine salt, which will
remain in solution. It is during the addition of the remaining second half of the diluted sulfuric acid that the super soluble dihydrazine sulfate is
converted to the slightly soluble monohydrazine sulfate which is precipitated. Because the solution has become hot from the neutralization process
completed earlier, a considerable amount of the monohydrazine sulfate being formed during the addition of the last half of the diluted sulfuric acid
will be held in the hot solution which will super saturate with the monohydrazine sulfate being formed, and then at a point where about two thirds of
the total sulfuric acid has been added, the hot super saturated solution will become cloudy and suddenly an avalanche precipitation of monhydrazine
sulfate crystals will occur, continuing that precipitation of crystals to the end of the addition of the remaining third of the sulfuric acid. Knowing
from observation that this is the manner in which the precipitation always occurs allows for the speed of the precipitation to be slowed for better
crystal development in the hot solution. When about sixty per cent of the diluted sulfuric acid has been added, the solution clarity is closely
observed and the instant that any turbidity or cloudiness is observed occurring, the drip rate of he sulfuric acid is reduced to a slow one drop per
second into the vigorously stirred hot solution. The very slow final neutralization and continuing vigorous stirring of the slowly cooling mixture for
one hour past the end of the addition, provides for a controlled growth of high purity and dense crystals of a desirable form. The stirring is then
discontinued and the flask is stoppered and placed into a cooling bath of melting ice overnight to complete the crystallization. Some effervescence of
dissolved carbon dioxide will be observed coming from the solution and this is normal.
Loosely stopper the flask because the continuing evolution of dissolved CO2 will gradually develop sufficient pressure to eject the stopper and send
it flying if the stopper is snug. A short length of string draped over the opening of the flask between the stopper and the inner surface of the glass
will break the seal sufficiently to slowly vent away any pressure from the effervescing carbon dioxide.
After cooling overnight in an ice water bath, the mixture should be stirred up one final time to dislodge fine bubbles of carbon dioxide from the mass
of crystals and to loosen any clumps of crystals for easier filtering. The stirbar is retrieved from the mixture and it is ready to filter. A 500 ml
portion of the cold supernatant liquid should be decanted into a wash bottle for use in rinsing residual crystals from the flask onto the filter. Most
of the liquid can be decanted from the mass of crystals and most of the wet slug of crystals will slide from the flask smoothly onto the filter, with
a bit of firm bumping of the flask bottom edge with the heel of the palm of the hand. A stream of liquid from the wash bottle is used to dislodge and
rinse residual crystals onto the filter. The drained but still wet crystals are flooded on the filter with about 150 ml of 70 per cent isopropyl
alcohol and with a glass rod are stirred into a thick slurry with the alcohol. As this alcohol rinse drains through the filter, a final rinse with
about 75 ml of anhydrous isopropyl alcohol is streamed in a spiral pattern onto the surface of the filter cake with a wash bottle. These alcohol
rinses will get rid of most of the residual salt water from the reaction mixture which is initially held in the filtered cystal mass by capillary
action. The alcohol rinsed crystals should be drained on the filter placed on a blotter to wick away excess liquid as much as possible and then air
dried on a warm glass tray.
The yield of dried sparkling white crystals of hydrazine sulfate is 221 to 236
grams, about 60 per cent of theory based on sodium hypochlorite. It is believed that the variation in yields is due for the most part to slight
variations in the composition of the commercially available 10 per cent solution of sodium hypochlorite. The solution is unstable in storage, so its
analysis changes as it sits on the shelf and gradually deteriorates. The yield of the synthesis varies according to the actual analysis of the
feedstock sodium hypochlorite solution at the time it is used for the synthesis. There may also be slight variations in the commercial sodium
hypochlorite solution analysis from lot to lot and slight variations in the analysis for the same product supplied from different manufacturers. The
rate of decomposition for the sodium hypochlorite solution is greatly reduced when it is stored in a cool location. At the warm outdoor temperatures
of summer days, the decomposition is accelerated, and after some passage of time the solution will decompose completely in storage.
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Nick F
Hazard to Others
Posts: 439
Registered: 7-9-2002
Member Is Offline
Mood: No Mood
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Shortened improved hydrazine sulphate.
I hope Mr. Anonymous does not mind, but I have produced an editted version of his write-up. It is not intended as a replacement, but I think it would
be more convenient to have this next to you while performing the synthesis, rather than the original. This is more in the form of step-by-step
instructions, rather than a description, as the original was. I have included some of the more important observations in italics inside square
brackets, although they may not come through that way when I copy/paste it here from Wordpad...
Also, may I have your permission to include my editted version on my website? It is still your work really, so I thought I should check with you
first.
----------------------------------------
Hydrazine Sulfate from urea and pool chlorinator is a synthesis which has been previously described. Outlined below is an improved OTC procedure.
--------------------
Experimental:
1) 1892 ml to 1900 ml of 10 per cent sodium hypochlorite (liquid pool chlorinator, or prepared fresh by bubbling chlorine through an appropriate
sodium hydroxide solution until the necessary increase in mass is achieved) was placed in a one gallon glass pickle jar which was sealed and chilled
to -10*C.
2) A 3" oval 60 gram stirbar was placed into the jar and the hypochlorite was stirred rapidly.
3) 170g of sodium hydroxide prills was added into the vortex over two minutes. Solid material must not be allowed to accumulate.
4) The jar was again sealed and cooled to -10*C.
5) An additional 85g of sodium hydroxide was added as before. The solution must be kept cold during the sodium hydroxide additions, this could be
achieved through the use of a salt/ice bath as long as the stirring is still as efficient, or with smaller additions and more "rest" in the
freezer, if necessary.
6) Again, seal the jar and return it to the freezer.
--------------------
7) Place 182g of urea in 100mL of hot distilled water in a one pint jar, with a threaded lid (eg, a large jam jar). Stir it until as much as possible
is dissolved.
8) In a second, similar jar is placed 2.5g of gelatine and 100mL of hot distilled water. Stir it until fully dissolved.
9) Combine the solutions formed in steps 7) and 8). The undissolved urea will now go into solution.
--------------------
10) Place a 4L Erlenmeyer flask on a large stirrer hotplate, and add a 3" (60g, or larger) oval stirbar, as in step 2).
11) Place a one gallon plastic funnel (or similar object) into the neck of the Erlenmeyer. The funnel must be adapted so as to provide a tight fit
into the neck of the flask (possibly window putty or similar could be used to seal it, as it can be removed afterwards). This funnel allows room for
the foaming.
12) Once the sodium hypochlorite/sodium hydroxide solution is at 5*C to 8*C, pour it into the Erlenmeyer, and start the stirring at about 40% of
maximum speed.
13) Quickly add, in one portion, the urea/gelatine solution, and raise the stirring speed to about 60% of maximum.
14) Loosely cover the top of the funnel, for example with cling-film or a plastic plate. Allow a gap to vent the carbon dioxide through.
[Original author's observations: After about fifteen minutes, usually the foam begins to subside very slowly. At twenty minutes the mixture is
stirring more freely still with the level of the foam having diminished further. A gradual slowly darkening in color towards orange will be observed
as the minutes pass and the flask may feel slightly warm to the touch. There will become visible an upwardly spiraling pattern of streaks in the foam
from the action of the stirrer and the foam will gradually stratify into two layers as it breaks up and begins to dissipate. The upper layer of foam
will show a more coarse texture to the bubbles and develop an open cell spongy appearance at the time when the foam is about to dissipate completely
[times and appearances may vary, this is general].]
15) At approximately twenty-five minutes, or when the height of the foam begins to drop, [with the volume of the reaction at around 3200mL],
supplemental heating is applied at a setting of 20%.
16) At thirty minutes [with the volume of the reaction at around 3100mL], heating is increased to 40%.
17) At thirty-five minutes [with the volume of the reaction at around 2900 ml], heating is increased to 60% [The color of the mixture is becoming a
distinct orange].
18) At forty to fifty minutes [the foam has subsided to a clear transparent dark orange solution], the stirring is reduced to 20%, and the heating
kept at 80%.
[My unconfirmed interpretation: the heating is increased from 60% to 80% gradually between thirty-five minutes and forty-five minutes, at which point
foaming should have ceased. The original author stated that "Good yields were observed with a reaction endpoint temperature of only 85 degrees
centigrade," thus, 80% heating should correspond to around 85*C.]
[Original author's observations: Over the next ten minutes the orange color will gradually fade at a visible rate in the completing reaction. The
color will fade to a pale yellow, very light ale colored, almost clear solution and this will indicate the endpoint of the reaction. The reaction
mixture is (preferably) heated an additional five minutes after color fade ceases or optionally may be heated until moisture is condensing on the
inner walls of the flask in the neck area of the flask. The heating is discontinued.]
--------------------
19) The overflow funnel is removed and the flask is quickly stoppered to exclude air.
20) The flask is removed from the hotplate stirrer, and placed into a pan of cold water to help speed the cooling of the contents. Occaisionally
remove the stopper to allow the pressure inside the flask to equalise with the atmosphere.
21) After about 30 minutes, place the stoppered flask into an ice bath for about one hour, to thoroughly chill the solution.
22) Measure out 650mL of 31.45% hydrochloric acid into a suitable container, and chill this in the ice bath.
23) Mix 175mL of cold distilled water and 200mL of 92.5% sulphuric acid, with care, in a 500mL Erlenmeyer flask.
24) Let the diluted sulphuric acid cool to almost room temperature, and then chill this in an ice bath or freezer.
--------------------
25) Return the chilled reaction mixture to the stirrer plate, and start stirring rapidly.
26) Add the 650mL of chilled hydrochloric acid at a rate of about 3 drops per second, but at a rate that does not cause excessive foaming, from an
addition funnel. To prevent too much contact with the air, the hydrazine solution can be protected by stuffing cotton wool or a similar material
loosely into the gap between the mouth of the Erlenmeyer and the addition funnel, but ensure that the carbon dioxide released is free to escape.
27) Close the tap on the addition funnel, and fill it with the chilled sulphuric acid solution prepared earlier.
28) Add the sulphuric acid to the rapidly stirred mixture at a rate of about 2 drops per second. As with the adition of the hydrochloric acid, reduce
the rate of addition if excessive foaming is encountered due to any remaining sodium carbonate in the solution.
29) When roughly two thirds, or slightly less, of the sulphuric acid has been added, the hot solution will start to become cloudy. As soon as any
cloudiness is observed, slow the rate of addition of the sulphuric acid to 1 drop per second, or slightly less. This results in a better quality
precipitate.
30) After all the sulphuric acid has been added, stop stirring, stopper the flask and place it into an ice bath, to finish the precipitation. Some
carbon dioxide may escape from the solution, so do not stopper the flask too tightly.
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31) When the mixture is thoroughly chilled, swirl the flask to allow any trapped bubbles to escape. Remove the stirbar.
32) Decant off as much of the supernatant liquid as possible without loosing any crystals.
33) Filter the remaining mass of crystals, and use some of the filtrate or decanted supernatant liquid to wash remaining crystals out of the flask and
into the filter.
34) The drained but still wet crystals are flooded on the filter with about 150 ml of 70% isopropyl alcohol and with a glass rod are stirred into a
thick slurry with the alcohol.
35) As the alcohol rinse drains through the filter, a final rinse with about 75 ml of anhydrous isopropyl alcohol is streamed in a spiral pattern onto
the surface of the filter cake with a wash bottle.
36) Place the drained mass of crystals in the filter onto a pile of absorbent paper, to suck out excess alcohol from between the crystals.
37) Dry the crystals in a warm, dry place.
--------------------
The yield of dried sparkling white crystals of hydrazine sulfate is 221 to 236
grams, about 60 per cent of theory based on sodium hypochlorite.
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Nick F
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Basement Chemist: "No Nick F, I dont mind."
Don't mind what..?
It seems Mr Anonymous wasn't too happy about the editted version, apparently I have missed important details. I'm not sure where, but...
Yes, I did forget to add that the solution should be stirred for one hour after the sulphuric acid has been added, that was a mistake, not a
deliberate omission. I overlooked it because it is somewhat buried in a huge mass of text. I will have to add that step in. That is exactly my point -
if you're trying to carry out the reaction with the original as your guide, it would be quite easy to overlook something if you were
concentrating on what was happening in your flask. The point-by-point version that I made is designed to have next to you during the reaction as
notes. As I said, it is not intended as a replacement, and anyone carrying out the reaction is assumed to be familiar with the original. Even so, it
is still the most detailed instruction for making hydrazine that I could find, apart from the originals that Mr Anonymous produced.
"There is a reason for everything , even the way the drain cleaner is diluted. Try it "carefully" as you suppose is okay and compare
results with the portionwise method I described to get around the thermally sensitive dye that is an impurity in the acid."
There is no way to get around the dye in the acid; you may convert it into substances that are no longer purple, but you will not remove any
impurities simply by mixing it with water, no-matter how you do it. If you decompose the dye with the heat of dilution of the acid, then you might
have a nicer looking product, but I can see no reason to assume that it would be any purer than if the dye was left purple.
"The proposition of making your own sodium hypochlorite by gassing NaOH with chlorine is not really a good idea for a non-industrial environment
. The liquid pool chlorinator is a cheaply available common article of commerce so why bother."
I can assure you that making your own hypochlorite solution from chlorine and sodium hydroxide is perfectly fine. That is precisely what I do if I
need a stronger hypochlorite solution than the 3% bleach that is available to me. Why do I bother? Because for me, and therefore probably others, pool
chlorinator is neither very cheap nor very common. And if I make it myself, then I can be sure of its purity - no metal ion nasties to interfere with
the reaction, and a precislely known concentration.
Do you have reason to belive that a 10% home-made solution will be less effective than a 10% purchased solution? If not, then it is a perfectly valid
comment to add. I merely presented it as another option, I never said that I advised doing it if you can get hold of 10% easily.
"The exotherm from the heat of solution of solid NaOH is rapid and energetic [I know that, I have used NaOH before!], and it would be a very
tedious process to manage the exotherm with salted ice, unless you had circulating brine coils directly in the hypochlorite solution. Otherwise you
could be there for hours adding the NaOH a teaspoon at a time while watching a thermometer.
Better to exploit the thermal mass of the solution and use that mass as a heat sink for absorbing the exotherm directly."
In the editted version, I use the same additions as you, and also the use of the freezer between additions, exactly as you described. I suggested that
a salt-ice bath may be used during the additions, when the container is not in the freezer.
A salt-ice bath can't do any harm, as long as your stirrer is still working effectively, as I said, so what is the problem in using one to
provide some additional cooling? It may be found that the benefit is slight, if any, but it's not going to make the solution any hotter, is it?
I think those are the main points you made in your e-mail to me.
Don't misunderstand me, I value the information that you have provided very greatly. But I can see no harm in having the version that I produced
to hand. And please, if you do e-mail me again to point out other things, try not to talk to me as if I'm a child. You are obviously very
intelligent, but I am not stupid either.
"but you didn't know that because you haven't done the synthesis you are editing."
Perhaps it was not intended (it is so hard to tell with type), but I detected a derrogatory tone in the e-mail, in the quote above for example. Maybe
it's just my paranoia though.
"So I would ask that no one edit a synthesis without experimental results to justify the merit and validity of the change."
I still maintain that I have not changed the actual procedure at all...
--------
Anyway, like I said, I do greatly value the information that you gave us and the benefit of your experience, I was just trying to put it into a form
that was easier to use.
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Iv4
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Long time since I was here.Anyways let me get this right:the sodium hypocchlorit rearnages the structure of urea so it forms hydrazine.Or does that
haoen only when he sulfate is added?If so could it be done with nitrate's or something?
[Edited on 9-9-2003 by Iv4]
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TechnologicallyRetarded
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Iv4, you are going to get your throat slit asking stuff like that... research the Hoffman Degredation:
http://en.wikipedia.org/wiki/Hoffman_degradation
Basically, an amide is reacted with a Hypohalite (Hypochlorite in most cases) to form a Nitrene which rearranges to an Isocyanate. On hydrolysis a
Carbamate results. This Carbamate loses CO2 to produce the respective Amine. The H2SO4 converts the Hydrazine produced to its respective Hydrogen
Sulfate which is relatively insoluble. I doubt the Nitrate would be at all insoluble.
Tr
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UnintentionalChaos
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Quote: Originally posted by TechnologicallyRetarded  | Iv4, you are going to get your throat slit asking stuff like that... research the Hoffman Degredation:
http://en.wikipedia.org/wiki/Hoffman_degradation
Basically, an amide is reacted with a Hypohalite (Hypochlorite in most cases) to form a Nitrene which rearranges to an Isocyanate. On hydrolysis a
Carbamate results. This Carbamate loses CO2 to produce the respective Amine. The H2SO4 converts the Hydrazine produced to its respective Hydrogen
Sulfate which is relatively insoluble. I doubt the Nitrate would be at all insoluble.
Tr |
Kindly read the last posting date before posting in a thread....there is a much longer thread on hydrazine from which this seems to be a failed
offshoot.
Department of Redundancy Department - Now with paperwork!
'In organic synthesis, we call decomposition products "crap", however this is not a IUPAC approved nomenclature.' -Nicodem
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DJF90
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I'm sure he had to dig deep to find this thread as it is so old!
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kclo4
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He probably didn't realize it was old, or that there was a bigger and better thread since it appears he is a new member, plus he is
TechnologicallyRetarded. 
*I just couldn't resist....*
He is at least answering an old unanswered question. It is much better then asking an already been answered question in an old thread. IMO
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TechnologicallyRetarded
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Apologies... and yes, my user name is fitting ~_~".
I am fairly new to forum's in general. Don't old threads get stopped? I do now realize I have posted a reply to a member who may not even be alive and
shan't do in future. I am also aware of the larger thread, this one is good for it's being so succinct - that's all. How long after a post would you
say a reply is permissible?
Thanks for taking it well kclo4 and again - sorry - Unintentional.
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DJF90
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Its good that you actually contributed something that was worth the resurrection of the thread. I have now made this my method of choice for making
hydrazine, when the lab is operational, as the yields far exceed that of the "traditional" method, and it looks simple. I assume just following the
general procedure for a hoffman degradation will work also? Although I think I will pre-make the bleach anyways (I'm sure I wanted some for somethign
else...).
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densest
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I did a quick web search for assays of hypochlorite in solution. Would this concentration information be useful to calculate the amount of bleach/pool
chlorine to start with?
None of the articles were free  , perhaps someone with university or corporate
access might check to see if the articles are useful.
I am admittedly lazy and didn't look up the procedure for 2 xOCl +2 KI + 2 H2O -> xOH + KOH + I2 and titration with Na2S2O3 to a clear endpoint. I
would assume one could calculate the stoichiometric quantity of sodium thiosulfate used to get the quantity of hypochlorite and that an excess of KI
is not going to confuse things.
http://www.ars.usda.gov/research/publications/publications.h... Spectrofluorometric Assay for Hypohalite and Peroxyacetic Acid Using Kojic Acid
http://cat.inist.fr/?aModele=afficheN&cpsidt=2231465 Spectrophotometric assay for hypochlorite/hypochlorous acid using
tris(2-carboxyethyl)phosphine Microchemical Journal, Volume 58, Number 2, February 1998 , pp. 218-224(7)
Quantitative spectrophotometric methods for determination of sodium hypochlorite in aqueous solutions DOI: 10.1002/jps.2600590824 Wiley Interscience
Journal of Pharmaceutical Science Volume 59 Issue 8, Pages 1168 - 1170
The last one is interesting - they would have you generate NCl3 and measure the absorption because it is such a strong absorber.... better dilute
that one well  At least it uses common OTC ingredients. Gotta look up kojic
acid to see if it's something one could get out of (for instance) a simple mold culture.
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dimrothCondenser
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sorry to post this here, but i didn't want to start a new thread for a simple question like this one, regarding the method given here for freebasing
the hydrazine sulfate with NaOH and obtaining a solution of hydrazine hydrate in methanol / 2-propanol.
Since i want to use hydrazine hydrate as a reductive in a Wolff-Kizhner reduction, wich is carried out in diethylene glycol, i was wondering if i
could just use the DEG instead of MeOH / IPA during the freebasing process. The original patents are talking about only using simple alcohols - what
problems could be caused by the additional hydroxyl-group of DEG?
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