chem1a

re me: -- i lied its mostly hexane not heptane re john .. - the msds for the only product in Aus named "shellite" states that the product is 100% volatile hydrocarbons, identifying the components as being pentane, hexane, heptane which together or seperatley seem to benamed as "naptha" or "petroleum ether". These will all boil off if evaporated and are not miscible with water. A wash with water will help dilute & seperate most anything that has managed to become dissolved in water absorbed by any of these solvents(if any has been absorbed at all). You could distill it if you really didnt trust the MSDS but i am not that sceptical and will happily settle for simply washing the product with dH2O - especially for something i am not eating in the end. If a person is concerned about purity or is extracting something for human consumption they should go to a chemical supplier and buy propper lab grade chemicals. Also as far as substitution of petroleum ether for diethylether in extractions goes -correct me if im wrong but as far as i am aware they have quite similar solvation properties and can "generally" be used interchangably for many extractions.

there is always the possibility that you have done serious damage that requires u only to move the wrong way to sever the cord .... could you be bothered checking up on that ?

Silencer Shellite from the hardware store is generally an ok substitute for backyard extractions that call for di-ethyl ether (though it most certainly is NOT di-ethyl ether - it is Naphtha which is synonymous with petroleum ether --- i believe it is mostly heptane ) ... if you dont trust it's purity wash it with distilled water before use (ie add water, shake, let seperate into layers - the shellite floats ... discard water layer from the bottom)

"Simply put: DONT TRY IT AT HOME." - thats good advice:) though if you still want to know more read up on davy - i believe he was the first to isolate Na this way. Detailed descriptions of his work should detail the equipment and proceedure used (though u can skip using the voltaic pile )

Na(s) can be isolated from molten NaCl under inert conditions (no oxidisers like oxygen present )....

i saw something on discovery about what was known as "the dryest city on earth" using suspended wires of sorts to do just this ...i cant for the life of me remember where it was, just that it was near the ocean but that high cliffs seperated it from the water & that none/very little of the humidity ever precipitated as rain. ../. this "wire" condensation system supplied the entire town's drinking water.

Ahhh .. that makes so much sense ! lol i cant believe i didnt think past the actual reaction to the isolation of the produced acids.... good to know H2SO4 doesnt boil away until higher temps - that makes conc H2SO4 much more accessible (i will make that 40 min drive now !) I will pull out my jar of NaCH3COO & distill away ! ... ive been looking forward to seeing solid GAA thanks all for your input

Can you please elaborate on the conditions mentioned in "not done properly" that lead to phosgene production so i can avoid them Also the extra ventilation in place to deal with liberated Chlorine gas should be enough to deal with this ww1 chem warfare agent shouldnt it ?(more specificly,"these" ww1 chem warfare agents - as both of them were used in the trench warfare) or are you recommending gas masks ? also update ... with fluro lamps, a blacklight & 6 hours of refluxing toluene is still toluene - i guess there was not enough UV energy to break CL2 into Cl. ....will try again tomorrow with a UV tanning lamp

Calculations for Iodine available not the iodine given from this reaction .... i dont know how these chems react sorry ... if u give an eqn i can calculate closer to actual yield NaIO3 Iodate Anion Iodine = 126.9g per mole Oxygen=15.9 per mole & we have 3 parts oxygen in this compound * 3 = 47.7 therefore 174.6 G for 1 mole Sodium Cation Na 22.99g per mole 1 mole substance = 197.59 BUT you have HAVE 350 g so 350g/197.59g = moles of substance = 1.77moles Mol Iodine relationship to Mol NaIO3 is 1:1 therefore max theoretical amount of iodine available 1.77mol * 126.9g = 224.8g Iodine present Also in that sample is Na 40.7g and 84.5G Oxygen (Test the math) 84.5 + 40.7 + 224.8 = 350 (100% of the original compositon)

good ethanoic acid (GAA) most esters toluene/xylene acetone Bad Benzyl chloride chlorine formic acid

edit: i apologise if this is in the wrong spot - i was unsure if it should go in organic chem or in "your experiments" as it is both.... I am trying to get to Benzyl alcohol 1) for the chllenge of getting there and 2) for use as flavouring in some soaps (my next project - if anyone has any good recipees let me know) that im planning on making for xmas for peeps. Anyhow the plan is to go Toluene---chlorination-->Benzyl Chloride ---Hydrolisys ---> Benzyl Alcohol (then possibly use alone or as an ester component) I am wondering how long the Ca(OCL)2 chlorination is supposed to take using equal volumes toluene:bleaching powder (or a slight excess of toluene to avoid Benzal chloride and trichloromethylbenzene formation) I have tried refluxing @110 c in the presence of sunlight (from a mirror) for 1/2 an hour and ended up with a recieving flask full of toluene, the latter portion of whic came across at 140c rather than toluene's 110c bp .. this still is not the 189c i was expecting - i can only attribute the low bp to the seemingly low concentration formed (i am guessing azetropy must have played a role). The last portion was very irritating to the eyes and nasal passages (much more so that the free chlorine the comes off of bleaching powder) so i am assuming it probably is the intended compound also note - the first time refluxing was attempted no uv light was used incase it led to substitution of the ring instead (are the bonds on the ring stornger than the methyl group's bonds?) - the bp of the fluid was 110c for the duration of the distillation and no irritating smell was noted obviously 1./2 hour was well an truely not long enough. so my question is: does anyone know just how long this reaction is actually supposed to take and furthermore if the energy saver globes (the fluro ones) release any UV light t all (to use instead of sunlight as it is very inconvenient)

Just a quick q is there any reason all the posts here (bar one) refer to the use of H2SO4 when making acids (eg nitric and ethanoic) from salts rather than any other strong acids. Is HCL less effective ? or is H2SO4 cheaper /more available where most of you are (H2SO4 is at least a 40 min drive from where i am for 5mol acid compared to HCL which is in every hardware and pool store) HCL appeared to be very effective in the production of boric acid from Borax... dissolved 100g borax in massive excess of HCL (200 ml) & heated to 60c (not all dissolved). Diluted acid borax mix with a futher 100ml H20 & kept at 60c then filtered. Refluxed resultant filtrate with ethanol & burnt to accquire a green/orange/blue flame. to confirm that the solid produced was indeed boric acid plain borax was refluxed with ethanol and burnt - only a blue/orange flame was obtained confirming suspicions that Triethyl borate had been created in the first refluxing step thereby confirming that Boric acid existed.

interestingly if you have a fan in your freezer and place ice cubes infront of the fan you will notice over a period of weeks the ice cubes shrinking .... they certainly are not at 100c but are very slowly evaporating