20% HCl = 20gHCl/100mL
(1.065 mols)
Is that correct? From my attempt at figuring this out I also think this means there is 3.883 grams of hydrogen chloride
I don't think it's unreasonable to be suspicious of an experiment using 2L of acid, lol. So what's your experiment here?
20% HCl = 20gHCl/100mL
Assuming w/v, it can be w/w as well.(1.065 mols)
Is that correct? From my attempt at figuring this out I also think this means there is 3.883 grams of hydrogen chloride
Molar mass of HCl is around 36.5 g/mol, without further analysis your mass seems to be ten times too low.
20% usually doesn't mean very accurate concentration, anything between 19-21 (or even 18-22) will do.
What is the concentration of the acid you have at hand?
Edit: nj question is not completely off topic, after all, we have some guidelines and forum rules (http://www.chemicalforums.com/index.php?topic=33740.0). You have not broken them as of now, but we have to be vigilant ;)
Generally 2L isn't a good scale to "experience chemistry." It's a good scale for a (very) amateur person dabbling around in chemistry to get a runaway reaction and boiling acid splashed on him. Anyway, hydrochloric acid is used for a couple not so nice syntheses, so elaborate a little and maybe you can avoid some unnecessary danger.
Or scale your rxn down a lot.
I found a lot of places to buy pure HCL online
This is crap, I used gaseous HCl all the time in my pilot plant with absolutely no problems. I used it to make solutions in ethyl acetate, ethanol etc.I found a lot of places to buy pure HCL online
Gaseous, compressed, in cylinders? Nobody sane will buy this stuff when they need a solution. Buy 38% solution and dilute.
For the record, I am doing a rxn on 0.3mmol scale currently, and it is done in 400mL of boiling concentrated hydrochloric acid. And it is not drug related at all. It is just the solvent.
So, why not just dilute 37% HCl?
Gaseous, compressed, in cylinders? Nobody sane will buy this stuff when they need a solution. Buy 38% solution and dilute.This is crap, I used gaseous HCl all the time in my pilot plant with absolutely no problems. I used it to make solutions in ethyl acetate, ethanol etc.
Gaseous, compressed, in cylinders? Nobody sane will buy this stuff when they need a solution. Buy 38% solution and dilute.This is crap, I used gaseous HCl all the time in my pilot plant with absolutely no problems. I used it to make solutions in ethyl acetate, ethanol etc.
As far as I can tell we are talking about water solution. When in need of water solution, would you start with gaseous HCl?
@ Discodermolide: Don´t tell such stories to the newbies here. Gaseous HCl is very nasty stuff. I have also experience with CO, SO2, ethylene, H2 of course and also phosgene, all in gas form. It´s always a pain...
@ Discodermolide: Don´t tell such stories to the newbies here. Gaseous HCl is very nasty stuff. I have also experience with CO, SO2, ethylene, H2 of course and also phosgene, all in gas form. It´s always a pain...
Note I said Pilot plant
@ Discodermolide: Don´t tell such stories to the newbies here. Gaseous HCl is very nasty stuff. I have also experience with CO, SO2, ethylene, H2 of course and also phosgene, all in gas form. It´s always a pain...
Note I said Pilot plant
I am with Discordermolide here, except for the Pilot Plant requirement. I always liked catalytic hydrogenations as the work-up was always easy, filter and evaporate. I don't want to generalize, as it depends on equipment at your disposal, experience, etc, but I can imagine it being a pain (HF, SF4) or a pleasure (H2, I can imagine others, though I haven't used them).
I don't mean to hihack this thread. I still don't understand why the poster escapes criticism for wanting to make HCl gas in the first place, let alone using it. How many of you that used HCl gas, made it? I am more than skeptical.
Hey guys! Back with an update... I got my 32% HCL in the mail and did some experiments... first of all... When I opened the box and took the bottle out they were wrapped in some absorbent (chemically inert to hcl) cloth. They were right to wrap the bottles in cloth because it sure did reek of HCL when I smelt the cloth. It burns... I'm guessing they didn't douse the bottles in HCL before they packed them so that must mean the HCL lost some of its potency. I'd like to think it lost about 1% maybe? Anyways... Onto my experiment... (not being illegal)
I tried refluxing a 20% HCL solution on its own. I had all of the safety precautions in full effect...
Results...
Refluxing HCL with a normal condenser will result in hydrogen chloride escaping. I think this is due to lack of surface area within the condenser...
Since HC has a lower bp than h2o wouldn't more hc boil out of the mixture than water? or is the world perfect and a perfect amount of each boils out at the same time? this is what I'm stuck on...
Dudeman, all I can say is you better have a legit fume hood.
Roughly, constant boiling HCl is 18% while conc HCl is 37% (I don't remember the actual values). When you reflux, there isn't enough water to absorb the HCl as the higher temperature.
There had been an earlier post in which someone advocated refluxing an ester in conc HCl. At the time, I thought about making a note about the HCl pouring out if you do this, but since the concept was basically correct, it would hydrolyze the ester, I let it go. Here is why you don't want to just do this. If you want to reflux HCl, dilute it to constant boiling HCl (~6N) first.
It is not a useless comment because you apparently have no clue about what you are working with. Based on that, a friendly reminder about safety protocols is in order.
yes, so be safe. Don't breathe it, get it in your eyes or on your skin. You don't need a high gaseous concentration to cause irritation of your respiratory tract and membranes. Wear gloves and goggles and run away if it's starting to smell... assuming you aren't doing this in a hood which seems very dangerous in light of the way the conversation went. If you are going to use HCl at home, nobody can stop you but do it "properly" and with knowledge. It could go bad very fast.
| An example of a negative azeotrope is hydrochloric acid at a concentration of 20.2% and 79.8% water (by weight). Hydrogen chloride boils at −84°C and water at 100°C, but the azeotrope boils at 110°C, which is higher than either of its constituents. The maximum temperature at which any hydrochloric acid solution can boil is 110°C. In general, a negative azeotrope boils at a higher temperature than any other ratio of its constituents. Negative azeotropes are also called maximum boiling mixtures or pressure minimum azeotrope. |
| If two solvents can form a negative azeotrope, then distillation of any mixture of those constituents will result in the residue being closer in composition to the azeotrope than the original mixture. For example, if a hydrochloric acid solution contains less than 20.2% hydrogen chloride, boiling the mixture will leave behind a solution that is richer in hydrogen chloride than the original. If the solution initially contains more than 20.2% hydrogen chloride, then boiling will leave behind a solution that is poorer in hydrogen chloride than the original. Boiling of any hydrochloric acid solution long enough will cause the solution left behind to approach the azeotropic ratio. |