Distilling hydrochloric acid

? The only idea that comes to mind is this: hydrogen chloride fumes are NASTY. Could you please tell us: do you really need concentrated HCl? What is the application?

Steve Bizub
- St Louis, Missouri
2004

A. Why don't you purchase some Conc. HCl from a chemical supply house and then dilute to the strength required. This is what most chemists would do.

Ronald Zeeman
Coil Coating - Brampton, Ontario, Canada
2004

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A. Dear sir, it is not advisable to distill HCl, because hydrogen chloride gas is dissolved in water to give the acid. If you distill the acid then acid vapours (HCl) will escape and will further reduce the concentration. Vapours from this acid will just inflame your nostrils and wreak havoc.

Regards,

Dinesh [last name deleted for privacy by Editor]
- Chennai, Tamilnadu, India
2004

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2004

Agree with Steve. A hydrochloric acid solution of 70 wt% HCl is only stable under very high pressure (about 5.15 MPa or 50.8 atm) HCl vapor at 30 °C) and is extremely dangerous. Before doing anything else, please read the safety info "Medical Management Guidelines (MMGs) for Hydrogen Chloride (HCl)" at
https://www.atsdr.cdc.gov/mmg/mmg.asp?id=758&tid=147

Two options for preparation of 70 wt% HCl solution: distillation (under some very specialized conditions) or addition of pressurized HCl gas. The US EPA's "Guidance for Reporting Hydrochloric Acid (acid aerosols including mists, vapors, gas, fog, and other airborne forms of any particle size)" contains most of the physical data necessary for distillation. http://www.epa.gov/tri/guide_docs/1999/hclguidance.pdf

Additional HCl solution data is at http://www.resistoflex.com/hci_graphs.htm#2 The freezing point curve indicates that partial freezing can only concentrate a 33% HCl solution to 40%; a composition corresponding to an HCl.3H2O complex.

The largest problem in distillation is the very high vapor pressure of the distillate. This, plus the health hazard and corrosiveness, requires the use of Teflon®-lined metal equipment rather than laboratory glassware. The change in composition of the still liquid is another consideration. The initial vapor will be ~90% HCl by weight, but by continuing the distillation until the remaining liquid reaches the azeotropic composition (~22.2 wt% HCl) and a total vaporization of ~22.6 wt%, the average distillate should be the desired 70 wt% HCl. To maintain a flow of vapor from the "boiler" to the condensing vessel, it may be necessary to solidify the condensate by keeping the latter at very low temperature with a dry ice/acetone or liquid nitrogen bath, while gradually raising the temperature of the still liquid. Use Pyrex glass boiling beads and avoid rapid heating to prevent "burping" of liquid. The condensing vessel should obviously be valved and detachable, and of suita! ble construction to withstand pressure, low temperature and corrosiveness. Perhaps, a 1 L Teflon®-coated, austenitic stainless steel pressure vessel, with appropriate valving, etc.

It is easier to add HCl gas under pressure to the 33% solution in order to reach the desired 70%. Again, use a 1 L Teflon®-coated SS vessel (e.g., a bomb calorimeter). Order a high-pressure cylinder of anhydrous HCl, an appropriate regulator, valving and tubing. Set the vessel on a weighing scale, fill ~90% full with the 33% HCl liquid, then add the desired weight of HCl gas. Close valving and give it some time to cool before using.

Ken Vlach [deceased]
- Goleta, California
Finishing.com honored Ken for his countless carefully researched responses. He passed away May 14, 2015.
Rest in peace, Ken. Thank you for your hard work which the finishing world, and we at finishing.com, continue to benefit from.

A. You can always add kitchen salt* to sulfuric acid* to get hydrochloric acid?

*must be 100% NaCl

*get it from hardware stores or uncharged car batteries (if you get it from the batteries, which is unadvised, filter out the chunks of lead).

"Jabir or Geber, is also credited with the invention and development of several chemical instruments that are still used today, such as the alembic, which made distillation easy, safe, and efficient. By distilling various salts together with sulfuric acid, Jabir discovered hydrochloric acid (from salt) and nitric acid (from saltpeter). By combining the two, he invented aqua regia, one of the few substances that can dissolve gold. Besides its obvious applications to gold extraction and purification, this discovery would fuel the dreams and despair of alchemists for the next thousand years. He is also credited with the discovery of citric acid (the sour component of lemons and other unripe fruits), acetic acid ⇦ this on eBay or Amazon [affil links] (from vinegar ⇦in bulk on eBay or Amazon [affil links] ), and tartaric acid ⇦ this on eBay or Amazon [affil links] (from wine-making residues)."

from:
- https://en.wikipedia.org/wiki/Geber

Kit Callahan
- Folsom, California, USA
2006

A. Concentrated (100%) HCl is a gas, you can't have 100% concentrated HCl in liquid form, the acid forms an azeotrope at about 30% concentration, so you cannot purify it further by distillation, you CAN have a slightly more concentrated HCl when you distill a mixture of 30% HCl with some concentrated (98%) sulfuric acid.

Marcial Cordova
- Hermosillo, Sonora, Mexico
2006

A. You can distill lower concentrations of HCl (less than 20%) also to produce up to 100 % HCl. For this you will need an extractant like H2SO4 or Calcium Chloride.

I suggest you produce 70% - 100% HCl at the point of use, and not store it.

Setting up a plant to produce such HCl is the option

Vinayak Madhekar
- Pune, Maharashtra, India
March 9, 2008

A. Hydrochloric acid is near saturation in water at about 33% to 40%, I believe, and higher concentrations would not be a reasonable solution to your problem as they really would only exist under laboratory conditions. Should you wish to have an acid with stronger qualities perhaps a different acid or a mix would give the field strength desired.

As for the salt gives hydrochloric acid, believe it or not I looked in the encyclopedia and found a 1600th century alchemist, Johann Rudolf Glauber, who's life work was highlighted by the discovery that hydrogen chloride gas is produced by the addition of sulfuric acid to table salt. Of course, one must bubble the HCl into water to make hydrochloric acid which, as indicated above, saturates near 33% at room temperature.

Dave Crippen
- Seattle, Washington
April 20, 2008

A. Hydrogen Chloride (HCl) is a gas, which can be produced by reacting Sulfuric acid with sodium chloride. However, an aqueous solution of HCl is saturated (at standard temperature and pressure) at around 40% concentration (like carbon dioxide in soda). Any solution which has been saturated under higher pressure to a higher concentration than this will go "flat" if exposed to normal atmospheric conditions, and return to 40% as the hydrogen Chloride escapes. Bubble hydrogen chloride gas (produced as said above) through water, and the gas will slowly saturate the solution. I wouldn't recommend this though, as hydrogen chloride is nasty stuff.

Austin Feathers
- Overland Park, Kansas, US
July 11, 2010

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A. The others are correct, hydrochloric above the 37% mark can only be produced under pressure, to force the escaping hydrogen chloride back into solution. Otherwise, at room temperature and pressure, the water saturates and no more hydrogen chloride will dissolve.

I do produce large amounts of hydrogen chloride at home using the salt / sulfuric method. Table salt works, anhydrous CaCl2 works better (more gas per unit mass of salt). The acid has to be near it's maximum distillable limit (98%). I also have thousands upon thousands of pounds worth of laboratory equipment to handle it and tens of other chemists providing tips on every detail.

It's doable at home. Get it wrong, however, and it's going to get very nasty, very quickly.

You should see the state of the area I generate the gas in, anything it touches it corrodes. Supposedly chemical safe plastics fall apart in minutes. The stainless is corroding, badly. I have often inhaled some of the gas, and even let others have a go to see what it's like. It is physically impossible not to have a minute long coughing seizure from one inhalation; I also smoke, so am used to ignoring the urge to cough.

There is another way to generate what is essentially pure 'hydrochloric', but that's harder and more dangerous again, so it doesn't really need discussing.

John Heritage
- Wallasey, Merseyside, United Kingdom
August 21, 2010

A. Since HCl is in nothing but water, can't you just use Driereite to purify the HCl by removing the water in the mixtures, which is also why it's almost impossible to distill upon mixture; the percentages are at the same degree of 110 for a water distill.

Brian Mag
- victoria, texas, usa
October 22, 2010

A. Extractive Distillation followed by high pressure HCl gas dissolution will give you an Ideal Solution to get high concentration HCl solution. However, since High Concentration HCl solution is unstable, it has to be generated only at the time of use.

Salting effect will work here.

Prashanth M
- Trivandrum, Kerala, India
August 24, 2011

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February 17, 2018

A. LOOK AT THE BOILING POINTS OF WATER AND HCL ACID!

WATER BOILS AT EXACTLY 100 °C - BUT AS WE ALL KNOW IT EVAPORATES AT LOWER TEMPERATURES!

HCL ACID - A BLEND OF HCL GAS AND H2O! BOILS AT 110 °C.

YOU CAN SAFELY DISTILL OUT THE WATER AT UNDER 110 °C A SINGLE DEGREE OVER AND YOUR JUST GOING TO GET A RESULTANT FLASK OF THE SAME CONCENTRATION YOU STARTED WITH!

THIS PROCESS WORKS THE SAME FOR SULFURIC ACID! WHICH IS EASIER AS IT'S BOIL POINT IS AROUND 300 °C.

*NOTE BUT BE WARNED IF YOU TAKE THE REMOVAL OF WATER TOO FAR GASES FROM EITHER PROCESS WILL CAUSE HCL GAS OR SULFURIC GAS TO TO LOST INTO THE AIR!

*THEREFORE BEING HUMAN, AS I HOPE EVERYONE HERE IS, YOU NEED A FUME HOOD!

DON'T BOTHER DOING ANYTHING LIKE THIS WITHOUT ONE AND ALL THE SAFETY EQUIPMENT RECOMMENDED IN CHEMISTRY LITERATURE BECAUSE THINGS CAN AND WILL GO WRONG.

HUGH MCRAE
- Adelaide, Australia.