HCl should be highly soluble in ethanol - nearly as soluble as it is in water. Some references suggest that as much as 78 parts per 100 parts ethanol are soluble at 0 C, decreasing to 69 parts at 20 C.

I suspect your problem could be (a) too high of temperature, (b) too large of bubbles, or (c) insufficient contacting time to absorb the HCl.

I agree with Larry and add to him you may need a catalyst to adsorb the HCl gas molecules on it. This is required to bring the the two materials in contact with each other. The catalyst may be porous plates of aluminum oxide you pass firstly HCl gas on it followed by a flow of ethanol. This process may run on long tubes in a closed flow system.

This is a conceptual answer by me to facilitate the reaction between a gas material and a liquid material.

You may look at the link: https://daim.idi.ntnu.no/masteroppgaver/013/13022/masteroppgave.pdf

Best wishes

The solution process must be exothermic also. With water the reaction is rather fast and may be violent. Sorry Dr Zekry but "catalyst" is not the right word for defining your description, which is a physical disparsion of a gas in aliquid. But I agree that a "frit" i.e. a fritted glass bubbler (porous alumina may be OK but expensive?), is the good solution to get the gas/liquid interface at maximum and soften the dissolution process.

Dr Zekry, very sorry for my remark, I did not understand completely your suggestion. Now I think that you suggest to adsorb the gas on a "basic" solid (alumina, or Al oxide), then transfer the adsorbed gas/solid in the Iiquid. I had a look at the link you gave, describing a process for removing HCl gas on such adsorbent in a reversible way. But I fear that when we put the HCl/Oxide in a polar liquid, the ionization process will conduct to formation of a chloride salt: HCl + Al2O3 (or Al(OH3)3 etc.) ---> Al(3+) + 3 Cl- (+ n H2O...).

Hi, you can check the link below for more information:

https://periodic-table-of-elements.org/SOLUBILITY/hydrogen_chloride