You could use an anion exchanger

This question is a bit  too open to answer. Some boundary conditions are further required for a solution.

You may try to dissolve your highly polar product in a solvent like diethyl ether / ethyl acetate and then wash with aqueous sodium bicarbonate solution.

@MP: I could easily guess why your answer was short. In fact, my suggestion is also based on certain assumptions and is not valid in some cases.

You can try using a polymer bound base that would mop up the acid and would only need filtering off the polymer at the end. A common one is DMA which is a tertiary amine and is normally very cheap to buy.

pour the content into sodium carbonate solution, then extract the organic material with chloroform

I use to remove any possible solvent (standardly, by evaporation in vacuum) and evaporate (and re-evaporate several times until success) with ethanol. Of course provided the product sustains ethanol, which should be very probable.

Dissolve your compound in Ethyl acetate and then purge ammonia gas. Ammonium chloride get ppt. out Then Filter it and remove ammonium chloride....

 You can pass it through Basic alumina column

If your compound is soluble in ether, then you can add an organic base (pyridine, TEA, DIPEA). the salt will precipitate and you can decant or filter the salt out. 

I assume the problem is that your compound has significant solubility in water.  On a small scale, you can pass a solution through an OH- form anion exchange resin to remove HCl, or a mixed bed (H+/OH-) ion exchange resin to remove all ionic species. (Essentially, it's Gajanan's method, but with the insoluble resin there's no worry about the salt being crystalline.)  Just stirring the resin with the reaction mixture is usually sufficient, but recovery of the product is better using a column.  Solvent should be polar - water and water-methanol are best at swelling and penetrating the resin beads.

This gets expensive for mole-scale reactions, unless you use a (Na+/Cl-) resin, such as those used for water softening and swimming pools.  They work just fine, but they leave sodium chloride in your final product. If no other ions are present, you'd get to the same endpoint simply by titrating with NaOH.

Note that the resin will bind all ions, so this is not an option if your product is ionizable in water.

is your product a solid or liquid?

is it sensible to water?

you can isolate it, than you wash with a bicarbonate solution.

I will suggest the use of pyridine or triethylamine in the reaction so as to trap the HCl as it is produced to form a soluble salt. In alternative, you can wash your product with bicarbonate solution

Thank you members for your kind feedback. My product is solid and soluble in polar solvents like water, methanol, ethanol etc. The problem is that the salt is also polar so it is getting difficult to separate it from the product in usual time and cost effective way. I have used triethylamine to scrub out HCl. It is forming triethylamine.hydrochloride salt which is again polar. If I wash the product with bicarbonate it will form chloride salt on neutralisation. Then how will I separate sodium chloride from my product?? If you can kindly explain!!

Please check whether your compound is soluble in ethyl acetate (EA).

Assuming that your compound is an organic one, you still have an option to drive it out from the aqueous solution into an organic phase. You may try to saturate the aqueous phase by adding sodium chloride.In case  Your organic solvent could be ethyl acetate, in case your compound is soluble in it (EA). This may work for you.

Wishing you best of luck.

Dr. Joy, which solvent are you using for this reaction for it will help members to suggest further possible and cost effective way of isolating your product.

you could neutralse your reaction using sodium bicarbonate followed by extract the reaction mixture with dichloromethane or chloroform 3x 20mL

https://www.researchgate.net/publication/282914150_How_to_successfully_convert_a_water-soluble_organic_onium_salt_into_its_free_base_or_change_its_anion_by_using_an_anion-exchanger_resin

Research How to successfully convert a water-soluble organic onium sa...

Efficient procedure for non acidic compounds: work up your solution with dry K2CO3. If your compound is acidic, you can wash your solution with NaCl solution or citric acid solution.

I'd like to know about solubility of your product and its functional groups until maybe someone figures out how it should be done.

If your product is solube in a solvent non miscible to water you can wash it with a K2CO3 diluted solution

If it is possible, aseotropic evaporation of reaction mixture, HCl flyes away with water, benzene or somethung else. If target is soluble in organic phase better than in water, but sensitive to alkaline media, try to wash with citric acid in water, it takes well some admitures like dymethylformamidex which dont' leave irganic layer at all.

If it is possible, aseotropic evaporation of reaction mixture, HCl flyes away with water, benzene or somethung else. If target is soluble in organic phase better than in water, but sensitive to alkaline media, try to wash with citric acid in water, it takes well some admitures like dymethylformamidex which dont' leave irganic layer at all.

If it is possible, aseotropic evaporation of reaction mixture, HCl flyes away with water, benzene or somethung else. If target is soluble in organic phase better than in water, but sensitive to alkaline media, try to wash with citric acid in water, it takes well some admitures like dymethylformamidex which dont' leave irganic layer at all.

Dissolve your compound in any polar solvent and wash that organic layer with sodium bicarbonate solution .

I'm answering too late, however, it can help others.

for these kinds of reaction conditions, the best way to remove HCl from the reaction mixture can be the Freeze-pump-thaw procedure.

Reaction of water and sodium ethoxide