# can pure molten hydrochloric acid conduct electricity?

by no idea
Tags: acid, conduct, electricity, hydrochloric, molten, pure
 P: 93 can pure molten hydrochloric acid conduct electricity?
 P: 736 Of course; HCl is an ionic solid; by definition, ionic solids are composed of anions and cations; when the solid is made liquid, you have free and mobile ions; thus, you can conduct electricity. Yes, pure molten HCl will conduct electricity
 PF Patron Sci Advisor P: 614 Well, I am not sure; hydrochloric acid is a gas which is used as aqueous solution. In high temperature you will not get it as a solid; it will evaporate. However, high temperature will possibly help its ionization.
P: 736

## can pure molten hydrochloric acid conduct electricity?

Would not the HCl gas conduct electricity as well? It has ions more mobile than that of its liquid form
 P: 42 Liquid HCl will probably be a poor conductor of electricity owing to the fact that it is a covalent compound and doesn't have terribly many ions floating about. Pure water will conduct electricity as a result of ions created by the reaction 2H2O <-> H3O+ + OH-, and there is probably an analagous equilibrium taking place with the HCl: 2HCl <-> H2Cl+ + Cl-. However, HCl is such a weak base that it will have little tendency to accept a proton to form H2Cl+, so this reaction will probably have very little effect (also it should be noted that pure water is still a poor conductor of electricity, even with the aforementioned equilibrium taking place).
P: 736
 Quote by Pyrovus Liquid HCl will probably be a poor conductor of electricity owing to the fact that it is a covalent compound
Silly mE! I forgot it was covalent... !!!
Ay!

 Quote by Pyrovus However, HCl is such a weak base
How? HCl is hydrochloric acid!, and it is a strong acid!! Strong acids will dissociate well in water!! Which means mobile ion availability in aqueous HCl solutions!--and thus will conduct electricity!
What Pyrovus means is that in the reaction $$2HCl \leftrightarrow H_2Cl^+ + Cl^-$$ HCl plays role of proton acceptor - so it is a Bronsted base.