How does strong and weak acid or base affect the conductivity of aqueous solutions?
We know electricity is the flow of electrons. The flow of ions can do the same thing. The more ions there are in a solution the greater the conductivity. Strong acids and bases dissociate into their respective ions more readily than weak acids and bases. This results in a greater number of ions in the solution, resulting in better conductivity. Same thing goes for solution concentration – the higher the solute concentration the more ions there are to flow in the solution, i.e. better conductivity. However, you pointed out a ‘strong’ acid is different to a ‘concentrated’ acid. A concentrated solution of a very weak acid will not conduct electricity – because a weak acid will not dissociate into it’s ions in water. So in conclusion strong concentrated acid or base electrolyte will vastly improve conductivity of aqueous solutions. A strong but unconcentrated or a weak acid/base will not improve electrical conductivity all that much. EDIT: I just read the answer below mine and I must say t
