How does strong acids conduct electricity in water? How do strong acids conduct electricity in water?
I have just studied ionization of water and I'm confused about some points.
First: I know that water ionizes  in a very small amount ($10^{-14}$) so it doesn't conduct electricity and if we add strong acid (or base) to it , it becomes a good conductor of electricity. My question here is how it conduct electricity although if a strong acid is in water its $\ce{H+}$ ions concentration  in water would range from $10^{-1}$ to $10^{-6}$ (which is avery small amount) to keep $K_w$ constant.
I'm confused so if you understood me please explain and tell me if I have something wrong
In water at 25 ºC $[H+]=[OH-]=10^{-7}M$, so a concentration of $[H+]=10^{-6}M$ is very low. With a strong acid like HCl you have to dissolve only around 35 micrograms in a liter of water to get this concentration.
Sea water on the other hand has a high conductivity and, in average, 35 grams per liter of salts dissolved in it. If you dissolve 35 grams of HCl en 1 liter of water you have $[H+]=1M$ and surely you can expect a high conductivity.
These are gross numbers, but I think they help to get the idea.
Conductivity of a solution depends on the free ions present on the mixture. With a strong acid you can get a high concentration of ions using a little quantity of acid. With a weak acid you need much more.