Does saline water lose conductivity over time? When current is passed through a beaker of salt water, the ions move towards the terminals (based on their charge– e.g., sodium ions to the cathode and chlorine ions to the anode).
Following this idea, should there not be a certain point when all the positive ions are on one side, and the negative on the other– with no further movement? So, in effect, causing the solution to not be conductive to electricity anymore?
EDIT: Would this be apparent if I were to do an experiment?
 A: No, all water has a small spontaneous rate of generating ion pairs.   There
is a fresh supply of ions generated as long as there is water, so it is
only when the water all leaves the system that conduction stops.
What an electric current does, is shift the equilibrium concentration
due to that spontaneous generation, so that there is excess (OH-) ions
around the positive terminal, and excess (H3O+) ions around the negative
terminal.    There may (or may not) be a reaction AT those terminals,
creating some chemical substances other than water and the electrode material.
Some generation of peroxide or hydrogen gas is certainly possible.
The concentration of those ions is represented by the pH of the water: near
the positive terminal (anode) the water will be basic, and near the negative
terminal it will be acidic.  When current is stopped, equilibrium quickly
will be reestablished, as the charged ions repel their similarly-charged
neighbors.
In the case of AC current, there may be no non-reversible chemical changes
at the electrodes, just a mess of oddly-charged ions which revert to
neutral water, or there might be evolution of hydrogen and oxygen (and loss
of water).
Salt raises some of the rates, and adds to the possible reactions, but
is not essential: the ionizing solvent, water, has its own conductivity.
A: Theoretically, yes.
At one point of time, all ions will be discharge  (even spectator ions, if any, theoretically,  will be discharged), after which the solution will lose conductivity.
A: Yes, that is exaclty what happens.
Of course, it would take a lot of time to discharge a very big countainer, but the fact that in any container the solution loses conductivity as all ions have adhered to the electrodes is what makes galvanic cells (a.k.a. the basis of the electric battery) not work forever.
With a bit of knowledge on redox reactions you can even calculate how much time it takes for the saline water to lose all its conductivity, but perhaps that would be a question more appropiate for the chemistry stack exchange.
