>According to http://www.chemguide.co.uk/physical/redoxeqia/introduction.html each electrode has an absolute electrode potential which is the difference between the positiveness and negativeness. So if we had a Zn plate in water and it has a negative charge of -5 on the metal. Would the absolute electrode potential be -5-5=-10? >So when we connect that zinc electrode to another electrode say copper. Copper so has it's own absolute electrode potential say -1-1=-2. So would the voltage recorded be -10-(-2)=-8V? Or would the absolute electrode potential be like -5-0=-5 since the solution in a cell is electrically neutral and so the potential differece recorded be -5-(-1)=-4V? So do we just take the difference in charge between the metal and the overall charge of the electrolyte to get the absolute electrode potential and the difference of the two absolute electrode potential is the voltmeter reading or am I wrong here? >Then now if we didn't have a salt bridge, how does the presence of more cations cause an opposite potential difference? The way I see it is like this: looking at the zinc electrode the negative charge on the zinc metal would remain constant but the solution outside becomes more positive. So initially it's absolute electrode potential was -5-0=-5 but soon it's -5-(1)=-6V and so on with the (1) continuing to increase. But even if keeps increasing there wouldn't be an opposite potential difference. So why would the reaction stop after a while?