Why is the pOH of 1 molar HCl 14 in an aqueous solution?
I was learning about strong bases and strong acids in chemistry within this context:
We have 1L of pure water at 25°C, and the pH of water is 7 and the pOH of water is 7, so it is a neutral solution.
Then we add 1 mole of HCl into the water. HCl, because it is such a strong acid, disassociates completely in the water. After some basic calculations, we found that the pH of HCl was 0 and the pOH was 14, but the way he showed this was using the water's pH and pOH - does this make sense?
So we found that the pH of water is 0, and then he did something funny and got a pOH of 14. Why is the pOH of this solution 14?
Here is the video, video mark, 10:02: Khan Academy - pH & pOH of Strong Acids and Bases