So initially, HOCl autoionize to H+ & OCl- until equiv point. But by adding OH-, it disrupts the would be equilibrium and neutralize the H+. Le Chatelier law's kick in and makes more H+ and eventually consume all of HOCl. Hence, you get Na+ OCl- solution. Is that logic correct?
Almost. In reality all of HOCl is never consumed, as the hydrolysis starts immediately when there is OCl
- base present in the solution.
Because hydrolysis occurs, what's left is just Na+ and OCl-, hence it's better to start using pOH instead of pH since there are no H+ left after equiv point. Is this logic correct?
Hard to say if it is correct or not. There is always some H
+ because we are in water. However, final solution is identical with the one obtained by dissolving solid NaOCl - thus you may treat it as containing (initially, before dissolution) only base OCl
-. If so, pOH calculation is much easier.
Hydrolysis always occurs in every problem right? Whether acidic or basic.
As long as we are in water, hydrolysis occurs always.