Absolutely correct.  With a strong acid and strong base titration, the end point is where the pH = 7.00 (Neutral).  As soon as you add one more drop of NaOH, the pH will shoot up into the basic range since NaOH is a strong base.  (And the addition of one drop to a neutral solution will cause a huge increase in the OH- concentration).  So while you're titrating, the solution will be clear until it suddenly becomes basic due to that addition of one extra drop of NaOH.

For a weak acid/strong base titration, a buffer range exists because as you are adding the base to the acid, you are forming water and the conjugate base of that acid.  Any combination of a weak acid and its conjugate base can be considered a buffer.  However, once you've added enough base to the solution, there won't be enough of the weak acid floating around to provide a buffer.

For strong acid and strong base titration, any indicator can be used. It is because the sharp pH change at the equivalent point.