Titration between acids / bases

Equivalence point or end-point (when equivalence volume is added such that no more acids nor bases are left, only left with salt)

SALT can be classified as
1) NEUTRAL (usually between strong acids and strong bases. pH = 7, due to hydration only)
2) ACIDIC (usually between strong acids and weak bases. pH < 7 due to conjugate acid of weak base)
3) BASIC  (usually between weak acids and strong bases. pH > 7 due to conjugate base of weak acid) 

If a base is weak, i.e. undergoes partial ionisation; then its conjugate acid also undergoes partial ionisation. Therefore, a weak base has its own Kb value, and thus its conjugate acid will have its own Ka value ( where Ka = Kw/Kb)

Reverse is true for weak acids and its conjugate bases.

In general, for any substance that behaves as a weak acid (recall, Lowry-Brosted theory states that acid donates H+), to calculate pH, 
- [H+] = sq. root (Ka.[acid])
-pH = -lg [H+]

In general, for any substance that behaves as a weak base (recall, Lowry-Brosted theory states that base accepts H+), to calculate pH, 
- [OH-] = sq. root (Kb.[base])
-pOH = -lg [OH-]
-pH = 14 – pOH

Thus a salt can behave as a weak acid or a weak base depending on whether it can accepts or donates H+

Hope this helps !