- #1
Titan97
Gold Member
- 450
- 18
If H2A2+ is being titrated with NaOH, a buffer forms.
The processes taking place are equilibrium between H2A2+ and HA+ ions, autoprotolysis of water and reaction of OH- ions with H2A2+ ions. As NaOH is added, the concentration of acid tends to decrease but because of the equilibrium
##H_2A^{2+} <=> HA^+ + H^+##, the decrease in concentration of acid is negligible.
Adding NaOH increases the amount of conjugate base which in turn increases the concentration of acid. Does this process never end? Whatever NaOH you add, the reacted Acid will form back.
The processes taking place are equilibrium between H2A2+ and HA+ ions, autoprotolysis of water and reaction of OH- ions with H2A2+ ions. As NaOH is added, the concentration of acid tends to decrease but because of the equilibrium
##H_2A^{2+} <=> HA^+ + H^+##, the decrease in concentration of acid is negligible.
Adding NaOH increases the amount of conjugate base which in turn increases the concentration of acid. Does this process never end? Whatever NaOH you add, the reacted Acid will form back.