- Joined
- Jun 13, 2006
- Messages
- 310
- Reaction score
- 0
Let's say we titrate weak monoprotic acid HA with strong base. At half-eq. point, There are equal concentration of A- and HA.
The dissociation reaction for HA is HA + H20 -> H3O+ + A-.
Since HA is weak acid, Ka is small, say 10^-10.
Then isn't the Keq for reverse reaction huge? which is 1/10^-10 = 10^10?
Then why isn't good amount of A- converted back to HA? I'm really confused. Would anyone please clarify? Thanks in advance.
The dissociation reaction for HA is HA + H20 -> H3O+ + A-.
Since HA is weak acid, Ka is small, say 10^-10.
Then isn't the Keq for reverse reaction huge? which is 1/10^-10 = 10^10?
Then why isn't good amount of A- converted back to HA? I'm really confused. Would anyone please clarify? Thanks in advance.