For a weak acid in an aqueous solution, what is the difference between the actual [HA] and the formal [HA]? (symbolized as F
suppose HA is the weak acid . HA can be dissociated into H+ and A- . there will be equilibrium estabilised between weak acid undissociated part and dissociated ions
suppose if intial concentration of HA is C . here HA is known to be formal HA ( initial )
once equilibrium is established some of the concentration decreases from ' C' . so the resulatant conentration = C- x
here weak acid is called actual acid . because the actual amount contributed can by known from here only
HA < ---------------------------> H+ + A-
C 0 0 -----------------------> initial
-x +x +x ------------------------> change
C-x x x ----------------------------> equailbrium
formal concentration = [HA] = C
actual concetration = [HA] = C- x
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