Problem- Although the dissociation of an acid is commonly written as indicated in Kw=[H+][OH-] = 1.0 E -14, better representations of the process and the resulting equilibrium expression are:
HA(aq) + H20(l) = H3O+ + A- K=[H3O+][A-]/[HA][H2O]
The equilibrium expression is usually simplified to Ka=[H+][A-]/[HA] by multiplying both sides of the equation by the concentration of water and defining a new constant, the acid dissociation constant, Ka as [K][H2O].
Is it a valid procedure to incorporate the water concentration into the acid dissociation constant?
I just need a general explanation of it please- Thanks!