given a diprotic acid, H2A, with two ionization constants of Ka1 = 1.6×10^-4 and Ka2 = 5.2×10^-11, calculate the ph for a .206 M solution of NaHA
Since we neglect second dissociation and consider the diprotic acid as monoprotic acid for our calculation.
Initial concentration (M) | 0.206 | 0 | 0 |
Change in concentration (M) | -x | x | x |
Equilibrium concentration (M) | 0.206-x | x | x |
The equilibrium constant
Since the value of Kb is small, we use the approximation
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