7.47. It has been found that the pH of a 0.01 M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its PKa.
7.47. It has been found that the pH of a 0.01 M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its PKa.
pH= −log [H+]=4.15
[H+]= antilog (−4.15)= 7.08*10−5
[A−]= [H+]=7.08*10−5
The concentration of undissociated acid is 0.01−0.000071=0.009929M.
HA+H2? O? H3? O++A−
Ka? = [H3? O+] [A−] / [HA]? = (7.08*10−5) (7.08*10−5)? / 0.009929
= 5.05*10−7
pKa? = −logKa? = −log5.05*10−7 ≈ 6.3
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