Calculate the pH at equivalence point when a solution of 0.10 M acetic acid is titrated with a solution of 0.10 M NaOH solution . K_(a)for acetic acid = 1.9xx10^(-5)

Calculate the pH at equivalence point when a solution of 0.10 M acetic

1.	Calculate the pH at equivalence point when a solution of 0.10 M acetic acid is titrated with a solution of 0.10 M NaOH solution . K_(a)for acetic acid = 1.9xx10^(-5)
Answer» Solution :At the EQUIVALENCE point, `CH_(3)CO ON a` is formed asn its concentration `=(0.1)/(2) M = 0.05 M`. It is a slat of weak acid and strong base. The formula for finding the pH of such a SALT is `pH = - (1)/(2) [log K_(w) + log K_(a) - log c]` `:. pH = - (1)/(2) [log 10^(-14)+log (1.9xx10^(-5))-log(5xx10^(-2))]` `=-(1)/(2) [-14 + (-5+0.2788)-(-2+0.6990)]=(1)/(2) (14+5-0.2788-2+0.6990)=(17.42)/(2) = 8.71`