Calcualte the pH at the equivalence point when a solution of `0.1M` acetic is titrated with a solution of `0.1M NaOH.(K_(a)for acid = 1.9xx10^(-5))`.

Calculate the pH at the equivalence point when a solution of 0.1 M acetic acid is titrated with a solution of 0.1 M NaOH. K_(a) for acid =1.9xx10^(-5) .

Calculate the pH at the equivalence point when a solution of 0.1 M acetic acid is titrated with a solution of 0.1 M NaOH. K_(a) for acid =1.9xx10^(-5) .

Calculate the pH at the equivalence point when a solution of 0.1M acetic acid is titrated with a solu- tion of 0.1M NaOH, K_a for acid =2 xx 10^(-5)-

Find the pH at equivalence points when a soluiton of 0.1M acetic acid is titrated with a solution of 0.3M NaOH K_(a) for acetic acid =7.5xx10^(-6)

Calculate OH^- concentration at the equivalent point when a solution of 0.1 M acetic acid is titrated with a solution of 0.1 M NaOH. Ka for the acid = 1.9 xx 10^(-5) .

Calculate the pH at the equivalence point when a solution of 0.1 M CH_3COOH is titrated with a solution of 0.1 M NaOH. K_a(CH_3COOH)= 1.8 xx 10^(-5)

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

Calculate the pH at the equivalence point during the titration of 0.1M, 25 mL CH_(3)COOH with 0.05M NaOH solution. [K_(a)(CH_(3)COOH) = 1.8 xx 10^(-5)]