What is the pH at equivalence point in the titration of 0.1 M `CH_(3)COOH` and 0.1 NaOH? (`K_(a)` for acetic acid is `1.8 xx 10^(-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)]

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)]

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)]

Calculate the percentage ionization of 0.01 M acetic acid in 0.1 M HCI. K_a of acetic acid is 1.8 xx 10^(-5)

Calculate the percentage ionization of 0.01 M acetic acid in 0.1 M HCI K_a of acetic acid is 1.8 xx 10^(-5)

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 CH_3COOH is titrated with a solution of 0.1 M NaOH. K_a(CH_3COOH)= 1.8 xx 10^(-5)