Calculate `[H^(+)]` at equivalent point between titration of 0.1 M, 25 mL of weak acid HA `(K_(a(HA)=10^(-5)` with 0.05 M NaOH solution:

Calculate [H^(+)] at equivalent point between titration of 0.1 M, 25 mL of weak acid HA (K_(a) (HA)=10^(-5)) with 0.05 M, 50ml of NaOH solution:

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 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 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) .

The equivalent point in a titration of 40.0mL of a sodium of a weak monoprotic acid occurs when 35.0mL of a 0.10M NaOH solutio has been added. The pH of the solution is 5.5 after the addition of 20.0mL of NaOH solution. What is the dissociation constant of the acid ?