When a solution of benzoic acid was titrated with `NaOH` the `pH` of the solution when half the acid neutralized was `4.2`. Dissociation constant of the acid is

The pH of 0.1 M solution of an organic acid is 4.0. Calculate the dissociation constant of the acid.

The equivalent point in titration of 40.0 ml of a solution of a weak monoprotic acid occurs when 35.0 of a 0.10 M NaOH solution has been added . The pH of the solution is 5.75 after the addition of 20.0 ml of NaOH solution . What is the dissociation constant of the acid ?

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 ?

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 ?

An organic monobasic weak acid is 50 % neutralised by adding NaOH. The pH of the solution is 5 . Acid dissociation constant for organic acid will be :

Calculate the the ratio of conjugate base// weak acid required to prepare an aqueous solution of benzoic acid and sodium benzote with pH of 4.5 . The acid dissociation constant of benzoic acid is 6.5 xx 10^(-5) .