Question

Given the Mass of acid dissolved in water, Volume of the solution, Molarity of a strong base used to titrate acid, and Volume of the base needed to reach the equilibrium point.

Calculate the molar mass of the acid.
Given the pH of the resulting solution after a given amount of base added, calculate Ka.
Calculate Kb
Calculate pH of solution at equilibrium point.

Answer 1

K_a = [H⁺][In^– ]

[HIn]

n_{HCl total} = n_{HCl neutralized by tablet} + n_{HCl neutralized by NaOH}(V_HCl × M_HCl) = (n_{HCl neutralized by tablet}) + (V_OH^– × M_OH^–)or (n_{HCl neutralized by tablet}) = (V_HCl × M_HCl) – (V_OH^– × M_OH^–)