Calculate the pH of solution in a titration experiment

The pKa of hypochlorous acid

The pKa of hypochlorous acid is 7.530. A 52.0 ml solution of 0.149 M sodium hypochlorite (NaOCl) is titrated with 0.293 M HCl. Calculate the pH of the solution.

What is the pH of the solution in the titration experiment? The pH of the buffer solution is 7.236 Explanation: Henderson - Hasselbalch equation of a buffer solution consisting of a weak acid and its conjugate base is given as: pH=pKa+log([conjugate base]/[weak acid]) The hypochlorous acid (HClO) is the weak acid and the conjugate base the hypochlorite anion (ClO⁻) is the conjugate base. The dissociation of the salt is given by: NaOCl(aq) ⇒ Na⁺(aq) + ClO⁻(aq) The salt dissociates at a ratio of 1:1 Substituting values to get: pH=pKa+log([conjugate base]/[weak acid]) pH=7.53+log(0.149M/0.293M) pH=7.53-0.2937 pH=7.236 The pH of the buffer solution is 7.236
← Gas effusion understanding the relative amounts of helium and argon What happens when a weakly dissociating compound is exposed to an electric current →

More Posts: