Question

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

Answer 1

The pH of the buffer solution is 7.236

Step-by-step explanation:

Henderson - Hasselbalch equation of a buffer solution consisting of a weak acid and its conjugate base is given as:

`pH=pK_a+log(([conjugate base])/([weak acid]))`

The hypochlorous acid (HCIO), 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 dissociate at a ratio of 1:1

Substituting values to get:

`pH=pK_a+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