Answer:
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:
[tex]pH=pK_a+log(\frac{[conjugate base]}{[weak acid]})[/tex]
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:
[tex]pH=pK_a+log(\frac{[conjugate base]}{[weak acid]})\\pH=7.53+log(\frac{0.149M}{0.293M})\\pH=7.53-0.2937\\pH=7.236[/tex]
The pH of the buffer solution is 7.236
