Answer:
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]))](https://img.qammunity.org/2021/formulas/chemistry/high-school/19sibpov38c282duszxu6ssfi7uwsozswb.png)
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](https://img.qammunity.org/2021/formulas/chemistry/high-school/c2pxr0cdttvxoh7059fml462w95ornv637.png)
The pH of the buffer solution is 7.236