Respuesta :
pH is calculated using Handerson- Hasselbalch Equation,
pH = pKa + log [Conjugate Base] / [Acid] --- (1)
Conjugate Base = NaClO
Acid = HClO
So,
pH = pKa + log [NaClO] / [HClO]
We are having concentration of acid and salt but missing with pKa,
pKa is calculated as,
pKa = -log Ka
Putting value of Ka,
pKa = -log 2.9 × 10⁻⁸
pKa = 7.53
Now,
Putting all values in eq. 1,
pH = 7.53 + log [0.099] / [0.158]
pH = 7.326
The pH of the buffer solution is 7.34
Concentration of HClO = 0.158 m
Concentration of NaClO = 0.099 m
[tex]K_a[/tex] for HClO = [tex]2.9\times 10^{-8}[/tex]
It is required to calculate the pH of the buffer solution.
What is a buffer solution?
A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small amount of strong acid or base is added to it.
The formula for calculating the pH of acidic buffer solution is
The Henderson - Hasselbalch equation states that for a buffer solution that consists of a weak acid and its conjugate base, the buffer pH is given by:
[tex]pH = p{Ka} + log\frac{[salt]}{[acid]}[/tex]
In this case, the buffer hypochlorous acid HClO is a weak acid, and its conjugate base is the hypochlorite anion ClO⁻ is delivered to the solution via sodium hypochlorite NaClO.
We know the value of [tex]K_a[/tex], firstly we have to calculate the value of [tex]pKa[/tex]
[tex]pKa= - log\ Ka[/tex]
[tex]pKa = - log (2.9\times10^{-8})\\pKa = 7.54[/tex]
[tex]pH = 7.54 + log\frac{[0.099]}{[0.158]}\\pH = 7.34[/tex]
Therefore, the pH of the buffer solution is 7.34
To learn more about the buffer solution, click here:
https://brainly.com/question/13833120
