Answer:
The concentration of hydrogen ion in the solution was [tex]7.24\times 10^{-7}[/tex].
Explanation:
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
[tex]pH=pK_a+\log(\frac{[salt]}{[acid]})[/tex]
[tex]pH=pK_a+\log(\frac{[NaX]}{[HX]})[/tex]
We are given:
[tex]K_a[/tex] = Acid dissociation constant of HX = [tex]8.64\times 10^{-7}[/tex]
[tex]pK_a=-\log[K_a]=-\log[8.64\times 10^{-7}]=6.06[/tex]
[tex][salt]=[NaX]=0.803 M[/tex]
[tex][acid]=[HX]=0.677 M[/tex]
pH = ?
Putting values in above equation, we get:
[tex]pH=6.06+\frac{0.803 M}{0.677 M}[/tex]
pH = 6.14
[tex]pH=-\log[H^+][/tex]
[tex]6.14=-\log[H^+][/tex]
[tex][H^+]=10^{-6.14}=7.24\times 10^{-7}[/tex]
The concentration of hydrogen ion in the solution was [tex]7.24\times 10^{-7}[/tex].
