Respuesta :
Answer:
The value of dissociation constant from this experimental data fro phenol is [tex]9.3576\times 10^{-11}[/tex].
Explanation:
[tex]C_6H_5OH\rightleftharpoons C_6H_5O^-+H^+[/tex]
Initially c 0 0
At eq'm [tex](c-c\alpha )[/tex] [tex]c\alpha [/tex] [tex]c\alpha [/tex]
Concentration of phenol , initially = c = 0.529 M
Degree of dissociation = [tex]\alpha =1.33\times 10^{-3} \%=1.33\times 10^{-5}[/tex]
An expression for dissociation constant is given as:
[tex]K_a=\frac{[C_6H_5O^-][H^+]}{[C_6H_5OH]}[/tex]
[tex]K_a=\frac{c\alpha \times c \alpha }{(c-c\alpha )}=\frac{c(\alpha )^2}{(1-\alpha )}[/tex]
[tex]K_a=\frac{0.529 M\times (1.33\times 10^{-5})^2}{(1-1.33\times 10^{-5})}[/tex]
[tex]K_a=9.3576\times 10^{-11}[/tex]
The value of dissociation constant from this experimental data fro phenol is [tex]9.3576\times 10^{-11}[/tex].
