Answer :
Answer:
[tex]\alpha =0.0009995[/tex]
Explanation:
Hello,
In this case, given the pH of the weak acid HA, we can obtain the concentration of hydrogen in the solution as shown below:
[tex]pH=-log([H^+]})[/tex]
[tex][H^+]=10^{-pH}=10^{-4.0}=1x10^{-4}M[/tex]
In such a way, the degree of ionization ([tex]\alpha[/tex]) is computed as:
[tex]Ka=\frac{\alpha ^2C_0}{1-\alpha}[/tex]
Whereas [tex]C_0[/tex] is 0.010 M and the acid dissociation constant is:
[tex]Ka=\frac{(1x10^{-4})^2}{1-1x10^{-4}}=1x10^{-4}[/tex]
Thus, solving for [tex]\alpha[/tex], we obtain:
[tex]\alpha =0.0009995[/tex]
Regards.