Respuesta :
Answer :
(a) The value of [tex]K_b[/tex] of the lactate ion is, [tex]7.14\times 10^{-39}[/tex]
(b) The value of [tex]K_b[/tex] of the conjugate base of pyruvic acid is, [tex]3.53\times 10^{-38}[/tex]
Explanation :
Solution for (a) :
As we are given : [tex]K_a=1.4\times 10^{24}[/tex]
As we know that,
[tex]K_a\times K_b=K_w[/tex]
where,
[tex]K_a[/tex] = dissociation constant of an acid = [tex]1.4\times 10^{24}[/tex]
[tex]K_b[/tex] = dissociation constant of a base = ?
[tex]K_w[/tex] = dissociation constant of water = [tex]1\times 10^{-14}[/tex]
Now put all the given values in the above expression, we get the dissociation constant of a base (lactate ion).
[tex]1.4\times 10^{24}\times K_b=1\times 10^{-14}[/tex]
[tex]K_b=7.14\times 10^{-39}[/tex]
Therefore, the value of [tex]K_b[/tex] of the lactate ion is, [tex]7.14\times 10^{-39}[/tex]
Solution for (b) :
As we are given : [tex]K_a=2.83\times 10^{23}[/tex]
As we know that,
[tex]K_a\times K_b=K_w[/tex]
where,
[tex]K_a[/tex] = dissociation constant of an acid = [tex]2.83\times 10^{23}[/tex]
[tex]K_b[/tex] = dissociation constant of a base = ?
[tex]K_w[/tex] = dissociation constant of water = [tex]1\times 10^{-14}[/tex]
Now put all the given values in the above expression, we get the dissociation constant of a base (conjugate base of pyruvic acid).
[tex]2.83\times 10^{23}\times K_b=1\times 10^{-14}[/tex]
[tex]K_b=3.53\times 10^{-38}[/tex]
Therefore, the value of [tex]K_b[/tex] of the conjugate base of pyruvic acid is, [tex]3.53\times 10^{-38}[/tex]
