Respuesta :
The answer is 5.8x10^-10. I did the math and checked other sources as well.
Answer: The base dissociation constant for a conjugate base is [tex]1.72\times 10^{-5}[/tex]
Explanation:
To calculate the base dissociation constant for the given acid dissociation constant, we use the equation:
[tex]K_w=K_b\times K_a[/tex]
where,
[tex]K_w[/tex] = Ionic product of water = [tex]10^{-14}[/tex]
[tex]K_a[/tex] = Acid dissociation constant = [tex]5.8\times 10^{-10}[/tex]
[tex]K_b[/tex] Base dissociation constant = ?
Putting values in above equation, we get:
[tex]10^{-14}=5.8\times 10^{-10}\times K_b\\\\K_b=0.172\times 10^{-4}=1.72\times 10^{-5}[/tex]
Hence, the base dissociation constant for a conjugate base is [tex]1.72\times 10^{-5}[/tex]
