Answer : The value of \(K_b\) is, \(7.7\times 10^{-8}\)
Explanation :
As we are given : \(K_a=1.3\times 10^{-7}\)
As we know that,
\(K_a\times K_b=K_w\)
where,
\(K_a\) = dissociation constant of an acid = \(1.3\times 10^{-7}\)
\(K_b\) = dissociation constant of a base = ?
\(K_w\) = dissociation constant of water = \(1\times 10^{-14}\)
Now put all the given values in the above expression, we get the dissociation constant of a base.
\(1.3\times 10^{-7}\times K_b=1\times 10^{-14}\)
\(K_b=7.7\times 10^{-8}\)
Therefore, the value of \(K_b\) is, \(7.7\times 10^{-8}\)
