I accidentally erased your post on the hydrolysis of various anions. The answer is

Kb(for the anion) = (Kw/Ka for the Ka for the acid) where Ka will be Ka for monoprotic acids, k2 for diprotic acids, or k3 for triprotic acids
So to make OH^- the smallest you want Ka to be the largest. For example,
........CO3^2- + HOH ==> HCO3^- + OH^- so Kb for CO3^2- is
Kb for CO3^2- = (Kw/k2 for H2CO3) = (x)(x)/(CO3^2-). Therefore, for OH to be the smallest you want Kw/Ka to be the smallest which makes Ka the largest.

To find the answer to the question on the hydrolysis of various anions, we can follow the provided formula:

Kb (for the anion) = (Kw / Ka for the acid)

This formula allows us to determine the value of Kb, the base hydrolysis constant, for different anions. The value of Kb tells us how much the anion hydrolyzes to produce hydroxide ions (OH^-) in an aqueous solution.

To determine the Kb for a specific anion, we need to consider the Ka for the corresponding acid. For monoprotic acids, we use the Ka value directly. For diprotic acids, we use the Ka2 value, and for triprotic acids, we use the Ka3 value.

In the given example of CO3^2- (carbonate ion), we can see that it hydrolyzes to produce bicarbonate ion (HCO3^-) and hydroxide ion (OH^-):

CO3^2- + HOH --> HCO3^- + OH^-

To find the Kb for CO3^2-, we use the formula:

Kb for CO3^2- = (Kw / k2 for H2CO3)

Here, Kw is the ionization constant for water, and k2 is the Ka value for the second ionization of the acid H2CO3 (carbonic acid).

To calculate the Kb, we need the value of Kw (which is a constant) and the value of k2 for H2CO3. The exact values for these constants can be obtained from reference sources or chemistry textbooks.

Based on the formula, to make OH^- concentration the smallest, we want Kw / Ka to be the smallest, which implies that Ka should be the largest. In other words, we want the acid to be weaker, leading to a smaller concentration of OH^-.

So, in summary, the formula Kb = (Kw / Ka) helps us calculate the base hydrolysis constant for various anions. To find the smallest OH^- concentration, we want the corresponding Ka value to be the largest, indicating a weaker acid.