Final answer:
By making use of the ion product of water and the given Ka values, we can calculate the Kb values of oxalic acid deprotonated forms, oxalate. The calculated Kb values are approximately 1.78 x 10^-13 and 1.84 x 10^-10.
Step-by-step explanation:
To calculate the two Kb values of oxalate from the given Ka values, you need to use the formulas of Ka, Kb and Kw. Firstly, understand that Ka*Kb=Kw, where Kw is the ion product of water, a constant equal to 1.0 * 10^-14. This relationship exists as a result of water being able to act as both an acid and a base.
For oxalic acid, we are given two Ka values: Ka1 = 5.62 x 10^-2 and Ka2 = 5.42 x 10^-5. To find the corresponding Kb values, rearrange the equation to solve for Kb (Kb=Kw/Ka), and insert the given Ka values into the equation:
- When Ka = 5.62 x 10^-2, Kb = 1.0 x 10^-14 / 5.62 x 10^-2 = 1.78 x 10^-13
- When Ka = 5.42 x 10^-5, Kb = 1.0 x 10^-14 / 5.42 x 10^-5 = 1.84 x 10^-10
So, the two Kb values of oxalate are approximately 1.78 x 10^-13 and 1.84 x 10^-10.
Learn more about Acid-Base Equilibrium