The equilibrium constant Kn for the neutralization of boric acid (H3BO3) and caffeine (C8H10N4O2) is 24. What is Kb for caffeine? The Ka of boric acid is 5.8 x 10^-10.

Verified step by step guidance

1. Step 1: Understand the relationship between the equilibrium constant (Kn) for the neutralization reaction and the individual constants (Ka and Kb). The reaction involves the neutralization of boric acid (H3BO3) with caffeine (C8H10N4O2), where Kn = Ka * Kb.
2. Step 2: Write the expression for the equilibrium constant Kn in terms of Ka and Kb. Since Kn = Ka * Kb, you can rearrange this equation to solve for Kb: Kb = Kn / Ka.
3. Step 3: Substitute the given values into the equation. You have Kn = 24 and Ka = 5.8 \times 10^{-10}. Substitute these values into the equation Kb = Kn / Ka.
4. Step 4: Perform the division to find Kb. Divide the value of Kn by the value of Ka to calculate Kb.
5. Step 5: Interpret the result. The calculated Kb will give you the base dissociation constant for caffeine, indicating its strength as a base in this neutralization reaction.