The Kb for a weak base is 4.9 × 10 -6. What is the value of Ka for for its conjugate acid? 2.0 x 10-9 4.9 × 104 4.0 × 10 -6 2.0 × 109 2.0 × 10 -5
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The equilibrium constant expression for this reaction is: Kb = [BH+][OH-]/[B][H2O] Since water is present in excess, we can assume that its concentration remains constant and write: Kb = [BH+][OH-]/[B] Now, we can use the relationship between Ka and Kb for a Show more…
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