Problem: The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

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We are being asked to calculate the K_b for a 0.1 M weak base (HB).

Step 1. Equilibrium reaction: HB_(aq) + H₂O_(l) ⇌ BH₂⁺_(aq) + OH^-_(aq)

$K_{b} = \frac{products}{reactants} = \frac{[{BH}_{2}] [{OH}^{-}]}{[HB]}$

$K_{b} = \frac{[x] [x]}{[0.1 - x]} K_{b} = \frac{x^{2}}{0.1 - x}$

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The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

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Problem: The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

FREE Expert Solution

Problem Details

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