A weak base, B, has basicity constant Kb = 2 × 10-5. The pH of any solution in which B = BH+ is

B + H2O ⇌ BH+ + OH- Kb = BH+ OH-B or Kb = OH- POH = 5-log 2 ∴ pH = 14 - pOH = 9 + log 2 = 9.3

A weak base, B, has basicity constant Kb = 2 × 10-5. The pH of any solution in which B = BH+ is

B + H2O ⇌ BH+ + OH- Kb = BH+ OH-B or Kb = OH- POH = 5-log 2 ∴ pH = 14 - pOH = 9 + log 2 = 9.3

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A weak base, B, has basicity constant $K_{b} = 2 \times 10^{- 5}$ . The pH of any solution in which $[B] = [B H^{+}]$ is

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4.7

7.0

9.3

9.7

answer is C.

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$B + H_{2} O ⇌ {BH}^{+} + {OH}^{-} K_{b} = \frac{[{BH}^{+}] [{OH}^{-}]}{[B]} or K_{b} = [{OH}^{-}] POH = 5 - \log 2 ∴ pH = 14 - pOH = 9 + \log 2 = 9.3$

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A weak base, B, has basicity constant Kb = 2 × 10-5. The pH of any solution in which B = BH+ is

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A weak base, B, has basicity constant $K_{b} = 2 \times 10^{- 5}$ . The pH of any solution in which $[B] = [B H^{+}]$ is