Practice question
Question
A weak base BOH has a Kb = 4.0 × 10⁻⁶ . What is the pH of a 0.01 M solution of BOH ?
Explanation
For BOH <=> B+ + OH- , Kb = (x²/0.01 - x) ≈ (x²/0.01) = 4.0 × 10⁻⁶ . Solving, x = [OH-] = sqrt4.0 × 10⁻⁸ = 2.0 × 10⁻⁴ . pOH = -log(2.0 × 10⁻⁴) ≈ 3.7 , pH = 14 - 3.7 = 10.3 .
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