Practice question
Question
A weak acid HB has Ka = 4.0 × 10⁻⁶ . If its 0.05 M solution is mixed with 0.025 M NaOH , what is the pH of the resulting solution?
Explanation
HB + OH- → B- + H₂O , moles: HB = 0.05 , OH- = 0.025 , after reaction: [HB] = 0.025 M , [B-] = 0.025 M . Buffer: pH = pKa + log ([B-]/[HB]) = -log(4.0 × 10⁻⁶) + log (0.025/0.025) = 5.4 + 0 = 5.4 .
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