Practice question
Question
A weak acid HY ( Ka = 2.0 × 10⁻⁵ ) is mixed with 0.01 M NaOH in a 2:1 volume ratio (acid:base). If the final [HY] = 0.04 M , what is the pH?
Explanation
Let volumes be 2V and V, total volume = 3V. Moles: HY = 0.04 × 3V , initial [HY] = 0.06 M , moles NaOH = 0.01V , [Y-] = (0.01V/3V) = 0.00333 M , remaining [HY] = 0.04 . pH = 4.7 + log (0.00333/0.04) = 4.7 - 1.08 = 3.62 .
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