Question 14.5: Consider the buffer system shown in the box below. The symbo...
Consider the buffer system shown in the box below. The symbol represents a mole of the weak acid; the symbol represents a mole of its conjugate base. The pH of the buffer is 6.0. What is K_{a} of the weak acid?
ANALYSIS
Information given: mol HB (3); mol B^{-} (2) pH (6.0)
Asked for: K_{a} for HB
STRATEGY
1. Find [H^{+}].
2. Substitute into Equation 14.2.
[H^+]= K_{a} \times \frac{n_{HB}}{n_{B^-}}\blacktriangleleft ⓘ (14.2)
ⓘIf you start with 0.20 mol HB and 0.10 mol B^-, [H^+] = 2K_{a}.
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