As the weak acid (HA) is titrated with a strong base (OH−), the neutralization reaction is:
HA...
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As the weak acid (HA) is titrated with a strong base (OH−), the neutralization reaction is:
HA + OH− → A− + H2O.
As the neutralization occurs, [HA] decreases and [A−] increases, allowing the solution to act as a buffer. Suppose 0.0015 mol HA and 0.0005 mol A− are present in 125 mL solution.
(a) What are the approximate concentrations of HA and A−?
(b) If the pKa of HA is 3.90, what is the pH of this solution?
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