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The k for acetic acid, HC2H3O2, is 1.8 * 10 ^ - 5 What is the ph of a buffer prepared with 1.0 m HC2H3O2 and 1.0 m C2H3O2-? HC2H3O2(aq) + H2O(l) = C2H3O2 (aq) + H3O+(aq)
Accepted Answer
The pH of the buffer can be calculated using the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
where:
pKa is the negative logarithm of the acid dissociation constant (Ka) for acetic acid (HC2H3O2).
[A-] is the concentration of the conjugate base (C2H3O2-)
[HA] is the concentration of the weak acid (HC2H3O2)
In this case:
pKa = -log(1.8 x 10^-5) = 4.74
[A-] = 1.0 M
[HA] = 1.0 M
Therefore, the pH of the buffer is:
pH = 4.74 + log(1.0/1.0) = 4.74
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