A buffer contains the weak acid HA and its conjugate base A-. The weak acid has a p Ka of 4.82 and the buffer has a pH of 4.25.
This is true of the relative concentration of the weak acid and its conjugate base in the buffer.
a) [HA} > [A-]
b) [Ha} < [A-]
c) [HA]=[A-]
1 answer:
From the henderson-hasslebalch equation: <span>pH=pKa+log<span><span>[<span>A−</span>]/</span><span>[HA]</span></span></span>
it's apparent that when pKa=pH, c. [HA]=[A^-].
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