An acid with a Ka of 2x10^-6 is used to make a buffer. what is the approximate pH of the solution if the buffer has equal concentrations of both the acid and its conjugate base?

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An acid with a Ka of 2x10^-6 is used to make a buffer. what is the approximate pH of the solution if the buffer has equal concentrations of both the acid and its conjugate base?

Chemistry
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Between 4-5 2-3 3-4 5-6
\[Ka = \frac{ [H ^{+}][A ^{-}] }{ [HA] }\]

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pH = pKa + log [A-/HA] I guess if the concentration of acid HA equals the conjugate base A- Log[1] = 0 So the pH would be equal to the pKa and I guess this would be where the greatest buffering capacity would be. PH = pKa
Yeah, definitely that's what I was thinking that looks right to me.

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