In a solution of 103.7 microM acetate buffer, what is the pH of the solution if

Question

In a solution of 103.7 microM acetate buffer, what is the pH of the solution if the concentration of acetate is 23.9 microM (just the deprotonated state)? The pKa of acetic acid is 4.76.
If someone could walk me through how to solve this problem it would be very appreciated!! In a solution of 103.7 microM acetate buffer, what is the pH of the solution if the concentration of acetate is 23.9 microM (just the deprotonated state)? The pKa of acetic acid is 4.76.
If someone could walk me through how to solve this problem it would be very appreciated!!
If someone could walk me through how to solve this problem it would be very appreciated!!

Explanation / Answer

For buffer,

pH = pKa + log(base/acid)

with,

[acetate] = 23.9 mM

[buffer] = 103.7 mM

So, [acetic acid] = 103.7 - 23.9 = 79.8 mM

Thus pH of buffer would be,

pH = 4.76 + log(23.9/79.8)

     = 4.236

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