Calculating pH of Acetic Acid/Sodium Acetate Solution

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SUMMARY

The pH of a solution created by mixing 200.0 mL of 0.400 M acetic acid and 200.0 mL of 1.00 M sodium acetate can be accurately calculated using the Henderson-Hasselbalch equation. The initial concentrations of acetic acid and sodium acetate must be adjusted for the final volume after mixing. The correct pH calculation involves determining the ratio of the concentrations of the conjugate base (sodium acetate) to the weak acid (acetic acid), leading to a pH value that differs from the initial incorrect calculation of 2.02.

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gsingh2011
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The problem is:
Calculate the pH of a solution created by mixing 200.0 mL of .400 M acetic acid and 200.0 mL of 1.00 M sodium acetate.

I got 2.02 for the pH, but according to other people in my class that's the wrong answer. Could someone explain how to do this? I used the Initial, Change, Equilibrium tables, if anyone knows how to do that..
 
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Can you go through your entire working? Perhaps look into the Henderson Hasselbalch equation or similar?
 

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