50 mL of 0.1 M acetic acid is mixed with 50 mL of 0.1 M sodium acetate (the conjugate base). The Ka of acetic acid is approximat
ely 1. 74 X 10 -5. What is the pH of the resulting solution?
1 answer:
Answer:
4.76
Explanation:
In this case, we have to start with the <u>buffer system</u>:
We have an acid () and a base (). Therefore we can write the <u>henderson-hasselbach reaction</u>:
If we want to calculate the pH, we have to <u>calculate the pKa</u>:
According to the problem, we have the <u>same concentration</u> for the acid and the base 0.1M. Therefore:
If we divide:
If we do the Log of 1:
So:
With this in mind, the pH is 4.76.
I hope it helps!
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