Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the ratio of [CH3COO-]/[CH3COOH] to have a pH of 4.00:
In the solution, identify the weak acid and the conjugate base. Recall from the Bronsted-Lowry definition that an acid is a proton (H+) donor and the base is a proton (H+) acceptor.
How much more acetic acid (pKa = 4.76) than acetate should be in solution to maintain a pH of 4.00?
a. 2.13 times more
b. 5.75 times more
c. 0.47 times more
d. 0.00 times more
e. 0.17 times more
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