What is the pH of a solution that is 0.1 M in both acetic acid and sodium acetat

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Question: What is the pH of a solution that is 0.1 M in both acetic acid and sodium acetate?

Options:

Correct Answer: 4.76

Solution:

Using Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]); pKa of acetic acid = 4.76, so pH = 4.76 + log(1) = 4.76

What is the pH of a solution that is 0.1 M in both acetic acid and sodium acetate?

What is the pH of a solution that is 0.1 M in both acetic acid and sodium acetate?

Step 1: Identify the components of the solution. We have acetic acid (HA) and sodium acetate (A-).
Step 2: Determine the concentrations of acetic acid and sodium acetate. Both are 0.1 M.
Step 3: Recall the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]).
Step 4: Find the pKa value for acetic acid, which is 4.76.
Step 5: Calculate the ratio of [A-] to [HA]. Since both are 0.1 M, the ratio is 0.1/0.1 = 1.
Step 6: Substitute the values into the Henderson-Hasselbalch equation: pH = 4.76 + log(1).
Step 7: Calculate log(1), which is 0.
Step 8: Add the values: pH = 4.76 + 0 = 4.76.

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