What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodiu

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Question: What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate?

Options:

Correct Answer: 4.74

Solution:

Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]). Here, pKa ≈ 4.74, so pH = 4.74 + log(1) = 4.74.

What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate?

What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate?

Step 1: Identify the components of the buffer solution. We have acetic acid (HA) and sodium acetate (A-).
Step 2: Determine the concentrations of the components. Both acetic acid and sodium acetate are at 0.1 M.
Step 3: Write down the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]).
Step 4: Find the pKa value for acetic acid. It is approximately 4.74.
Step 5: Calculate the ratio of the concentrations. Since both are 0.1 M, the ratio [A-]/[HA] = 0.1/0.1 = 1.
Step 6: Calculate the logarithm of the ratio. log(1) = 0.
Step 7: Substitute the values into the Henderson-Hasselbalch equation: pH = 4.74 + 0.
Step 8: Simplify the equation to find the pH: pH = 4.74.

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