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Calculate the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sod
Calculate the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate.
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Practice Questions
1 question
Q1
Calculate the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate.
4.76
5.76
6.76
7.76
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Using Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]); pKa of acetic acid = 4.76, so pH = 4.76 + log(1) = 4.76
Questions & Step-by-step Solutions
1 item
Q
Q: Calculate the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate.
Solution:
Using Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]); pKa of acetic acid = 4.76, so pH = 4.76 + log(1) = 4.76
Steps: 8
Show Steps
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: 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 the concentrations: [A-] (sodium acetate) is 0.1 M and [HA] (acetic acid) is 0.1 M. So, [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 = 4.76 + 0.
Step 8: Simplify the equation to find the pH: pH = 4.76.
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