The pH of a buffer solution prepared by using 0.04 M of C6H5COONa and 0.02 M C6H5COOHsolutions is(Note: Ka of acid is 6.4 × 10−5 at 25°C)A. 3.89B. 4.19C. 4.49D. 6.19
Question
The pH of a buffer solution prepared by using 0.04 M of C6H5COONa and 0.02 M C6H5COOHsolutions is(Note: Ka of acid is 6.4 × 10−5 at 25°C)A. 3.89B. 4.19C. 4.49D. 6.19
Solution
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
where:
- [A-] is the concentration of the base (C6H5COONa in this case)
- [HA] is the concentration of the acid (C6H5COOH in this case)
- pKa is the negative logarithm of the acid dissociation constant (Ka)
First, we need to calculate the pKa from the given Ka. The pKa is calculated as follows:
pKa = -log(Ka) = -log(6.4 × 10−5) = 4.19
Then, we substitute the values into the Henderson-Hasselbalch equation:
pH = 4.19 + log(0.04/0.02) = 4.19 + log(2) = 4.19 + 0.3 = 4.49
So, the pH of the buffer solution is 4.49. Therefore, the correct answer is C. 4.49.
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