What is the pH of a buffer that contains 0.5 M ammonia(base) and 0.8 M ammonium chloride(acid)? (pKa = 9.248).
Question
What is the pH of a buffer that contains 0.5 M ammonia (base) and 0.8 M ammonium chloride (acid)? (pKa = 9.248)
Solution
To solve this problem, we can use the Henderson-Hasselbalch equation, which is:
pH = pKa + log([A-]/[HA])
where:
- [A-] is the concentration of the base, which is ammonia (NH3) in this case.
- [HA] is the concentration of the acid, which is ammonium chloride (NH4Cl) in this case.
Given:
- pKa = 9.248
- [A-] = 0.5 M (concentration of ammonia)
- [HA] = 0.8 M (concentration of ammonium chloride)
Substitute these values into the Henderson-Hasselbalch equation:
pH = 9.248 + log(0.5/0.8)
Now, calculate the log(0.5/0.8) and add the result to 9.248 to find the pH.
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