In blood (pH=7.4), aspirin has pKa of 3.4. What is the ratio of A− to HA?
A
1:10000
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B
1000:1
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C
10000:1
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D
100:1
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Solution
The correct option is C 10000:1 Given, pKa=3.4,pH=7.4 Using Henderson-Hasselbalch equation: pH=pKa+log([conjugate base][acid] pH=pKa+log([A−][HA] 7.4=3.4+log([A−][HA]) 7.4=3.4=log([A−][HA] 4=log([A−][HA] 104=[A−][HA] [A−]:[HA]=10000:1