Respuesta :
Answer : a) [tex]\frac{[A^-]}{[HA]}=10^{4}[/tex]
b) [tex]\frac{[A^-]}{[HA]}=0.01[/tex]
Explanation : Given,
a) pH = 7.4
[tex]pK_a[/tex] for aspirin = 3.4
Using Henderson Hesselbach equation :
[tex]pH=pK_a+\log \frac{[Salt]}{[Acid]}[/tex]
Concentration of salt [tex](A^-)[/tex] = ?
Concentration of acid [tex](HA)[/tex] = ?
[tex]pH=pK_a+\log \frac{[A^-]}{[HA]}[/tex]
Now put all the given values in this expression, we get:
[tex]7.4=3.4+\log \frac{[A^-]}{[HA]}[/tex]
[tex]\frac{[A^-]}{[HA]}=10^{4}[/tex]
b) pH = 1.4
Using Henderson Hesselbach equation :
[tex]pH=pK_a+\log \frac{[A^-]}{[HA]}[/tex]
Now put all the given values in this expression, we get:
[tex]1.4=3.4+\log \frac{[A^-]}{[HA]}[/tex]
[tex]\frac{[A^-]}{[HA]}=0.01[/tex]
The pKa is the acid dissociation constant. The ratio of A to HA in the blood is, 10000, and in the stomach is 0.01.
What is the acid dissociation constant?
The acid dissociation constant or pKa has been the dissociation of the compound into ions at specified pH.
The relation between pKa and pH can be given as:
[tex]\rm pH=pKa\;+\;log\;\dfrac{acid}{salt}[/tex]
The pKa of aspirin is 3.4.
- The ratio of acid (A) to salt (HA) in blood is given as:
[tex]\rm 7.4=3.4\;+\;log\;\dfrac{A}{HA} \\\dfrac{A}{HA}=10000[/tex]
- The ratio of acid (A) to salt (HA) in the stomach is given as:
[tex]\rm 7.4=1.4\;+\;log\;\dfrac{A}{HA} \\\dfrac{A}{HA}=0.01[/tex]
Learn more about acid dissociation constant, here:
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