The [tex]K_{a}[/tex] of phenylacetic acid is 4.76008×[tex]10^{-5}[/tex], when the pH of the solution is 2.62.
As we know,
pH = -log[[tex]H^{+}[/tex]]
[[tex]H^{+}[/tex]] = [tex]10^{-pH}[/tex]
[[tex]H^{+}[/tex]] = [tex]10^{-2.62}[/tex]
[[tex]H^{+}[/tex]] = 2.39×[tex]10^{-3}[/tex]
Also to find [tex]K_{a}[/tex] of phenylacetic acid we know another relation as:
[[tex]H^{+}[/tex]] = [tex]\sqrt{K_{a} .c}[/tex]
2.39×[tex]10^{-3}[/tex] = [tex]\sqrt{K_{a} .0.12}[/tex]
[tex]K_{a}[/tex] = 4.76008×[tex]10^{-5}[/tex]
Therefore, the [tex]K_{a}[/tex] of phenylacetic acid is 4.76008×[tex]10^{-5}[/tex], when the pH of the solution is 2.62.
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