It has been found that the pH of a 0.01 M sol | vedclass

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Question

Let the organic acid be $HA$.

$\Rightarrow HA \longleftrightarrow H ^{+}+ A$

Concentration of $HA =0.01 \,M \,pH$

$=4.15$

$-\log \left[ H

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Vedclass · Answer

Let the organic acid be $HA$.

$\Rightarrow HA \longleftrightarrow H ^{+}+ A$

Concentration of $HA =0.01 \,M \,pH$

$=4.15$

$-\log \left[ H ^{+}ight]=4.15$

$\left[ H ^{+}ight]=7.08 	imes 10^{-5}$

Now, $K_{a}=\frac{\left[ H ^{+}ight]\left[ A ^{-}ight]}{[ HA ]}$

$\left[ H ^{+}ight]=\left[ A ^{-}ight]=7.08 	imes 10^{-5}$

$[ HA ]=0.01$

Then,  $K_{a}=\frac{\left(7.08 	imes 10^{-5}ight)\left(7.08 	imes 10^{-5}ight)}{0.01}$

$K_{a}=5.01 	imes 10^{-7}$

$p K_{a}=-\log K_{a}$

$=-\log \left(5.01 	imes 10^{-7}ight)$

$p K_{a}=6.3001$

It has been found that the $pH$ of a $0.01$ $M$ solution of an organic acid is $4.15 .$ Calculate the concentration of the anion, the ionization constant of the acid and its $p{K_a}$

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