The pH of a 0.1 M aqueous solution of a | vedclass

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Question

Given:-

$\mathrm{pH}=3$

Concentration $\longrightarrow 0.1 \mathrm{M}$

Weak acid $\longrightarrow$ HA

$\mathrm{HA} \rightleftharpoons \mat

Vedclass · Accepted Answer

$1$

Vedclass · Answer

Given:-

$\mathrm{pH}=3$

Concentration $\longrightarrow 0.1 \mathrm{M}$

Weak acid $\longrightarrow$ HA

$\mathrm{HA} ightleftharpoons \mathrm{H}^{\oplus}+\mathrm{A}^{\ominus}$

$\mathrm{C} \quad 0 \quad 0$

$\mathrm{C}(1-\alpha) \quad \mathrm{C} \alpha \quad \mathrm{C} \alpha$

$\left[\mathrm{H}^{+}ight]=\mathrm{C} \alpha$

$\Rightarrow-\log \left[\mathrm{H}^{+}ight]=3$

$\Rightarrow\left[\mathrm{H}^{+}ight]=10^{-3}$

$\Rightarrow 10^{-3}=0.1 	imes \alpha$

$\Rightarrow \alpha=10^{-2}$

$\Rightarrow \alpha=1 \%$

The $pH$ of a $0.1\ M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation ?......$\%$

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