(A) For a weak acid,the degree of dissociation $\alpha$ is given by the formula $\alpha = \sqrt{\frac{K_a}{C}}$.Given:Concentration $C = 0.1 \ mol \ L

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(A) For a weak acid,the degree of dissociation $\alpha$ is given by the formula $\alpha = \sqrt{\frac{K_a}{C}}$.Given:Concentration $C = 0.1 \ mol \ L^{-1} = 10^{-1} \ M$.Dissociation constant $K_a = 10^{-5}$.Substituting the values into the formula:$\alpha = \sqrt{\frac{10^{-5}}{10^{-1}}}$$\alpha = \sqrt{10^{-4}}$$\alpha = 10^{-2} = 0.01$.Thus,the degree of dissociation is $0.01$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)pH of weak Acids and weak Bases

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The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

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A
$0.01$
B
$0.5$
C
$0.1$
D
$1.0$

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6-2.Equilibrium-II (Ionic Equilibrium)

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pH of weak Acids and weak Bases

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The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

Similar Questions

If the degree of dissociation is $1.30\%$,what is the $K_a$ for $0.1 \ M \ CH_3COOH$?

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

Dissociation constant for a monobasic acid is $10^{-4}$. What is the $pH$ of the monobasic acid? (If $\%$ dissociation $= 2\,\%$)

If the dissociation constant of an acid $HA$ is $1 \times 10^{-5}$,the $pH$ of a $0.1 \ M$ solution of the acid will be approximately

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