(B) For a weak base $BOH$,the dissociation is $BOH \rightleftharpoons B^{+} + OH^{-}$.The dissociation constant $K_b = \frac{[B^{+}][OH^{-}]}{[BOH]} =

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(B) For a weak base $BOH$,the dissociation is $BOH \rightleftharpoons B^{+} + OH^{-}$.The dissociation constant $K_b = \frac{[B^{+}][OH^{-}]}{[BOH]} = \frac{c \alpha^2}{1-\alpha} \approx c \alpha^2$.Given $K_b = 1.0 \times 10^{-12}$ and $c = 0.01 \ M = 10^{-2} \ M$.$1.0 \times 10^{-12} = 10^{-2} \times \alpha^2 \implies \alpha^2 = 10^{-10} \implies \alpha = 10^{-5}$.$[OH^{-}] = c \alpha = 10^{-2} \times 10^{-5} = 1.0 \times 10^{-7} \ M$.

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

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The dissociation constant of a base $BOH$ at $25^{\circ} C$ is $1.0 \times 10^{-12}$. The concentration of $OH^{-}$ in a $0.01 \ M$ aqueous solution is .......

A
$1.0 \times 10^{-5} \ M$
B
$1.0 \times 10^{-7} \ M$
C
$2.0 \times 10^{-6} \ M$
D
$1.0 \times 10^{-14} \ M$

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6-2.Equilibrium-II (Ionic Equilibrium)

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pH of weak Acids and weak Bases

At $25 \, ^\circ C$,the equilibrium constant for a base $BOH$ is $1.0 \times 10^{-12}$. What will be the concentration of hydroxide ions in a $0.01 \, M$ aqueous solution of the base?

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The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........

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The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

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Dimethyl amine $(CH_3)_2NH$ is a weak base and its ionization constant is $5.4 \times 10^{-5}$. Calculate $[OH^{-}]$,$[H_3O^{+}]$,$pOH$ and $pH$ of its $0.2 \ M$ solution at equilibrium.

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Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues,leads to pain and a feeling of fatigue. In a $0.10 \ M$ aqueous solution,lactic acid is $3.7 \%$ dissociated. The value of the dissociation constant,$K_a,$ for this acid will be:

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The dissociation constant of a base $BOH$ at $25^{\circ} C$ is $1.0 \times 10^{-12}$. The concentration of $OH^{-}$ in a $0.01 \ M$ aqueous solution is .......

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At $25 \, ^\circ C$,the equilibrium constant for a base $BOH$ is $1.0 \times 10^{-12}$. What will be the concentration of hydroxide ions in a $0.01 \, M$ aqueous solution of the base?

The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........

The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

Dimethyl amine $(CH_3)_2NH$ is a weak base and its ionization constant is $5.4 \times 10^{-5}$. Calculate $[OH^{-}]$,$[H_3O^{+}]$,$pOH$ and $pH$ of its $0.2 \ M$ solution at equilibrium.

Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues,leads to pain and a feeling of fatigue. In a $0.10 \ M$ aqueous solution,lactic acid is $3.7 \%$ dissociated. The value of the dissociation constant,$K_a,$ for this acid will be:

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