At 25,^o C, the dissociation const | vedclass

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(d) ${K_b} = \frac{{{C^2}{\alpha ^2}}}{{C(1 - \alpha )}} = C{\alpha ^2}$ assuming $\alpha < < 1$;$1 - \alpha 	ilde -1$

${10^{ - 12}} = {10^{

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$1.0 	imes {10^{ - 7}}\,mol\;{L^{ - 1}}$

Vedclass · Answer

(d) ${K_b} = \frac{{{C^2}{\alpha ^2}}}{{C(1 - \alpha )}} = C{\alpha ^2}$ assuming $\alpha < < 1$;$1 - \alpha 	ilde -1$

${10^{ - 12}} = {10^{ - 2}} 	imes {\alpha ^2}$; ${\alpha ^2} = {10^{ - 10}}$; $\alpha = {10^{ - 5}}$

$[O{H^ - }] = C\alpha = .01 	imes {10^{ - 5}} = {10^{ - 7}}$

At $25\,^o C$, the dissociation constant of a base $BOH$ is $1.0 \times {10^{ - 12}}$. The concentration of Hydroxyl ions in $0.01\, M$ aqueous solution of the base would be

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