Chemistry - Ionic Equilibrium Question with Solution | TestHub

$$\begin{array}{c}\mathrm{C}=0.01\mathrm{M}\\ {\mathrm{K}}_b=1\times 10^{-12}\text{ at }25^{\circ }\mathrm{C}\\ \mathrm{BOH}\rightleftharpoons {\mathrm{B}}^{+}+{\mathrm{OH}}^{-}\\ \mathrm{C}00\end{array}$$ at eq. $\mathrm{C}-\mathrm{C}\alpha \mathrm{C}\alpha \mathrm{C}\alpha$ $$\begin{array}{rl}\left[{\mathrm{OH}}^{-}\right]& =\mathrm{C}\alpha \\ \left[{\mathrm{OH}}^{-}\right]& =\sqrt{{\mathrm{K}}_b\mathrm{C}}=\sqrt{1\times 10^{-12}\times 10^{-2}}\end{array}$$ $$\left[{\mathrm{OH}}^{-}\right]=10^{-7}\mathrm{mol}{\mathrm{L}}^{-1}$$ Related Theory The activities of the solutes are approximated with molarities. The dissociation constant is an immediate consequence of the law of mass action which describes equilibria in a more general way. The dissociation constant is also sometimes called ionization constant when applied to salts.