The pOH at which water is maximum dissociated | vedclass

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(B) At $25\,^{\circ}C$,the dissociation of water is represented as: $H_2O \rightleftharpoons H^{+} + OH^{-}$According to the common ion effect,the pre

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$7$

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(B) At $25\,^{\circ}C$,the dissociation of water is represented as: $H_2O \rightleftharpoons H^{+} + OH^{-}$According to the common ion effect,the presence of either $H^{+}$ or $OH^{-}$ ions suppresses the dissociation of water.At $pOH = 7$,the concentration of $OH^{-}$ is $10^{-7} \, M$ and $[H^{+}]$ is $10^{-7} \, M$. This represents the neutral point where the concentration of both ions is minimal and equal,allowing for the standard equilibrium dissociation.If $pOH = 14$,the solution is highly basic,$[OH^{-}]$ is very high,and the reaction shifts backward.If $pOH = 0$,the solution is highly acidic,$[H^{+}]$ is very high,and the reaction shifts backward.Therefore,the dissociation of water is maximum at $pOH = 7$.

The $pOH$ at which water is maximum dissociated at $25\,^{\circ}C$ is

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