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(A) The ionic product of water,denoted as $K_w$,is the product of the molar concentrations of hydronium ions $(H_3O^+)$ and hydroxide ions $(OH^-)$ in

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$[H_3O^+][OH^-]$

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(A) The ionic product of water,denoted as $K_w$,is the product of the molar concentrations of hydronium ions $(H_3O^+)$ and hydroxide ions $(OH^-)$ in water at a given temperature.For pure water,the dissociation reaction is $2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)$.The equilibrium constant expression is $K_c = \frac{[H_3O^+][OH^-]}{[H_2O]^2}$.Since the concentration of water is considered constant,the ionic product is defined as $K_w = [H_3O^+][OH^-]$.

Which equation represents the calculation of the ionic product for distilled water?

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