In the equilibrium HClO_4 + H_2O rightlefthar | vedclass

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(D) According to the Brønsted-Lowry theory,an acid-base pair differs by a single proton $(H^+)$. In the reaction $HClO_4 + H_2O \rightleftharpoons H_3

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$ClO_4^-$ is the conjugate base of $HClO_4$

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(D) According to the Brønsted-Lowry theory,an acid-base pair differs by a single proton $(H^+)$. In the reaction $HClO_4 + H_2O \rightleftharpoons H_3O^{+} + ClO_4^-$,$HClO_4$ acts as an acid and loses a proton to form its conjugate base,$ClO_4^-$. Similarly,$H_2O$ acts as a base and gains a proton to form its conjugate acid,$H_3O^{+}$. Therefore,$ClO_4^-$ is the conjugate base of $HClO_4$.

In the equilibrium $HClO_4 + H_2O \rightleftharpoons H_3O^{+} + ClO_4^-$,which of the following statements is correct?

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