Which of the following acts as an acid in an | vedclass

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(C) $1$. $HOCl$ (hypochlorous acid) acts as a Bronsted-Lowry acid in aqueous solution by donating a proton $(H^+)$ to water: $HOCl + H_2O \rightleftha

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$HOCl$ and $B(OH)_3$

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(C) $1$. $HOCl$ (hypochlorous acid) acts as a Bronsted-Lowry acid in aqueous solution by donating a proton $(H^+)$ to water: $HOCl + H_2O \rightleftharpoons H_3O^+ + OCl^-$.$2$. $B(OH)_3$ (boric acid) acts as a Lewis acid in aqueous solution by accepting a lone pair of electrons from water: $B(OH)_3 + 2H_2O \rightleftharpoons [B(OH)_4]^- + H_3O^+$.$3$. Since both compounds exhibit acidic behavior in aqueous solution,the correct option is $C$.

Which of the following acts as an acid in an aqueous solution?

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