QuestionMay 19, 2025

Identify the Bronsted acid(s)in the reaction. HIO_(3)(aq)+H_(2)O(l)leftharpoons H_(3)O^+(aq)+IO_(3)^-(aq) HIO_(3) HIO_(3) and H_(3)O^+ H_(2)O H_(2)O and HIO_(3)

Identify the Bronsted acid(s)in the reaction. HIO_(3)(aq)+H_(2)O(l)leftharpoons H_(3)O^+(aq)+IO_(3)^-(aq) HIO_(3) HIO_(3) and H_(3)O^+ H_(2)O H_(2)O and HIO_(3)
Identify the Bronsted acid(s)in the reaction. HIO_(3)(aq)+H_(2)O(l)leftharpoons H_(3)O^+(aq)+IO_(3)^-(aq) HIO_(3) HIO_(3) and H_(3)O^+ H_(2)O H_(2)O and HIO_(3)

Solution
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Answer

HIO_{3} and H_{3}O^{+} Explanation 1. Identify Bronsted Acids A Bronsted acid is a species that donates a proton (H⁺) in a chemical reaction. In the given equilibrium reaction, HIO_{3} donates a proton to water (H_{2}O), forming H_{3}O^{+} and IO_{3}^{-}. Therefore, HIO_{3} acts as a Bronsted acid. Additionally, H_{3}O^{+} can also donate a proton back to IO_{3}^{-}, making it a Bronsted acid as well. 2. Determine Correct Options Based on the identification of Bronsted acids, both HIO_{3} and H_{3}O^{+} are Bronsted acids in this reaction.

Explanation

1. Identify Bronsted Acids<br /> A Bronsted acid is a species that donates a proton (H⁺) in a chemical reaction. In the given equilibrium reaction, $HIO_{3}$ donates a proton to water ($H_{2}O$), forming $H_{3}O^{+}$ and $IO_{3}^{-}$. Therefore, $HIO_{3}$ acts as a Bronsted acid. Additionally, $H_{3}O^{+}$ can also donate a proton back to $IO_{3}^{-}$, making it a Bronsted acid as well.<br /><br />2. Determine Correct Options<br /> Based on the identification of Bronsted acids, both $HIO_{3}$ and $H_{3}O^{+}$ are Bronsted acids in this reaction.
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