Lewis, Brønsted-Lowry, and Arrhenius Definitions - AP Chemistry

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Question

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Answer

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

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Question

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

Answer

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ becomes $\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$ . Since $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ accepted a proton, it must be the Lewis base.

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Question

What is the pH of a solution?

Answer

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

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Question

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

Answer

There are three main definitions for acids and bases: the Lewis acids and bases, Bronsted-Lowry acids and bases, and Arrhenius acids and bases.

A Lewis acid is a species which can accept an electron pair from a donor. An example of a Lewis acid is $Fe^{2+}$ ; as a cation, it can accept an electron pair. A Lewis base is a species which can donate an electron pair. An example of a Lewis base is $OH^{-}$ ; as an anion, it can donate an electron pair.

A Bronsted-Lowry acid is a species which can donate a proton. An example of a Bronsted-Lowry acid is , which can donate its hydrogen ion. A Bronsted-Lowry base is a species which can accept a proton from a donor. An example of a Bronsted-Lowry base is $OH^{-}$ , which can accept a hydrogen ion in order to become water.

An Arrhenius acid is a species which releases hydrogen ions into solution. An example of an Arrhenius acid is $HNO_{3}$ . When this compound dissolves in aqueous solution, it produces $H^{+}$ and $NO_{3}^{-}$ . An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is . When this compound dissolves in aqueous solution, it produces $Li^{+}$ and $OH^{-}$ .

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Question

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Answer

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

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Question

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Answer

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

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Question

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

Answer

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ becomes $\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$ . Since $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ accepted a proton, it must be the Lewis base.

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Question

What is the pH of a solution?

Answer

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

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Question

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

Answer

There are three main definitions for acids and bases: the Lewis acids and bases, Bronsted-Lowry acids and bases, and Arrhenius acids and bases.

A Lewis acid is a species which can accept an electron pair from a donor. An example of a Lewis acid is $Fe^{2+}$ ; as a cation, it can accept an electron pair. A Lewis base is a species which can donate an electron pair. An example of a Lewis base is $OH^{-}$ ; as an anion, it can donate an electron pair.

A Bronsted-Lowry acid is a species which can donate a proton. An example of a Bronsted-Lowry acid is , which can donate its hydrogen ion. A Bronsted-Lowry base is a species which can accept a proton from a donor. An example of a Bronsted-Lowry base is $OH^{-}$ , which can accept a hydrogen ion in order to become water.

An Arrhenius acid is a species which releases hydrogen ions into solution. An example of an Arrhenius acid is $HNO_{3}$ . When this compound dissolves in aqueous solution, it produces $H^{+}$ and $NO_{3}^{-}$ . An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is . When this compound dissolves in aqueous solution, it produces $Li^{+}$ and $OH^{-}$ .

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Question

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Answer

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

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Question

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Answer

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

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Question

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

Answer

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ becomes $\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$ . Since $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ accepted a proton, it must be the Lewis base.

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Question

What is the pH of a solution?

Answer

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

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Question

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

Answer

There are three main definitions for acids and bases: the Lewis acids and bases, Bronsted-Lowry acids and bases, and Arrhenius acids and bases.

A Lewis acid is a species which can accept an electron pair from a donor. An example of a Lewis acid is $Fe^{2+}$ ; as a cation, it can accept an electron pair. A Lewis base is a species which can donate an electron pair. An example of a Lewis base is $OH^{-}$ ; as an anion, it can donate an electron pair.

A Bronsted-Lowry acid is a species which can donate a proton. An example of a Bronsted-Lowry acid is , which can donate its hydrogen ion. A Bronsted-Lowry base is a species which can accept a proton from a donor. An example of a Bronsted-Lowry base is $OH^{-}$ , which can accept a hydrogen ion in order to become water.

An Arrhenius acid is a species which releases hydrogen ions into solution. An example of an Arrhenius acid is $HNO_{3}$ . When this compound dissolves in aqueous solution, it produces $H^{+}$ and $NO_{3}^{-}$ . An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is . When this compound dissolves in aqueous solution, it produces $Li^{+}$ and $OH^{-}$ .

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Question

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Answer

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

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Question

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Answer

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

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Question

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

Answer

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ becomes $\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$ . Since $\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ accepted a proton, it must be the Lewis base.

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Question

What is the pH of a solution?

Answer

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

Compare your answer with the correct one above

Question

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

Answer

There are three main definitions for acids and bases: the Lewis acids and bases, Bronsted-Lowry acids and bases, and Arrhenius acids and bases.

A Lewis acid is a species which can accept an electron pair from a donor. An example of a Lewis acid is $Fe^{2+}$ ; as a cation, it can accept an electron pair. A Lewis base is a species which can donate an electron pair. An example of a Lewis base is $OH^{-}$ ; as an anion, it can donate an electron pair.

A Bronsted-Lowry acid is a species which can donate a proton. An example of a Bronsted-Lowry acid is , which can donate its hydrogen ion. A Bronsted-Lowry base is a species which can accept a proton from a donor. An example of a Bronsted-Lowry base is $OH^{-}$ , which can accept a hydrogen ion in order to become water.

An Arrhenius acid is a species which releases hydrogen ions into solution. An example of an Arrhenius acid is $HNO_{3}$ . When this compound dissolves in aqueous solution, it produces $H^{+}$ and $NO_{3}^{-}$ . An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is . When this compound dissolves in aqueous solution, it produces $Li^{+}$ and $OH^{-}$ .

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Question

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Answer

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

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Lewis, Brønsted-Lowry, and Arrhenius Definitions - AP Chemistry

Identify the Bronsted-Lowry acid in the following equation:

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that becomes , which it lost an , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that becomes . Since accepted a proton, it must be the Lewis base.

What is the pH of a solution?

PH is defined as , where is hydronium concentration). In order to do this we simply take : =

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor. In the forward reaction, is a proton donor. In the backward reaction, is the proton donor. The acids in this reaction are and .

Identify the Bronsted-Lowry acid in the following equation:

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that becomes , which it lost an , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that becomes . Since accepted a proton, it must be the Lewis base.

What is the pH of a solution?

PH is defined as , where is hydronium concentration). In order to do this we simply take : =

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor. In the forward reaction, is a proton donor. In the backward reaction, is the proton donor. The acids in this reaction are and .

Identify the Bronsted-Lowry acid in the following equation:

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that becomes , which it lost an , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that becomes . Since accepted a proton, it must be the Lewis base.

What is the pH of a solution?

PH is defined as , where is hydronium concentration). In order to do this we simply take : =

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor. In the forward reaction, is a proton donor. In the backward reaction, is the proton donor. The acids in this reaction are and .

Identify the Bronsted-Lowry acid in the following equation:

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that becomes , which it lost an , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

Recall that a Lewis base accepts a proton, while a Lewis acid donates a proton. Looking at the equation, we can see that becomes . Since accepted a proton, it must be the Lewis base.

What is the pH of a solution?

PH is defined as , where is hydronium concentration). In order to do this we simply take : =

Which type of acid is defined by its ability to produce hydrogen ions in aqueous solution?

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor. In the forward reaction, is a proton donor. In the backward reaction, is the proton donor. The acids in this reaction are and .

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .

Identify the Bronsted-Lowry acid in the following equation:

$\text{H}_2\text{O}+\text{C}_3\text{H}_6\text{O}^-\rightarrow\text{OH}^-+\text{C}_3\text{H}_7\text{O}$

Recall that a Bronsted-Lowry acid donates a proton. From the equation, we can see that $\text{H}_2\text{O}$ becomes $\text{OH}^-$ , which it lost an $\text{H}^+$ , or a proton. Thus, water must be the Bronsted-Lowry acid.

Identify the Lewis Base in the following reaction:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-(aq)\rightleftharpoons \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-(aq)+\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}(aq)$

PH is defined as $-log_{10}${H+}$ , where is hydronium concentration). In order to do this we simply take $-log_{10}${8M}$ :

$pH=-log_{10}${concentration of H+}$

= $pH=-log_{10}${8M}=.9$

$\textrm{HClO}_{2}(aq)\textrm{ + H}_{2}\textrm{O}(l)\rightleftharpoons\textrm{ClO}_{2}\textrm{ }^{-}(aq)\textrm{ + H}_{3}\textrm{O}^{+}(aq)$

According to the Brønsted-Lowry definition of acids and bases, which species in the reaction are acids?

Remember a Brønsted-Lowry acid is defined as a proton donor.

In the forward reaction, $\textrm{HClO}_{2}$ is a proton donor. In the backward reaction, $\textup{H}_3\textup{O}^+$ is the proton donor.

The acids in this reaction are $\textrm{HClO}_{2}$ and $\textup{H}_3\textup{O}^+$ .