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College Chemistry : Lewis, Brønsted-Lowry, and Arrhenius Definitions

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Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Identify the Bronsted-Lowry acid in the following equation:

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

Possible Answers:

$\text{C}_3\text{H}_7\text{O}$ $\displaystyle \text{C}_3\text{H}_7\text{O}$

$\text{OH}^-$ $\displaystyle \text{OH}^-$

$\text{H}_2\text{O}$ $\displaystyle \text{H}_2\text{O}$

$\text{C}_3\text{H}_6\text{O}^-$ $\displaystyle \text{C}_3\text{H}_6\text{O}^-$

Correct answer:

$\text{H}_2\text{O}$ $\displaystyle \text{H}_2\text{O}$

Explanation:

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

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Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Identify the Lewis Base in the following reaction:

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

Possible Answers:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-$ $\displaystyle \text{CH}_3\text{CH}_2\text{CH}_2\text{S}^-$

$\text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$ $\displaystyle \text{CH}_3\text{CH}_2\text{CH}_2\text{OH}$

$\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ $\displaystyle \text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$

$\text{CH}_3\text{CH}_2\text{CH}_2\text{SH}$ $\displaystyle \text{CH}_3\text{CH}_2\text{CH}_2\text{SH}$

Correct answer:

$\text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$ $\displaystyle \text{CH}_3\text{CH}_2\text{CH}_2\text{O}^-$

Explanation:

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

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Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

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

Possible Answers:

Bronsted-Lowry acid

Lewis acid

None of these

Arrhenius acid

Correct answer:

Arrhenius acid

Explanation:

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 $Fe^{2+}$ $\displaystyle Fe^{2+}$; 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 $OH^{-}$ $\displaystyle OH^{-}$; 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 HCl $\displaystyle HCl$, 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 $OH^{-}$ $\displaystyle OH^{-}$, 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 $HNO_{3}$ $\displaystyle HNO_{3}$. When this compound dissolves in aqueous solution, it produces $H^{+}$ $\displaystyle H^{+}$ and $NO_{3}^{-}$ $\displaystyle NO_{3}^{-}$. An Arrhenius base is a species which releases hydroxide ions into solution. An example of an Arrhenius base is LiOH $\displaystyle LiOH$. When this compound dissolves in aqueous solution, it produces $Li^{+}$ $\displaystyle Li^{+}$ and $OH^{-}$ $\displaystyle OH^{-}$.

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Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

What is the pH of a $\displaystyle 8M$ HCl $\displaystyle HCl$ solution?

Possible Answers:

-.9 $\displaystyle -.9$

$\displaystyle .9$

2.10 $\displaystyle 2.10$

-1.10 $\displaystyle -1.10$

1.10 $\displaystyle 1.10$

Correct answer:

$\displaystyle .9$

Explanation:

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

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

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

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Example Question #31 : Acid Base Reactions

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

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

Possible Answers:

$\textrm{H}_{2}\textrm{O, ClO}_{2}^{-}$ $\displaystyle \textrm{H}_{2}\textrm{O, ClO}_{2}^{-}$

There are no acids in the reaction

$\textrm{H}_{2}\textrm{O, H}_{3}\textrm{O}^{+}$ $\displaystyle \textrm{H}_{2}\textrm{O, H}_{3}\textrm{O}^{+}$

$\textrm{HClO}_{2}\textrm{, H}_{3}\textrm{O}^{+}$ $\displaystyle \textrm{HClO}_{2}\textrm{, H}_{3}\textrm{O}^{+}$

$\textrm{HClO}_{2}\textrm{, ClO}_{2}^{-}$ $\displaystyle \textrm{HClO}_{2}\textrm{, ClO}_{2}^{-}$

Correct answer:

$\textrm{HClO}_{2}\textrm{, H}_{3}\textrm{O}^{+}$ $\displaystyle \textrm{HClO}_{2}\textrm{, H}_{3}\textrm{O}^{+}$

Explanation:

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

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

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

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College Chemistry : Lewis, Brønsted-Lowry, and Arrhenius Definitions

Study concepts, example questions & explanations for College Chemistry

All College Chemistry Resources

Example Questions

Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Example Question #1 : Lewis, Brønsted Lowry, And Arrhenius Definitions

Example Question #31 : Acid Base Reactions

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