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College Chemistry : Acid-Base Reactions

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Example Question #31 : Acid Base Reactions

$KOH(aq)\ +\ HCN(aq)\ \rightleftharpoons\ H_{2}O(l)\ +\ KCN(aq)$

KOH reacts with HCN in aqueous solution according to the chemical equation provided. If it took $29.0\ mL$ of a $0.12\ M$ KOH solution to titrate $30.0\ mL$ of an HCN solution, what was the concentration of original HCN solution?

Possible Answers:

$0.0030\ M$

$0.24\ M$

$0.12\ M$

$11.0\ M$

Correct answer:

$0.12\ M$

Explanation:

Using the concentration of KOH as a conversion factor, we can convert the volume of KOH to moles by dimensional analysis:

$\frac{0.12\ moles}{L}\times0.029\ L=0.0035\ moles\ KOH$

At the equivalence point of the titration:

$moles\ of\ KOH=moles\ of\ HCN=0.0035\ moles$

$Molarity=\frac{0.0035\ moles}{0.030\ L}=0.12\ M$

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Example Question #1 : Strong And Weak Acids/Bases

$CH_{3}COOH(aq)\ +\ H_{2}O(l)\rightleftharpoons\ H_{3}O^{+}(aq)\ +\ CH_{3}COO^{-}(aq)$

Determine the acid dissociation constant expression for the given reaction.

Possible Answers:

$K_{a}=\frac{[CH_{3}COOH]}{[H_{3}O^{+}][CH_{3}COO^{-}]}$

$K_{a}=\frac{[H_{3}O^{+}][CH_{3}COO^{-}]}{[CH_{3}COOH]}$

$K_{a}=\frac{[H_{3}O^{+}][CH_{3}COO^{-}]}{[CH_{3}COOH][H_{2}O]}$

$K_{a}=\frac{[CH_{3}COOH][H_{2}O]}{[H_{3}O^{+}][CH_{3}COO^{-}]}$

Correct answer:

$K_{a}=\frac{[H_{3}O^{+}][CH_{3}COO^{-}]}{[CH_{3}COOH]}$

Explanation:

Acid dissociation constant which is denoted as $K_{a}$ is the equilibrium constant for the ionization of an acid. Therefore, the numerator contains the product of the concentrations of the substances on the product side of the chemical equation. The denominator contains the product of the concentrations of the substances on the reactant side of the chemical equation. $H_{2}O$ is omitted in the acid dissociation constant expression because as the solvent it is in excess and therefore the change in its concentration is negligible in comparison to the other substances in solution.

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

Identify the Bronsted-Lowry acid in the following equation:

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

Possible Answers:

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

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

$\text{OH}^-$

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

Correct answer:

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

Explanation:

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

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Example Question #31 : Acid Base Reactions

Identify the Lewis Base in the following reaction:

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

Possible Answers:

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

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

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

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

Correct answer:

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

Explanation:

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

Arrhenius acid

None of these

Lewis 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 $Fe^{2+}$ ; 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 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 $OH^{-}$ , 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 LiOH . When this compound dissolves in aqueous solution, it produces $Li^{+}$ and $OH^{-}$ .

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

What is the pH of a HCl solution?

Possible Answers:

-1.10

1.10

-.9

2.10

Correct answer:

Explanation:

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

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

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

Possible Answers:

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

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

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

There are no acids in the reaction

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

Correct answer:

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

Explanation:

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

In the forward reaction, $\textrm{HClO}_{2}$ 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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College Chemistry : Acid-Base Reactions

Study concepts, example questions & explanations for College Chemistry

All College Chemistry Resources

Example Questions

Example Question #31 : Acid Base Reactions

Example Question #1 : Strong And Weak Acids/Bases

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

Example Question #31 : Acid Base Reactions

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

All College Chemistry Resources

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