Chapter 10, Problem 10.33UKC

(a)

Interpretation Introduction

Interpretation:

The given reaction ${\text{HF+OH}}^{\text{-}}\to {\text{H}}_{\text{2}}{\text{O+F}}^{\text{-}}$ should be matched with the given boxes.

Concept Introduction:

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$

Reaction between Acid and Base: When an acid reacts with the base $H^{+}$ from acid and ${\text{OH}}^{\text{-}}$ from base are neutralized that result in formation of salt and water.

Answer to Problem 10.33UKC

The box 2 matches with the given reaction.

Explanation of Solution

Analyzing the given boxes shows that there are 9${\text{OH}}^{\text{-}}$ and ${\text{3H}}^{\text{+}}$. The second box explains that in order to get that situation with 9 unreacted ${\text{OH}}^{\text{-}}$ ions the acid with should contain one proton with it. Hence it matches with the given reaction since the given reaction ${\text{HF+OH}}^{\text{-}}\to {\text{H}}_{\text{2}}{\text{O+F}}^{\text{-}}$ contains one proton for donation.

(b)

Interpretation Introduction

Interpretation:

The given reaction $H_{2}S{O}_3+2O{H}^{-}\to 2H_{2}O+S{O}_3^{2-}$ should be matched with the given boxes.

Concept Introduction:

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$

Reaction between Acid and Base: When an acid reacts with the base $H^{+}$ from acid and ${\text{OH}}^{\text{-}}$ from base are neutralized that result in formation of salt and water.

Answer to Problem 10.33UKC

The box 3 matches with the given reaction.

Explanation of Solution

Analyzing the given boxes shows that there are 9${\text{OH}}^{\text{-}}$ and ${\text{3H}}^{\text{+}}$. The third box explains that in order to get that situation with 6 unreacted ${\text{OH}}^{\text{-}}$ ions the acid with should contain two protons with it. Hence it matches with the given reaction since the given reaction contains two proton for donation as two water molecules are formed.

(c)

Interpretation Introduction

Interpretation:

The given $H_{3}P{O}_4+3O{H}^{-}\to 3H_{2}O+P{O}_4^{3-}$ reaction should be matched with the given boxes.

Concept Introduction:

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$

Reaction between Acid and Base: When an acid reacts with the base $H^{+}$ from acid and ${\text{OH}}^{\text{-}}$ from base are neutralized that result in formation of salt and water.

Answer to Problem 10.33UKC

The box 1 matches with the given reaction.

Explanation of Solution

Analyzing the given boxes shows that there are 9${\text{OH}}^{\text{-}}$ and ${\text{3H}}^{\text{+}}$. The first box explains that in order to get that situation with 3 unreacted ${\text{OH}}^{\text{-}}$ ions the acid should contain three protons with it. Hence it matches with the given reaction since the given reaction contains 3 protons for donation as three water molecules are formed.