Chapter 16, Problem 56A

(a)

Interpretation Introduction

Interpretation:

The given conjugate acid-base pairneeds to be identified. Also, the correct conjugate acid-base pairs should be written if the given pair is incorrect.

Concept introduction:

The concept of conjugate acid-base pair is given by Bronsted-Lowry.

According to it,

Acid is a substance which donate hydrogen ion and Base is a substance which accept hydrogen ion.

When acid donates $H^{+}$ , the species form is conjugate base and when base accepts $H^{+}$ , the species formed is conjugate acid.

Answer to Problem 56A

  $\begin{array}{l}{H}_{2}O:Acid\\ O{H}^{-}:Conjugatebase\end{array}$

Explanation of Solution

  $2H_{2}O\rightleftharpoons H_3{O}^{+}+O{H}^{-}$

So,

  $\begin{array}{l}{H}_{2}O:Acid\\ O{H}^{-}:Conjugatebase\end{array}$

(b)

Interpretation Introduction

Interpretation:

The given conjugate acid-base pair needs to be identified. Also, the correct conjugate acid-base pairs should be written if the given pair is incorrect.

Concept introduction:

The concept of conjugate acid-base pair is given by Bronsted-Lowry.

According to it,

Acid is a substance which donate hydrogen ion and Base is a substance which accept hydrogen ion.

When acid donates $H^{+}$ , the species form is conjugate base and when base accepts $H^{+}$ , the species formed is conjugate acid.

Answer to Problem 56A

The given pair is not conjugate acid-base pair.

Correct pairs are:

  $\begin{array}{l}{H}_{2}S{O}_4/HS{O}_4{}^{-}\\ HS{O}_4{}^{-}/S{O}_4{}^{2-}\end{array}$

Explanation of Solution

For $H_{2}S{O}_4$

  $H_{2}S{O}_4\rightleftharpoons H^{+}+HS{O}_4{}^{-}$

So,

  $\begin{array}{l}{H}_{2}S{O}_4:Acid\\ HS{O}_4{}^{-}:Conjugatebase\end{array}$

For $HS{O}_4{}^{-}$

  $HS{O}_4{}^{-}\rightleftharpoons H^{+}+S{O}_4{}^{2-}$

So,

  $\begin{array}{l}HS{O}_4{}^{-}:Acid\\ S{O}_4{}^{2-}:Conjugatebase\end{array}$

(c)

Interpretation Introduction

Interpretation:

The given conjugate acid-base pair needs to be identified. Also, the correct conjugate acid-base pairs should be written if the given pair is incorrect.

Concept introduction:

The concept of conjugate acid-base pair is given by Bronsted-Lowry.

According to it,

Acid is a substance which donate hydrogen ion and Base is a substance which accept hydrogen ion.

When acid donates $H^{+}$ , the species form is conjugate base and when base accepts $H^{+}$ , the species formed is conjugate acid.

Answer to Problem 56A

  $\begin{array}{l}{H}_{3}P{O}_4:Acid\\ H_{2}P{O}_4{}^{-}:Conjugatebase\end{array}$

Explanation of Solution

  $H_{3}P{O}_4\rightleftharpoons H^{+}+H_{2}P{O}_4{}^{-}$

So,

  $\begin{array}{l}{H}_{3}P{O}_4:Acid\\ H_{2}P{O}_4{}^{-}:Conjugatebase\end{array}$

(d)

Interpretation Introduction

Interpretation:

The given conjugate acid-base pair needs to be identified. Also, the correct conjugate acid-base pairs should be written if the given pair is incorrect.

Concept introduction:

The concept of conjugate acid-base pair is given by Bronsted-Lowry.

According to it,

Acid is a substance which donate hydrogen ion and Base is a substance which accept hydrogen ion.

When acid donates $H^{+}$ , the species form is conjugate base and when base accepts $H^{+}$ , the species formed is conjugate acid.

Answer to Problem 56A

  $\begin{array}{l}H{C}_2{H}_3{O}_2:Acid\\ C_2{H}_3{O}_2{}^{-}:Conjugatebase\end{array}$

Explanation of Solution

  $H{C}_2{H}_3{O}_2\rightleftharpoons H^{+}+C_2{H}_3{O}_2{}^{-}$

So,

  $\begin{array}{l}H{C}_2{H}_3{O}_2:Acid\\ C_2{H}_3{O}_2{}^{-}:Conjugatebase\end{array}$