Chapter 9, Problem 9.94P

Interpretation Introduction

(a)

Interpretation:

Thebalanced chemical equation of acid-base reaction between the aqueous solution of ${\text{HNO}}_{\text{3}}$ and $\text{LiOH}$ needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance. It purposed the concept of conjugated acid-base pair. A Bronsted acid gives ${\text{H}}^{\text{+}}$ ion to form conjugated base whereas a Bronsted base accepts ${\text{H}}^{\text{+}}$ ion to form its conjugated acid.

  $\begin{array}{l}{\text{ HA + H}}_{\text{2}}\text{O }\underset{}{\to }{\text{ A}}^{\text{-}}{\text{ + H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Bronsted + Bronsted Conjugated Conjugated}\\ \text{ Acid base base acid}\end{array}$

Overall the reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction.

Answer to Problem 9.94P

  $\begin{array}{l}{\text{ HNO}}_{\text{3}}{}_{\text{(aq) }}{\text{+ LiOH}}_{\text{(aq)}}\underset{}{\to }{\text{ LiNO}}_{\text{3}}{}_{\text{(aq) }}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}\\ \text{ Acid + Base Salt + Water }\end{array}$

Explanation of Solution

Nitric acid ${\text{HNO}}_{\text{3}}$ is soluble in water. Here ${\text{HNO}}_{\text{3}}$ acts as an acid as it gives ${\text{H}}^{\text{+}}$ ion and forms ${\text{NO}}_{\text{3}}{}^{-}$ ion. Lithium hydroxide $\text{LiOH}$ is also soluble in water and acts as a base as it gives ${\text{OH}}^{\text{-}}$ ion and forms ${\text{Li}}^{\text{+ }}$ ion. The ${\text{H}}^{\text{+}}$ ion from ${\text{HNO}}_{\text{3}}$ must be accepted by ${\text{OH}}^{\text{-}}$ ion from $\text{LiOH}$ which results in the formation of ${\text{H}}_{\text{2}}\text{O}$ . Hence in the given reaction ${\text{HNO}}_{\text{3}}$ is an acid and $\text{LiOH}$ is a base. The reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction. The complete balance acid-base equation of ${\text{HNO}}_{\text{3}}$ with $\text{LiOH}$ must be written as:

  $\begin{array}{l}{\text{ HNO}}_{\text{3}}{}_{\text{(aq) }}{\text{+ LiOH}}_{\text{(aq)}}\underset{}{\to }{\text{ LiNO}}_{\text{3}}{}_{\text{(aq) }}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}\\ \text{ Acid + Base Salt + Water }\end{array}$

Interpretation Introduction

(b)

Interpretation:

The balanced chemical equation ofacid-base reaction between the aqueous solution of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ and $\text{NaOH}$ needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance. It purposed the concept of conjugated acid-base pair. A Bronsted acid gives ${\text{H}}^{\text{+}}$ ion to form conjugated base whereas a Bronsted base accepts ${\text{H}}^{\text{+}}$ ion to form its conjugated acid.

  $\begin{array}{l}{\text{ HA + H}}_{\text{2}}\text{O }\underset{}{\to }{\text{ A}}^{\text{-}}{\text{ + H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Bronsted + Bronsted Conjugated Conjugated}\\ \text{ Acid base base acid}\end{array}$

Overall the reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction.

Answer to Problem 9.94P

  $\begin{array}{l}{\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\text{(aq) }}{\text{+ 2 NaOH}}_{\text{(aq)}}\underset{}{\to }{\text{ Na}}_{\text{2}}{\text{SO}}_4{}_{\text{(aq) }}{\text{+ 2 H}}_{\text{2}}{\text{O}}_{\text{(l)}}\\ \text{ Acid + Base Salt Water }\end{array}$

Explanation of Solution

Sulfuric acid ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ is soluble in water. Here ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ acts as an acid as it gives ${\text{H}}^{\text{+}}$ ion and forms ${\text{SO}}_{\text{4}}{}^{2-}$ ion. Calcium hydroxide $\text{NaOH}$ is also soluble in water and acts as a base as it gives ${\text{OH}}^{\text{-}}$ ion and forms ${\text{Na}}^{\text{+ }}$ ion. The ${\text{H}}^{\text{+}}$ ion from ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ must be accepted by ${\text{OH}}^{\text{-}}$ ion from $\text{NaOH}$ which results in the formation of ${\text{H}}_{\text{2}}\text{O}$ . Hence in the given reaction ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ is an acid and $\text{NaOH}$ is a base. The reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction. The complete balance acid-base equation of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ with $\text{NaOH}$ must be written as:

  $\begin{array}{l}{\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\text{(aq) }}{\text{+ 2 NaOH}}_{\text{(aq)}}\underset{}{\to }{\text{ Na}}_{\text{2}}{\text{SO}}_4{}_{\text{(aq) }}{\text{+ 2 H}}_{\text{2}}{\text{O}}_{\text{(l)}}\\ \text{ Acid + Base Salt Water }\end{array}$

Interpretation Introduction

(c)

Interpretation:

The balanced chemical equation ofacid-base reaction between the aqueous solution of $\text{HCl}$ and ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance. It purposed the concept of conjugated acid-base pair. A Bronsted acid gives ${\text{H}}^{\text{+}}$ ion to form conjugated base whereas a Bronsted base accepts ${\text{H}}^{\text{+}}$ ion to form its conjugated acid.

  $\begin{array}{l}{\text{ HA + H}}_{\text{2}}\text{O }\underset{}{\to }{\text{ A}}^{\text{-}}{\text{ + H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Bronsted + Bronsted Conjugated Conjugated}\\ \text{ Acid base base acid}\end{array}$

Overall the reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction.

Answer to Problem 9.94P

  $\begin{array}{l}{\text{2 HCl}}_{\text{(aq) }}{\text{+ K}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}\underset{}{\to }{\text{ 2 KCl}}_{\text{(aq) }}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ + CO}}_{\text{2(g)}}\\ \text{ Acid + Base Salt Water Carbon dioxide}\end{array}$

Explanation of Solution

Hydrochloric acid $\text{HCl}$ is soluble in water. Here $\text{HCl}$ acts as an acid as it gives ${\text{H}}^{\text{+}}$ ion and forms ${\text{I}}^{-}$ ion. Potassium carbonate ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ is also soluble in water and acts as a base. The ${\text{H}}^{\text{+}}$ ion from $\text{HCl}$ must be accepted by ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ which results in the formation of ${\text{H}}_{\text{2}}\text{O}$ . Hence in the given reaction $\text{HI}$ is an acid and ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ is a base. The reaction of $\text{HCl}$ with ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ forms $\text{KCl}$ as salt and ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}$ . Since ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}$ is unstable so it readily decomposes to ${\text{H}}_{\text{2}}\text{O}$ and ${\text{CO}}_{\text{2(g)}}$ . Thus the complete balance acid-base equation of $\text{HCl}$ with ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ must be written as:

  $\begin{array}{l}{\text{2 HCl}}_{\text{(aq) }}{\text{+ K}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}\underset{}{\to }{\text{ 2 KCl}}_{\text{(aq) }}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ + CO}}_{\text{2(g)}}\\ \text{ Acid + Base Salt Water Carbon dioxide}\end{array}$

Interpretation Introduction

(d)

Interpretation:

The balanced chemical equation of acid-base reaction between the aqueous solution of $\text{HI}$ and ${\text{NaHCO}}_{\text{3}}$ needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance. It purposed the concept of conjugated acid-base pair. A Bronsted acid gives ${\text{H}}^{\text{+}}$ ion to form conjugated base whereas a Bronsted base accepts ${\text{H}}^{\text{+}}$ ion to form its conjugated acid.

  $\begin{array}{l}{\text{ HA + H}}_{\text{2}}\text{O }\underset{}{\to }{\text{ A}}^{\text{-}}{\text{ + H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Bronsted + Bronsted Conjugated Conjugated}\\ \text{ Acid base base acid}\end{array}$

Overall the reaction of acid and base forms salt and water as the product. This reaction is called a neutralization reaction.

Answer to Problem 9.94P

  $\begin{array}{l}{\text{HI}}_{\text{(aq) }}{\text{+ NaHCO}}_{\text{3}}{}_{\text{(aq)}}\underset{}{\to }{\text{ NaI}}_{\text{(aq) }}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ + CO}}_{\text{2(g)}}\\ \text{Acid + Base Salt Water Carbon dioxide}\end{array}$

Explanation of Solution

Hydroiodic acid $\text{HI}$ is soluble in water. Here $\text{HI}$ acts as an acid as it gives ${\text{H}}^{\text{+}}$ ion and forms ${\text{I}}^{-}$ ion. Sodium hydrogen carbonate ${\text{NaHCO}}_{\text{3}}$ is also soluble in water and acts as a base. The ${\text{H}}^{\text{+}}$ ion from $\text{HI}$ must be accepted by ${\text{NaHCO}}_{\text{3}}$ which results in the formation of ${\text{H}}_{\text{2}}\text{O}$ . Hence in the given reaction $\text{HI}$ is an acid and ${\text{NaHCO}}_{\text{3}}$ is a base. The reaction of $\text{HI}$ with ${\text{NaHCO}}_{\text{3}}$ forms $\text{ NaI}$ as salt and ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}$ . Since ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}$ is unstable so it readily decomposes to ${\text{H}}_{\text{2}}\text{O}$ and ${\text{CO}}_{\text{2(g)}}$ . Thus the complete balance acid-base equation of $\text{HI}$ with ${\text{NaHCO}}_{\text{3}}$ must be written as:

  $\begin{array}{l}{\text{HI}}_{\text{(aq) }}{\text{+ NaHCO}}_{\text{3}}{}_{\text{(aq)}}\underset{}{\to }{\text{ NaI}}_{\text{(aq) }}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ + CO}}_{\text{2(g)}}\\ \text{Acid + Base Salt Water Carbon dioxide}\end{array}$