Chapter 5, Problem 5.38AP

(a)

Interpretation Introduction

Interpretation:

The given reaction should be identified as whether precipitation, neutralization, or redox reaction.

Concept introduction:

Reactions of ionic compounds can be grouped into three and they are,

1. 1. Precipitation reaction: A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.
2. 2. Acid- base neutralization reaction: it is a double displacement reaction in which an acid and a base react to form an ionic compound (salt) and water.
3. 3. Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.

A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.

The term solubility reveals the amount of a given substance that can be dissolved in a certain amount of solvent.

• If a compound contains ammonium ion $N{H}_4^{+}$ and group IA cations such as $L{i}^{+},N{a}^{+},K^{+},R{b}^{+}andC{s}^{+}$ as cation then it is probably soluble.
• A compound is probably soluble if it contains one of the following anions:

  Halide: $C{l}^{-},B{r}^{-}and{I}^{-}exceptA{g}^{+},H{g}_2^{2+},andP{b}^{2+}compounds$

  Nitrate ($N{O}_3^{-}$), perchlorate $\left(Cl{O}_4^{-}\right)$, acetate $\left(C{H}_{3}CO{O}^{-}\right)$, and sulfate $\left(S{O}_4^{2-}\right)$ , except $B{a}^{2+},H{g}_2^{2+},andP{b}^{2+}sulfates$

• General solubility guidelines for ionic compounds in water

  $\begin{array}{cc}\text{Soluble}& \text{Exceptions}\\ \text{Ammonium}\text{compounds}\left({\text{NH}}_{\text{4}}^{\text{+}}\right)& \text{None}\\ \text{Lithium}\text{compounds}\left({\text{Li}}^{\text{+}}\right)& \text{None}\\ \text{Sodium}\text{compounds}\left({\text{Na}}^{\text{+}}\right)& \text{None}\\ \text{Potassium}\text{compounds}\left({\text{K}}^{\text{+}}\right)& \text{None}\\ \text{Nitrates}\left({\text{NO}}_{\text{3}}^{\text{-}}\right)& \text{None}\\ \text{Perchlorates}\left({\text{ClO}}_{\text{4}}^{\text{-}}\right)& \text{None}\\ \text{Acetates}\left({\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}\right)& \text{None}\\ \text{Chlorides}\left({\text{Cl}}^{\text{-}}\right)& \\ \text{Bromides}\left({\text{Br}}^{\text{-}}\right)& {\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\\ \text{Iodides}\left({\text{I}}^{\text{-}}\right)& \\ \text{Sulfates}\left({\text{SO}}_{\text{4}}^{\text{2-}}\right)& {\text{Ba}}^{\text{2+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The given reaction should be identified as whether precipitation, neutralization, or redox reaction.

Concept introduction:

In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.

Coefficient is a number placed before a formula in a chemical equation.

A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.

Reactions of ionic compounds can be grouped into three and they are

1. 1. Precipitation reaction: A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.
2. 2. Acid- base neutralization reaction: it is a double displacement reaction in which an acid and a base react to form an ionic compound (salt) and water.
3. 3. Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Oxidation: Losing electrons, increasing oxidation number.

Reduction: Gaining electron, decreasing oxidation number.

(c)

Interpretation Introduction

Interpretation:

The given reaction should be identified as whether precipitation, neutralization, or redox reaction.

Concept introduction:

In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.

Coefficient is a number placed before a formula in a chemical equation.

A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.

Reactions of ionic compounds can be grouped into three and they are,

1. 1. Precipitation reaction: A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.
2. 2. Acid- base neutralization reaction: it is a double displacement reaction in which an acid and a base react to form an ionic compound (salt) and water.
3. 3. Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.

The number of electrons an atom tends to give up or gain in a chemical reaction is called oxidation number.

Oxidation: Losing electrons, increasing oxidation number.

Reduction: Gaining electron, decreasing oxidation number.

(d)

Interpretation Introduction

Interpretation:

The given reaction should be identified as whether precipitation, neutralization, or redox reaction.

Concept introduction:

In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.

Coefficient is a number placed before a formula in a chemical equation.

A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.

Reactions of ionic compounds can be grouped into three and they are,

1. 1. Precipitation reaction: A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.
2. 2. Acid- base neutralization reaction: it is a double displacement reaction in which an acid and a base react to form an ionic compound (salt) and water.
3. 3. Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.

A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.

The term solubility reveals the amount of a given substance that can be dissolved in a certain amount of solvent.

• If a compound contains ammonium ion $N{H}_4^{+}$ and group IA cations such as $L{i}^{+},N{a}^{+},K^{+},R{b}^{+}andC{s}^{+}$ as cation then it is probably soluble.
• A compound is probably soluble if it contains one of the following anions:

  Halide: $C{l}^{-},B{r}^{-}and{I}^{-}exceptA{g}^{+},H{g}_2^{2+},andP{b}^{2+}compounds$

  Nitrate ($N{O}_3^{-}$), perchlorate $\left(Cl{O}_4^{-}\right)$, acetate $\left(C{H}_{3}CO{O}^{-}\right)$, and sulfate $\left(S{O}_4^{2-}\right)$ , except $B{a}^{2+},H{g}_2^{2+},andP{b}^{2+}sulfates$

• General solubility guidelines for ionic compounds in water

  $\begin{array}{cc}\text{Soluble}& \text{Exceptions}\\ \text{Ammonium}\text{compounds}\left({\text{NH}}_{\text{4}}^{\text{+}}\right)& \text{None}\\ \text{Lithium}\text{compounds}\left({\text{Li}}^{\text{+}}\right)& \text{None}\\ \text{Sodium}\text{compounds}\left({\text{Na}}^{\text{+}}\right)& \text{None}\\ \text{Potassium}\text{compounds}\left({\text{K}}^{\text{+}}\right)& \text{None}\\ \text{Nitrates}\left({\text{NO}}_{\text{3}}^{\text{-}}\right)& \text{None}\\ \text{Perchlorates}\left({\text{ClO}}_{\text{4}}^{\text{-}}\right)& \text{None}\\ \text{Acetates}\left({\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}\right)& \text{None}\\ \text{Chlorides}\left({\text{Cl}}^{\text{-}}\right)& \\ \text{Bromides}\left({\text{Br}}^{\text{-}}\right)& {\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\\ \text{Iodides}\left({\text{I}}^{\text{-}}\right)& \\ \text{Sulfates}\left({\text{SO}}_{\text{4}}^{\text{2-}}\right)& {\text{Ba}}^{\text{2+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\end{array}$

(e)

Interpretation Introduction

Interpretation:

The given reaction should be identified as whether precipitation, neutralization, or redox reaction.

Concept introduction:

In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.

Coefficient is a number placed before a formula in a chemical equation.

A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.

Reactions of ionic compounds can be grouped into three and they are,

1. 1. Precipitation reaction: A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.
2. 2. Acid- base neutralization reaction: it is a double displacement reaction in which an acid and a base react to form an ionic compound (salt) and water.
3. 3. Oxidation-reduction reaction: Both the oxidation and reduction reaction occurs together in a chemical reaction. It is also known as redox reaction.

A precipitation reaction takes place when two solutions of well soluble substances together form a poorly soluble salt.

The term solubility reveals the amount of a given substance that can be dissolved in a certain amount of solvent.

• If a compound contains ammonium ion $N{H}_4^{+}$ and group IA cations such as $L{i}^{+},N{a}^{+},K^{+},R{b}^{+}andC{s}^{+}$ as cation then it is probably soluble.
• A compound is probably soluble if it contains one of the following anions:

  Halide: $C{l}^{-},B{r}^{-}and{I}^{-}exceptA{g}^{+},H{g}_2^{2+},andP{b}^{2+}compounds$

  Nitrate ($N{O}_3^{-}$), perchlorate $\left(Cl{O}_4^{-}\right)$, acetate $\left(C{H}_{3}CO{O}^{-}\right)$, and sulfate $\left(S{O}_4^{2-}\right)$ , except $B{a}^{2+},H{g}_2^{2+},andP{b}^{2+}sulfates$

• General solubility guidelines for ionic compounds in water

  $\begin{array}{cc}\text{Soluble}& \text{Exceptions}\\ \text{Ammonium}\text{compounds}\left({\text{NH}}_{\text{4}}^{\text{+}}\right)& \text{None}\\ \text{Lithium}\text{compounds}\left({\text{Li}}^{\text{+}}\right)& \text{None}\\ \text{Sodium}\text{compounds}\left({\text{Na}}^{\text{+}}\right)& \text{None}\\ \text{Potassium}\text{compounds}\left({\text{K}}^{\text{+}}\right)& \text{None}\\ \text{Nitrates}\left({\text{NO}}_{\text{3}}^{\text{-}}\right)& \text{None}\\ \text{Perchlorates}\left({\text{ClO}}_{\text{4}}^{\text{-}}\right)& \text{None}\\ \text{Acetates}\left({\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}\right)& \text{None}\\ \text{Chlorides}\left({\text{Cl}}^{\text{-}}\right)& \\ \text{Bromides}\left({\text{Br}}^{\text{-}}\right)& {\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\\ \text{Iodides}\left({\text{I}}^{\text{-}}\right)& \\ \text{Sulfates}\left({\text{SO}}_{\text{4}}^{\text{2-}}\right)& {\text{Ba}}^{\text{2+}}\text{,}{\text{Hg}}_{\text{2}}^{\text{2+}}\text{,}\text{and}{\text{Pb}}^{\text{2+}}\text{compounds}\end{array}$