Chapter 5.3, Problem 5.5P

(a)

Interpretation Introduction

Interpretation: Predict the given reaction whether it is a precipitation reaction or not. If it is a precipitation reaction, its balanced chemical equation should be written.

Concept introduction:

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: Predict the given reaction whether it is a precipitation reaction or not. If it is a precipitation reaction, its balanced chemical equation should be written.

Concept introduction:

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

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