Chapter 7.2, Problem 7.1SC

Interpretation Introduction

(a)

Interpretation:

If pairs of solutions are mixed, whether a solid is formed or not should be identified with balanced chemical equation.

Concept Introduction:

A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.

There are following solubility rules:

1. The salts formed from sodium, potassium and ammonium ions are soluble in nature.

All sulfate salts are soluble except ${\text{CaSO}}_4$, ${\text{PbSO}}_4$ and ${\text{BaSO}}_4$.

2. All nitrate salts are soluble. The formula of nitrate polyatomic ion is ${\text{NO}}_3^{-}$.
3. All the salts formed from chloride, bromide and iodide are soluble except those with ${\text{Pb}}^{2+}$ and ${\text{Ag}}^{+}$.
4. All sulfate salts are insoluble except ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{3}}$, ${\text{K}}_{\text{2}}{\text{SO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{SO}}_{\text{3}}$.
5. All sulfides are insoluble except ${\text{Na}}_{\text{2}}\text{S}$, ${\text{K}}_{\text{2}}\text{S}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}\text{S}$.
6. All oxides and hydroxides are insoluble except ${\text{Na}}_{\text{2}}\text{O}$ /NaOH, ${\text{K}}_{\text{2}}\text{O}$ /KOH and $\text{BaO}/\text{Ba}{\left(\text{OH}\right)}_{\text{2}}$.
7. All carbonates are insoluble except ${\text{Na}}_{\text{2}}{\text{CO}}_3$, ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{CO}}_{\text{3}}$.

Interpretation Introduction

(b)

Interpretation:

If pairs of solutions are mixed, whether a solid is formed or not should be identified with balanced chemical equation.

Concept Introduction:

A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.

There are following solubility rules:

1. The salts formed from sodium, potassium and ammonium ions are soluble in nature.

All sulfate salts are soluble except ${\text{CaSO}}_4$, ${\text{PbSO}}_4$ and ${\text{BaSO}}_4$.

2. All nitrate salts are soluble. The formula of nitrate polyatomic ion is ${\text{NO}}_3^{-}$.
3. All the salts formed from chloride, bromide and iodide are soluble except those with ${\text{Pb}}^{2+}$ and ${\text{Ag}}^{+}$.
4. All sulfate salts are insoluble except ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{3}}$, ${\text{K}}_{\text{2}}{\text{SO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{SO}}_{\text{3}}$.
5. All sulfides are insoluble except ${\text{Na}}_{\text{2}}\text{S}$, ${\text{K}}_{\text{2}}\text{S}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}\text{S}$.
6. All oxides and hydroxides are insoluble except ${\text{Na}}_{\text{2}}\text{O}$ /NaOH, ${\text{K}}_{\text{2}}\text{O}$ /KOH and $\text{BaO}/\text{Ba}{\left(\text{OH}\right)}_{\text{2}}$.
7. All carbonates are insoluble except ${\text{Na}}_{\text{2}}{\text{CO}}_3$, ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{CO}}_{\text{3}}$.

Interpretation Introduction

(c)

Interpretation:

If pairs of solutions are mixed, whether a solid is formed or not should be identified with balanced chemical equation.

Concept Introduction:

A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.

There are following solubility rules:

1. The salts formed from sodium, potassium and ammonium ions are soluble in nature.

All sulfate salts are soluble except ${\text{CaSO}}_4$, ${\text{PbSO}}_4$ and ${\text{BaSO}}_4$.

2. All nitrate salts are soluble. The formula of nitrate polyatomic ion is ${\text{NO}}_3^{-}$.
3. All the salts formed from chloride, bromide and iodide are soluble except those with ${\text{Pb}}^{2+}$ and ${\text{Ag}}^{+}$.
4. All sulfate salts are insoluble except ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{3}}$, ${\text{K}}_{\text{2}}{\text{SO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{SO}}_{\text{3}}$.
5. All sulfides are insoluble except ${\text{Na}}_{\text{2}}\text{S}$, ${\text{K}}_{\text{2}}\text{S}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}\text{S}$.
6. All oxides and hydroxides are insoluble except ${\text{Na}}_{\text{2}}\text{O}$ /NaOH, ${\text{K}}_{\text{2}}\text{O}$ /KOH and $\text{BaO}/\text{Ba}{\left(\text{OH}\right)}_{\text{2}}$.
7. All carbonates are insoluble except ${\text{Na}}_{\text{2}}{\text{CO}}_3$, ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{CO}}_{\text{3}}$.