Chapter 4.2, Problem 1PE

(a)

Interpretation Introduction

Interpretation:

The compounds $FeS$ have to be classified as soluble or insoluble compound.

Concept Introduction:

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}\text{,}{\text{K}}^{\text{+}}\text{,}{\text{NH}}_{\text{4}}{}^{\text{+}}$, salts of nitrate $\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)$, chlorate $\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)$, perchlorate $\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)$, acetate $\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}\text{,}{\text{Br}}^{\text{-}}\text{and}{\text{I}}^{\text{-}}$ are soluble. But some of the halides whose cations are ${\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}{}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of F^-are soluble. But some of the fluoride salt of ${\text{Mg}}^{\text{+2}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of  sulfate $\left({\text{SO}}_{\text{4}}{}^{\text{-2}}\right)$ are soluble. But sulfates of $A{g}^{\text{+}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Insoluble compounds in water:

Most of the salts of are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,  are soluble in water.

(b)

Interpretation Introduction

Interpretation:

The compound $Ca{\left(OH\right)}_2$ has to be classified as soluble or insoluble compound.

Concept Introduction

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}\text{,}{\text{K}}^{\text{+}}\text{,}{\text{NH}}_{\text{4}}{}^{\text{+}}$, salts of nitrate $\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)$, chlorate $\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)$, perchlorate $\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)$, acetate $\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}\text{,}{\text{Br}}^{\text{-}}\text{and}{\text{I}}^{\text{-}}$ are soluble. But some of the halides whose cations are ${\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}{}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of F^-are soluble. But some of the fluoride salt of ${\text{Mg}}^{\text{+2}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of sulfate $\left({\text{SO}}_{\text{4}}{}^{\text{-2}}\right)$ are soluble. But sulfates of $A{g}^{\text{+}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Insoluble compounds in water:

Most of the salts of are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,  are soluble in water.

(c)

Interpretation Introduction

Interpretation:

The compound $\text{Co}{\left({\text{NO}}_{\text{3}}\right)}_{\text{3}}$ has to be classified as soluble or insoluble compound.

Concept Introduction

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}\text{,}{\text{K}}^{\text{+}}\text{,}{\text{NH}}_{\text{4}}{}^{\text{+}}$, salts of nitrate $\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)$, chlorate $\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)$, perchlorate $\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)$, acetate $\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.

Almost all the salts of ${\text{Cl}}^{\text{-}}\text{,}{\text{Br}}^{\text{-}}\text{and}{\text{I}}^{\text{-}}$ are soluble. But some of the halides whose cations are ${\text{Ag}}^{\text{+}}\text{,}{\text{Hg}}_{\text{2}}{}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of F^-are soluble. But some of the fluoride salt of ${\text{Mg}}^{\text{+2}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Salts of  sulfate $\left({\text{SO}}_{\text{4}}{}^{\text{-2}}\right)$ are soluble. But sulfates of $A{g}^{\text{+}}\text{,}{\text{Ca}}^{\text{+2}}\text{,}{\text{Sr}}^{\text{+2}}\text{,}{\text{Ba}}^{\text{+2}}\text{,}{\text{Pb}}^{\text{+2}}$ are insoluble.

Insoluble compounds in water:

Most of the salts of are insoluble but some of the salts of NH₄⁺, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,  are soluble in water.