Chapter 3, Problem 16PS

Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when the compound dissolves in water.

(a) NiCl₂

(b) Cr(NO₃)₃

(c) Pb(NO₃)₂

(d) BaSO₄

Interpretation Introduction

Interpretation:

Water solubility of the given compounds and ions produced by the compounds should be analyzed.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

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

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

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

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

Insoluble compounds in water:

Most of the salts of $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{ and}\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and $\text{BaS}$ are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 16PS

Water soluble compound.  Produced ions are ${\text{Ni}}^{\text{2+}}{\text{and Cl}}_{}^{\text{-}}$.

Explanation of Solution

The given compound Nickel (II) chloride which is soluble in water.

${\text{NiCl}}_2$ is dissolves in water, Nickel(II) chloride is composed of ${\text{Ni}}^{\text{2+}}{\text{and Cl}}_{}^{\text{-}}$, and it became ions in water.

  

Interpretation Introduction

Interpretation:

Water solubility of the given compounds and ions produced by the compounds should be analyzed.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

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

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

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

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

Insoluble compounds in water:

Most of the salts of $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{ and}\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and $\text{BaS}$ are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 16PS

Water soluble compound.  Produced ions are ${\text{Cr}}^{\text{3+}}{\text{and NO}}_{\text{3}}{}^{\text{-}}$.

Explanation of Solution

The given compound is Chromium (III) nitrate which is soluble in water.

${\text{Cr(NO}}_3{)}_3$ is dissolves in water, Chromium(III) nitrate is composed of ${\text{Cr}}^{\text{3+}}{\text{and NO}}_3^{\text{-}}$, and it became ions in water.

  

Interpretation Introduction

Interpretation:

Water solubility of the given compounds and ions produced by the compounds should be analyzed.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

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

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

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

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

Insoluble compounds in water:

Most of the salts of $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{ and}\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and $\text{BaS}$ are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 16PS

Water soluble compound.  Produced ions are.${\text{Pb}}^{\text{2+}}{\text{and NO}}_{\text{3}}^{-}$.

Explanation of Solution

The given compound is Lead (II) nitrate which is soluble in water.

${\text{Pb(NO}}_{\text{3}}{\text{)}}_{\text{2}}$ is dissolves in water, Lead(II) nitrate is composed of ${\text{Pb}}^{\text{2+}}\left(\text{aq}\right){\text{ + 2 NO}}^{\text{-}}{}_{\text{3}}\left(\text{aq}\right)$, and it became ions in water.

  

Interpretation Introduction

Interpretation:

Water solubility of the given compounds and ions produced by the compounds should be analyzed.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Soluble compounds in water

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

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

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

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

Insoluble compounds in water:

Most of the salts of $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{ and}\left({\text{S}}^{\text{2-}}\right)$ are insoluble but some of the salts of NH₄⁺, alkali metal cations and $\text{BaS}$ are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 16PS

This compound insoluble in water.

Explanation of Solution

The given compound is Barium sulfate which is insoluble in water.