Chapter 3, Problem 20PS

Which compound or compounds in each of the following groups is (are) soluble in water?

(a) BaSO₄, Ba(NO₃)₂, BaCO₃

(b) Na₂SO₄, NaClO₄, NaCH₃CO₂

(c) AgBr, KBr, Al₂Br₆

Interpretation Introduction

Interpretation:

Water solubility of the given 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.  List of solubility of the compound is given below,

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ 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, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$ is soluble and others are insoluble.

Explanation of Solution

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

$\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$ is dissolves in water, barium nitrate is composed of ${\text{Ba}}^{\text{2+}}{\text{and NO}}_{\text{3}}^{\text{2-}}$, and it became ions in water it soluble in water and others are insoluble.

  

Interpretation Introduction

Interpretation:

Water solubility of the given 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.  List of solubility of the compound is given below,

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ 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, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

All are water soluble.

Explanation of Solution

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.  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ is soluble in water.  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ is dissolves in water, sodium sulfate is composed of ${\text{Na}}^{\text{+}}{\text{and SO}}_4^{2-}$, and it became ions in water it soluble in water.

  

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble. ${\text{NaClO}}_{\text{4}}$ is soluble in water, sodium perchlorate is composed of ${\text{Na}}^{\text{+}}{\text{and ClO}}_4^{-}$, and it became ions in water it soluble in water.

  

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble.  ${\text{NaCH}}_{\text{3}}{\text{CO}}_{\text{2}}$ is soluble in water.  ${\text{NaCH}}_{\text{3}}{\text{CO}}_{\text{2}}$ is dissolves in water, sodium acetate is composed of ${\text{Na}}^{\text{+}}{\text{and CH}}_{\text{3}}{\text{CO}}_2^{-}$, and it became ions in water it soluble in water.

  

Interpretation Introduction

Interpretation:

Water solubility of the given 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. List of solubility of the compound is given below,

Soluble compounds in water

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ 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 are $\left({\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}\right)$ 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 $\text{carbonate }\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)\text{, phosphate }\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)\text{, Oxalate }\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)\text{, Chromate }\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)\text{, sulfide }\left({\text{S}}^{\text{2-}}\right)$ 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, $\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\text{and Sr}{\left(\text{OH}\right)}_{\text{2}}$ are soluble in water.

Answer to Problem 20PS

${\text{KBr and Al}}_{\text{2}}{\text{Br}}_{\text{6}}$ are water soluble and silver bromide is water insoluble.

Explanation of Solution

Almost all the salts of ${\text{Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, NH}}_{\text{4}}{}^{\text{+}}\text{, salts of nitrate }\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)\text{, chlorate }\left({\text{ClO}}_{\text{3}}{}^{\text{-}}\right)\text{, Perchlorate }\left({\text{ClO}}_{\text{4}}{}^{\text{-}}\right)\text{, Acetate }\left({\text{CH}}_{\text{3}}{\text{CO}}_{\text{2}}{}^{\text{-}}\right)$ are soluble. $\text{KBr}$ is dissolves in water, potassium bromide is composed of ${\text{K}}^{\text{+}}{\text{and Br}}^{\text{-}}$, and it became ions in water, it soluble in water.

  

${\text{Al}}_{\text{2}}{\text{Br}}_{\text{6}}$ is dissolves in water, aluminium bromide is composed of ${\text{Al}}^{\text{3+}}{\text{and Br}}_{}^{\text{-}}$, and it became ions in water, it soluble in water.

  

Silver bromide is water insoluble.