Chapter 3, Problem 30QRT

Predict whether each compound is soluble in water. Indicate which ions are present in solution for the water-soluble compounds.

1. (a) Ammonium nitrate
2. (b) Barium sulfate
3. (c) Potassium acetate
4. (d) Calcium carbonate
5. (e) Sodium perchlorate

Interpretation Introduction

Interpretation:

The solubility of the given Ammonium nitrate in water has to be identified. The ions present in the aqueous solution of Ammonium nitrate has to be identified.

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:

All ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$ group and ${\text{NH}}_4^{+}$ compound are soluble, all nitrates $\left({\text{NO}}_{\text{3}}{}^{\text{-}}\right)$ 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 namely ${\text{Ag}}^{\text{+}}{\text{, Hg}}_{\text{2}}{}^{\text{2+}}{\text{, Pb}}^{\text{2+}}$ are insoluble.

Most of the sulfates are soluble except ${\text{CaSO}}_{\text{4}}{\text{, SrSO}}_{\text{4}}{\text{, BaSO}}_{\text{4}}{\text{ and PbSO}}_{\text{4}}$ are insoluble.

All the 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.

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 ${\text{Ca}}^{\text{2+}}{\text{, Sr}}^{\text{2+}}{\text{, Ba}}^{\text{2+}}{\text{, Pb}}^{\text{2+}}{\text{, Ag}}^{\text{+}}$ are insoluble.

Insoluble compounds in water:

All phosphates $\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)$ and carbonates $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)$ are insoluble except ${\text{NH}}_4^{+}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$.

All chromates $\left({\text{CrO}}_{\text{4}}{}^{\text{2-}}\right)$ are insoluble except ${\text{NH}}_4^{+}$, ${\text{Mg}}^{\text{2+}}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$.

All hydroxides are insoluble except ${\text{NH}}_4^{+}$, ${\text{Mg}}^{\text{2+}}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$. $\text{Sr}{\left(\text{OH}\right)}_{\text{2}}\text{, Ba}{\left(\text{OH}\right)}_{\text{2}}\text{, and Ca}{\left(\text{OH}\right)}_{\text{2}}$ are slightly soluble.

All oxalates $\left({\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\right)$ are insoluble except ${\text{NH}}_4^{+}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$.

All sulfides $\left({\text{S}}^{\text{2-}}\right)$ are insoluble except ${\text{NH}}_4^{+}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$ and Group 2A ($\text{MgS, CaS, and BaS}$ are sparingly 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.

Dissociation:

When ionic compound dissolved in water it produced cation and anion, this process is called as dissociation.

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

Explanation of Solution

The given compound is shown below,

   Ammonium nitrate (${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$)

All ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$ group and ${\text{NH}}_4^{+}$ compound are soluble, therefore Ammonium nitrate (${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$) is soluble in water.

The dissociation of Ammonium nitrate (${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$) is given below,

  ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}\to {\text{ NH}}_4^{+}{\text{(aq) + NO}}_3^{-}\text{(aq)}$

Therefore, Ammonium nitrate (${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$) is dissolved in water (dissociation) gives ${\text{NH}}_4^{+}\text{(aq) }$ and ${\text{NO}}_3^{-}\text{(aq)}$.

Interpretation Introduction

Interpretation:

The solubility of the given Barium sulfate in water has to be identified. The ions present in the aqueous solution of Barium sulfate has to be identified.

Concept introduction:

Refer to part (a)

Explanation of Solution

The given compound is shown below,

   Barium sulfate

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

, therefore Barium sulfate (${\text{BaSO}}_{\text{4}}$) is insoluble in water and it can’t undergo dissociation.

Interpretation Introduction

Interpretation:

The solubility of the given Potassium acetate in water has to be identified. The ions present in the aqueous solution of Potassium acetate has to be identified.

Concept introduction:

Refer to part (a)

Explanation of Solution

The given compound is shown below,

   Potassium acetate

All the 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, therefore Potassium acetate (${\text{KCH}}_{\text{3}}\text{COO}$) is soluble in water.

The dissociation of Potassium acetate (${\text{KCH}}_{\text{3}}\text{COO}$) is given below,

  ${\text{KCH}}_{\text{3}}\text{COO }\to {\text{ K}}^{\text{+}}{\text{(aq) + CH}}_{\text{3}}{\text{COO}}^{\text{-}}\text{(aq)}$

Therefore, Potassium acetate (${\text{KCH}}_{\text{3}}\text{COO}$) is dissolved in water (dissociation) gives ${\text{K}}^{\text{+}}\text{(aq)}$ and ${\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}\text{(aq)}$.

Interpretation Introduction

Interpretation:

The solubility of the given Calcium carbonate in water has to be identified. The ions present in the aqueous solution of Calcium carbonate has to be identified.

Concept introduction:

Refer to part (a)

Explanation of Solution

The given compound is shown below,

   Calcium carbonate

All phosphates $\left({\text{PO}}_{\text{4}}{}^{\text{3-}}\right)$ and carbonates $\left({\text{CO}}_{\text{3}}{}^{\text{2-}}\right)$ are insoluble except ${\text{NH}}_4^{+}$ and Group ${\text{1A (Li}}^{\text{+}}{\text{, Na}}^{\text{+}}{\text{, K}}^{\text{+}}{\text{, Rb}}^{\text{+}}{\text{, Cs}}^{\text{+}}\text{)}$, therefore Calcium carbonate (${\text{CaCO}}_3$) is insoluble in water and it can’t undergo dissociation.

Interpretation Introduction

Interpretation:

  The solubility of the given Sodium perchlorate in water has to be identified. The ions present in the aqueous solution of Sodium perchlorate has to be identified.

Concept introduction:

Refer to part (a)

Explanation of Solution

The given compound is shown below,

  Sodium perchlorate

All the 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, therefore Sodium perchlorate (${\text{NaClO}}_{\text{4}}$) is soluble in water.

The dissociation of Sodium perchlorate (${\text{NaClO}}_{\text{4}}$) is given below,

  ${\text{NaClO}}_{\text{4}}\to {\text{ Na}}^{\text{+}}{\text{(aq) + ClO}}_4^{-}\text{(aq)}$

Therefore, Sodium perchlorate (${\text{NaClO}}_{\text{4}}$) is dissolved in water (dissociation) gives ${\text{Na}}^{\text{+}}\text{(aq)}$ and ${\text{ClO}}_4^{-}\text{(aq)}$.