Chapter 12, Problem 12.133CQ

Interpretation Introduction

(a)

Interpretation:

The net ionic equation of the given reaction should be determined.

Concept Introduction:

The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.

There are following rules of solubility of an ionic compound in the water:

1. The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
2. The salts of nitrate ion are commonly soluble.
3. The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
4. Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
5. Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
6. Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
7. The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
8. Carbonates are insoluble.
9. Chromates are insoluble.
10. Phosphates are also insoluble such as calcium phosphate and silver phosphate.
11. Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation of the given reaction should be determined.

Concept Introduction:

The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.

There are following rules of solubility of an ionic compound in the water:

1. The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
2. The salts of nitrate ion are commonly soluble.
3. The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
4. Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
5. Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
6. Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
7. The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
8. Carbonates are insoluble.
9. Chromates are insoluble.
10. Phosphates are also insoluble such as calcium phosphate and silver phosphate.
11. Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation of the given reaction should be determined.

Concept Introduction:

The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.

There are following rules of solubility of an ionic compound in the water:

1. The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
2. The salts of nitrate ion are commonly soluble.
3. The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
4. Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
5. Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
6. Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
7. The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
8. Carbonates are insoluble.
9. Chromates are insoluble.
10. Phosphates are also insoluble such as calcium phosphate and silver phosphate.
11. Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.

Interpretation Introduction

(d)

Interpretation:

The net ionic equation of the given reaction should be determined.

Concept Introduction:

The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.

There are following rules of solubility of an ionic compound in the water:

1. The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
2. The salts of nitrate ion are commonly soluble.
3. The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
4. Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
5. Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
6. Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
7. The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
8. Carbonates are insoluble.
9. Chromates are insoluble.
10. Phosphates are also insoluble such as calcium phosphate and silver phosphate.
11. Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.