Frank Textbook Solutions: Study Of Acids, Bases and Salts

 Page 1


Chapter 3. Study Of Acids, Bases and Salts
PAGE NO : 62
Solution 1: 
Solution 2:
1. (i) Hydrogen chloride HCl 
(ii) Nitric acid HNO3
2. (i) Carbonic acid H2CO3 
(ii) Oxalic acid (COOH)2
3. (i) Sulphuric acid H2SO4 
(ii) Hydrogen chloride HCl
4. (i) Carbonic acid H2CO3 
(ii) Acetic acid
Solution 3: 
 
 
Page 2


Chapter 3. Study Of Acids, Bases and Salts
PAGE NO : 62
Solution 1: 
Solution 2:
1. (i) Hydrogen chloride HCl 
(ii) Nitric acid HNO3
2. (i) Carbonic acid H2CO3 
(ii) Oxalic acid (COOH)2
3. (i) Sulphuric acid H2SO4 
(ii) Hydrogen chloride HCl
4. (i) Carbonic acid H2CO3 
(ii) Acetic acid
Solution 3: 
 
 
pH = -log10 [H3O+]
2. The three applications of pH scale are:
It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.
Solution 5:
 
Solution 6:
 
 
 
Solution 4:
1. The pH of a solution is defined as the negative logarithm (base 10) of the hydronium
ion concentration present in the solution.
Page 3


Chapter 3. Study Of Acids, Bases and Salts
PAGE NO : 62
Solution 1: 
Solution 2:
1. (i) Hydrogen chloride HCl 
(ii) Nitric acid HNO3
2. (i) Carbonic acid H2CO3 
(ii) Oxalic acid (COOH)2
3. (i) Sulphuric acid H2SO4 
(ii) Hydrogen chloride HCl
4. (i) Carbonic acid H2CO3 
(ii) Acetic acid
Solution 3: 
 
 
pH = -log10 [H3O+]
2. The three applications of pH scale are:
It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.
Solution 5:
 
Solution 6:
 
 
 
Solution 4:
1. The pH of a solution is defined as the negative logarithm (base 10) of the hydronium
ion concentration present in the solution.
3. An acid in a solution furnishes the ions:
 
Hydronium / Hydrogen ion and a negative ion.
Solution 8:
 
PAGE NO : 63
 
Solution 9:
1. CaO
2. NaOH
3. CuO
4. Cu[(OH)2]
5. H2CO3
6. Ferric hydroxide [Fe (OH)3].
7. CuO
8. NH3
Solution 10:
 
Anhydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid
 
because anhydrous means without water and we know that the property of acidity is
 
shown by a substance only when it is dissolved in water or its aqueous solution is
 
prepared.
Solution 7:
1. Base in solution furnishes the ions:
Hydroxide ion/ oxide ion and a metallic ion.
2. A weak alkali furnishes the ions:
Hydroxide ion and metallic ion and molecules of weak alkali./
Page 4


Chapter 3. Study Of Acids, Bases and Salts
PAGE NO : 62
Solution 1: 
Solution 2:
1. (i) Hydrogen chloride HCl 
(ii) Nitric acid HNO3
2. (i) Carbonic acid H2CO3 
(ii) Oxalic acid (COOH)2
3. (i) Sulphuric acid H2SO4 
(ii) Hydrogen chloride HCl
4. (i) Carbonic acid H2CO3 
(ii) Acetic acid
Solution 3: 
 
 
pH = -log10 [H3O+]
2. The three applications of pH scale are:
It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.
Solution 5:
 
Solution 6:
 
 
 
Solution 4:
1. The pH of a solution is defined as the negative logarithm (base 10) of the hydronium
ion concentration present in the solution.
3. An acid in a solution furnishes the ions:
 
Hydronium / Hydrogen ion and a negative ion.
Solution 8:
 
PAGE NO : 63
 
Solution 9:
1. CaO
2. NaOH
3. CuO
4. Cu[(OH)2]
5. H2CO3
6. Ferric hydroxide [Fe (OH)3].
7. CuO
8. NH3
Solution 10:
 
Anhydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid
 
because anhydrous means without water and we know that the property of acidity is
 
shown by a substance only when it is dissolved in water or its aqueous solution is
 
prepared.
Solution 7:
1. Base in solution furnishes the ions:
Hydroxide ion/ oxide ion and a metallic ion.
2. A weak alkali furnishes the ions:
Hydroxide ion and metallic ion and molecules of weak alkali./
Solution 11: 
Solution 12: 
Strength of an acid measures the ease with which the acid can ionize to produce hydrogen 
or hydronium ions when dissolved in water. Those acids which can easily ionize to form 
hydrogen ions are called strong acids while those which can partially ionize to form 
hydrogen ions are called weak acids. 
Strength of an acid depends upon many factors such as:
1. Molecular structure of the acid
2. The temperature
3. Properties of the solvent
Solution 13: 
Page 5


Chapter 3. Study Of Acids, Bases and Salts
PAGE NO : 62
Solution 1: 
Solution 2:
1. (i) Hydrogen chloride HCl 
(ii) Nitric acid HNO3
2. (i) Carbonic acid H2CO3 
(ii) Oxalic acid (COOH)2
3. (i) Sulphuric acid H2SO4 
(ii) Hydrogen chloride HCl
4. (i) Carbonic acid H2CO3 
(ii) Acetic acid
Solution 3: 
 
 
pH = -log10 [H3O+]
2. The three applications of pH scale are:
It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.
Solution 5:
 
Solution 6:
 
 
 
Solution 4:
1. The pH of a solution is defined as the negative logarithm (base 10) of the hydronium
ion concentration present in the solution.
3. An acid in a solution furnishes the ions:
 
Hydronium / Hydrogen ion and a negative ion.
Solution 8:
 
PAGE NO : 63
 
Solution 9:
1. CaO
2. NaOH
3. CuO
4. Cu[(OH)2]
5. H2CO3
6. Ferric hydroxide [Fe (OH)3].
7. CuO
8. NH3
Solution 10:
 
Anhydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid
 
because anhydrous means without water and we know that the property of acidity is
 
shown by a substance only when it is dissolved in water or its aqueous solution is
 
prepared.
Solution 7:
1. Base in solution furnishes the ions:
Hydroxide ion/ oxide ion and a metallic ion.
2. A weak alkali furnishes the ions:
Hydroxide ion and metallic ion and molecules of weak alkali./
Solution 11: 
Solution 12: 
Strength of an acid measures the ease with which the acid can ionize to produce hydrogen 
or hydronium ions when dissolved in water. Those acids which can easily ionize to form 
hydrogen ions are called strong acids while those which can partially ionize to form 
hydrogen ions are called weak acids. 
Strength of an acid depends upon many factors such as:
1. Molecular structure of the acid
2. The temperature
3. Properties of the solvent
Solution 13: 
Solution 14: 
Solution B with pH value 9 will give pink colour with phenolphthalein. 
Concept Insight: Bases give pink colour with phenolphthalein because a base will 
abstract two protons from phenolphthalein and the resulting phenolphthalein ion provides 
pink colour to the solution.
Solution 15: 
Two indicators for identification of acid are methyl red and Thymol blue.
Solution 16: 
Solution 17: