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Which one of the following solutions has lowest conducting power:
- a)0.1 M CH3COOH
- b)0.1 M NaCl
- c)0.1 M KNO3
- d)0.1 M HCl
Correct answer is option 'A'. Can you explain this answer?
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Which one of the following solutions has lowest conducting power:a)0.1...
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Which one of the following solutions has lowest conducting power:a)0.1...
**Answer:**
To determine the solution with the lowest conducting power, we need to consider the dissociation of the solutes in water. The greater the degree of dissociation, the higher the conducting power of the solution.
**Dissociation of the solutes:**
a) CH3COOH (acetic acid):
CH3COOH ⇌ CH3COO- + H+
b) NaCl (sodium chloride):
NaCl ⇌ Na+ + Cl-
c) KNO3 (potassium nitrate):
KNO3 ⇌ K+ + NO3-
d) HCl (hydrochloric acid):
HCl ⇌ H+ + Cl-
**Factors affecting the degree of dissociation:**
1. Nature of the solute: Strong acids and strong bases dissociate completely in water, while weak acids and weak bases dissociate to a lesser extent.
2. Concentration of the solution: Higher concentrations tend to increase the degree of dissociation.
**Explanation:**
a) 0.1 M CH3COOH (acetic acid):
Acetic acid is a weak acid and does not dissociate completely in water. It only partially ionizes into CH3COO- and H+. Therefore, the conducting power of this solution will be lower compared to the others.
b) 0.1 M NaCl (sodium chloride):
Sodium chloride is an ionic compound and dissociates completely into Na+ and Cl- ions in water. This solution will have a higher conducting power compared to acetic acid.
c) 0.1 M KNO3 (potassium nitrate):
Potassium nitrate is also an ionic compound and dissociates completely into K+ and NO3- ions in water. This solution will have a higher conducting power compared to acetic acid.
d) 0.1 M HCl (hydrochloric acid):
Hydrochloric acid is a strong acid and dissociates completely into H+ and Cl- ions in water. This solution will have a higher conducting power compared to acetic acid.
Therefore, the solution with the lowest conducting power is 0.1 M CH3COOH (acetic acid) due to its weak acid nature and partial dissociation in water.
To determine the solution with the lowest conducting power, we need to consider the dissociation of the solutes in water. The greater the degree of dissociation, the higher the conducting power of the solution.
**Dissociation of the solutes:**
a) CH3COOH (acetic acid):
CH3COOH ⇌ CH3COO- + H+
b) NaCl (sodium chloride):
NaCl ⇌ Na+ + Cl-
c) KNO3 (potassium nitrate):
KNO3 ⇌ K+ + NO3-
d) HCl (hydrochloric acid):
HCl ⇌ H+ + Cl-
**Factors affecting the degree of dissociation:**
1. Nature of the solute: Strong acids and strong bases dissociate completely in water, while weak acids and weak bases dissociate to a lesser extent.
2. Concentration of the solution: Higher concentrations tend to increase the degree of dissociation.
**Explanation:**
a) 0.1 M CH3COOH (acetic acid):
Acetic acid is a weak acid and does not dissociate completely in water. It only partially ionizes into CH3COO- and H+. Therefore, the conducting power of this solution will be lower compared to the others.
b) 0.1 M NaCl (sodium chloride):
Sodium chloride is an ionic compound and dissociates completely into Na+ and Cl- ions in water. This solution will have a higher conducting power compared to acetic acid.
c) 0.1 M KNO3 (potassium nitrate):
Potassium nitrate is also an ionic compound and dissociates completely into K+ and NO3- ions in water. This solution will have a higher conducting power compared to acetic acid.
d) 0.1 M HCl (hydrochloric acid):
Hydrochloric acid is a strong acid and dissociates completely into H+ and Cl- ions in water. This solution will have a higher conducting power compared to acetic acid.
Therefore, the solution with the lowest conducting power is 0.1 M CH3COOH (acetic acid) due to its weak acid nature and partial dissociation in water.
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