Kohlrausch's Law, Class 12 Chemistry NCERT Solutions

1. Conductivity of a solution depends upon:

Nature of electrolyte

Nature of solvent

Temperature

All of the above

Question 1 of 15

2. Limiting Ionic conductivity is defined as:

Conducting power of one gram of ions at a given temperature and concentration

Conducting power of one mole of electrolyte at a given temperature and concentration

Conducting power of one mole of ions at a given temperature at infinite dilution

Conducting power of one gram mole of ions at a given temperature and concentration

Question 2 of 15

D.None of these

Question 3 of 15

4. Which of the following statements is correct?

Molar conductivity of a strong electrolyte decreases with dilution

Molar conductivity of a strong and weak electrolyte decreases with dilution

Molar conductivity of a weak electrolyte decreases with dilution

Molar conductivity of a strong and weak electrolyte increases with dilution

Question 4 of 15

5. Molar conductivity for a compound AB is 145.0 Scm²mol^-1 and for CB is 110.1 Scm²mol^-1. Limiting molar conductivity for A⁺ is 73.5 Scm²mol^-1. What is limiting molar conductivity for C⁺?

326.6 S cm² mol^-1

38.6 S cm² mol^-1

181.6 S cm² mol^-1

90.8 S cm² mol^-1

Question 5 of 15

6. Limiting molar conductivity of acetic acid can be calculated using:

Kohlrausch s Law Multiple Choice Questions for CBSE Class 12 Chemistry Topperlearning

Question 6 of 15

280 S cm^{2^{mol^-1}}

330.98 S cm^{2^{mol^-1}}

203.6 S cm^{2^{mol^-1}}

90.98 S cm^{2^{mol^-1}}

Question 7 of 15

8. Kohlrausch’s Law shows that:

at infinite dilution the ionic conductivity of ions is additive.

at infinite dilution the ionic conductivity of all the ions of the electrolyte become equal.

at infinite dilution the concentration of the electrolyte becomes unity.

at infinite dilution the concentration of ions increases.

Question 8 of 15

9. Conductivity of a solution contained within 1 centimetre cube volume is known as:

Resistance

Molar conductivity

Conductivity

Conductance

Question 9 of 15

10. Kohlrausch’s Law is applicable:

to aqueous solution of strong electrolytes

applicable to electrolytes dissolved in a solvent of low polarity only.

to electrolytes at temperature above room temperature.

to electrolytic solutions at infinite dilution

Question 10 of 15

11. At 300K molar conductivity of solution A is 350 units, and at infinite dilution the molar conductivity of the same sample is 480 unit. Predict the percentage dissociation of the electrolyte.

73.0%

37.0%

63.0%

137.0%

Question 11 of 15

12. For weak electrolytes ∧m^o cannot to be calculated by extrapolation of ∧m^o vs (c)^1/2 graph. Which of the following is not the reason?

∧m⁰ increases steeply on dilution especially near lower concentrations.

Weak electrolytes ionize completely in solution

∧m for weak electrolytes does not vary linearly with dilution.

Weak electrolytes dissociated to a much lesser extent as compared to strong electrolytes and therefore, ∧m⁰ of weak electrolytes is low. It becomes even low at lower concentration.

Question 12 of 15

13.