MCQ Kohlrausch’s Law, Class 12 Chemistry

1. There will be total 15 MCQ in this test.
2. Please keep a pen and paper ready for rough work but keep your books away.
3. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number.
4. No negative marking for incorrect choice.
5. Please click on “Finish the Test” when you want to exit.
6. All the best – Happy Studying

1. Conductivity of a solution depends upon:

Nature of electrolyte

Nature of solvent

Temperature

All of the above

Your comments:

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

Your comments:

Question 2 of 15

3. A.B.C.D.None of these

A

B

C

D

Your comments:

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

Your comments:

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

Your comments:

Question 5 of 15

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

A

B

C

D

Your comments:

Question 6 of 15

7.

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}

Your comments:

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.

Your comments:

Question 8 of 15

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

Resistance

Molar conductivity

Conductivity

Conductance

Your comments:

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

Your comments:

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%

Your comments:

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.

Your comments:

Question 12 of 15

13.

A

B

C

D

Your comments:

Question 13 of 15

14. The molar conductivities at infinite dilution in water at 25OC for NaOAC and HCl are 91.0 and 426.2 S cm² mol^-1 respectively. To calculate  ,the additional value required is:

∧ ⁰NaOH

∧ ⁰H2O

∧ ⁰NaCl

∧ ⁰KCl

Your comments:

Question 14 of 15

15. With increase in temperature the degree of dissociation of electrolyte:

Increases

Depends on the enthalpy change of dissolution

Decreases

Depends on the nature of salt

Your comments:

Question 15 of 15

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