JEE Main - Conductance in electrolytic solutions molar conductivities and Kohlrausch's law One Line Questions & Answers

1. The molar conductivity of a 0.1 M solution of KCl is 12.95 S cm² mol⁻¹. If the limiting molar conductivity of KCl is 149.9 S cm² mol⁻¹, what is the degree of dissociation? — 0.086

2. The molar conductivity of a 0.01 M solution of a weak acid HA is 150 S cm² mol⁻¹, and its limiting molar conductivity is 300 S cm² mol⁻¹. What is the degree of dissociation of HA? — 0.5

3. The molar conductivity of CaSO₄ at infinite dilution is approximately 130 S cm² mol⁻¹. If Λm°(Ca²⁺) = 59.5 S cm² mol⁻¹ and Λm°(SO₄²⁻) = 160 S cm² mol⁻¹, what would be the expected molar conductivity of CaSO₄ at infinite dilution based on Kohlrausch's law? — 219.5 S cm² mol⁻¹

4. If the limiting molar ionic conductivities of K⁺ and OH⁻ are 73.5 S cm² mol⁻¹ and 198.0 S cm² mol⁻¹ respectively, what is the limiting molar conductivity of KOH? — 271.5 S cm² mol⁻¹

5. The molar conductivity of BaCl₂ at infinite dilution is 280 S cm² mol⁻¹. If the molar conductivity of Ba²⁺ and Cl⁻ ions are 127 and 71 S cm² mol⁻¹ respectively, what is the molar conductivity of Ba²⁺ at infinite dilution? — 127 S cm² mol⁻¹

6. The limiting molar conductivity of NaCl, Na⁺, and Cl⁻ are 126.4, 50.1, and 71.4 S cm² mol⁻¹ respectively. What is the limiting molar conductivity of HCl? — 197.8 S cm² mol⁻¹

7. According to Kohlrausch's law, Λm°(CH₃COOH) = Λm°(CH₃COO⁻) + Λm°(H⁺). If Λm°(CH₃COONa) = 91.0 S cm² mol⁻¹, Λm°(HCl) = 426.16 S cm² mol⁻¹, and Λm°(NaCl) = 126.45 S cm² mol⁻¹, calculate Λm°(CH₃COOH). — 309.71 S cm² mol⁻¹

8. The molar conductivity of AgCl at infinite dilution is 138.3 S cm² mol⁻¹. If Λm°(Ag⁺) = 61.9 S cm² mol⁻¹, what is Λm°(Cl⁻)? — 76.4 S cm² mol⁻¹

9. In the context of conductance, the term 'electrolytic cell' refers to: — The part of the circuit containing the electrolytic solution between two electrodes.

10. Conductivity (κ) is defined as the conductance of: — A solution of unit volume

11. Conductance of a solution is inversely proportional to: — Resistance

12. The molar conductivity of an electrolyte is defined as: — Conductance of solution containing one mole of electrolyte

13. Which of the following is a measure of the ability of an ion to move in an electric field? — Ionic mobility

14. Which of the following statements about the effect of temperature on conductivity is TRUE? — Conductivity of electrolytes increases with increasing temperature.

15. The molar conductivity of a strong electrolyte decreases with concentration due to: — Both B and C

16. What is the main reason for the decrease in molar conductivity of strong electrolytes with increasing concentration? — Reduced ionic mobility due to inter-ionic attraction and increased viscosity

17. Kohlrausch's law is applicable at: — Infinite dilution

18. The phenomenon that explains the increase in molar conductivity of weak electrolytes with dilution is: — Increased dissociation

19. What happens to the conductivity of an electrolytic solution upon dilution? — It decreases

20. The molar conductivity of a solution of concentration C can be expressed as Λm = Λm° - A√C for dilute solutions, where A is a constant. This equation is known as: — Debye-Hückel-Onsager equation

21. The cell constant (G*) of a conductivity cell is given by: — Area / Length

22. Conductance of a solution is directly proportional to: — Area of cross-section

23. Which ion has the highest ionic mobility in aqueous solution? — Cs⁺

24. Which ion exhibits the lowest molar conductivity at infinite dilution in aqueous solution among alkali metals? — Li⁺

25. For a weak electrolyte like acetic acid, as the concentration decreases (dilution increases): — Molar conductivity increases

26. Which of the following factors affects the conductivity of an electrolytic solution? — All of the above

27. The unit of conductance (G) is: — Siemens (S)

28. The degree of dissociation of a weak electrolyte at a given concentration can be determined using: — Kohlrausch's Law

29. Kohlrausch's law states that at infinite dilution, the molar conductivity of an electrolyte is the sum of the contributions of the individual ions. This law is a consequence of: — The independence of ionic migration

30. Which of the following methods is used to measure the conductivity of electrolytic solutions? — Conductometry

31. The relationship between resistance (R), resistivity (ρ), length (l), and area of cross-section (A) is given by: — R = ρ * (l/A)

32. Conductance (G) is the reciprocal of: — Resistance (R)

33. The unit of cell constant is: — m⁻¹

34. The unit of conductivity (κ) is: — S cm⁻¹

35. What is the SI unit of molar conductivity? — S m² mol⁻¹

36. The unit of resistance (R) is: — Ohm (Ω)

37. Which of the following statements about the mobility of ions is INCORRECT? — Smaller ions have higher mobility in aqueous solutions due to less hydration.

38. For a strong electrolyte, the plot of Λm versus √C is a: — Straight line with negative slope

39. Kohlrausch's law is particularly useful for determining the molar conductivity of: — Weak electrolytes at infinite dilution

40. Molar conductivity increases with the dilution for: — Both strong and weak electrolytes

41. The transport number of an ion is defined as the fraction of the total charge carried by: — That particular ion

42. According to Kohlrausch's law, the molar conductivity of an electrolyte at infinite dilution is equal to the sum of: — The ionic conductances of the ions

43. The molar conductivity of an electrolyte solution is a measure of: — The ability of the solution to conduct electricity per mole of electrolyte

44. The limiting molar conductivity of an electrolyte is the molar conductivity at: — Zero concentration

45. The molar conductivity of a weak electrolyte approaches a maximum value at: — Zero concentration

46. The relationship between conductivity (κ) and resistivity (ρ) is: — κ = 1/ρ

47. Conductivity (κ) is related to conductance (G) and cell constant (G*) by: — κ = G * G*

48. Molar conductivity of a strong electrolyte at infinite dilution is represented by: — Λm°

49. The relationship between conductivity (κ) and molar conductivity (Λm) is: — Λm = 1000 * κ / C

Conductance in electrolytic solutions molar conductivities and Kohlrausch's law - One Line Questions