• iamal
• February 12, 2026

Master Strong and Weak Electrolyte Conductivity MCQs with Proven Success Strategies

Understanding the concept behind strong and weak electrolyte conductivity mcqs is essential for mastering electrochemistry at the Class 11 and Class 12 level. The behavior of electrolytes in solution directly influences conductivity, molar conductivity, degree of ionization, and overall ionic mobility. When aspirants prepare using strong and weak electrolyte conductivity mcqs, they gain clarity about how ionic dissociation affects current flow in aqueous systems.

Strong electrolytes are substances that completely dissociate into ions in aqueous solution. Examples include HCl, NaCl, KNO₃, and other soluble salts. Because they produce a large number of ions per unit volume, their conductivity is high. This is one of the primary ideas tested repeatedly in strong and weak electrolyte conductivity mcqs. The presence of freely moving ions allows efficient transport of charge through the solution.

Weak electrolytes, on the other hand, partially dissociate in water. Common examples include acetic acid (CH₃COOH) and ammonium hydroxide (NH₄OH). Since only a fraction of the molecules ionize, the total number of charge carriers is much lower compared to strong electrolytes. This difference forms the conceptual backbone of many strong and weak electrolyte conductivity mcqs.

Specific conductivity (κ) depends on the number of ions present in a given volume of solution. Strong electrolytes generally show high specific conductivity at moderate concentrations. However, as dilution increases, specific conductivity decreases because the number of ions per unit volume decreases. These dilution-based trends are frequently analyzed in strong and weak electrolyte conductivity mcqs to test conceptual understanding.

Molar conductivity (Λm) behaves differently. For strong electrolytes, molar conductivity increases slightly with dilution due to reduced interionic interactions. For weak electrolytes, molar conductivity increases sharply with dilution because ionization increases significantly. This sharp increase is a central focus area in strong and weak electrolyte conductivity mcqs, as it highlights the contrast between complete and partial dissociation.

The Debye–Hückel–Onsager equation describes the variation of molar conductivity with concentration for strong electrolytes. Weak electrolytes, however, follow Ostwald’s dilution law. Aspirants often encounter theory-based questions derived from these relationships while practicing strong and weak electrolyte conductivity mcqs.

Another critical factor is degree of dissociation (α). For weak electrolytes, α increases with dilution, leading to higher molar conductivity. For strong electrolytes, α is nearly 1 even at moderate concentrations. The link between α and conductivity is a recurring concept emphasized in strong and weak electrolyte conductivity mcqs.

Temperature also plays a role. As temperature increases, ionic mobility increases due to decreased viscosity of the solvent. Both strong and weak electrolytes show increased conductivity at higher temperatures, though the mechanism differs slightly. Temperature dependence is another commonly tested idea in strong and weak electrolyte conductivity mcqs.

Graphical interpretation is equally important. A plot of molar conductivity versus √C for strong electrolytes yields a straight line with a negative slope. For weak electrolytes, the curve is non-linear. Recognizing these graphical differences is essential when solving strong and weak electrolyte conductivity mcqs.

Limiting molar conductivity (Λm°) represents molar conductivity at infinite dilution. At this stage, ions behave independently. Strong electrolytes approach Λm° smoothly, whereas weak electrolytes require extrapolation due to incomplete ionization at higher concentrations. Many conceptual applications of Λm° appear in strong and weak electrolyte conductivity mcqs.

Strong and Weak Electrolyte Conductivity MCQs with Answers

1. Zeta potential is:
A. Potential required to bring about coagulation of a colloidal sol
B. Potential required to give the particle a speed of 1 cm s⁻¹
C. Potential difference between fixed charged layer and the diffused layer having opposite charges
D. Potential energy of the colloidal particles
Answer: C

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2. The molar conductivity of 0.007 M acetic acid is 20 S cm² mol⁻¹. What is the dissociation constant of acetic acid?
A. 2.5 × 10⁻⁵ mol⁻¹ L
B. 2.50 × 10⁻⁴ mol⁻¹ L
C. 1.75 × 10⁻⁴ mol L⁻¹
D. 1.75 × 10⁻⁵ mol⁻¹ L
Answer: D

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3. Given λ°Mg²⁺ = 106 and λ°SO₄²⁻ = 160 S cm² mol⁻¹. The value of λ°MgSO₄ is:
A. 271.6
B. 266
C. 390
D. 126
Answer: B

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4. Molar conductivities of KCl, NaCl and KNO₃ are 100, 120 and 90 S cm² mol⁻¹. Molar conductivity of NaNO₃ is:
A. 110
B. 290
C. 310
D. 120
Answer: A

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5. Conductivity of HCl solution is ___ × 10⁻² S m⁻¹:
A. 57
B. 56
C. 58
D. 59
Answer: A

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6. Molar conductivity of BaSO₄ at infinite dilution is:
A. 280
B. 426
C. 288
D. 860
Answer: C

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7. Molar conductivity of AgCl is:
A. 121.6
B. 111.4
C. 130.6
D. 150.2
Answer: A

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8. Electrolyte X is:
A. HCl
B. NaCl
C. KNO₃
D. CH₃COOH
Answer: D

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9. False statement is:
A. Ionic mobilities increase with T
B. CBaSO₄(T₂) > CBaSO₄(T₁)
C. CNaCl(T₂) > CNaCl(T₁)
D. CNaCl >> CBaSO₄ at given T
Answer: D

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10. Same value for constant A in Debye-Huckel-Onsager equation:
A. MgSO₄, NaSO₄
B. NH₄Cl, NaBr
C. NaBr, MgSO₄
D. NaCl, CaCl₂
Answer: B

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11.  Which among the following statements is incorrect for interstitial compounds?
(i) They are very hard and rigid
(ii) They have higher melting point than pure metal
(iii) They do not show conductivity
(iv) They are chemically reactive
Answer: D

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12. Cell constant is:
A. 1.1
B. 1.29
C. 0.56
D. 2.8
Answer: B

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13. Molar conductivity is:
A. 5.0 ohm⁻¹ cm² mol⁻¹
B. 5.0 ohm⁻¹ cm¹ mol⁻¹
C. 2.5 ohm⁻¹ cm¹ mol⁻¹
D. 2.0 ohm⁻¹ cm¹ mol⁻¹
Answer: A

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14. Conductivity decreases on dilution due to:
A. Decrease in number of ions per unit volume
B. Increase in ionic mobility
C. Increase in percentage ionisation
D. Increase in number of ions
Answer: A

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15. S₁: Conductivity always increases with decrease in the concentration of electrolyte.
S₂: Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the following is
A. S₁ true, S₂ false
B. S₁ false, S₂ true
C. Both true
D. Both false
Answer: B

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16. Degree of dissociation is:
A. 0.28
B. 0.3
C. 0.5
D. 0.125
Answer: D

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17. Decreasing order is:
A. A > C > B
B. C > B > A
C. B > C > A
D. A > B > C
Answer: A

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18. Conductivity corresponds to:
A. 1:1 electrolyte
B. 1:2 electrolyte
C. 1:3 electrolyte
D. 1:4 electrolyte
Answer: B

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19. Least conductivity complex:
A. Penta aqua chloro chromium (III) chloride
B. Tetra aqua dichloro chromium (III) chloride
C. Hexa aqua dichloro chromium (III) chloride
D. Tri aqua trichlorido chromium (III)
Answer: D

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20. Mass of silver deposited is:
A. 1.08 g
B. 10.8 g
C. 21.6 g
D. 108 g
Answer: B

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21. λ° CaCl₂ is:
A. 215
B. 340
C. 126
D. 261
Answer: D

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22. Ratio is:
A. 10⁵ cm³ mol⁻¹
B. 10³ cm³ mol⁻¹
C. 10 cm³ mol⁻¹
D. 10⁴ cm³ mol⁻¹
Answer: A

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23. Boiling point is:
A. 375.6 K
B. 376.3 K
C. 378.1 K
D. 380.3 K
Answer: A

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24. Molar conductivity is:
A. 5 × 10⁻³ S cm² mol⁻¹
B. 2 × 10⁻³ S cm² mol⁻¹
C. 200 S cm² mol⁻¹
D. 0.02 S cm² mol⁻¹
Answer: D

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25. Dissociation constant is:
A. 1.0 × 10⁻⁵
B. 2.25 × 10⁻⁴
C. 2.25 × 10⁻⁵
D. 2.25 × 10⁻³
Answer: C

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26. Not straight line graph:
A. HCl
B. NaCN
C. NaCl
D. HCN
Answer: D

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27. Least specific conductance:
A. 0.002 N
B. 0.1 N
C. 0.2 N
D. 2 N
Answer: A

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28. SI unit of conductivity