Electrolytic Conductance of Acids, Bases, and Salts
Chemistry ⇒ Acids, Bases, and Salts
Electrolytic Conductance of Acids, Bases, and Salts starts at 10 and continues till grade 12.
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See sample questions for grade 11
A solution of acetic acid shows much lower conductance than that of HCl at the same concentration. Give a reason.
A student measures the conductance of 0.1 M NaCl and 0.1 M CH₃COOH. The conductance of NaCl is much higher. Explain why, based on the nature of the electrolytes.
Describe how you would determine the molar conductance at infinite dilution for a weak electrolyte using Kohlrausch’s Law.
Explain the difference between specific conductance and molar conductance.
Explain why the conductance of a 0.1 M NaOH solution is higher than that of a 0.1 M NH₄OH solution.
Explain why the conductance of a solution increases with dilution.
Explain why the molar conductance of strong electrolytes increases only slightly with dilution, while that of weak electrolytes increases sharply.
If the specific conductance of a 0.01 M KCl solution is 0.00141 S cm⁻¹ and the cell constant is 1.1 cm⁻¹, what is the measured conductance?
State Kohlrausch’s Law of Independent Migration of Ions.
The conductance of a solution increases with temperature. State one reason for this observation.
Explain why the molar conductance of a strong electrolyte approaches a limiting value at infinite dilution, but does not increase indefinitely with further dilution.
State and explain the effect of temperature on the electrolytic conductance of a salt solution.
