Which of the following statements is incorrect with respect to the plot of molar conductivity (Λm) versus square root of concentration (1/√c) for electrolytes in solution?
For strong electrolytes, a straight line with positive slope is obtained.
The graph of **molar conductivity (Λm)** versus the square root of concentration (**1/√c**) shows different behaviors for strong and weak electrolytes:
- For **strong electrolytes**, the plot typically gives a straight line with a **negative slope**, as the molar conductivity decreases with the square root of the concentration. This is because as the concentration decreases, the ions become more dissociated, leading to a decrease in conductivity at low concentrations.
- For **weak electrolytes**, the relationship is not linear, and hence a straight line is not obtained.
- For **strong electrolytes**, the graph is expected to show a straight line with a **negative slope**, and the extrapolated intercept represents the limiting molar conductivity (**Λm0**).
Therefore, the incorrect statement is **Option 3**: **For strong electrolytes, a straight line with positive slope is obtained** (this is not true; the slope is negative).
Important Questions from Electrochemistry
What is the numerical value of one Faraday in Coulombs?
Which term of molar conductivity is used when the concentration of electrolyte approaches zero?
Kohlrausch law is related to which of the following term?
Identify transition metal complexes which are not octahedral in shape.
(A) [Co(NH₃)₆]³⁺
(B) [Ni(CO)₄]
(C) [CoCl(NH₃)₅]²⁺
(D) [CoCl₂(NH₃)₄]⁺
(E) [PtCl₄]²⁻
Choose the correct answer from the options given below:
The product of complete hydrolysis of XeF₆ in the following reaction is:
XeF₆ + H₂O → ? HF
