Back to notes
Differentiate between strong and weak electrolytes with examples.
Press to flip
Strong electrolytes (e.g., NaOH, KCl) dissociate nearly completely in solution, whereas weak electrolytes (e.g., CH₃COOH, NH₃) only partially dissociate.
Provide an example of a strong electrolyte and explain why it is classified as such.
Hydrochloric acid (HCl) is an example of a strong electrolyte because it dissociates nearly 100% into its ions (H⁺ and Cl⁻) in solution.
Describe the relationship between conductance (G), conductivity (κ), and the dimensions of the cell (l and A).
Conductance (G) is related to conductivity (κ) and the dimensions of the cell by the formula G = κ × (l/A), where l is the distance between electrodes and A is the cross-sectional area.
How does the conductivity (κ) of an electrolyte solution change with ion concentration and temperature?
Conductivity typically increases with higher ion concentration and increased temperature as both factors facilitate better ion mobility.
What is the inverse relationship between conductance and resistance?
Conductance (G) is the inverse of resistance (R), given by G = 1/R.
How does molar conductivity (Λm) change with dilution, and why?
Molar conductivity (Λm) increases with dilution because the ions in solution experience less interaction with each other, enhancing their mobility.
Why is detailed understanding and practice important in mastering electrochemistry?
Because electrochemistry involves complex concepts and calculations that are crucial for exams such as JEE Mains, NEET, and EAMCET, understanding and practice help ensure clarity and proficiency.
What is the defining difference between electrolytes and non-electrolytes?
Electrolytes dissociate into ions in solution, allowing the solution to conduct electricity, whereas non-electrolytes do not dissociate into ions and do not conduct electricity.
What factors affect the conductance of an electrolyte solution?
Factors affecting conductance include the number of ions present, the mobility of the ions, the nature of the electrolyte, ion concentration, and temperature.
Calculate the molar conductivity if the conductivity (κ) of a solution is 0.05 S/cm and its molarity (M) is 0.01 M.
Using the formula Λm = κ × 1000/M, we get Λm = 0.05 × 1000/0.01 = 5000 S cm² mol⁻¹.
Define molar conductivity (Λm) and its relation to conductivity (κ) and molarity (M).
Molar conductivity (Λm) is the conductivity of an electrolyte solution divided by its molarity (M). It is given by the formula: Λm = κ × 1000/M.
Explain how to calculate equivalent conductivity (Λeq) given conductivity (κ) and normality (N) of the solution.
Equivalent conductivity (Λeq) can be calculated using the formula Λeq = κ × 1000/N.
What role does resistivity (ρ) play in determining conductivity (κ)?
Conductivity (κ) is the reciprocal of resistivity (ρ), given by κ = 1/ρ.
Explain the significance of the cell constant in calculating conductivity.
The cell constant accounts for the geometry of the container in which the conductivity is measured and is used to convert measured conductance (G) to conductivity (κ) using the formula κ = G × (l/A).
What are the units of molar conductivity and equivalent conductivity?
The units of molar conductivity (Λm) are S cm² mol⁻¹, and the units of equivalent conductivity (Λeq) are S cm² equivalent⁻¹.
Previous
Next