Why Do Different Electrolytes Have Varying Molar Conductivities?

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SUMMARY

The discussion focuses on the varying molar conductivities of different electrolytes, specifically highlighting strong electrolytes like HCl, NaCl, and weak electrolytes such as CH3COOH. Strong electrolytes dissociate completely in water, resulting in higher molar conductivities, while weak electrolytes only partially dissociate, leading to lower conductivities. The limiting molar conductivities provided are 426.1 S·cm²/mol for HCl, 126.5 S·cm²/mol for NaCl, and 91.05 S·cm²/mol for CH3COONA. The exercise also involves calculating the degree of dissociation (α) and the dissociation constant (K) for CH3COOH at a concentration of 0.6 M.

PREREQUISITES
  • Understanding of strong and weak electrolytes
  • Knowledge of molar conductivity and its significance
  • Familiarity with the concept of degree of dissociation (α)
  • Basic skills in equilibrium constant calculations
NEXT STEPS
  • Calculate the degree of dissociation (α) for CH3COOH using the formula α = (Λm / Λ°) where Λm is the molar conductivity and Λ° is the limiting molar conductivity.
  • Research the dissociation constant (K) for weak acids and how to derive it from molar conductivity.
  • Explore the differences in dissociation behavior between strong acids and bases versus weak acids.
  • Study the impact of concentration on the conductivity of electrolytes.
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Chemistry students, educators, and professionals interested in understanding electrolyte behavior, conductivity measurements, and acid-base dissociation principles.

physicist888
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strong and weak electrolytes-need help pleasez

hi all
i need help to solve the following exercise

Given: strong electrolyt limiting molar conductivity of ion i ( S.Cm2/mol)
HCl 426.1
CH3COONA 91.05
HF 405
NaCl 126.5
1- why did thos electrolyts has a different molar conductivity?
2- calculate the degree of dissociation alpha and the constant of dissociation K for a weak electrolyt CH3COOH dilute at 0.6. given the molar conductivity equal 195.3 Cm2/mol. (show the calculation in details)
 
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Why does everyone have questions like these? :(
 
Are there any formulas? And are you calculating the equillibrium constant? Please re-write the question clearer with units. I will try to help you o:)


I think the answer to the first question is because strong acids such as HCL and HF dissociate completely in water making them strong electrolytes. NaCl is a strong base so it also dissociates completely in water. Weak acids such as carboxylic acids dissociate partially in water giving them a weaker electrical current.
 

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