Why Do Different Electrolytes Have Varying Molar Conductivities?

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Different electrolytes exhibit varying molar conductivities due to their degree of dissociation in water, with strong electrolytes like HCl and NaCl fully dissociating, while weak electrolytes like acetic acid (CH3COOH) only partially dissociate. The molar conductivities provided indicate that strong acids and bases have higher values compared to weak acids. To calculate the degree of dissociation (alpha) and the dissociation constant (K) for CH3COOH at a concentration of 0.6, the molar conductivity of 195.3 S.Cm2/mol can be used in conjunction with relevant formulas. Understanding these concepts is crucial for solving related exercises and determining equilibrium constants. The discussion highlights the importance of clarity in questions and the need for detailed calculations.
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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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