Why Do Different Electrolytes Exhibit Varying Molar Conductivities?

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Different electrolytes exhibit varying molar conductivities due to factors such as ion mobility and the size of solvent shells surrounding the ions. Strong electrolytes like HCl and NaCl show higher conductivities compared to weak electrolytes like CH3COOH, which have lower degrees of dissociation. The degree of dissociation (alpha) and dissociation constant (K) can be calculated using the molar conductivity values provided. Ionic conductivity is influenced by the ability of ions to move freely in the solvent, with smaller ions typically exhibiting greater mobility. Understanding these principles is crucial for analyzing electrolyte behavior in solutions.
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strong and weak electrolytes-need help pleasez

hi all
i need help to solve the following exercise

Given: those are a strong electrolyt limiting , and we give the molar conductivity for each ion in ( 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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The conductivities here are ionic in nature. That is, the conduction requires that the ion be mobile in the solvent. Ions with smaller solvent shells will be more mobile than ions with larger solvent shells. Ions that form better hydrogen bonds will conduct better than those that form weaker hydrogen bonds.

Show me the formula for ionic conductivity that has the K term for dissociation contained within and we can talk about the second question.
 

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