Why Do Different Electrolytes Exhibit Varying Molar Conductivities?

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SUMMARY

The discussion focuses on the varying molar conductivities of strong and weak electrolytes, specifically analyzing HCl, CH3COONA, HF, and NaCl. The molar conductivities provided are 426.1 S·cm²/mol for HCl, 91.05 S·cm²/mol for CH3COONA, 405 S·cm²/mol for HF, and 126.5 S·cm²/mol for NaCl. Factors influencing these differences include ion mobility, solvent shell size, and hydrogen bonding capabilities. Additionally, the calculation of the degree of dissociation (α) and the dissociation constant (K) for acetic acid (CH3COOH) at a concentration of 0.6 M is requested, with a molar conductivity of 195.3 S·cm²/mol.

PREREQUISITES
  • Understanding of strong and weak electrolytes
  • Knowledge of molar conductivity and its significance
  • Familiarity with ionic conductivity formulas
  • Basic principles of ion mobility and solvent interactions
NEXT STEPS
  • Calculate the degree of dissociation (α) for acetic acid (CH3COOH) using the provided molar conductivity
  • Research the relationship between ion mobility and solvent shell size
  • Explore the concept of hydrogen bonding and its effect on ionic conductivity
  • Learn about the dissociation constant (K) for weak electrolytes and its calculation methods
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Chemistry students, educators, and researchers interested in electrolyte behavior, ionic conductivity, and the principles of dissociation in solutions.

physicist888
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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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