Kinetic Salt Effect - Size of Ions

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SUMMARY

The kinetic salt effect describes how the rate constant of a reaction varies with the ionic strength of a solution. It is established that ionic strength is influenced by molality and ion charges, but ionic radius does not significantly impact this effect. In the discussion, it is concluded that the kinetic salt effect will differ between solutions of 0.1 M NaCl and 0.1 M HCl due to the differing charge to mass ratios of the ions involved, particularly highlighting that hydrogen has a higher charge to mass ratio than sodium.

PREREQUISITES
  • Understanding of ionic strength and its calculation
  • Familiarity with the concept of rate constants in chemical reactions
  • Knowledge of the properties of ions, including charge to mass ratio
  • Basic grasp of molality and its role in solution chemistry
NEXT STEPS
  • Research the mathematical relationship between ionic strength and reaction rates
  • Explore the concept of charge to mass ratio in detail
  • Investigate the differences in ionic behavior between various salts and acids
  • Learn about the implications of ionic radius in solution chemistry
USEFUL FOR

Chemists, chemical engineers, and students studying reaction kinetics and solution chemistry will benefit from this discussion.

RandyP
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Hello,

Throwing out a question to see if anyone has some insight.

The kinetic salt effect describes the variation of the rate constant of a reaction with respect to the ionic strength of the solution. The mathematical relationship considers the ionic strength (molality/ion charges) of the solution, but as described there would be no effect of ionic radius. Does anyone know if ionic radius can play a role in this? For example, would the magnitude of the kinetic salt effect be identical for a solution of 0.1 M NaCl as it would for 0.1M HCl? Thanks
RP
 
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Probably not since the charge to mass ratio is higher for hydrogen than it is for sodium. That will affect the ionic strength of the solution.
 

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