Dilution & Strength: Is More Concentrated Better?

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SUMMARY

The discussion centers on the comparison of dilute and concentrated acids, specifically addressing the misconception that a dilute acid is stronger than a concentrated one. According to Ostwald's dilution law, the degree of dissociation for dilute acids is higher, making them better electrolytes. However, the pH of concentrated acids is significantly higher, indicating greater acidity. The relationship between concentration and strength is clarified through the equation Ka=(conc.)*alpha*alpha, leading to the conclusion that concentrated acids are indeed stronger despite the higher dissociation in dilute solutions.

PREREQUISITES
  • Understanding of Ostwald's dilution law
  • Knowledge of acid dissociation constants (Ka)
  • Familiarity with pH calculations
  • Basic concepts of electrolytes and their behavior
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  • Research the implications of Ostwald's dilution law in practical applications
  • Study the relationship between pH and concentration in various acid-base reactions
  • Explore the concept of weak vs. strong electrolytes in detail
  • Learn about the calculation of acid dissociation constants (Ka) for different acids
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Chemistry students, educators, and professionals in the field of chemical engineering or analytical chemistry who seek to deepen their understanding of acid strength and electrolyte behavior.

aim1732
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Is it right to say that a dilute acid is stronger than the same acid which has higher molarity?
By Ostwald's dilution law I can say that dissociation degree for the dilute sample is more. So it is a better electrolyte. But I also find that pH for concentrated sample is appreciably more.
Ka=(conc.)*alpha*alpha(for weak electrolytes)
So [H+]=sqrt(Ka*conc.)
Actually I can not stomach what I have heard-that a dilute acid is stronger than its concentrated counterpart. I have always thought the more concentrated the stronger it is.
 
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Hey! I'm very very sorry that I cannot help you with your problem but I was just wondering if you could help me out very quickly? I would like to post a question of my own but I'm having trouble finding out where to do so!
So sorry for the unhelpful post, good luck though! :)
 
SoConfused__ said:
Hey! I'm very very sorry that I cannot help you with your problem but I was just wondering if you could help me out very quickly? I would like to post a question of my own but I'm having trouble finding out where to do so!
So sorry for the unhelpful post, good luck though! :)


Never mind. Please check your Member Profile.
 

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