K-value missing in acid-base problem?

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SUMMARY

The discussion centers on calculating the initial concentration of hydrofluoric acid (HF) needed to achieve a pH of 1.5. The key point raised is the necessity of the acid dissociation constant (Ka) for HF, which is essential for solving the problem. Participants emphasize the importance of consulting a reliable source for the Ka value of HF, as it is not provided in the original question. The correct application of the Ka value is crucial for determining the concentration accurately.

PREREQUISITES
  • Understanding of acid-base chemistry, specifically pH calculations.
  • Familiarity with the concept of acid dissociation constants (Ka).
  • Knowledge of hydrofluoric acid (HF) properties and behavior in aqueous solutions.
  • Ability to use equilibrium expressions in chemical calculations.
NEXT STEPS
  • Research the Ka value of hydrofluoric acid (HF) from reliable chemical databases.
  • Learn how to calculate pH from concentration using the formula pH = -log[H+].
  • Study the principles of chemical equilibrium and how they apply to weak acids.
  • Explore additional resources on acid-base titration and its calculations.
USEFUL FOR

Chemistry students, educators, and professionals involved in chemical analysis or laboratory work, particularly those focusing on acid-base reactions and pH calculations.

alingy2
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What initial concentration of HF (aq) in water would give a solution with a pH = 1.5?

I think the K value is missing... How could we solve this problem?
 
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alingy2 said:
What initial concentration of HF (aq) in water would give a solution with a pH = 1.5?

I think the K value is missing... How could we solve this problem?

Hey there!
I'm sure you know the K of water - what you're looking for is the Ka value of HF. Have you not been given the value?
 
Is there a table of Ka values in your book?
 

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