K-value missing in acid-base problem?

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To determine the initial concentration of HF needed for a solution with a pH of 1.5, the Ka value of HF is essential. The discussion highlights that the K value for water is not relevant, and instead, the focus should be on the dissociation constant of HF. Participants suggest checking textbooks or resources for the Ka value if it hasn't been provided. Without this value, solving the problem accurately is challenging. Understanding the relationship between pH and concentration through the Ka value is crucial for finding the solution.
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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?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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