You have 0.5 L of air at 203 k in an expendable container at constant pressure. You heat the container to 273 k. What is the vol
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The question is incomplete, complete question is :
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that x is small? ( for HF is
.)
[HF] = 0.280 M
Express your answer to two decimal places.
Answer:
The pH of an 0.280 M HF solution is 1.87.
Explanation:3
Initial concentration if HF = c = 0.280 M
Dissociation constant of the HF =
Initially
c 0 0
At equilibrium :
(c-x) x x
The expression of disassociation constant is given as:
Solving for x, we get:
x = 0.01346 M
So, the concentration of hydrogen ion at equilibrium is :
The pH of the solution is ;
The pH of an 0.280 M HF solution is 1.87.
Answer:
of HA is 6.80
Explanation:
Acid dissociation constant () of HA is represented as-
Where species inside third bracket represents equilibrium concentrations
Now, plug in all the given equilibrium concentration into above equation-
So,
Hence