What is the pH of a 0.384 M aqueous solution of hydrofluoric acid? Ka (HF) = 7.1x10-4
The answer to this question is quite simple
We need to know 2 formulas
1
Ka = [H+] [F-] / [HF]
Since concentration Of [H+] and [F-] is same
So
Ka = [H+]2 / [ HF]
[ H+] = √ Ka × [HF]
[H+] = √ (0.384× 7.1×10-4)
[H+] = √ 0.00027264
= 0.016511814
Now we know
pH = -log[H+]
So
pH = -log [0.016511814]
= 1.78
So the pH of solution is
1.78
I hope this helps. If you have any query or want more detailed explanation, feel free to ask in the comments section below.
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