Which of the following result(s) is/are correct for the equilibrium state in a solution originally having 0.1M−CH3COOH and 0.1M−HCl? Ka of CH3COOH=1.8×10−5.
A
[H+]=0.1M
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B
[CH3COO−]=1.8×10−5M
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C
Degree of dissociation of acetic acid =1.8×10−4
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D
[H+] from water 10−13M
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Solution
The correct option is A[H+]=0.1M [H+]=0.1M→H+Concentration The introduction of HCl into an acetic acid solution would shift the equilibrium of the acetic acid forward forming less ions. This is Le-Chatlier's principle, since acetic acid is weak acid.