Asked by Bailey
I Just don't know what to do, I think I understand, but im not sure because all of the compounds are liquid. I would know how to do it if they were aqueous, and just the water is liquid, but they are all liquid.
Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH
of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is
CH3COOH(l) + H2O(l) H3O+(l) + CH3CO2-(l)
Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH
of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is
CH3COOH(l) + H2O(l) H3O+(l) + CH3CO2-(l)
Answers
Answered by
bobpursley
from your equation, let x be concentration of H3O+
ka=x^2/(.1-x)
but PH=2.37, or
x=10^-2.37
x^2=10^-4.74
ka= 1.81970086e-5/(.1-0.0043)
ka=0.00019014638=1.9e-4
ka=x^2/(.1-x)
but PH=2.37, or
x=10^-2.37
x^2=10^-4.74
ka= 1.81970086e-5/(.1-0.0043)
ka=0.00019014638=1.9e-4
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