Let's call CH3CH2COOH, just to save some time typing, HP.
HP ==> H+ + P^-
Ka = (H^+)(P^-)/(HP)
Initial concns:
(HP) = 1.97E-2
(H^+)= 0
(P^-) = 0
Equilibrium concns:
(H^+) = 5.00E-4
(P^-) = 5.00E-4
(HP) = 1.97E-2 - 5.00E-4
Plug those equilibrium values into the Ka expression and solve for K.
Calculate the equilibrium constant for the weak acid, CH3CH2CO2H, if the aqueous solution of CH3CH2CO2H that has an initial concentration of 1.97E-2 M has a [H+] of 5.00E-4.
CH3CH2CO2H <=> CH3CH2CO2 + H
i know that to figure out the equilibrium constant it is kc = products/reactants
and i have to do something with the ICE table...but i don't know how to apply it...
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