HC2H3O2 (aq)  ↔  C2H3O2- (aq) + H+ (aq)   At equilibrium at 25 ºC, a 0.100 M solution of acetic acid has the following concentrations:   [HC2H3O2] = 0.0990 M   [C2H3O2-] = 1.33×10-3 M     [H+] =  1.33×10-3 M     Please determine the equilibrium constant, Keq for the reaction above at 25 ºC.

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Acetic acid is a well-known weak acid.  Weak acids are acids that only partially dissociate.  Thus acetic acid can dissociate into the acetate ion and a proton in aqueous solution.  The relevant chemical reaction is below:  


HC2H3O2 (aq)  ↔  C2H3O2- (aq) + H+ (aq)  


At equilibrium at 25 ºC, a 0.100 M solution of acetic acid has the following concentrations:  


[HC2H3O2] = 0.0990 M  


[C2H3O2-] = 1.33×10-3 M  

 

[H+] =  1.33×10-3 M  

 

Please determine the equilibrium constant, Keq for the reaction above at 25 ºC.  

 

Question 2 options:

 

A) 

5.71×104

 

B) 

0.100

 

C) 

1.75×10-7

 

D) 

1.79×10-5

 

E) 

5.71×106

 

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