You might develop a table like this one: Is the ionization of acetic acid a rela

Question

You might develop a table like this one: Is the ionization of acetic acid a relatively complete reaction, or is it a partial one that represents an equilibrium? What general pattern do you observe in the concentration of acetic acid versus pH? Compare the relationship among the three values ([H^+], [C2H3O2^-], [H C2H3O2]) for each initial concentration of acetic acid. Try different mathematical operations (multiply, divide, etc.). You can try multiplying all three or a combination of multiplying and dividing (i.e., dividing one by the product of the other two, etc.).

Explanation / Answer

Acetic acid will form the next equilibrium:

HAc <-> H+ and Ac-

Ka = [H+][Ac-]/[HAc]

NOTE

for every 1 mol of HAc you will have in solution 1 mol of H+

therefore, the concentration of H+ is always hte same as Ac-

The concentration of HAc is always that of the initial concentration minus the concentration in equilibrium:

Then #)

NOTE i will supose pH and [H+] data is correct

1) M= 0.1 pH = 3.18; [H+] = 6.6*10^-4 ; Since [H+] = [Ac] = 6.6*10^-4 ; [HAc] = M - [H+] = 0.1 -6.6*10^-4

2) M= 0.01 pH = 3.28; [H+] = 5.25*10^-4 ; Since [H+] = [Ac] = 5.25*10^-4 [HAc] = M - [H+] = 0.01 -5.25*10^-4

3) M = 0.001 pH= 3.83; [H+] = 1.48*10^-4 ; Since [H+] = [Ac] = 1.48*10^-4 [HAc] = M - [H+] = 0.001 -1.48*10^-4

4) M= 0.0001 pH= 5.42; [H+] = 3.8*10^-6 ; Since [H+] = [Ac] = 3.8*10^-6 ; [HAc] = M - [H+] = 0.0001-3.8*10^-6

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