Help with Le Chatelier's Principle

Write the equalibrium equation for the ionization of acetic acid. What would happen to the concentration of acetic acid if sodium acetate is added to the solution? Suggest a method to verify your conclusion.

Thanks

You can write it any of these ways:

HC2H3O2 <------------> H+ + C2H3O2-
or, if you're an organic chemist
CH3COOH <-----------------> H+ + C2H3O2-

A Bronsted-Lowry enthusiast would write
HC2H3O2 + H2O <----------------> H3O+ + C2H3O2-
or
CH3COOH + H2O<------------> H3O+ + CH3COO-

If you added sodium acetate, you would be increasing the concentration of acetate ion, the C2H3O2-, and, from Lechatelier's principle, this would drive the reaction to the left increasing the concentration of molecular HC2H3O2. It would lower the concentration of H+ and therefore lower the pH, which is how you could verifty it - use a pH meter and check the pH before and after you add the sodium acetate.

HC2H3O2 --> H+ + C2H3O2-
1) adding NaC2H3O2 would cause a huge production of C2H3O2- but not from the acetic acid, this would remain as acetic acid due to the common ion effect and that NaC2H3O2 is much more soluble than HC2H3O2

NaC2H3O2 --> Na+ + C2H3O2-, the pH will be basic whereas the pH of acetic acid dissociation will be acidic

NaC2H3O2 + H2O --> HC2H3O2 + Na+ + OH-, pH > 7
HC2H3O2 + H2O --> H+ + C2H3O2-, pH < 7