[Luisa2901]

Do you have any suggestions about this question?

Calculate the mass of solid sodium acetate that must be added to 200 mL of a solution containing 0.200 mol/L silver nitrate and 0.100 mol/L nitric acid so that silver acetate (Ksp = 2.30x10^-3) begins to precipitate.

I know that AgNO3 is a soluble salt and HNO3 is a strong acid, so the initial concentrations of Ag+ and H+ will be 0.2 mol/L and 0.1 mol/L. I am having trouble figuring out how the H+ of the acid will affect the equilibrium.

Nac2h3O2---> Na+ + C2H3O2-
C2H302- +Ag+ ---> AgC2H302

[Borek]

Acetic acid is a weak one, isn't it?

[Luisa2901]

So I have to consider that C2H302- will react with the H+ of HNo3 to form acetic acid?

Nac2h3O2---> Na+ + C2H3O2-
x                         x        x

C2H302- + H+---> HC2H3O2   K=1/ka (acetic acid)
     x          0.1         0
     -y         -y          y
    x-y        0.1-y       y

C2H302- +Ag+ ---> AgC2H302
  x-y -z     0.2- z                             

[Borek]

So I have to consider that C2H302- will react with the H+ of HNo3 to form acetic acid?

Yes.

Not sure what you are trying to do with z, you are looking for the moment where nothing precipitated yet.