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### Topic: solubility equilibrium  (Read 454 times)

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#### Luisa2901

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##### solubility equilibrium
« on: December 09, 2023, 12:49:57 PM »

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
« Last Edit: December 09, 2023, 01:02:14 PM by Luisa2901 »

#### Borek

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##### Re: solubility equilibrium
« Reply #1 on: December 09, 2023, 04:09:52 PM »
Acetic acid is a weak one, isn't it?
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#### Luisa2901

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##### Re: solubility equilibrium
« Reply #2 on: December 09, 2023, 05:18:55 PM »
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
« Last Edit: December 09, 2023, 06:12:15 PM by Luisa2901 »

#### Borek

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##### Re: solubility equilibrium
« Reply #3 on: December 09, 2023, 05:46:38 PM »
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.
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