Calculate the solubility of silver oxalate, ag2c2o4, in pure water. ksp = 1.0 × 10-11 a. 1.4 × 10-4 m b. 8.2 × 10-5 m c. 5.4 × 10-5 m d. 3.2 × 10-6 m e. 2.5 × 10-12 m

Chemical reaction (dissociation) of silver oxalate in water: 
Ag₂C₂O₄(s) → 2Ag⁺(aq) + C₂O₄²⁻(aq).
Ksp(Ag₂C₂O₄) = [Ag⁺]²·[C₂O₄²⁻].
[C₂O₄²⁻] = x; solubility of oxalate ion.

[Ag⁺] = 2[C₂O₄²⁻] = 2x
1.0·10⁻¹¹ = (2x)² · x = 4x³.

x = ∛1.0·10⁻¹¹ ÷ 4.

x = 1.4·10⁻⁴ M.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

the product of the pressure and volume is also constant