Calculate the solubility of Ag₂SO₄ [K_sp = 1.2 × 10^-5] in a 2.0 M AgNO₃ solution. A) 6.0 × 10^-6 mol/L B) 1.2 × 10^-5 mol/L C) 3.0 × 10^-6 mol/L D) 1.4 × 10^-2 mol/L E) none of these

Question

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The solubility product constant (Ksp) for Ag₂SO₄ is given as: K_sp = 1.2 × 10^-5 The balanced equation for the dissolution of Ag₂SO₄ in water is: Ag₂SO₄(s) ⇌ Ag+ (aq) + S1U1B2O4S2- (aq) Using the 2.0 M AgNO3 solution, we can assume that the initial concentration of Ag+ ions is 2.0 M. We can use an ICE table to determine the final concentration of Ag+ ions and S2- ions at equilibrium: | | Ag+ | S1U1B2O4S2- | |-------|----------|-------------| | I | 2.0 M | 0 | | C | -x | +x | | E | 2.0 - x | x | The solubility product expression is: K_sp = [Ag+][S1U1B2O4S2-] = (2.0 - x)(x) Substituting the value of Ksp and solving for x gives: 1.2 × 10^-5 = (2.0 - x)(x) x = 3.0 × 10^-6 Therefore, the solubility of Ag₂SO₄ is 3.0 × 10^-6 mol/L in a 2.0 M AgNO3 solution. The correct choice is C.

Calculate the Solubility of Ag2SO4 [Ksp = 1

Calculate the Solubility of Ag₂SO₄ [K_sp = 1