What is the concentration of [Ag⁺] in a saturated solution of Ag₂SO₄? The K_sp of Ag₂SO₄ is 1.50 × 10⁻⁵.

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The solubility product (Ksp) for Ag2SO4 is given as 1.50 × 10^−5. The dissociation of Ag2SO4 in water can be represented as Ag2SO4(s) ⇌ 2Ag+(aq) + SO4^2−(aq). From the stoichiometry of the dissolution, for every mole of Ag2SO4 that dissolves, 2 moles of Ag+ ions are produced. Let the solubility of Ag2SO4 be S mol/L. Then, the concentration of Ag+ ions will be 2S and the concentration of SO4^2− ions will be S. The Ksp expression is Ksp = [Ag+]^2[SO4^2−] = (2S)^2(S) = 4S^3. Substituting the given Ksp value, we get 4S^3 = 1.50 × 10^−5. Solving for S gives S ≈ 0.0155 M. Since the concentration of Ag+ ions is twice the solubility of Ag2SO4, the concentration of Ag+ in the solution is 2 × 0.0155 M = 0.0310 M.

What Is the Concentration of [Ag+] in a Saturated Solution

What Is the Concentration of [Ag⁺] in a Saturated Solution