Determine the molar solubility of CaSO₄ in a solution containing 0.14 M Na₂SO₄.K_sp (CaSO₄)= 2.4 × 10^-5. A) 3.4 × 10^-6 M B) 1.7 × 10^-4 M C) 5.8 × 10^-10M D) 4.9 × 10^-3 M E) 0.10 M

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The balanced equation for the dissolution of CaSO₄ is: CaSO₄(s) ⇌ CaS1U1B2+(aq) + SO4S1U1B2-(aq) The solubility product expression is: Ksp = [CaS1U1B2+][SO4S1U1B2-] Let x be the molar solubility of CaSO₄ in mol/L. Then, at equilibrium: [CaS1U1B2+] = x [SO4S1U1B2-] = x Substituting into the Ksp expression, we get: Ksp = x^2 Ksp is given as 2.4 × 10^-5 and can be converted to: Ksp = 2.4 × 10^-5 Now, the problem also tells us that the solution contains 0.14 M Na₂SO₄. Since Na₂SO₄ is a soluble salt, it will dissociate completely in solution: Na₂SO₄(s) → Na+ + SO4S1U1B2- We can use stoichiometry to find the concentration of SO4S1U1B2- in solution, which is the same as [SO4S1U1B2-] for the dissolution of CaSO₄: [SO4S1U1B2-] = 0.14 M Now, we can use the Ksp expression to solve for x: Ksp = x^2 2.4 × 10^-5 = x^2 x = sqrt(2.4 × 10^-5) x = 1.55 × 10^-3 M Therefore, the molar solubility of CaSO₄ is 1.55 × 10^-3 M, which is equivalent to 1.55 × 10^-4 mol/L, or 1.55 × 10^-4 M. The closest answer choice is B, 1.7 × 10^-4 M.

Determine the Molar Solubility of CaSO4 in a Solution Containing

Determine the Molar Solubility of CaSO₄ in a Solution Containing