When 200 mL of 0.10 M BaCl₂ is added to 100 mL of 0.30 M Na₂SO₄, the number of moles of BaSO₄ (solubility product = 1.1 × 10^-10) precipitated is ________.

Question

Quizplus · Accepted Answer

The correct answer is A.The number of moles of BaSO4 precipitated can be calculated using the solubility product constant and the concentrations of the reactants. The solubility product constant for BaSO4 is 1.1 × 10^-10. The concentration of Ba2+ in the solution is 0.10 M and the concentration of SO42- in the solution is 0.30 M. The reaction between Ba2+ and SO42- is:Ba2+ + SO42- → BaSO4The number of moles of BaSO4 precipitated can be calculated using the following equation:Ksp = [Ba2+][SO42-]1.1 × 10^-10 = (0.10 M)(0.30 M)[BaSO4] = 3.7 × 10^-9 MThe number of moles of BaSO4 precipitated is:moles of BaSO4 = (3.7 × 10^-9 M)(0.200 L) = 0.020 mol

When 200 ML of 0