A researcher filled a 5.00 L flask with water and slowly added small amounts of CaC₂O₄. A small amount of precipitate was noticed after 0.0305 grams were added. What is the maximum value of K_sp for this compound?

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Quizplus · Accepted Answer

The solubility product (Ksp) is calculated using the concentration of ions at equilibrium. The molar mass of CaC2O4 is approximately 128.1 g/mol. The moles of CaC2O4 added is 0.0305 g / 128.1 g/mol = 2.38×10^-4 mol. In a 5.00 L solution, the concentration is 4.76×10^-5 M. Since CaC2O4 dissociates into Ca^2+ and C2O4^2-, Ksp = [Ca^2+][C2O4^2-] = (4.76×10^-5)^2 = 2.3×10^-9.

A Researcher Filled a 5