4. The following precipitation reaction can be used to determine the amount of copper ions dissolved in solution.
A chemist added 5.00 × 10−2 L of a solution containing 0.173 mol L−1 Na3PO4(aq) to a 5.00 × 10−2 L sample containing CuCl2(aq). This resulted in a precipitate. The chemist filtered, dried, and weighed the precipitate. If 1.21 g of Cu3(PO4)2(s) were obtained, and assuming no copper ions remained in solution, calculate the following:
a. the concentration of Cu2+(aq) ions in the sample solution.
b. the concentrations of Na+(aq), Cl−(aq), and PO43−(aq) in the reaction solution (supernatant) after the precipitate was removed.