Problem- Part A) In your experiment one of the reagents was limiting and the other was in excess. Therefore after the lead(II)iodide precipitated from the solution, there were spectator ions left in the solution and also the unreacted excess reagent. Assuming complete precipitation of lead (II) iodide, calculate the concentrations of each type of ion (Pb2+, K+, NO3-, I-) present in the solution after the PbI2 precipitated out.

Reaction is: Pb(NO3)2(aq) + 2KI(aq) ---> PbI2(s) + 2KNO3(aq)

2.0 ml of 0.250M Pb(NO3)2 and 7.0 ml of 0.250M KI

Part B) Chemists always report the yield (as a %) when they perform a reaction, because it shows how efficient the reaction is as a method of preparing the desired product. When would it be important to report both the total yield and the isolated yield of a reaction? In general, does it matter very much for reactions in lab experiments?

Justify your solution