5.00 mL of 0.0120 M Pb(NO2)2 are mixed with 3.00 mL 0.0300 M KI. And diluted to a final volume of 10.00 mL with KNO3 solvent. A yellow precipitate of PbI2 forms. The precipitate is separated from the supernatant solution which is analyzed for [I-]. The concentration of I- in the test solution is calculated from the graph to be 1.82 x 10-3 M.
Calculate the following:
a. Initial [Pb+2] (after mixing but before precipitating)
b. Initial [I-] (after mixing but before precipitating)
c. Equilibrium [I-] = (graph [I-] x 10.0 mL/3.00 mL)
d. [I-] reacted to form precipitate
e. [Pb+2] reacted to form precipitate
f. Equilibrium [Pb+2]
g. Ksp of PbI2
h. Tube #1 is analyzed by taking 3.00 mL of the saturated solution of PbI2 and treating it with acid and KNO2 and diluted to 10.00 mL. This diluted solution is then analyzed in a spectrophotometer and found to have [I-] of 1.59 x 10-3 M using the regression equation from the graph. Calculate the Ksp of PbI2 using this data.