Question
I've a solution 0.002M of Pb(NO3)2:
What is the minimum concentration of iodide ions (I-) necessary to observe the precipitation of PbI2?
What mass of KI should be added to observe the precipitation of PbI2 from the 25 mL volume lead nitrate solution?
What is the minimum concentration of iodide ions (I-) necessary to observe the precipitation of PbI2?
What mass of KI should be added to observe the precipitation of PbI2 from the 25 mL volume lead nitrate solution?
Answers
................Pb(NO3)2 ==> Pb^2+ + 2NO3^-
I...............0.002..................0............0
C............-0.002.............0.002.......0.002*2
E.................0.................0.002.......0.004
..........PbI2 ==> Pb^2+ + 2I^-
Ksp = (Pb^2+)(I^-)^2
Look up Ksp and substitute.
You know (Pb^2+) from the Pb(NO3)2 equilibrium.
Solve for (I^-) in mols//L. Convert to mols/25 mL. Convert to grams KI/25 mL.
Post your work if you get stuck.
I...............0.002..................0............0
C............-0.002.............0.002.......0.002*2
E.................0.................0.002.......0.004
..........PbI2 ==> Pb^2+ + 2I^-
Ksp = (Pb^2+)(I^-)^2
Look up Ksp and substitute.
You know (Pb^2+) from the Pb(NO3)2 equilibrium.
Solve for (I^-) in mols//L. Convert to mols/25 mL. Convert to grams KI/25 mL.
Post your work if you get stuck.
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