A student mixed 5.00 ml of 0.0120 M Pb(NO3)2 with 4.00 mL of 0.0300 M KI and 1.00 mL of 0.20 M KNO3 and observed the formaton of a yellow precipitate. Show all calculations. The concentration of I- at equilibrium is experimentally determined to be 6.5E-5 a. How many moles of I- precipitated? b. How many moles of Pb2+ remain in solution? c. What is the concentration of Pb2+ in the equilibrium solution? (The volume of the equilibrium solution is still 10 ml) d. Determine Ksp of
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A student mixed 5.00 ml of 0.0120 M Pb(NO3)2 with 4.00 mL of 0.0300 M KI and 1.00 mL of 0.20 M KNO3 and observed the formaton of a yellow precipitate. Show all calculations.
The concentration of I- at equilibrium is experimentally determined to be 6.5E-5
a. How many moles of I- precipitated?
b. How many moles of Pb2+ remain in solution?
c. What is the concentration of Pb2+ in the equilibrium solution? (The volume of the equilibrium solution is still 10 ml)
d. Determine Ksp of PbI2 from this data. Show all work please.
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