If the initial concentrations are {Pb (CH3CO2) 2} = 0.165 M and {NH4I} = 0.466 M, how many grams of PbI2 will precipitate out of solution?

76.065 g of PbI2.

Explanation:

Equation of the reaction:

Pb (CH3CO2) 2 (aq) + 2NH4I - -> PbI2 (s) + 2NH4 (CH3CO2) (aq)

Given:

Pb (CH3CO2) 2 = 0.165 M

NH4I = 0.466 M

Since molar concentration = number of moles/volume

Calculating the number of moles of the limiting reagent,

0.165 moles of Pb (CH3CO2) 2 in 0.466 moles of NH4I all in the same volume of solution and by stoichiometry, since 1 mole of Pb (CH3CO2) 2 reacts with 2 moles of NH4I.

Therefore, Pb (CH3CO2) 2 is the limiting reagent.

Using stoichiometry, 1 mole of Pb (CH3CO2) 2 reacted to form 1 mole of PbI2 precipitate.

Number of moles of PbI2 = 0.165 moles

Molar mass of PbI2 = 207 + (127 * 2)

= 461 g/mol

Mass = molar mass * number of moles

= 461 * 0.165

= 76.065 g of PbI2.