Pb(NO3)2 + 2 AgI -> 2 AgNO3 + PbI2
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300.0 mL of 0.375 mol/L Pb(NO3)2 is mixed with 250.0 mL of 1.20 mol/L KI a) Write the balanced chemical equation (including states) for the reaction that occurs between Lead (II) Nitrate and Potassium Iodide. (2T) b) What is the Precipitate that forms (1T) c) What mass of precipitate will theoretically form? Include all your steps, sig figs and units. (6T, 1C)
Vishal S.
When 75.0 $\mathrm{mL}$ of a 0.100 $\mathrm{M}$ lead(Il) nitrate solution is mixed with 100.0 $\mathrm{mL}$ of a 0.190 $\mathrm{M}$ potassium iodide solution, a yellow-orange precipitate of lead(II) iodide is formed. (a) What mass in grams of lead(II) iodide is formed, assuming the reaction goes to completion? (b) What is the molarity of each of the ions $\mathrm{Pb}^{2+}, \mathrm{K}^{+}, \mathrm{NO}_{3}$ , and $\mathrm{I}^{-}$ in the resulting solution?
When $75.0 \mathrm{~mL}$ of a $0.100 \mathrm{M}$ lead(II) nitrate solution is mixed with $100.0 \mathrm{~mL}$ of a $0.190 \mathrm{M}$ potassium iodide solution, a yelloworange precipitate of lead(II) iodide is formed. (a) What mass in grams of lead(II) iodide is formed, assuming the reaction goes to completion? (b) What is the molarity of each of the ions $\mathrm{Pb}^{2+}, \mathrm{K}^{+}, \mathrm{NO}_{3}^{-}$, and I in the resulting solution?
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