Problem: A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.Determine the percent yield.

FREE Expert Solution

Recall molarity (M):

molarity(M)=moles soluteL solution


2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)


Calculate the mass of PbCl2 produced from each reactant:

PbCl2 from KCl

molar mass PbCl2 = 278.1 g/mol

mass PbCl2=27.6 mL×10-3 L1 mL×1.62 mol KCl1 L                                 ×1 mol PbCl22 mol KCl×278.1 g PbCl21 mol PbCl2

mass PbCl2 = 6.21 g


PbCl2 from Pb(NO3)2

molar mass PbCl2 = 278.1 g/mol

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Problem Details
A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:

2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)


The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

Determine the percent yield.

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