Balanced equation: K2SO4(aq) + Pb(C2H3O2)2(aq) → 2 KC2H3O2(aq) + PbSO4(s)
Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters).
Determine the limiting reactant, which is the reactant that forms the less amount of product.
Molar mass PbSO4 = 303.26 g/mol
The mass of PbSO4 formed by 57.5mL sample of a 0.112 M K2SO4 is:
You may want to reference (Pages 152 - 157)Section 4.4 while completing this problem.
A 57.5mL sample of a 0.112 M potassium sulfate solution is mixed with 35.0mL of a 0.110 M lead(II) acetate solution and the following precipitation reaction occurs:
K2SO4(aq) + Pb(C2H3O2)2(aq) → 2 KC2H3O2(aq) + PbSO4(s)
The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the theore©tical yield.
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